Atomic Timeline (AKA The 7 Dead Dudes of Atomic Theory) Timeline Construction • Use the adding machine tape to make your Atomic Timeline •
Download ReportTranscript Atomic Timeline (AKA The 7 Dead Dudes of Atomic Theory) Timeline Construction • Use the adding machine tape to make your Atomic Timeline •
Slide 1
Atomic Timeline
(AKA The 7 Dead Dudes of Atomic Theory)
Slide 2
Timeline Construction
• Use the adding machine tape to make your
Atomic Timeline
• Make sure you include…
•
•
•
•
Name
Date
Important Information
Picture/or/Symbol
Slide 3
1) Democritus – 460 BC
• First to develop the idea that matter was
made of particles called Atoms
• The term “Atoms” comes from the Greek
word “atomos” which means “undivisible”
Slide 4
2) John Dalton - 1803
• Proposed atomic theory
• An atom is indivisible, indestructible, tiny
sphere.
• Determined that elements have unique
atomic masses
Slide 5
3) Joseph John Thomson - 1898
• Discovered Electrons
• Proposed an atomic model known as the “plum
pudding” model
Slide 6
4) Ernest Rutherford - 1911
• Discovered positively charged nucleus by
probing atoms of gold foil with positively
charged particles.
• Proposed atomic model with massive nucleus
with electrons in a circle around it in a solar
system model
Slide 7
5) Niels Bohr - 1913
• Developed atomic model that placed
electrons in specific energy levels to explain
why they did not spiral toward and collide
with the nucleus
• Proposed the model with electrons in specific
orbits around the nucleus
Slide 8
6) James Chadwick - 1932
• Discovered neutron as a neutral particle in
the nucleus
• The discovery explained why the mass of an
atom could not be attributed entirely to the
mass of the protons
Nucleus
(+) Positive Protons
(0) Neutral Neutrons
Slide 9
7) Erwin Schrodinger – 1933
• Described electrons as waves with their
probable location viewed as a cloud and
introduced a mathematical model of the
atom
e-
Slide 10
Highlights
1. Democritus
First – Atomos - Indivisible
2. John Dalton
Atomic Theory
3. J.J. Thomson
Electrons - “Plum Pudding”
4.
5.
6.
7.
+ Charged Nucleus – Gold Foil
Electrons Specific NRG Levels
Neutrons (Jimmy Neutron)
Electron Cloud Wave
Ernest Rutherford
Niels Bohr
James Chadwick
Erwin Schrodinger
Slide 11
Way to Remember the Order of the
Scientists for the Atomic Theory…
•
•
•
•
•
•
•
Democritus Democritus
Discovered Dalton
Tiny Thomson
Round Rutherford
Circular Chadwick
Ball-like Bohr
Spheres Schrodinger
Slide 12
Indivisible Electron
Greek
Dalton
Nucleus
Orbit
Electron
Cloud
X
X
Thomson
X
Rutherford
X
X
Bohr
X
X
Wave
X
X
X
X
Slide 13
Don’t Sweat the
Small Stuff!
Slide 14
Size of Atoms
• Tiny!
• Tinier than the cells and germs.
• Too small to be seen with ordinary
microscopes
• Atoms are so small that it would take 100
million atoms placed side by side to form a
row only 1 cm long which is about the width
of your pinky finger!
Slide 15
How Small is the Small Stuff?
• Let’s check it out…
• http://www.micro.magnet.fsu.edu/primer/jav
a/scienceopticsu/powersof10
• http://www.cellsalive.com/howbig.htm
• http://www.strangematterexhibit.com/struc
ture.html
• http://learn.genetics.utah.edu/content/begin
/cells/scale/
• http://www.azonano.com/Details.asp?Article
ID=1780
Slide 16
What’s the Matter?
Matter
Slide 17
What’s the Matter?
“Stuff” that
Everything
is made of!
Made of
Atoms
Matter
Has Mass=
The Amount
of Matter
in an Object
Has Volume=
Takes Up
Space
Slide 18
What was the “Small Stuff” anyway?
•Atoms
•Elements
•Molecules
•Compounds
Slide 19
Atoms
• Basic unit of matter
• The smallest particle of a substance that has
all of the properties of that substance.
• Example= the element Gold is made of gold
atoms
Slide 20
Elements
• A pure substance made of only one kind of
atom.
• Examples= Gold, Hydrogen, Carbon, etc.
• Elements are found on the Periodic Table of
Elements.
• Here is a song about them…
http://www.privatehand.com/flash/elements.h
tml
Slide 21
Molecules
• Made up of two or more atoms joined tightly
together.
• Small particle of the entire substance or
compound
• Atoms in a molecule may be of the same
element or of different elements.
• Examples= 1 molecule of the element oxygen
or 1 molecule of the compound water H2O
Slide 22
Compounds
• A substance whose molecules contain atoms
of different elements combined chemically.
• Most matter exists as compounds.
• Examples= Water, Carbon Dioxide, etc.
Slide 23
What is the difference between a
Compound and a Molecule?
• A molecule is formed when two or more
atoms join together chemically.
• Molecules can be made up of atoms joined
together or elements joined together which
form compounds
• A compound is a molecule that contains at
least two different elements.
Slide 24
Compound vs. Molecule
• All compounds are molecules but not all
molecules are compounds!
• Molecules that are made of two atoms joined
together are not compounds
• Compound = entire substance
• Molecule = small particle of entire substance
Slide 25
Atom
•Smallest part of a substance
•Has all of the properties of that substance
Molecule
Element
•Pure Substance
•Made of 1 kind
of atom
•2 or more atoms
joined tightly
together
•Smallest part
of compound
Compound
•Molecules
containing
atoms
of different
elements
Slide 26
Atom
• Smallest part of a
substance
• Has all of the properties
of that substance
Slide 27
Element
• Pure Substance
• Made of 1 kind of
atom
Slide 28
Molecule
•2 or more atoms
joined tightly
together
•Smallest part
of compound
Slide 29
Compound
• Molecules containing
atoms of different
elements
Slide 30
Chemical Bonding
•
Elements bond together to form compounds
•
2 Main Types of Bonding…
1. Colvalent = sharing of e-
1. Ionic = giving or taking of e-
Slide 31
Covalent Bonding = Sharing e• Covalent Bond= sharing of electrons that
occurs between 2 non-metals
Ex) Water H2O
H
= Hydrogen’s Electron
O
H
= Oxygen’s Electrons
Slide 32
Ionic Bonding = give or take eIonic Bond= giving or taking of electrons that
occurs between metals and non-metals
Ex) Salt NaCl – Na give outer e- to Cl
Na
Na1+
Cl
Cl1-
Slide 33
Ions
• An ion is an atom or molecule which has lost
or gained one or more electrons, making it
positively or negatively charged.
• A negatively charged ion, which has more
electrons in its electron shells than it has
protons in its nuclei, is known as an anion
• Conversely, a positively-charged ion, which
has fewer electrons than protons, is known
as a cation
Slide 34
Ions (con’t)
• An ion consisting of a single atom is called a
monatomic ion, but if it consists of two or
more atoms, it is a polyatomic ion. Polyatomic
ions containing oxygen, such as carbonate
and sulfate, are called oxyanions.
• Ions are represented by the presence of a
superscript indicating the sign of the net
electric charge and the number of electrons
lost or gained, if more than one. For example:
H+ and SO42−.
Slide 35
Elements in the Earth & Air
1.
2.
3.
4.
5.
6.
7.
Element
Oxygen
Silicon
Aluminum
Iron
Calcium
Potassium
Sodium
Symbol
Use
O
Breathing
Si
Glass/Rocks
Al
Foil/Cans
Fe
Steel
Ca
Bones/Teeth
K
Bones/Muscles
Na
Salt
Slide 36
Elements In Our Bodies
Ca 1.6%
N 2.4%
Other 3.3%
H 10.2%
C 17.5%
O 65%
Slide 37
Nucleus
P+
&
NO
1st = 2 e2nd = 8 e3rd = 18 e-
Slide 38
Periodic Table
• Atomic # = # of p+ = # of e• # of n0 = Atomic Mass – Atomic #
• Period #s = # of orbitals/shells
• 7 Periods = 7 shell max
Slide 39
“Playing” with the Periodic Table…
• Draw the orbitals on your paper plate
• Use play-doh to represent protons, neutrons,
and electrons
• Choose a different color for each
• Start with simple elements and work your
way up!
Slide 40
Nucleus
P+
&
NO
1st = 2 e2nd = 8 e3rd = 18 e-
Slide 41
Acting Out Bohr
Models!
Nucleus
P+
&
NO
1st = 2 e2nd = 8 e3rd = 18 e-
Slide 42
Periodic Tables
• Check out the Periodic Table in Pictures and
in Words
• Use your other Periodic Table to Color Code
the Metals, Nonmetals, and Metalloids
• On the other side, color code the
Groups/Families
Slide 43
Slide 44
Awesome Websites…
•
•
•
•
•
•
•
•
•
http://www.visual-literacy.org/periodic_table/periodic_table.html
http://www.everypoet.com/absurdities/elements/
http://sciencespot.net/Pages/kdzchem2.html
http://www.middleschoolscience.com/chemistry.htm
http://www.middleschoolscience.com/atomicmusicalchairs.pdf
http://www.science-class.net/Chemistry/Chemistry.htm
http://elements.wlonk.com/Elements_Pics_11x8.5.pdf
http://elements.wlonk.com/Elements_Words_11x8.5.pdf
http://www.learner.org/interactives/periodic/index.html
Slide 45
Blue= Metals
Pink= Metalloids
Yellow= Nonmetals
Slide 46
How to Read the
Periodic Table
Tracy Arrington-Payne
SI560
Slide 47
The Periodic Table Is . .
• A table of all known elements,
• A useful tool for scientists,
• And, it arranges elements according
to their properties.
Slide 48
The Inventor
• Created by Dmitri Mendeleev.
• Mendeleev was a teacher who
was discouraged by his teaching
tools and decided to create his
own.
• He made note cards of the
elements known at that time and
arranged them. When there
wasn’t an element to fit a certain
spot, he left it open and
predicted an element would be
found later to fill it.
Slide 49
Reading a Periodic Table
• When reading a periodic table . . . .
–
–
–
–
Look at the box
Look at the columns (group or family)
Look at the rows (periods)
Look at the location of metals, nonmetals, and
semiconductors
Slide 50
Using the Box
• Each box represents a different element.
• Each box contains information that tells . .
–
–
–
–
The elements name
The elements symbol
The atomic number of the element
The atomic weight of the number
Slide 51
Example
• Name – Oxygen
Oxygen
8
• Atomic Number – 8
• Atomic Symbol – O
• Atomic Weight – 16.00
O
16.00
Slide 52
Using the Columns
• Each column of elements is called a family or
group.
• Elements in a family have similar but not
identical properties.
• The number for the column sometimes
indicates the number of electrons in outer
shells of the element.
• Elements in a group have the same number of
electrons in their outer orbital.
Slide 53
Families or Groups
•Elements in the red group
have 1 electron in their outer
shell.
•Elements in the orange
group have 2 electrons in
their outer shell.
•As you keep counting the
colored columns, you add an
additional electron.
•Purple has 8 electrons in its
outer shell.
•(Don’t include the white
group)
Slide 54
Slide 55
Using the Rows
• Rows represent an elements period.
• Elements in a period are not alike in
properties.
• Even though some squares are skipped in
between, all of the rows go from left to
right.
Slide 56
Using the Rows
• As a rule. . . .
– the first element in a period is usually an active
solid.
– the last element in a period is always a noble gas.
• Atomic size decreases from left to right
across a period.
• And generally, atomic mass increases form
left to right across a period, although there
are exceptions.
Slide 57
Example
•Every element in the top
row (first period) has one
orbital for its electrons.
•Every element in the
second row (the second
period) have two orbitals
available.
•Atoms on the left are
usually larger and lighter.
•Atoms on the right are
usually smaller and heavier.
Slide 58
Slide 59
Metals, Nonmetals, and
Semiconductors
Some periodic tables are color coded to show what
elements are metals, nonmetals, and
semiconductors.
In general, elements located in the left two-thirds
or so of the periodic table are metals. The
nonmetals are on the right side of the table.
The dividing line between the metals and
nonmetals are elements called semiconductors.
Slide 60
The gray area represents the metals.
The yellow area represents the semiconductors.
The blue area represents the nonmetals.
Slide 61
Conclusion
• The Periodic Table is an excellent tool for
looking at elements and the key to using it is
to understand the code of it structure.
• Using the boxes, columns, and rows will help
you learn about the properties of elements.
Slide 62
I. Metals, Metalloids, and Non-Metals
II. 7 Periods/Rows
III. 18 Groups/Families
Slide 63
I. Metals, Metalloids, & Non-Metals
Metals
left
• On the _______ of the staircase/zig-zag
(except for hydrogen)
• Most are shiny, hard, and dense.
• They conduct (transmit) electricity and heat.
high melting and
• They have mostly _______
boiling points.
• They are malleable (pounded into shapes) and
ductile (drawn into wire).
• Ex) Aluminum is a metal that is pounded into
aluminum foil.
Slide 64
Metalloids
on
• 7 elements _____
the staircase/zig-zag
both
• Properties of _______
metals and nonmetals.
• Ex) Silicon is a metalloid. It conducts
electricity like a metal and is brittle like a
non-metal. It is used to make microchips.
Slide 65
Non-Metals
right of the staircase/zig-zag
• To the _______
• Most have low melting points
• Are dull and brittle if solid.
poor
• Most are _______
conductors of heat and
electricity.
• Ex) Sulfur is a non-metal. It is often used to
make fertilizer.
Slide 66
II. 7 Periods/Rows
The Period # = the # of Electron
Shells/Orbitals/Energy Levels
1. This period contains the two __________
lightest
known elements, hydrogen (H) and helium (He).
Each element has 2 electron shell.
2. The elements in this period have 2 electron
shells. The gases that make up most of our
____________,
atmosphere nitrogen(N) and oxygen(O),
are found in this period.
3 electron
3. The elements in this period have ___
shells. Sodium (Na) and chlorine(Cl) are found
in this period.
Slide 67
4. The elements in this period have 4 electron
shells. This period includes the element iron
(Fe), a commonly used _____.
metal
5. The elements in this period have 5 electron
shells. Silver (___)
Ag is found in this period
6. With 6 electron shells, some of these
__________
heavier elements are unstable and
radioactive. This period includes gold (Au),
lead (Pb) and radioactive radon (Rn).
7. With 7 electron shells, these are the
heaviest elements. Many are
________________
- some so unstable
radioactive
that they fall apart almost instantly.
Uranium (U) is found in this period
Slide 68
III. 18 Columns/Groups/Families
1.
2.
3.
4.
5.
6.
7.
8.
Alkali Metals
Alkaline Earth Metals
Transition Metals
BCNO Family
Halogens
Noble Gases
Lanthanides
Actinides
Slide 69
1. Alkali Metals – Group 1 (far left of table)
• The metals are Lithium, Sodium, Potassium, Rubidium,
Cesium, and Francium.
• Hydrogen, a non-metal, is in the family because of its
reactivity
________________.
electron in their outer shells.
• All have 1 __________
• They are all soft and very reactive.
↑ as we read down the table.
• Their reactivity ___
• They so reactive because they have 1 valence electron
that can easily be given away.
• All of these metals are soft, silvery white, with low
melting points.
blow
up
• Hydrogen will _______
____
upon any contact with
flames.
burn the skin if
• The metals are so reactive they will _______
touched.
Slide 70
1. Alkali Metals (con’t)
• They tarnish rapidly and react violently with
water
__________.
salts
• They easily form _______
with the halogens.
never found in their pure forms in nature,
• They are _______
only found as compounds
• The metals in this family are easy to identify because
colors
they give off a different _________
when burned:
Lithium = crimson, Sodium = yellow, Potassium = violet,
Rubidium = reddish-violet, Cesium = blue, and Francium =
Rare Little is Known
Uses
• Important _________Lithium = Grease, Lubricants,
Aircraft Parts, & Batteries, Sodium = Salt and Gasoline,
Potassium = More Expensive than Na & less widely used
but used in fertilizer and photography.
Slide 71
2. The Alkaline Earth Metals – Group 2
• 6 metals: Berylium, Magnesium, Calcium,
Strontium, Barium, and Radium.
soft
• Are _______
and bright silvery-white in color.
high
• Have high melting points and _______
densities.
2 electrons in their outer shells.
• All have ___
• Are all reactive and react with water.
less
• Are __________
reactive than the alkali metals.
↑ as we read down the
• Have reactivity that ___
table.
• Will oxidize or tarnish in air, but can be handled
humans
by __________.
• Are __________
never found in nature in their pure
forms.
Slide 72
2. Alkaline Earth (con’t)
– Are good conductors of electricity
– Burn in different colors: Magnesium = Bright White,
Calcium = Orange-Red, Strontium = Bright Red,
Barium = Yellowish-Green, and Radium = Crimson
fireworks because of their bright colors
– Used in ____________
– Beryllium is often added to other metals to make hard
alloys
metal __________,
used to make rocket nose cones,
and in nuclear reactors.
– Magnesium is used in aircraft and photographic
equipment.
– Calcium is used with other metals to make reactive
alloys.
– Radium is radioactive and is used in the treatment of
cancer
__________.
Slide 73
3. The Transition Metals – Groups 3-12
largest family on the Periodic Table with 40
• The __________
members.
• Some of the more common and widely used members of
this family include iron, nickel, copper, zinc, silver, and
gold.
metals
• They are all __________hard, shiny, and strong.
• Fairly stable, reacting slowly or not at all with air and
water.
• Most of them have very _______
high melting points and
boiling points.
Mercury is one exception- it is a liquid at room
• ____________
temperature.
• Most are good ____________
conductors of heat and electricity.
• Most will dissolve in an acid, however, __________
gold
resists acids.
oxygen
• Most can bond to _________
in more ways than one,
making different compounds.
Slide 74
3. Transition Metals (con’t)
• Most can be pounded into sheets or shapes
ductile
(____________)
or drawn into a wire (____________)
malleable
• Most can form colored compounds with oxygen.
strong
• Many can form __________
metal alloys (a mixture of
metals).
• Form a bridge between the very reactive metals on the
left side and the less reactive metals on the right.
• Very similar so that it is difficult to detect differences
from one column to the next.
• First elements in groups 8,9, 10 called the iron triad
because they are the only ones known to create a
magnetic field.
• Many uses because of their properties- construction
materials, pipes, wires, coins, jewelry, aircrafts, cars,
bicycles, cooking utensils, paints, cleaners, etc.
Slide 75
4. The BCNO Family – Groups 13-16
25 members
• Large family with ___
• Some of the more common members of this family
include carbon, nitrogen, oxygen, aluminum, silicon, sulfur,
arsenic, tin, and lead.
divided
• This family is sometimes __________
into two or four
separate families.
diverse
• Most __________
family of elements.
lightest
• Name is from the ____________
of the elements in
each column- Boron, Carbon, Nitrogen, and Oxygen.
• There are metals, nonmetals, and metalloids in this family
gases
• Some members are _______
at room temp like nitrogen
solids
and oxygen, but most are __________.
Slide 76
4. The BCNO Family (con’t)
• They are reactive, but selective with which
bond
elements they will __________.
• Most will bond with oxygen & oxygen will bond
with __________
itself
bond
• Members of each column tend to _______
with
other elements in a similar fashion
• Oxygen supports combustion.
• Many uses- essential to life (carbon, oxygen,
nitrogen, and phosphorus), metals are used in
electronics, nonmetals are used as
insulators on wires, poisons, fertilizers, in
____________
scuba gear, soap, glass-making, solder, aircraft,
weapons, drink cans, foil, pots, and pans.
Slide 77
5. The Halogens – Group 17
• All have seven electrons in their outer shells and are
____________
poisonous non-metals.
• Most reactive of all nonmetals, but are poor conductors of
____________
electricity
down
• Their reactivity decreases as we read __________
the
table.
5 elements- fluorine,
• Very small family consisting of only ___
chlorine, bromine, iodine, and astatine
room temperature fluorine and chlorine are gases,
• At _______
bromine is a liquid, and iodine and astatine are solids
Very reactive and never found in their pure forms in
• ______
nature.
• Combine with alkali metals to form a family of chemical
salts
compounds - __________.
Slide 78
5. The Halogens (con’t)
• Fluorine is added to toothpaste and water to
prevent tooth decay and combines with uranium to
form __________
fuel.
nuclear
• Chlorine is added to water supplies and swimming
pools to kill germs. It is widely used in bleach and
salt.
Bromine
• ____________
is used as a gasoline additive,
photograph developer, fire retardant, and an
insecticide. It is also used to kill germs in water
supplies.
• Iodine is added to salt to reduce thyroid disease.
It is also used as a film developer and as a
disinfectant in water supplies.
no
• Astatine is very rare, very radioactive, and has ___
uses.
Slide 79
6. The Noble Gases - Group 18
• They are very non-reactive because they have
_____
outer shells…inert.
full
rarest
• These are some of the __________
and heaviest
elements.
• Six gases- helium, neon, argon, krypton, xenon, and
radon
Colorless tasteless, and odorless
• __________,
• Do not mix with others- do not gain, share, lose
electrons.
• Chemically stable because they have a full outer
energy level.
• Helium, neon, and argon will _____
not combine with
other elements
• Xenon, krypton, and radon will combine with other
elements, but difficult process.
Slide 80
6. The Noble Gases (con’t)
• When an electrical current is passed through one
of these gases it will glow in a characteristic
__________
ex) neon has a characteristic orangecolor
red glow
air and is used in balloons
• Helium is lighter than _____
and blimps
• Ne, Ar, Kr, & Xe are used in lights b/c of the colors
they make in light bulbs because they ___
do ___
not
react with the metal (tungsten) that makes the
filament.
Radon
• __________
is radioactive and is used in the
treatment of cancer.
• Argon is the most abundant Noble Gas, making up
one percent of the atmosphere.
Slide 81
7. Lanthanides
• 1st of the 2 rows at the bottom of the table
• 15 elements known as the _______
Earth
rare
Elements along with the Actinides
• Soft, shiny, silvery metals
• Malleable with high conductivity
• Reactive
• Burns in oxygen or air
• Oxidizes or tarnishes rapidly
Slide 82
7. Lanthanides (con’t)
except for poor
• Similar to transition metals _______
conductors
• React in similar manner because they are found
nature
together in _______
spark
• Produce _______
when struck
• Alloys made with iron are used to make flints for
cigarette lighters
• Uses: glass, welders’ goggles, nuclear reactors,
petroleum, color TV screens, computer monitors
(because they produce colors when combined
with phosphorus)
• Example of colors are Europium = red and
green
Terbium = _______
Slide 83
8. Actinides
bottom
• Very last row at the _______
• 15 elements known as the Rare Earth Elements
along with the Lanthanides
• All radioactive, reactive, silvery metals
• Actinium, thorium, protactinium, and uranium are
all natural
• Neptunium and plutonium were once thought to
manmade but found small
be synthetic or __________,
amounts in nature.
• _____
All
other members are synthetic
Slide 84
8. Actinides (con’t)
• After Curium, all are very radioactive and have
been produced in such small
_______ amounts that
little is known about them
• Uranium is the most stable and is used for
nuclear fuel, power plants, weapons, as a pigment
in glass and ceramics.
• Plutonium is used in nuclear weapons and to power
space exploration equipment.
• Curium is used to power satellites and was used
to test moon soils.
Americium
• ____________
is used in smoke detectors.
Slide 85
Review
•
•
•
•
Metals – To the Left & are More Reactive
Metalloids on Stairs
Non-Metals to the Right Less Reactive
7 Periods/Rows/HorizontalRow
– # indicates the # of e- shells/orbitals/energy levels
• 18 Groups/Families/Vertical
– Elements have similar properties within families
• Chemical Reactivity
– Metals increase from right to left & top to bottom
– Nonmetals increase from left to right & bottom to top
Slide 86
Periodic Table Quiz
1.
2.
3.
4.
5.
Who was the first to develop the Periodic Table?
a.
b.
c.
Henry Mosely
Niels Bohr
Dmitri Mendeleev
a.
b.
c.
Atomic Mass
Atomic Number
Atomic Theory
a.
b.
c.
Solids
Liquids
Gases
a.
b.
c.
Metals, Nonmetals, and Metalloids
Metals, Solids, and Liquids
Metals, Nonmetals, and Gases
a.
b.
c.
To the Left of the Staircase/Zig-Zag
On the Staircase/Zig-Zag
To the Right of the Staircase/Zig-Zag
The modern Periodic Table is designed according to increasing
Most of the elements are
The Periodic Table is divided into which of the following 3 properties?
Where on the Periodic Table are the Metalloids located?
Slide 87
6. What are the horizontal rows on the periodic table called?
a.
b.
c.
Periods
Groups
Families
a.
b.
c.
7
12
18
a.
b.
c.
Rows
Periods
Families
a.
b.
c.
7
12
18
a.
b.
c.
Increases
Decreases
Stays the Same
7. How many rows are there?
8. What are the vertical columns on the periodic table called?
9. How many columns are there?
10. As you move across the Periodic Table from left to right,
what happens to the reactivity of the elements?
Slide 88
Chemistry Review
Slide 89
Atoms
Slide 90
Atoms
•
•
•
•
•
•
•
•
•
Atomic Theory
Atomic Structure
Small
Protons (+), Neutrons (0), Electrons (-)
Nucleus
Orbitals
Elements, Compounds, Molecules
2, 8, 18
Periodic Table
Slide 91
Periodic Table
Slide 92
•
•
•
•
•
•
•
•
•
•
•
Periodic Table
118 Elements
1st created by Dmitri Mendeleev
1st arranged by Atomic Mass now Atomic #
7 Rows or Periods & 18 Columns or Families
Metals (left of staircase), Non-Metals (right of
staircase), and Metalloids (on staircase)
Solids, Liquids, Gases
Staircase – Zig Zag
Atomic Structure
Symbols, Atomic # & Atomic Mass
# of P & # of E = Atomic #
Atomic Mass – Atomic # = # of N
Slide 93
Atomic Theory
Slide 94
Atomic Theory
•
•
•
•
•
•
•
•
Evolution of the Model of the Atom
Democritus - Atomos
John Dalton – Atomic Theory
JJ Thomson – Plum Pudding
Ernest Rutherford – Gold Foil
James Chadwick – Neutron
Niels Bohr – Electron Shells
Erwin Schrodinger – Wave Model
Slide 95
Atomic Structure
Slide 96
Atomic Structure
•
•
•
•
•
•
•
•
•
Nucleus with Protons & Neutrons
Electron Shells/Orbitals/Levels
Electrons = approx. ½ size of P & N
2, 8, 18
Periodic Table Rows = # of Shells
7 Shell Max
Periodic Table Columns = # of Valence eElectron Cloud
Wave Model
Slide 97
Elements
Slide 98
Elements
•
•
•
•
•
•
•
•
118
Each with their own properties
Made of atoms
Combine same atoms = Molecules
Combine different atoms = Compounds
1, 2, or 3 letter symbols
Arranged on table by increasing atomic #
Found in nature or manmade
Slide 99
Chemical Bonding
Slide 100
Chemical Bonding
• Atoms joined together chemically to form
either molecules or compounds
• Covalent Bonds = Sharing of Electrons by 2
Non-Metals
• Ionic Bonds = Giving & Taking of Electrons by
a Metal and a Non-Metal
• Toothpicks are used to represent bonding
with molecular models
Slide 101
Chemical Reactions
Slide 102
Chemical Reactions
•
•
•
•
Reactants = Start With
Products = End With
Reactants → Products
4 Types of Chemical Reactions:
1.
2.
3.
4.
Synthesis
Decomposition
Single Displacement
Double Displacement
Slide 103
Matter
Slide 104
Matter
•
•
•
•
•
•
•
What everything is made up of
Has Mass and Volume
Made of Atoms
Atoms make up Elements
Elements make up Compounds
Most of the world is made of Chemical
Compounds
States/Phases of Matter…
1. Solid 2. Liquid 3. Gas 4. Plasma
Slide 105
States of Matter
Slide 106
States of Matter
• Solid – definite shape and volume
• Liquid – takes shape of container & has
definite volume
• Gas – takes shape & volume of container
• Plasma – ex) sun, stars, fire, etc.
• Evaporation – liquid to a gas
• Condensation – gas to a liquid
• Sublimation – solid to a gas
• Melting, Boiling, & Freezing
Slide 107
Physical vs. Chemical
Changes
Slide 108
Physical vs. Chemical Changes
• Physical Change = still the same substance
• Chemical Change = creates a new substance
• Examples of Physical Changes = crushing,
cutting, melting, boiling, freezing, breaking,
mixing, etc.
• Examples of Chemical Changes = reacting,
burning, fizzing, rusting, cooking, etc.
Slide 109
Mixtures
Slide 110
Mixtures
• Mixture is physically combined – no chemical
reaction occurs!
• Solution = solute dissolves in a solvent
Ex) sugar water, kool-aid, salt water, etc.
• Suspension = large particles settle out
Ex) muddy water, Italian salad dressing, etc.
• Colloid = matter is dispersed throughout
Ex) Jell-O, paint, mayonnaise, milk, fog, etc.
• Homogeneous = the same matter throughout
• Heterogeneous = different matter
throughout
Atomic Timeline
(AKA The 7 Dead Dudes of Atomic Theory)
Slide 2
Timeline Construction
• Use the adding machine tape to make your
Atomic Timeline
• Make sure you include…
•
•
•
•
Name
Date
Important Information
Picture/or/Symbol
Slide 3
1) Democritus – 460 BC
• First to develop the idea that matter was
made of particles called Atoms
• The term “Atoms” comes from the Greek
word “atomos” which means “undivisible”
Slide 4
2) John Dalton - 1803
• Proposed atomic theory
• An atom is indivisible, indestructible, tiny
sphere.
• Determined that elements have unique
atomic masses
Slide 5
3) Joseph John Thomson - 1898
• Discovered Electrons
• Proposed an atomic model known as the “plum
pudding” model
Slide 6
4) Ernest Rutherford - 1911
• Discovered positively charged nucleus by
probing atoms of gold foil with positively
charged particles.
• Proposed atomic model with massive nucleus
with electrons in a circle around it in a solar
system model
Slide 7
5) Niels Bohr - 1913
• Developed atomic model that placed
electrons in specific energy levels to explain
why they did not spiral toward and collide
with the nucleus
• Proposed the model with electrons in specific
orbits around the nucleus
Slide 8
6) James Chadwick - 1932
• Discovered neutron as a neutral particle in
the nucleus
• The discovery explained why the mass of an
atom could not be attributed entirely to the
mass of the protons
Nucleus
(+) Positive Protons
(0) Neutral Neutrons
Slide 9
7) Erwin Schrodinger – 1933
• Described electrons as waves with their
probable location viewed as a cloud and
introduced a mathematical model of the
atom
e-
Slide 10
Highlights
1. Democritus
First – Atomos - Indivisible
2. John Dalton
Atomic Theory
3. J.J. Thomson
Electrons - “Plum Pudding”
4.
5.
6.
7.
+ Charged Nucleus – Gold Foil
Electrons Specific NRG Levels
Neutrons (Jimmy Neutron)
Electron Cloud Wave
Ernest Rutherford
Niels Bohr
James Chadwick
Erwin Schrodinger
Slide 11
Way to Remember the Order of the
Scientists for the Atomic Theory…
•
•
•
•
•
•
•
Democritus Democritus
Discovered Dalton
Tiny Thomson
Round Rutherford
Circular Chadwick
Ball-like Bohr
Spheres Schrodinger
Slide 12
Indivisible Electron
Greek
Dalton
Nucleus
Orbit
Electron
Cloud
X
X
Thomson
X
Rutherford
X
X
Bohr
X
X
Wave
X
X
X
X
Slide 13
Don’t Sweat the
Small Stuff!
Slide 14
Size of Atoms
• Tiny!
• Tinier than the cells and germs.
• Too small to be seen with ordinary
microscopes
• Atoms are so small that it would take 100
million atoms placed side by side to form a
row only 1 cm long which is about the width
of your pinky finger!
Slide 15
How Small is the Small Stuff?
• Let’s check it out…
• http://www.micro.magnet.fsu.edu/primer/jav
a/scienceopticsu/powersof10
• http://www.cellsalive.com/howbig.htm
• http://www.strangematterexhibit.com/struc
ture.html
• http://learn.genetics.utah.edu/content/begin
/cells/scale/
• http://www.azonano.com/Details.asp?Article
ID=1780
Slide 16
What’s the Matter?
Matter
Slide 17
What’s the Matter?
“Stuff” that
Everything
is made of!
Made of
Atoms
Matter
Has Mass=
The Amount
of Matter
in an Object
Has Volume=
Takes Up
Space
Slide 18
What was the “Small Stuff” anyway?
•Atoms
•Elements
•Molecules
•Compounds
Slide 19
Atoms
• Basic unit of matter
• The smallest particle of a substance that has
all of the properties of that substance.
• Example= the element Gold is made of gold
atoms
Slide 20
Elements
• A pure substance made of only one kind of
atom.
• Examples= Gold, Hydrogen, Carbon, etc.
• Elements are found on the Periodic Table of
Elements.
• Here is a song about them…
http://www.privatehand.com/flash/elements.h
tml
Slide 21
Molecules
• Made up of two or more atoms joined tightly
together.
• Small particle of the entire substance or
compound
• Atoms in a molecule may be of the same
element or of different elements.
• Examples= 1 molecule of the element oxygen
or 1 molecule of the compound water H2O
Slide 22
Compounds
• A substance whose molecules contain atoms
of different elements combined chemically.
• Most matter exists as compounds.
• Examples= Water, Carbon Dioxide, etc.
Slide 23
What is the difference between a
Compound and a Molecule?
• A molecule is formed when two or more
atoms join together chemically.
• Molecules can be made up of atoms joined
together or elements joined together which
form compounds
• A compound is a molecule that contains at
least two different elements.
Slide 24
Compound vs. Molecule
• All compounds are molecules but not all
molecules are compounds!
• Molecules that are made of two atoms joined
together are not compounds
• Compound = entire substance
• Molecule = small particle of entire substance
Slide 25
Atom
•Smallest part of a substance
•Has all of the properties of that substance
Molecule
Element
•Pure Substance
•Made of 1 kind
of atom
•2 or more atoms
joined tightly
together
•Smallest part
of compound
Compound
•Molecules
containing
atoms
of different
elements
Slide 26
Atom
• Smallest part of a
substance
• Has all of the properties
of that substance
Slide 27
Element
• Pure Substance
• Made of 1 kind of
atom
Slide 28
Molecule
•2 or more atoms
joined tightly
together
•Smallest part
of compound
Slide 29
Compound
• Molecules containing
atoms of different
elements
Slide 30
Chemical Bonding
•
Elements bond together to form compounds
•
2 Main Types of Bonding…
1. Colvalent = sharing of e-
1. Ionic = giving or taking of e-
Slide 31
Covalent Bonding = Sharing e• Covalent Bond= sharing of electrons that
occurs between 2 non-metals
Ex) Water H2O
H
= Hydrogen’s Electron
O
H
= Oxygen’s Electrons
Slide 32
Ionic Bonding = give or take eIonic Bond= giving or taking of electrons that
occurs between metals and non-metals
Ex) Salt NaCl – Na give outer e- to Cl
Na
Na1+
Cl
Cl1-
Slide 33
Ions
• An ion is an atom or molecule which has lost
or gained one or more electrons, making it
positively or negatively charged.
• A negatively charged ion, which has more
electrons in its electron shells than it has
protons in its nuclei, is known as an anion
• Conversely, a positively-charged ion, which
has fewer electrons than protons, is known
as a cation
Slide 34
Ions (con’t)
• An ion consisting of a single atom is called a
monatomic ion, but if it consists of two or
more atoms, it is a polyatomic ion. Polyatomic
ions containing oxygen, such as carbonate
and sulfate, are called oxyanions.
• Ions are represented by the presence of a
superscript indicating the sign of the net
electric charge and the number of electrons
lost or gained, if more than one. For example:
H+ and SO42−.
Slide 35
Elements in the Earth & Air
1.
2.
3.
4.
5.
6.
7.
Element
Oxygen
Silicon
Aluminum
Iron
Calcium
Potassium
Sodium
Symbol
Use
O
Breathing
Si
Glass/Rocks
Al
Foil/Cans
Fe
Steel
Ca
Bones/Teeth
K
Bones/Muscles
Na
Salt
Slide 36
Elements In Our Bodies
Ca 1.6%
N 2.4%
Other 3.3%
H 10.2%
C 17.5%
O 65%
Slide 37
Nucleus
P+
&
NO
1st = 2 e2nd = 8 e3rd = 18 e-
Slide 38
Periodic Table
• Atomic # = # of p+ = # of e• # of n0 = Atomic Mass – Atomic #
• Period #s = # of orbitals/shells
• 7 Periods = 7 shell max
Slide 39
“Playing” with the Periodic Table…
• Draw the orbitals on your paper plate
• Use play-doh to represent protons, neutrons,
and electrons
• Choose a different color for each
• Start with simple elements and work your
way up!
Slide 40
Nucleus
P+
&
NO
1st = 2 e2nd = 8 e3rd = 18 e-
Slide 41
Acting Out Bohr
Models!
Nucleus
P+
&
NO
1st = 2 e2nd = 8 e3rd = 18 e-
Slide 42
Periodic Tables
• Check out the Periodic Table in Pictures and
in Words
• Use your other Periodic Table to Color Code
the Metals, Nonmetals, and Metalloids
• On the other side, color code the
Groups/Families
Slide 43
Slide 44
Awesome Websites…
•
•
•
•
•
•
•
•
•
http://www.visual-literacy.org/periodic_table/periodic_table.html
http://www.everypoet.com/absurdities/elements/
http://sciencespot.net/Pages/kdzchem2.html
http://www.middleschoolscience.com/chemistry.htm
http://www.middleschoolscience.com/atomicmusicalchairs.pdf
http://www.science-class.net/Chemistry/Chemistry.htm
http://elements.wlonk.com/Elements_Pics_11x8.5.pdf
http://elements.wlonk.com/Elements_Words_11x8.5.pdf
http://www.learner.org/interactives/periodic/index.html
Slide 45
Blue= Metals
Pink= Metalloids
Yellow= Nonmetals
Slide 46
How to Read the
Periodic Table
Tracy Arrington-Payne
SI560
Slide 47
The Periodic Table Is . .
• A table of all known elements,
• A useful tool for scientists,
• And, it arranges elements according
to their properties.
Slide 48
The Inventor
• Created by Dmitri Mendeleev.
• Mendeleev was a teacher who
was discouraged by his teaching
tools and decided to create his
own.
• He made note cards of the
elements known at that time and
arranged them. When there
wasn’t an element to fit a certain
spot, he left it open and
predicted an element would be
found later to fill it.
Slide 49
Reading a Periodic Table
• When reading a periodic table . . . .
–
–
–
–
Look at the box
Look at the columns (group or family)
Look at the rows (periods)
Look at the location of metals, nonmetals, and
semiconductors
Slide 50
Using the Box
• Each box represents a different element.
• Each box contains information that tells . .
–
–
–
–
The elements name
The elements symbol
The atomic number of the element
The atomic weight of the number
Slide 51
Example
• Name – Oxygen
Oxygen
8
• Atomic Number – 8
• Atomic Symbol – O
• Atomic Weight – 16.00
O
16.00
Slide 52
Using the Columns
• Each column of elements is called a family or
group.
• Elements in a family have similar but not
identical properties.
• The number for the column sometimes
indicates the number of electrons in outer
shells of the element.
• Elements in a group have the same number of
electrons in their outer orbital.
Slide 53
Families or Groups
•Elements in the red group
have 1 electron in their outer
shell.
•Elements in the orange
group have 2 electrons in
their outer shell.
•As you keep counting the
colored columns, you add an
additional electron.
•Purple has 8 electrons in its
outer shell.
•(Don’t include the white
group)
Slide 54
Slide 55
Using the Rows
• Rows represent an elements period.
• Elements in a period are not alike in
properties.
• Even though some squares are skipped in
between, all of the rows go from left to
right.
Slide 56
Using the Rows
• As a rule. . . .
– the first element in a period is usually an active
solid.
– the last element in a period is always a noble gas.
• Atomic size decreases from left to right
across a period.
• And generally, atomic mass increases form
left to right across a period, although there
are exceptions.
Slide 57
Example
•Every element in the top
row (first period) has one
orbital for its electrons.
•Every element in the
second row (the second
period) have two orbitals
available.
•Atoms on the left are
usually larger and lighter.
•Atoms on the right are
usually smaller and heavier.
Slide 58
Slide 59
Metals, Nonmetals, and
Semiconductors
Some periodic tables are color coded to show what
elements are metals, nonmetals, and
semiconductors.
In general, elements located in the left two-thirds
or so of the periodic table are metals. The
nonmetals are on the right side of the table.
The dividing line between the metals and
nonmetals are elements called semiconductors.
Slide 60
The gray area represents the metals.
The yellow area represents the semiconductors.
The blue area represents the nonmetals.
Slide 61
Conclusion
• The Periodic Table is an excellent tool for
looking at elements and the key to using it is
to understand the code of it structure.
• Using the boxes, columns, and rows will help
you learn about the properties of elements.
Slide 62
I. Metals, Metalloids, and Non-Metals
II. 7 Periods/Rows
III. 18 Groups/Families
Slide 63
I. Metals, Metalloids, & Non-Metals
Metals
left
• On the _______ of the staircase/zig-zag
(except for hydrogen)
• Most are shiny, hard, and dense.
• They conduct (transmit) electricity and heat.
high melting and
• They have mostly _______
boiling points.
• They are malleable (pounded into shapes) and
ductile (drawn into wire).
• Ex) Aluminum is a metal that is pounded into
aluminum foil.
Slide 64
Metalloids
on
• 7 elements _____
the staircase/zig-zag
both
• Properties of _______
metals and nonmetals.
• Ex) Silicon is a metalloid. It conducts
electricity like a metal and is brittle like a
non-metal. It is used to make microchips.
Slide 65
Non-Metals
right of the staircase/zig-zag
• To the _______
• Most have low melting points
• Are dull and brittle if solid.
poor
• Most are _______
conductors of heat and
electricity.
• Ex) Sulfur is a non-metal. It is often used to
make fertilizer.
Slide 66
II. 7 Periods/Rows
The Period # = the # of Electron
Shells/Orbitals/Energy Levels
1. This period contains the two __________
lightest
known elements, hydrogen (H) and helium (He).
Each element has 2 electron shell.
2. The elements in this period have 2 electron
shells. The gases that make up most of our
____________,
atmosphere nitrogen(N) and oxygen(O),
are found in this period.
3 electron
3. The elements in this period have ___
shells. Sodium (Na) and chlorine(Cl) are found
in this period.
Slide 67
4. The elements in this period have 4 electron
shells. This period includes the element iron
(Fe), a commonly used _____.
metal
5. The elements in this period have 5 electron
shells. Silver (___)
Ag is found in this period
6. With 6 electron shells, some of these
__________
heavier elements are unstable and
radioactive. This period includes gold (Au),
lead (Pb) and radioactive radon (Rn).
7. With 7 electron shells, these are the
heaviest elements. Many are
________________
- some so unstable
radioactive
that they fall apart almost instantly.
Uranium (U) is found in this period
Slide 68
III. 18 Columns/Groups/Families
1.
2.
3.
4.
5.
6.
7.
8.
Alkali Metals
Alkaline Earth Metals
Transition Metals
BCNO Family
Halogens
Noble Gases
Lanthanides
Actinides
Slide 69
1. Alkali Metals – Group 1 (far left of table)
• The metals are Lithium, Sodium, Potassium, Rubidium,
Cesium, and Francium.
• Hydrogen, a non-metal, is in the family because of its
reactivity
________________.
electron in their outer shells.
• All have 1 __________
• They are all soft and very reactive.
↑ as we read down the table.
• Their reactivity ___
• They so reactive because they have 1 valence electron
that can easily be given away.
• All of these metals are soft, silvery white, with low
melting points.
blow
up
• Hydrogen will _______
____
upon any contact with
flames.
burn the skin if
• The metals are so reactive they will _______
touched.
Slide 70
1. Alkali Metals (con’t)
• They tarnish rapidly and react violently with
water
__________.
salts
• They easily form _______
with the halogens.
never found in their pure forms in nature,
• They are _______
only found as compounds
• The metals in this family are easy to identify because
colors
they give off a different _________
when burned:
Lithium = crimson, Sodium = yellow, Potassium = violet,
Rubidium = reddish-violet, Cesium = blue, and Francium =
Rare Little is Known
Uses
• Important _________Lithium = Grease, Lubricants,
Aircraft Parts, & Batteries, Sodium = Salt and Gasoline,
Potassium = More Expensive than Na & less widely used
but used in fertilizer and photography.
Slide 71
2. The Alkaline Earth Metals – Group 2
• 6 metals: Berylium, Magnesium, Calcium,
Strontium, Barium, and Radium.
soft
• Are _______
and bright silvery-white in color.
high
• Have high melting points and _______
densities.
2 electrons in their outer shells.
• All have ___
• Are all reactive and react with water.
less
• Are __________
reactive than the alkali metals.
↑ as we read down the
• Have reactivity that ___
table.
• Will oxidize or tarnish in air, but can be handled
humans
by __________.
• Are __________
never found in nature in their pure
forms.
Slide 72
2. Alkaline Earth (con’t)
– Are good conductors of electricity
– Burn in different colors: Magnesium = Bright White,
Calcium = Orange-Red, Strontium = Bright Red,
Barium = Yellowish-Green, and Radium = Crimson
fireworks because of their bright colors
– Used in ____________
– Beryllium is often added to other metals to make hard
alloys
metal __________,
used to make rocket nose cones,
and in nuclear reactors.
– Magnesium is used in aircraft and photographic
equipment.
– Calcium is used with other metals to make reactive
alloys.
– Radium is radioactive and is used in the treatment of
cancer
__________.
Slide 73
3. The Transition Metals – Groups 3-12
largest family on the Periodic Table with 40
• The __________
members.
• Some of the more common and widely used members of
this family include iron, nickel, copper, zinc, silver, and
gold.
metals
• They are all __________hard, shiny, and strong.
• Fairly stable, reacting slowly or not at all with air and
water.
• Most of them have very _______
high melting points and
boiling points.
Mercury is one exception- it is a liquid at room
• ____________
temperature.
• Most are good ____________
conductors of heat and electricity.
• Most will dissolve in an acid, however, __________
gold
resists acids.
oxygen
• Most can bond to _________
in more ways than one,
making different compounds.
Slide 74
3. Transition Metals (con’t)
• Most can be pounded into sheets or shapes
ductile
(____________)
or drawn into a wire (____________)
malleable
• Most can form colored compounds with oxygen.
strong
• Many can form __________
metal alloys (a mixture of
metals).
• Form a bridge between the very reactive metals on the
left side and the less reactive metals on the right.
• Very similar so that it is difficult to detect differences
from one column to the next.
• First elements in groups 8,9, 10 called the iron triad
because they are the only ones known to create a
magnetic field.
• Many uses because of their properties- construction
materials, pipes, wires, coins, jewelry, aircrafts, cars,
bicycles, cooking utensils, paints, cleaners, etc.
Slide 75
4. The BCNO Family – Groups 13-16
25 members
• Large family with ___
• Some of the more common members of this family
include carbon, nitrogen, oxygen, aluminum, silicon, sulfur,
arsenic, tin, and lead.
divided
• This family is sometimes __________
into two or four
separate families.
diverse
• Most __________
family of elements.
lightest
• Name is from the ____________
of the elements in
each column- Boron, Carbon, Nitrogen, and Oxygen.
• There are metals, nonmetals, and metalloids in this family
gases
• Some members are _______
at room temp like nitrogen
solids
and oxygen, but most are __________.
Slide 76
4. The BCNO Family (con’t)
• They are reactive, but selective with which
bond
elements they will __________.
• Most will bond with oxygen & oxygen will bond
with __________
itself
bond
• Members of each column tend to _______
with
other elements in a similar fashion
• Oxygen supports combustion.
• Many uses- essential to life (carbon, oxygen,
nitrogen, and phosphorus), metals are used in
electronics, nonmetals are used as
insulators on wires, poisons, fertilizers, in
____________
scuba gear, soap, glass-making, solder, aircraft,
weapons, drink cans, foil, pots, and pans.
Slide 77
5. The Halogens – Group 17
• All have seven electrons in their outer shells and are
____________
poisonous non-metals.
• Most reactive of all nonmetals, but are poor conductors of
____________
electricity
down
• Their reactivity decreases as we read __________
the
table.
5 elements- fluorine,
• Very small family consisting of only ___
chlorine, bromine, iodine, and astatine
room temperature fluorine and chlorine are gases,
• At _______
bromine is a liquid, and iodine and astatine are solids
Very reactive and never found in their pure forms in
• ______
nature.
• Combine with alkali metals to form a family of chemical
salts
compounds - __________.
Slide 78
5. The Halogens (con’t)
• Fluorine is added to toothpaste and water to
prevent tooth decay and combines with uranium to
form __________
fuel.
nuclear
• Chlorine is added to water supplies and swimming
pools to kill germs. It is widely used in bleach and
salt.
Bromine
• ____________
is used as a gasoline additive,
photograph developer, fire retardant, and an
insecticide. It is also used to kill germs in water
supplies.
• Iodine is added to salt to reduce thyroid disease.
It is also used as a film developer and as a
disinfectant in water supplies.
no
• Astatine is very rare, very radioactive, and has ___
uses.
Slide 79
6. The Noble Gases - Group 18
• They are very non-reactive because they have
_____
outer shells…inert.
full
rarest
• These are some of the __________
and heaviest
elements.
• Six gases- helium, neon, argon, krypton, xenon, and
radon
Colorless tasteless, and odorless
• __________,
• Do not mix with others- do not gain, share, lose
electrons.
• Chemically stable because they have a full outer
energy level.
• Helium, neon, and argon will _____
not combine with
other elements
• Xenon, krypton, and radon will combine with other
elements, but difficult process.
Slide 80
6. The Noble Gases (con’t)
• When an electrical current is passed through one
of these gases it will glow in a characteristic
__________
ex) neon has a characteristic orangecolor
red glow
air and is used in balloons
• Helium is lighter than _____
and blimps
• Ne, Ar, Kr, & Xe are used in lights b/c of the colors
they make in light bulbs because they ___
do ___
not
react with the metal (tungsten) that makes the
filament.
Radon
• __________
is radioactive and is used in the
treatment of cancer.
• Argon is the most abundant Noble Gas, making up
one percent of the atmosphere.
Slide 81
7. Lanthanides
• 1st of the 2 rows at the bottom of the table
• 15 elements known as the _______
Earth
rare
Elements along with the Actinides
• Soft, shiny, silvery metals
• Malleable with high conductivity
• Reactive
• Burns in oxygen or air
• Oxidizes or tarnishes rapidly
Slide 82
7. Lanthanides (con’t)
except for poor
• Similar to transition metals _______
conductors
• React in similar manner because they are found
nature
together in _______
spark
• Produce _______
when struck
• Alloys made with iron are used to make flints for
cigarette lighters
• Uses: glass, welders’ goggles, nuclear reactors,
petroleum, color TV screens, computer monitors
(because they produce colors when combined
with phosphorus)
• Example of colors are Europium = red and
green
Terbium = _______
Slide 83
8. Actinides
bottom
• Very last row at the _______
• 15 elements known as the Rare Earth Elements
along with the Lanthanides
• All radioactive, reactive, silvery metals
• Actinium, thorium, protactinium, and uranium are
all natural
• Neptunium and plutonium were once thought to
manmade but found small
be synthetic or __________,
amounts in nature.
• _____
All
other members are synthetic
Slide 84
8. Actinides (con’t)
• After Curium, all are very radioactive and have
been produced in such small
_______ amounts that
little is known about them
• Uranium is the most stable and is used for
nuclear fuel, power plants, weapons, as a pigment
in glass and ceramics.
• Plutonium is used in nuclear weapons and to power
space exploration equipment.
• Curium is used to power satellites and was used
to test moon soils.
Americium
• ____________
is used in smoke detectors.
Slide 85
Review
•
•
•
•
Metals – To the Left & are More Reactive
Metalloids on Stairs
Non-Metals to the Right Less Reactive
7 Periods/Rows/HorizontalRow
– # indicates the # of e- shells/orbitals/energy levels
• 18 Groups/Families/Vertical
– Elements have similar properties within families
• Chemical Reactivity
– Metals increase from right to left & top to bottom
– Nonmetals increase from left to right & bottom to top
Slide 86
Periodic Table Quiz
1.
2.
3.
4.
5.
Who was the first to develop the Periodic Table?
a.
b.
c.
Henry Mosely
Niels Bohr
Dmitri Mendeleev
a.
b.
c.
Atomic Mass
Atomic Number
Atomic Theory
a.
b.
c.
Solids
Liquids
Gases
a.
b.
c.
Metals, Nonmetals, and Metalloids
Metals, Solids, and Liquids
Metals, Nonmetals, and Gases
a.
b.
c.
To the Left of the Staircase/Zig-Zag
On the Staircase/Zig-Zag
To the Right of the Staircase/Zig-Zag
The modern Periodic Table is designed according to increasing
Most of the elements are
The Periodic Table is divided into which of the following 3 properties?
Where on the Periodic Table are the Metalloids located?
Slide 87
6. What are the horizontal rows on the periodic table called?
a.
b.
c.
Periods
Groups
Families
a.
b.
c.
7
12
18
a.
b.
c.
Rows
Periods
Families
a.
b.
c.
7
12
18
a.
b.
c.
Increases
Decreases
Stays the Same
7. How many rows are there?
8. What are the vertical columns on the periodic table called?
9. How many columns are there?
10. As you move across the Periodic Table from left to right,
what happens to the reactivity of the elements?
Slide 88
Chemistry Review
Slide 89
Atoms
Slide 90
Atoms
•
•
•
•
•
•
•
•
•
Atomic Theory
Atomic Structure
Small
Protons (+), Neutrons (0), Electrons (-)
Nucleus
Orbitals
Elements, Compounds, Molecules
2, 8, 18
Periodic Table
Slide 91
Periodic Table
Slide 92
•
•
•
•
•
•
•
•
•
•
•
Periodic Table
118 Elements
1st created by Dmitri Mendeleev
1st arranged by Atomic Mass now Atomic #
7 Rows or Periods & 18 Columns or Families
Metals (left of staircase), Non-Metals (right of
staircase), and Metalloids (on staircase)
Solids, Liquids, Gases
Staircase – Zig Zag
Atomic Structure
Symbols, Atomic # & Atomic Mass
# of P & # of E = Atomic #
Atomic Mass – Atomic # = # of N
Slide 93
Atomic Theory
Slide 94
Atomic Theory
•
•
•
•
•
•
•
•
Evolution of the Model of the Atom
Democritus - Atomos
John Dalton – Atomic Theory
JJ Thomson – Plum Pudding
Ernest Rutherford – Gold Foil
James Chadwick – Neutron
Niels Bohr – Electron Shells
Erwin Schrodinger – Wave Model
Slide 95
Atomic Structure
Slide 96
Atomic Structure
•
•
•
•
•
•
•
•
•
Nucleus with Protons & Neutrons
Electron Shells/Orbitals/Levels
Electrons = approx. ½ size of P & N
2, 8, 18
Periodic Table Rows = # of Shells
7 Shell Max
Periodic Table Columns = # of Valence eElectron Cloud
Wave Model
Slide 97
Elements
Slide 98
Elements
•
•
•
•
•
•
•
•
118
Each with their own properties
Made of atoms
Combine same atoms = Molecules
Combine different atoms = Compounds
1, 2, or 3 letter symbols
Arranged on table by increasing atomic #
Found in nature or manmade
Slide 99
Chemical Bonding
Slide 100
Chemical Bonding
• Atoms joined together chemically to form
either molecules or compounds
• Covalent Bonds = Sharing of Electrons by 2
Non-Metals
• Ionic Bonds = Giving & Taking of Electrons by
a Metal and a Non-Metal
• Toothpicks are used to represent bonding
with molecular models
Slide 101
Chemical Reactions
Slide 102
Chemical Reactions
•
•
•
•
Reactants = Start With
Products = End With
Reactants → Products
4 Types of Chemical Reactions:
1.
2.
3.
4.
Synthesis
Decomposition
Single Displacement
Double Displacement
Slide 103
Matter
Slide 104
Matter
•
•
•
•
•
•
•
What everything is made up of
Has Mass and Volume
Made of Atoms
Atoms make up Elements
Elements make up Compounds
Most of the world is made of Chemical
Compounds
States/Phases of Matter…
1. Solid 2. Liquid 3. Gas 4. Plasma
Slide 105
States of Matter
Slide 106
States of Matter
• Solid – definite shape and volume
• Liquid – takes shape of container & has
definite volume
• Gas – takes shape & volume of container
• Plasma – ex) sun, stars, fire, etc.
• Evaporation – liquid to a gas
• Condensation – gas to a liquid
• Sublimation – solid to a gas
• Melting, Boiling, & Freezing
Slide 107
Physical vs. Chemical
Changes
Slide 108
Physical vs. Chemical Changes
• Physical Change = still the same substance
• Chemical Change = creates a new substance
• Examples of Physical Changes = crushing,
cutting, melting, boiling, freezing, breaking,
mixing, etc.
• Examples of Chemical Changes = reacting,
burning, fizzing, rusting, cooking, etc.
Slide 109
Mixtures
Slide 110
Mixtures
• Mixture is physically combined – no chemical
reaction occurs!
• Solution = solute dissolves in a solvent
Ex) sugar water, kool-aid, salt water, etc.
• Suspension = large particles settle out
Ex) muddy water, Italian salad dressing, etc.
• Colloid = matter is dispersed throughout
Ex) Jell-O, paint, mayonnaise, milk, fog, etc.
• Homogeneous = the same matter throughout
• Heterogeneous = different matter
throughout