Transcript Day 6 Bonding Atoms. HONORS
Slide 1
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 2
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 3
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 4
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 5
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 6
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 7
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 8
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 9
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 10
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 11
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 12
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 13
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 14
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 15
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 16
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 17
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 18
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 19
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 2
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 3
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 4
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 5
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 6
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 7
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 8
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 9
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 10
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 11
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 12
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 13
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 14
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 15
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 16
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 17
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 18
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements
Slide 19
Identify elements by their properties and
placement on the periodic table.
On the periodic table:
The horizontal rows are called ____________
The vertical columns are called ___________
Links:
What Holds a Molecule Together?
Ionic Bonding: Interactive Tutorial
- Ionic Bonds
Ionic Bonds
• You and a friend walk past a market that
sells apples for 40 cents each and pears for
50 cents each. You have 45 cents and want
an apple. Your friend also has 45 cents but
wants a pear.
Atoms like to have a filled
outer shell of electrons.
Sometimes, by transferring
electrons from one atom to
another, electron shells are
filled. The atom that gives
away an electron will take
a positive charge, and the
receiving atom will have a
negative charge. The
charged atoms or ions will
be attracted to each other,
and form bonds.
- Ionic Bonds
Ions and Ionic Bonds
• Ionic bonds form as a result of the
attraction between positive and negative
ions.
Ionic compounds and ionic bonding
When metals react with non-metals, electrons are transferred
from the metal atoms to the non-metal atoms, forming ions. The
resulting compound is called an ionic compound.
Consider reactions between metals and non-metals, for example
•sodium + chlorine
sodium chloride
•magnesium + oxygen
magnesium oxide
•calcium + chlorine
calcium chloride
In each of these reactions, the metal atoms give electrons to the
non-metal atoms, so that the metal atoms become positive ions
and the non-metal atoms become negative ions. There is a strong
electrostatic force of attraction between these oppositely-charged
ions, called an ionic bond. The animation shows ionic bonds
being formed in sodium chloride, magnesium oxide and calcium
chloride.
- Ionic Bonds
Properties of Ionic Compounds
• In general, ionic compounds are hard, brittle
crystals that have high melting points. When
dissolved in water or melted, they conduct
electricity.
Some atoms like to share
electrons to complete their outer
shell. Like this oxygen atom. It
needs 2 electrons to follow the
2/8/8 rule. In this case to make
water, you would need 2
hydrogen atoms. By sharing
electrons the hydrogen atom is
also able to complete it’s electron
shell. Hydrogen bonds are
primarily covalent bonds and a
regular covalent bond is very
strong.
Oxygen
- Covalent Bonds
How Covalent Bonds Form
• The force that holds atoms together in a
covalent bond is the attraction of each atom’s
nucleus for the shared pair of electrons.
- Covalent Bonds
How Covalent Bonds Form
• The oxygen atom in water and the nitrogen atom in
ammonia are each surrounded by eight electrons as
a result of sharing electrons with hydrogen atoms.
- Covalent Bonds
How Covalent Bonds Form
• An oxygen molecule contains one double bond,
while a carbon dioxide molecule has two double
bonds. A nitrogen molecule contains one triple
bond.
Covalent compounds - simple molecules
Covalent bonds form between non-metal atoms. Each bond consists of a shared
pair of electrons, and is very strong. Covalently-bonded substances fall into two
main types:
1.simple molecules, and
2.giant covalent structures.
Simple molecules
These contain only a few atoms held together by strong covalent bonds. An
example is carbon dioxide (CO2), whose molecules contain one atom of carbon
bonded with two atoms of oxygen.
Hydrogen chloride, ammonia, methane, chlorine, and water are also
examples of simple molecules with covalent bonds. All these substances
have very strong bonds between the atoms, but much weaker forces
holding the molecules together. When one of these substances melts or
boils, it is these weak 'intermolecular forces' that break, not the strong
covalent bonds. This means that simple molecular substances are gases,
liquids or solids with low melting points and low boiling points.
On the Inside
• BY YOURSELF complete BOTH sides
of the “On the Inside” worksheet.
You do NOT have to draw the Oxygen
Atom
GO ON
Website
Click the link below & then click LAUNCH
http://www.pbslearningmedia.org/resource/ls
ps07.sci.phys.matter.theatom/the-atom/
Now try this more challenging website &
click on ATOM BUILDER ACTIVITY
http://www.pbs.org/wgbh/aso/tryit/atom/#
**Hint: Use “The Atom Builder Guide”
links at bottom of page for help
Interactive Periodic Table Game
CLICK ON PICTURE:
___Ductile
c
Able to be pulled into
a long wire
d
___Malleable
___Brittle
g
Able to be
hammered or rolled
into a shape
Easily broken and is not
able to be molded or
shaped
___
k Conductor of
electricity
Allows
electricity to
flow freely
___
l Conductor
of heat
Allows heat to flow
freely
n
___Dull
Not shiny
___Soft
m
Not hard
i
___Shiny
Lusterous
at a high temp.
___
h high boiling Boils
so is usually a liquid
point
at room temperature
Melts at high temp.
j
___High melting so is usually a solid
point
at room temperature
___
f Semiconductor
a
___Opaque
Will carry electricity
only under certain
conditions
Not clear or
transparent
___Density
b
___Reactive
e
D=M÷V,
determines is it
will sink or float
Will quickly &
easily combine
with other
elements