Metals and nonmetals The Basics Reactivity Reactions with metals The Periodic Table is divided into…. Metals The Periodic Table is divided into…. and non-metals Metals all have similar physical properties… •They.
Download ReportTranscript Metals and nonmetals The Basics Reactivity Reactions with metals The Periodic Table is divided into…. Metals The Periodic Table is divided into…. and non-metals Metals all have similar physical properties… •They.
Slide 1
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 2
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 3
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 4
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 5
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 6
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 7
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 8
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 9
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 10
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 11
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 12
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 13
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 14
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 15
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 16
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 17
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 18
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 19
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 20
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 21
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 22
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 23
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 24
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 25
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 26
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 27
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 28
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 29
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 30
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 31
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 32
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 33
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 34
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 35
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 36
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 37
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 38
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 39
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 40
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 41
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 2
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 3
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 4
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 5
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 6
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 7
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 8
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 9
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 10
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 11
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 12
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 13
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 14
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 15
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 16
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 17
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 18
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 19
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 20
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 21
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 22
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 23
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 24
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 25
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 26
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 27
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 28
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 29
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 30
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 31
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 32
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 33
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 34
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 35
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 36
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 37
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 38
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 39
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 40
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.
Slide 41
Metals and nonmetals
The Basics
Reactivity
Reactions
with metals
The Periodic Table is divided into….
Metals
The Periodic Table is divided into….
and non-metals
Metals all have similar
physical properties…
•They have high melting and boiling points (except mercury)
•They conduct electricity and heat.
•They have a high density.
•They are shiny (lustrous).
•They are malleable (can be moulded)
•They are ductile (can be stretched)
Non-metals….
• Have low melting and boiling points.
• Are brittle.
•
Do not conduct heat or electricity well.
(except carbon)
Different metals are suitable for
different jobs.
Gold, silver and platinum are very unreactive but very
malleable - making them suitable for jewellery
Copper is malleable, ductile and it conducts heat
and electricity well.
It is also unreactive making it suitable
for holding and carrying water.
Aluminium is a reactive
metal, but it forms a
coating of very stable
aluminium oxide.
This, together with its lightness and malleability
gives it many uses from window frames to
insulation foil.
Iron ore is common
and iron itself is
very strong.
It can be moulded into
many shapes
As it forms, iron oxide
constantly flakes away
exposing more of the iron
underneath.
Remember:
Unfortunately iron is quite
brittle (for a metal) and also
oxidises (rusts) easily.
Only iron oxide is called
rust.
No other metal rusts!
Like aluminium, zinc oxidises
to form a stable coating of
zinc oxide which protects the
iron underneath it.
This is called galvanising.
To prevent this happening,
iron is often covered with a
thin layer of zinc.
Lead is very dense, unreactive and
malleable - making it suitable for fishing
weights and roof sealing.
Lead fumes have been linked
to brain damage so it is now
considered too toxic to be
used inside houses (e.g. as in
old-fashioned water pipes)
Back
Sodium, Calcium and Magnesium
These three metals are all far too reactive to be
much use in their pure form.
They all make important compounds though.
Sodium
Sodium metal is so reactive it has to be kept in oil to keep
it away from the oxygen in the air..
Without the oil, sodium quickly oxides into useless sodium
oxide
All the same, sodium is essential for both plants and animals.
The commonest source of sodium is common table salt –
Sodium Chloride.
Calcium
Calcium is less reactive than sodium, but it still oxidises
too rapidly for the pure metal to have any uses.
Calcium compounds, however, are very important.
Calcium carbonate makes up about 10% of the earth’s surface
– limestone, marble and chalk.
Calcium compounds are essential for life – such as for making
bones and milk.
Magnesium
Magnesium is less reactive then sodium or calcium.
It is still too reactive to have any uses in its pure form though.
Magnesium is easily obtainable from salts in sea water
Amongst other things, magnesium is essential for making
chlorophyll.
…. so Group 1
metals are the
most reactive
Reactivity
Metals get more reactive as you
move left in the periodic table
…They also get
more reactive
as you go down
the table
Reactivity
Group 1 metals are
the most reactive.
Reactivity
then Group 2
and potassium
is more
reactive
than
sodium
Reactivity
These
group 1
metals
are too
reactive
to be
allowed
in labs.
On the other hand, its difficult
to get copper and zinc to do
anything!
Metals all form
(They do this by LOSING electrons)
Most non- metals form
(They do this by GAINING electrons)
Groups 1 – 13 form positive ions
Na+
Mg2+
Al3+
Group 14 elements don’t form ions
This is because they have 4
electrons in their outer shell. It
isn’t easier to gain 4 more or
lose 4 - so they don’t do either!
Groups 15, 16 and 17 all gain electrons to form negative ions
N3S2-
Cl-
Group 18 elements don’t form ions either.
This is because they already have
the full 8 electrons in their outer
shell.
3
11
Li
Na
Group 1 metals all
have one electron in
their outer shell.
19
K
Rb
Cs
Fr
They can lose this
electron to form a
1+ positive ion
For instance:
3
11
Li
Na
lithium
lithium + electron
ion
19
K
Li
Li+
+
Rb
Cs
Fr
+
e-
3
11
Li
Na
19
K
Rb
Cs
Fr
+
Li+
3
11
Li
Na
19
K
Rb
Cs
Fr
Li+
+
Na+
3
11
Li
Li+
Na
Na+
19
K
Rb
Cs
Fr
K+
+
3
11
Li
Li+
Na
Na+
19
K
K+
Rb
Rb+
Cs
Cs+
Fr
Fr+
4
12
Be
Mg
20
Ca
2+
Group 2 metals
have 2 electrons
in their outer
shell….
Sr
Ba
Ra
Be
2+
Mg
Ca
Sr
….. so they
form 2+ ions
Ba
Ra
2+
2+
2+
2+
Some metals, like iron, can form
2+ or 3+ ions
Fe
Fe2+
+
2 e-
Fe
Fe3+
+
3 e-
Non-metals can form two
types of ion:
Monatomic ions
Polyatomic ions
(the ion is made from just
one non-metal element)
(the ion is made from more than one
non-metal element)
Cl - = chloride
I - = iodide
Br - = bromide
OH-
= hydroxide
SO42NO -
= sulphate
= nitrate
O 2- = oxide
S 2- = sulphide
CO32-
= carbonate
3
HCO32- = hydrogen carbonate
Metal and non-metals join together to
make IONIC compounds.
2Cu
copper
Mg
magnesium
+ O2
oxygen
+ Cl2
chlorine
2CuO
copper oxide
MgCl2
magnesium
chloride
Reactions with Metals.
1. Metals react with oxygen to from oxides.
2. Metals react with water to form hydroxides and
hydrogen gas.
3. Metals react with acids to form salts and hydrogen
gas.
1. Metals react with oxygen (O2) to
form oxides.
sodium
4Na
+
calcium
+
2Ca
+
iron
+
4Fe
+
+
oxygen
O2
oxygen
sodium oxide
2Na2O
calcium oxide
2CaO
oxygen
iron oxide
3O2
2Fe2O3
O2
2. Metals react with water to produce
hydroxides and hydrogen gas.
sodium hydroxide + hydrogen gas
sodium
+
water
2Na
+
2H2O
calcium
+
water
calcium hydroxide + hydrogen gas
Ca
+
2H2O
2NaOH
Ca(OH)2
+
+
*Soluble hydroxides are called alkalis*
H2
H2
3. Metals react with acids to form
salts and hydrogen gas
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
potassium + sulphuric acid potassium sulphate + hydrogen
2K
+
H2SO4
K2SO4
+
H2
Naming Salts
The metal forms the first
part of the salt’s name.
potassium + hydrochloric acid potassium chloride + hydrogen
2K
+
2HCl
2KCl
+
H2
The non-metal forms
the second part of the
salt’s name.