What’s the Matter?
Matter
What’s the Matter? p. 7
“Stuff” that
Everything
is made of!
Made of
Atoms
Can be a solid,
liquid, gas,
or plasma
Matter
Has Mass=
The Amount
of Matter
in an Object
Has Volume=
Takes Up
Space
What’s the Matter?
“Stuff” that
Everything
is made of!
Made of
Atoms
Can be a solid,
liquid, gas,
or plasma
Matter
Has Mass=
The Amount
of Matter
in an Object
Has Volume=
Takes Up
Space
States of Matter Brainstorm p. 2
1. How many states of matter are there?
2. What are the states of matter?
3. Draw what you think the particles look like on a
microscopic level
4. Describe their motion.
#
S.O.M.
How it Looks…
How it
Moves…
1
Size &
Shape
Ex)
Solid
OOOOOOOOOOOOOOO
OOOOOOOOOOOOOOO
OOOOOOOOOOOOOOO
Tightly Packed Together
& Bonded!
Slow
Definite Ice Cube
(vibrate Volume &
Desk
Shape
in place)
2
Liquid
OO O O OO
O
O O O O
O O
OO O OO O
Loosely Packed Together
with Some Bonds!
3
Gas
4
Plasma
Fast
Takes
Shape of
Container &
Definite
Volume
Water
Juice
O
O O O
O
O
O
O
O O
Spread Apart with No
Bonds!
Faster
Takes
Shape &
Volume of
Container
Steam
Air
e-O
O OeO O
O
Oe- O
O
e-O
O
OeSpread Apart & Charged!
Fastest!
Electrically
Charged
Gas!
Stars
Lightning
O
O
O
SOM Animations
• http://www.chemtutor.com/sta.htm
• http://www.kentchemistry.com/links/Matter/HeatingC
urve.htm
Phase Change Graph
Phase Change Graph
K
Kelvin
˚
Celsius
˚F
Fahrenheit
Can you freeze air?
• Nitrogen (what 78% of the air is made of)
freezes at -210 degrees Celsius. Oxygen (air is
about 20% oxygen) freezes at -222.65 degrees
Celsius. So if you want to have a block of solid
air it would have to be at least 222.65 degrees
below zero.
Can gold become a gas?
• Any element can become a gas; you just need to heat it past its
boiling point. For gold, that’s 2,856 degrees Celsius (5,173 degrees
Fahrenheit), which is hotter than the temperature in an arc furnace
so it’s difficult to just boil a bar of gold. But you can create small
amounts of gold gas by bombarding it with a high-energy beam of
electrons in a vacuum. This knocks atoms of gold free from the solid
mass and they’ll fly around and coat anything in the vacuum
chamber. Electron beam vapour deposition is used to create very
thin gold coatings for the electronics, medical and space industries.
Gold coatings can also be used as a lubricant in machinery.
• http://www.howitworksdaily.com/science/can-gold-become-a-gas/
Summary Chart p. 5
Change of
State
Direction
Endo (take in) or
Exo (give off)
Thermic (Heat)
Example
Melting
Solid Liquid
Endo
Ice melts into liquid water
at 0˚C, 32˚F, or 273K
Freezing
Liquid Solid
Exo
Liquid water freezes into
ice at 0˚C, 32˚F, or 273K
Vaporization
Liquid
Gas
Endo
Liquid water vaporizes
into steam at 100˚C,
212˚F, or 373K
Condensation
Gas
Liquid
Exo
Steam condenses into
liquid water at 100˚C,
212˚F, or 373K
Sublimation
Solid
Gas
Endo
Solid Dry Ice sublimes
into a gas at -78˚C
(Evaporation)
4 States of Matter S.O.M.
1. Solid
2. Liquid
3. Gas
4. Plasma
Plasma
• In plasma TVs, little pockets of gas are excited
with electricity disrupting the normal balance of
atoms so there are lots of free ions and electrons,
turning them into plasma, which creates a light.
• If you super cool gas, you get a BEC superatom
wave. Warm it up, and the wave will return to a
gas.
• http://www.sciencelearn.org.nz/ScienceStories/Strange-Liquids/States-of-matter
Dry Ice
• What is Dry Ice?
– Solid Carbon Dioxide
• I thought Carbon Dioxide was a Gas!?
– YES, but at a temperature of -109.3 degrees Fahrenheit it
is a SOLID!
• Why is Mr. Horinger Wearing Gloves?
– Because Dry ice is soooooo cold that it can actually burn
your skin!
Dry Ice & Halloween
• Why is it used at Halloween time?
– Because it goes through a cool process known as
SUBLIMATION that creates a fog-like effect
• What is SUBLIMATION?
– Sublimation is when a Solid skips the liquid phase
and goes right to a Gas!
Solid
Gas
General (Physical) Properties
• Physical properties may be
observed without changing the
nature of the matter.
• Boiling point is a physical
property
– When a liquid boils, the vapor
may be condensed to get the
liquid back
– The liquid is still the same
substance
What are some Physical Properties?
• Properties you can see, such as color, shape,
hardness, and texture
• Properties that are easily measured, such as mass,
volume, density, melting point, boiling point
– Note! Freezing and melting point are the same temperature!
– Density = Mass ÷ Volume
• Is the ability to be attracted to a magnet a physical
property?
How do we measure mass and
volume?
• Mass is measured on a balance or scale.
Common units are grams, milligrams, and
kilograms
• Liquid volume is measured with a graduated
cylinder. Common units are liters and
milliliters
• Solid volumes may be calculated with
formulas or by water displacement Common
units are cm3 or milliliters.
Let’s Try Some More Density Problems
1) If the mass of a rock is 500g and its volume is
25cm3, what is its density?
2) If the density of a liquid is 1.2 g/ml, and its
volume is 10ml, what is its mass?
3) If Bob’s mass is 80kg and his density is
1.6kg/l, what is his volume?
Answers: D = M ÷ V
• 1) 500g ÷ 25cm3 =
20g/cm3
• 2) 1.2g/ml x 10ml =
12g
• 3) 80kg ÷ 1.6kg/l = 50L
M
D
V
WEIGHT
• Weight is the pull of gravity on mass.
• Weight changes in response to gravitational
pull.
• A person’s mass will remain the same on the
earth or on the moon, but she will only weigh
1/6 as much on the moon.
PHASES OF MATTER
The most common phases of matter are solid,
liquid, and gas
Plasma is a high energy phase found in stars
When a substance changes phase, energy
(heat) is lost or gained, but temperature
remains the same.
The northern lights are caused by plasma streams from
the sun hitting our atmosphere. This causes electrons in
atmospheric gases to be excited to a higher energy level,
And when they drop back down, a photon of light is emitted.
Types of Phase Changes
• Solid to liquid:
Melting
• Liquid to gas:
Vaporization
• Gas to liquid:
Condensation
• Liquid to solid:
Freezing
• Solid to gas:
Sublimation
Temperature Doesn’t Change During a
Phase Change!
Physical vs. Chemical
Properties vs. Changes
BrainPOP Property Changes
Physical OR Chemical Properties?
Does not change the identity of the matter
Observed with your senses
Flammability
Color
Odor
Reactivity
Mass
Volume
Conduction of Heat
Changes into a new substance with different properties
State of Matter – Solid, Liquid, Gas
Change of State – Melting, Freezing, Boiling
Physical
OR Chemical
Properties?
Malleability,
Ductility, or Solubility
Shape
Density
Not as easy to observe
Length
Reactivity with water, oxygen, or air
Hardness or Luster
Heat of combustion
Specific Heat
Sublimation, Evaporation, or Condensation
New substances are formed
pH
PhysicalBoiling,
OR Chemical
Changes?
Melting, Freezing
Burning
Mixing, Crushing
Sanding
Cooking
Often easy to observe
Do not change the substance
Producing Heat, Light, or Odor
Affects 1 or more properties of a substance.
Crushing or Breaking
Reacting
Color Changes
Fizzingor Foaming
Physical OR
Chemical
Smashing
a pumpkinChanges?
Chewing gum
Digesting a sandwich
Wood rotting
Smells like coffee and is brown
Tastes bitter
Dissolves in water
Milk souring
Iron rusting
Crushing a can
Mixing cake batter
Decomposing an apple
Physical OR Chemical Changes?
Breaking glass
Cutting a piece of pie
Baking Soda & Vinegar
Slicing Bread
Crumpling paper
Boiling water
Kool-aid dissolving in water
Cracking an egg
Baking a cake
Burning a marshmallow
Melting an ice cube
Chemical Properties and Changes
• Chemical properties describe a substances’
ability to change into a different substance. A
chemical change is the process by which the
substance changes.
Examples of Chemical Properties
• Flammability
• Ability to support burning
• Ability to combine with other chemicals in a
chemical reaction.
Examples of Chemical Changes
•
•
•
•
•
•
•
Rusting
Photosynthesis
Explosions
Burning
Digestion
Baking food
Fermentation
What are indicators of a chemical
change?
•
•
•
•
•
•
Gas given off
Heat absorbed or released
Light given off
Color change
Oxidation of a metal
New substances are formed
Physical Change
vs.
Chemical Change
Physical Change
A change in a substance
that does not change the
identity of the substance.
Physical Change
Examples:
•Ice melting
•Ripping paper in half
•Mixing ice tea mix in water
•Chewing your food
Chemical Change
A change in a substance
that results in a new
substance being formed.
Physical Properties of Matter
•
•
•
•
•
•
•
•
•
•
•
•
•
Does not change the identity of the matter
Observed with your senses
Color
Odor
Mass
Volume
Conduction of Heat
State of Matter – Solid, Liquid, Gas
Change of State – Melting, Freezing, Boiling
Malleability
Ductility
Solubility
Density
Chemical Properties
• Changes into a new substance with different
properties
• Not as easy to observe as physical properties.
• Flammability
• Reactivity
• You can observe chemical properties only in
situations in which the identity of the
substance could change!
•
•
•
•
•
•
•
•
•
•
•
•
•
Physical Properties vs. Chemical Properties
of Matter p.14
Does not change the identity of
the matter
Observed with your senses
Color
Odor
Mass
Volume
Conduction of Heat
State of Matter – Solid, Liquid,
Gas
Change of State – Melting,
Freezing, Boiling
Malleability
Ductility
Solubility
Density
• Changes into a new
substance with different
properties
• Not as easy to observe as
physical properties.
• Flammability
• Reactivity
• Chemical Changes always
include Physical Changes
• You can observe chemical
properties only in situations
in which the identity of the
substance could change!
Physical Changes
•
•
•
•
•
•
•
•
•
•
Affects one or more physical properties of a substance.
Boiling
Melting
Freezing
Crushing
Breaking
Mixing
Sanding, etc.
Often easy to observe
Do not change the substance.
Chemical Changes
• When one or more substances are changed into
entirely new substances with different properties.
• Reacting
• Burning
• Color Changes
• Fizzing
• Foaming
• Heating
• Producing Heat, Light, or Odor
•
•
•
•
•
•
•
•
•
•
Physical Changes vs. Chemical Changes
of Matter p.15
Affects one or more physical
properties of a substance.
Boiling
Melting
Freezing
Crushing
Breaking
Mixing
Sanding, etc.
Often easy to observe
Do not change the substance.
• When one or more
substances are changed into
entirely new substances
with different properties.
• Reacting
• Burning
• Color Changes
• Fizzing
• Foaming
• Heating
• Producing Heat, Light, or
Odor
Bohr Atom
Model
p. 7
Nucleus
P+
&
NO
1st = 2 e2nd = 8 e3rd = 18 e-
4th = 32 e5th = 32 e6th = 18 e7th = 8 e-
The shell # = row # on
Periodic Table!
The Atoms Family Song
http://www.televisiontunes.com/Addams_Family.html
1st Verse:
They’re tiny and they’re teeny,
Much smaller than a beany,
They never can be seeny,
The Atoms Family.
2nd Verse:
Together they make gases,
And liquids like molasses,
And all the solid masses,
The Atoms Family
Chorus
3rd Verse:
Neutrons can be found,
Where protons hang around;
Electrons they surround
The Atoms Family.
Chorus:
They are so small.
(Snap, snap)
They’re round like a ball.
(Snap, snap)
They make up the air.
They’re everywhere.
Can’t see them at all.
(Snap, snap)
Welcome to Matterville
(where everything matters!)
In the center of Matterville, there is a
place called the Nucleus Arcade, where two
members of the Atoms Family like to hang
out. Perky Patty Proton, like her sisters, is
quite large with a huge smile and eyes that
sparkle (+). Patty is always happy and has a
very positive personality. Nerdy Nelda
Neutron is large like Patty, but she has a
boring, flat mouth and eyes with zero
expression (o). Her family is very apathetic
and neutral about everything. Patty, Nelda,
and their sisters spend all their time at the
arcade.
Around the Nucleus Arcade, you will
find a series of roadways that are used by
another member of the Atoms Family,
Enraged Elliott Electron. Elliott races madly
around the Arcade on his bright red chrome-plated
Harley-Davidson. He rides so fast that
no one can be sure where he is at any time.
Elliott is much smaller than Patty and Nelda
and he is always angry because these bigger
relatives will not let him in the Arcade. He
has a frown on his face, eyes that are squinted
with anger, and a very negative (-) attitude.
The first energy street can only hold
only two Electron brothers. The second
energy street, called the Energy Freeway,
can hold 8 brothers. The third energy
street, called the Energy Superhighway,
can hold 18 of the brothers.
The morale of Matterville is stable as
long as each negative Electron brother is
balanced out by one positive Proton sister.
The number of residents in Matterville
depends on the Proton and Neutron families.
Challenge: What would happen to the morale
of Matterville if one Elliott Electron was
kidnapped?
Morale of Matterville
The morale of Matterville is stable as long as it
has the same number of protons (+) and
electrons (-).
If someone kidnaps one Elliott Electron, the
morale of Matterville would become positive
(more protons).
If one Elliott Electron were to move to
Matterville, the morale would be negative
(more electrons).
1st Energy
Street
Nucleus
P+
&
NO
1st = 2 e2nd = 8 e3rd = 18 e-
2nd Energy
Freeway
3rd Super
Highway
“ATOMS Family” p. 8
Perky Patty Proton (p+)
Nerdy Nelda Neutron (n0)
Enraged Elliot Electron (e-)
Name: Patty Proton (p+)
Description:
– Has a Happy & Positive Personality +
– Larger than e- & about the same size as no
– # of protons = # of electrons = atomic #
Favorite Activity:
– Hanging out in the Nucleus Arcade
++
U
Name: Nelda Neutron (no)
Description:
– Has a Boring Personality = No Charge or Neutral
- Larger than e- & about the same size as p+
- Atomic Mass – Atomic # = # of Neutrons
Favorite Activity:
– Hanging out in the Nucleus Arcade
00
Name: Elliott Electron (e-)
Description:
– Has a Negative Personality – Smaller than P+ & No
– # of electrons = # of protons = atomic #
Favorite Activity:
– Hangs far outside the Nucleus Arcade in the ecloud (empty space)
-∩
1)
2) D
e-
3) T
p+
p+
4) B
http://education.jlab.org/atomtour/listofparticles.html
5) 1000 miles!
If the Nucleus was the size of an
,
Electrons would be 5 Football Fields Away!
Word Wall p.”51”
#
Word
Definition
1
Atom
Tiny, makes up all matter
2
Proton
+ charge, n nucleus,
larger than e-
3
Neutron
4
Electron
5
Periodic
Table
O charge, n nucleus,
larger than e- charge, outside nucleus,
smaller than p+ & nO
Organizes all 118 elements
according to their
properties
*not drawn to scale!*
Pic/Symbol
Word Wall p.51
#
Word
Definition
Pic/Symbol
1
Atom
Tiny, makes up all matter
2
Proton
+ charge, n nucleus, larger than
e-
3
Neutron
O charge, n nucleus,
larger than e-
4
Electron
- charge, outside nucleus,
smaller than p+ & nO
5
Periodic
Table
Organizes all 118 elements
according to their properties
6
Bohr Model
Shows electron levels
2, 8, 8 or 18
7
Lewis
Structure
Valence electron dot model
Ne
8
Valence
Outermost e- on last shell
e-
How Small Is Small? Flow Map p.8
1) Milky Way
Galaxy
6) Earth
2) Stars
7) Florida
3) Sun
8) Science
Lab
13) Nucleus of
Plant Cell
4) Planets
9) Oak Tree
14) DNA
19) Protons p+ &
Neutrons no
5) Earth’s
Moon
10) Branch
15) e- cloud of
Carbon Atom!
20) Quarks!
11) Leaf
12) Cells
16) e- electrons
17) Empty
Space
18) Nucleus of
Carbon Atom
Dude
Date
Discovery
460 BC
“Atomos” Indivisible
John
Dalton
1803
Father of
Atomic Theory
JJ
Thomson
1898
Plum Pudding
Model of Electrons
Ernest
Rutherford
1911
Gold Foil Experiment
Nucleus
Niels
Bohr
1913
Electrons in Specific
Energy Levels
James
Chadwick
1932
Neutrons are neutral
(Jimmy Neutron)
No
Erwin
Schrodinger
1933
Electron Cloud
Wave Model
e-
Democritus
Drawing
e-
e-
+
Way to Remember the Order of the Scientists
for the Atomic Theory…
1.Democritus Democritus
2.Dalton Discovered
3.Thomson Tiny
4.Rutherford Round
5.Bohr Ball-like
6.Chadwick Circular
7.Schrodinger Spheres
Electron
Proton
Neutron
Negative
+
Positive
0
Neutral
Location:
Inside or Outside the Nucleus?
Outside
Inside
Inside
How much mass?
A lot or a little?
Little
A lot
A lot
X
X
Electrical Charge
(+,-, or 0)
Which 2 have about equal mass?
Which 2 equal each other in an atom &
are the same as the atomic #?
Which 2 are added together as the
atomic mass of the atom?
X
X
X
X
The Atoms Family - Atomic Math
Challenge
Atomic Number
Symbol
Name
Atomic Mass
electrons
protons
Atomic number equals the number of
____________ or
________________.
Atomic mass equals the number ofprotons
______________ +neutrons
_______________.
What was the “Small Stuff” anyway?
•Atoms
•Elements
•Molecules
•Compounds
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
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.ht
ml
Elements in the Earth & Air
Element
1. Oxygen
2. Silicon
3. Aluminum
4. Iron
5. Calcium
6. Potassium
7. Sodium
Symbol
Use
O
Breathing
Si
Glass/Rocks
Al
Foil/Cans
Fe
Steel
Ca
Bones/Teeth
K Bones/Muscles
Na
Salt
Elements In Our Bodies
N 2.4%
Ca 1.6%
Other 3.3%
H 10.2%
C 17.5%
O 65%
3)
6) Color Code Metals, Non-Metals, & Metalloids – 3 Different Colors
Blue= 93 Metals
Pink= 7 Metalloids
Yellow= 18 Nonmetals
14-year-old girl dies after inhaling helium
PHILIP CAULFIELD Thursday, February 23, 2012
•
A small town in southwest Oregon is in shock and a 27-year-old woman is facing criminal charges after a 14-yearold girl died after huffing helium during a booze- and pot-fueled bash over the weekend.
•
Ashley Long, an eighth-grader from Eagle Point, told her parents she was headed to a sleepover last Saturday, but
instead went to a party hosted by a friend's big sister, where she downed mixed drinks before taking hits from an
8-gallon helium canister, The Associated Press reported.
CBS/AP) EAGLE POINT, Ore. - Authorities say 14-year-old Ashley Long died last weekend after inhaling helium at a party
in Medford, Ore.
•
Police say the older sister of one of Long's friends was throwing the party, which included alcohol and marijuana.
•
After drinking on the drive over, and downing more drinks in the condo, Ashley took her turn on a tank of helium
that everyone else was inhaling to make their voices sound funny.
•
"My daughter didn't want to do it," said Long's stepfather, Justin Earp, calling the teen a victim of peer pressure.
"They put a mask up to her face. They said it would be OK. `It's not gonna hurt you. It'll just make you laugh and
talk funny.'"
•
Instead of merely experiencing a voice change, Long passed out and later died at a hospital, the result of an
obstruction in a blood vessel caused by inhaling helium from a pressurized tank.
•
Dr. Mark Morocco, associate professor of emergency medicine at the Ronald Reagan Medical Center in Los
Angeles, said what happens is similar to when a scuba diver surfaces too quickly. A gas bubble gets into the
bloodstream and can block blood flow to the brain, causing a stroke.
•
Police have arrested 27-year-old Katherine McAloon, who lived in the condo, on charges of providing alcohol and
marijuana to minors. Four men who were at the party have been questioned by police, but have not been
charged, said Medford Police Lt. Mike Budreau. More charges may be filed after police turn over their evidence to
the district attorney.
Covalent Bonding = Sharing e-
• Covalent Bond= sharing of valence electrons (ve-)
that occurs between 2 non-metals
Ex) Water H2O
H
X
X
= Hydrogen’s Electron
O
X
H
= Oxygen’s Electrons
Ionic Bonding = give or take eIonic Bond= giving or taking of valence electrons
(ve-) that occurs between metals and nonmetals
Ex) Salt NaCl – Na give outer e- to Cl
NaX
Cl
X
Na1+
Cl1-
Types of Chemical Reactions
What is a Chemical Reaction?
• A change in substances and a change in
energy.
• Chemical changes are a result of chemical
reactions.
• Neither matter or energy is created or
destroyed in a chemical reaction---only
changed.
Parts of a Chemical Reaction
• Reactants = What you start with
• Products = What you end up with
• → = yields sign
• REACTANTS → PRODUCTS
1) Synthesis Reactions
• To visualize a synthesis reaction look at the
following cartoon:
• In the cartoon, the skinny bird (reactant) and
the worm (reactant) combine to make one
product, a fat bird.
ENERGY OF CHEMICAL REACTIONS
• Chemical reactions always involve a change in
energy.
• Energy is cannot be created or destroyed.
• Energy is absorbed or released in chemical
reactions.
• Chemical reactions can be described as
Exothermic Reactions
• Chemical reactions in which energy is released
are exothermic.
• The energy that is released was originally
stored in the chemical bonds of the reactants.
• Often the heat given off causes the product(s)
to feel hot.
• Any reaction that involves combustion
(burning) is an exothermic chemical reaction.
Endothermic Reactions
• Chemical reactions in which energy is
absorbed are endothermic.
• Energy is required for the reaction to occur.
• The energy absorbed is often heat energy or
electrical energy.
• Adding electrical energy to metal oxides can
separate them into the pure metal and
oxygen.
• Adding electrical energy to sodium chloride
can cause the table salt to break into its
original sodium and chlorine parts.
p. 23 Matter Map #1
Made up of only
1 type of atom
When 2 or more
different elements
chemically combine
I. Metals, Metalloids, and Non-Metals
II. 7 Periods/Rows
III. 18 Groups/Families
I. Metals, Metalloids, & Non-Metals
left
Metals
• On the _______ of the staircase/zig-zag
(except for hydrogen)
• Most are shiny, hard, and dense.
high
• They conduct (transmit)
electricity and heat.
• They have mostly _______ melting and boiling
points.
• They are malleable (pounded into shapes) and
ductile (drawn into wire).
• Ex) Aluminum is a metal that is pounded into
8 Metalloids
on
X
Ununseptium was just discovered recently & is a metalloid! Cross off the 7 and put an 8!
• 7 elements _____ the staircase/zig-zag
both
• Properties of _______ metals and non-metals.
• Ex) Silicon is a metalloid. It conducts electricity
like a metal and is brittle like a non-metal. It is
used to make microchips.
Non-Metals
right
• To the _______ of the staircase/zig-zag
• 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.
II. 7 Periods/Rows
The Period # = the # of Electron Shells/Orbitals/Energy
Levels
1. This period contains the two __________
known
lightest
elements, hydrogen (H) and helium (He). Each
1X shell.
element has only 2 electron
I made another mistake! I know…I can’t believe it either! Cross off the 2 and put a 1!
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. The elements in this period have ___ electron shells.
Sodium (Na) and chlorine(Cl) are found 3in this period.
4. The elements in this period have 4 electron
metal
shells. This period includes
the element iron
(Fe), a commonly used _____.
5. The elements inAg
this period have 5 electron
shells. Silver (___) is found in this period
heavier
6. With
6 electron shells, some of these
__________ 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
radioactive
elements.
Many are ________________ some so unstable that they fall apart almost
instantly. Uranium (U) is found in this period
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
• All have 1 __________
in their outer shells.
• They are all soft and very reactive.
↑we read down the table.
• Their reactivity ___ as
• They are 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.
• Hydrogen will _______ ____ upon any contact with flames.
blow
up
• The metals are so reactive they will _______ the skin if touched.
burn
1. Alkali Metals (con’t)
•water
They tarnish rapidly and react violently with __________.
salts
• They easily form _______ with the halogens.
never found in their pure forms in nature, only
• They are _______
found as compounds
• The metals in this family are easy to identify because they
give off a different _________colors
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.
2. The Alkaline Earth Metals – Group 2
• 6 metals: Berylium, Magnesium, Calcium, Strontium,
Barium, and Radium.
soft and bright silvery-white in color.
• Are _______
high
• Have high melting points and _______
densities.
• All have ___2electrons in their outer shells.
• Are all reactive and react with water.
less reactive than the alkali metals.
• Are __________
• Have reactivity that ___ as ↑
we read down the table.
• Will oxidize or tarnish in air, but can be handled by
__________.
humansfound in nature in their pure forms.
• Are __________
never
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
– Used in ____________
because of their bright colors
– Beryllium is often added to other metals to make hard metal
alloys
__________,
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
3. __________
Thelargest
Transition
Metals
Groups
• The
family on the
Periodic–Table
with 403-12
members.
• Some of the more common and widely used members of this
family include iron, nickel, copper, zinc, silver, and gold.
• They are all __________- hard, shiny, and strong.
• Fairly stable, reacting slowly or not at all with air and water.
metals
• Most of them have very _______ melting points and boiling
points.
• ____________ is one exception- it is a liquid at room
high
temperature.
• Most are good ____________ of heat and electricity.
Mercury
• Most will dissolve in an acid, however, __________ resists acids.
• Most can bond to _________
in more ways than one, making
conductors
different compounds.
gold
oxygen
3. Transition Metals (con’t)
•
•
•
•
•
•
•
ductile
malleable
Most can be pounded into sheets or shapes
(____________) or drawn into a wire (____________)
strong
Most can form colored compounds with oxygen.
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,
4. The BCNO Family – Groups 13-16
25
• Large family with ___ members
• Some of the more common members of this family include
carbon, nitrogen, oxygen, aluminum, silicon, sulfur,
divided
arsenic, tin, and lead.
• This family is sometimes __________ into two or four
diverse
separate
families.
lightest
• Most __________ family
of elements.
• Name is from the ____________ of the elements in each
column- Boron, Carbon, Nitrogen, and Oxygen.
gases and metalloids in this family
• There are metals, nonmetals,
• Some members are _______solids
at room temp like nitrogen
and oxygen, but most are __________.
4. The BCNO Family (con’t)
bond with which
• They are reactive, but selective
elements they will __________.
• Mostitself
will bond with oxygen & oxygen will bond
bond
with __________
• 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
insulators
electronics,
nonmetals are used as ____________
on wires, poisons, fertilizers, in scuba gear, soap,
glass-making, solder, aircraft, weapons, drink cans,
5. The Halogens – Group 17
• Allpoisonous
have seven electrons in their outer shells and are
____________ non-metals.
electricity
• Most
reactive of all nonmetals, but are poor conductors of
down
____________
• Their reactivity decreases as we read __________ the table.
• Very small family consisting of only ___5elements- fluorine,
chlorine, bromine, iodine, and astatine
room
• At _______ temperature fluorine and chlorine are gases,
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 - __________.
5. The Halogens (con’t)
• Fluorine is added to toothpaste and water to prevent
nuclear
tooth decay
and combines with uranium to form
__________ fuel.
• Chlorine is added to water supplies and swimming
pools to kill germs. It is widely used in bleach and
Bromine
salt.
• ____________ 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
no
water supplies.
• Astatine is very rare, very radioactive, and has ___
Noble Gases
Group
18 outer
• They6.
areThe
very non-reactive
because -they
have _____
shells…inert.
full
rarest
• These are some of the __________
and heaviest elements.
• Six gases- helium, neon, argon, krypton, xenon, and radon
• __________, tasteless, and odorless
• Do not
mix
with
othersdo
not
gain,
share,
lose
electrons.
Colorless
• Chemically stable because they have a full outer energy
level.
• Helium, neon, and argon will _____ combine with other
elements
• Xenon, krypton, and radon will combine with other
elements, but difficult process. not
6. The Noble Gases (con’t)
• When an electrical current is passed through one of
color
these
gases it will glow in a characteristic
__________ ex) neon hasair
a characteristic orange-red
glow
• Helium is lighter than _____ and is used in balloons
and blimps
docolors
not
• Ne, Ar, Kr, & Xe are used in lights b/c of the
they make in light bulbs because they ___ ___ 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.
7. Lanthanides
• 1st of the 2 rows at the bottom
of the table
rare
• 15 elements known as the _______ Earth
Elements along with the Actinides
• Soft, shiny, silvery metals
• Malleable with high conductivity
• Reactive
• Burns in oxygen or air
• Oxidizes or tarnishes rapidly
7. Lanthanides (con’t)
•
•
•
•
•
•
except
Similar to transition metals _______ for poor
conductors
nature
React in similar
manner because they are found
togetherspark
in _______
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 ofgreen
colors are Europium = red and Terbium
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
manmade
• Neptunium and plutonium
were once thought to
be synthetic or __________, but found small
Allamounts in nature.
• _____ other members are synthetic
8. Actinides (con’t)
small
• After Curium, all are very
radioactive and have
been produced in such _______ 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.
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
Word Wall p.51
#
Word
Definition
Pic/Symbol
1
Atom
Tiny, makes up all matter
2
Proton
+ charge, n nucleus, larger than
e-
3
Neutron
O charge, n nucleus,
larger than e-
4
Electron
- charge, outside nucleus,
smaller than p+ & nO
5
Periodic
Table
Organizes all 118 elements
according to their properties
6
Bohr Model
Shows electron levels
2, 8, 8 or 18
7
Lewis
Structure
Valence electron dot model
Ne
8
Valence
Outermost e- on last shell
e-
#
S.O.M.
How it Looks…
How it
Moves…
1
Size &
Shape
Ex)
Solid
OOOOOOOOOOOOOOO
OOOOOOOOOOOOOOO
OOOOOOOOOOOOOOO
Tightly Packed Together
& Bonded!
Slow
Definite Ice Cube
(vibrate Volume &
Desk
Shape
in place)
2
Liquid
OO O O OO
O
O O O O
O O
OO O OO O
Loosely Packed Together
with Some Bonds!
3
Gas
4
Plasma
Fast
Takes
Shape of
Container &
Definite
Volume
Water
Juice
O
O O O
O
O
O
O
O O
Spread Apart with No
Bonds!
Faster
Takes
Shape &
Volume of
Container
Steam
Air
e-O
O OeO O
O
Oe- O
O
e-O
O
OeSpread Apart & Charged!
Fastest!
Electrically
Charged
Gas!
Stars
Lightning
O
O
O
4 States of Matter S.O.M.
1. Solid
2. Liquid
3. Gas
Solid
Liquid
Gas
Has a fixed volume and shape Assumes the shape of the part Assumes the shape & volume
of the container which it
of its container
occupies
Plasma
Electrically Charged Gas
Rigid - particles are locked
into place
They cannot slide past one
another
Particles can move/slide past
one another
Particles can move past one
another
Electrons have escaped the
orbits around the nucleus!
Particles move slowly
They vibrate in place
Particles move faster than a
solid and slower than a gas
Particles Move Fast
Particles move extremely Fast
Smart Start
The Periodic Table has 7 rows
called periods and 18 columns
called families. The metals are
to the left of the staircase and
the non-metals are to the
right. The metalloids are on
the staircase.
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!
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
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.ht
ml
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
Compounds
• A substance whose molecules contain atoms
of different elements combined chemically.
• Most matter exists as compounds.
• Examples= Water, Carbon Dioxide, etc.
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.
Atom
•Smallest part of a substance
•Has all of the properties of that substance
•Join together to make elements
Element
•Pure Substance
•Made of 1 kind
of atom
Separated in
Nuclear Reactions
Molecule
•2 or more atoms
joined tightly
together
•Smallest part
of compound
Compound
•Molecules
containing
atoms
of different
elements
Atom
• Smallest part of a substance
• Has all of the properties of
that substance
Element
• Pure Substance
• Made of 1 kind of atom
Molecule
•2 or more atoms
joined tightly
together
•Smallest part
of compound
Compound
• Molecules containing
atoms of different
elements
Pure elements?
Elements made of SINGLE
ATOMS?
An element made of
MOLECULES?
Mixture of TWO elements?
Mixture of THREE elements?
Pure compounds?
Mixture of TWO compounds?
Pure elements? A, C, D, E, F, H
Elements made of SINGLE
ATOMS? A, D, E, H
An element made of MOLECULES?
C, F
Mixture of TWO elements?
E, F
Mixture of THREE elements? H
Pure compounds? B, G
Mixture of TWO compounds? B
Physical vs. Chemical Properties
CHARACTERISTICS
PHYSICAL PROPERTIES (
) - can be observed or measured
WITHOUT
__________ changing the identity
of the matter. Observed with your
________________.
C______ O______ SENSES
Mass V__________
OLOR
DOR
OLUME
1) Thermal Conductivity= transfer of __________.
HEAT
Ex)
METALS
= GOOD
CONDUCTORS
2) State
of Matter=
the physical
form in which a substance exists.
S__________ L__________ G__________ P__________
Ex)
OLID
IQUID
AS
LASMA
NEON IS A GAS AT ROOM TEMP
POUNDED
3) Malleability= the ability to be __________
into thin
__________. SHEETS
Ex) Aluminum Foil
4)Ductility= the ability to be drawn or pulled into a
__________.WIRE
Ex) Copper
DISSOLVE
5) Solubility= the ability to __________
in another
substance.
Ex) SALT WATER
VOLUME
6) Density= Mass per unit __________.
Ex) WATER ~ 1G/ML
• CHEMICAL PROPERTIES = describes a substance
based on its ability to change into a _____
NEW with different properties. Not as easy to
substance
observe as physical properties.
• 1) Flammability= the ability to __________
BURN
• 2) Reactivity= when 2 substances get together
and
something __________. Many substances react
readily with________, ________,CHANGES
&/or ________.
WATER
• *You can observe chemical properties
only in
AIR
situations
in which theOXYGEN
identity of the substance
could change!*
Physical vs. Chemical Changes
PHYSICAL CHANGE= a change that affects one or more
physical properties of a substance.
ELTING
REEZING
HINTS: Breaking, M__________,F__________,
C__________,
RUSHING B__________,
OILING Sanding, etc.
PHYSICAL PROPERTIES CAN BE OBSERVED OR MEASURED
WITHOUT CHANING ITS IDENTITY
& A PHYSICAL CHANGE AFFECTS 1 OR MORE OF THOSE
PROPERTIES!
PHYSICAL CHANGES ARE OFTEN EASY TO __________
OBSERVE
BECAUSE THEY DO NOT CHANGE THE IDENTITY OF THE
SUBSTANCE.
CHEMICAL CHANGE= when one or more substances are changed into
entirely _____ substancesNEW
with completely _____________
DIFFERENT
properties.
These changes are not easy to undo. If possible, it would
take another reaction to do so.
HINTS: Reacting, B__________, Color Changes, Fizzing, Fire, Heating,
URNING
Producing _______, Light,
or Odor.
HEAT
CHEMICAL PROPERTIES ARE A SUBSTANCE’S _________ TO GO
THROUGH A CHANGE.
ABILITY
A CHEMICAL CHANGE IS THE ACTUAL __________ WHERE THAT
PROCESS
SUBSTANCE CHANGES INTO ANOTHER!
YOU CANNOT __________ CHEMICAL CHANGES USING PHYSICAL
UNDO
MEANS BECAUSE
NEW SUBSTANCES ARE FORMED! HOWEVER, SOME
CHEMICAL CHANGES _____ _____ REVERSED UNDER THE RIGHT
MAYCHANGES!
BE
CONDITIONS BY OTHER CHEMICAL
Physical Properties of Matter
•
•
•
•
•
•
•
•
•
•
•
•
•
Does not change the identity of the matter
Observed with your senses
Color
Odor
Mass
Volume
Conduction of Heat
State of Matter – Solid, Liquid, Gas
Change of State – Melting, Freezing, Boiling
Malleability
Ductility
Solubility
Density
Chemical Properties
• Changes into a new substance with different
properties
• Not as easy to observe as physical properties.
• Flammability
• Reactivity
• You can observe chemical properties only in
situations in which the identity of the
substance could change!
•
•
•
•
•
•
•
•
•
•
•
•
•
Physical Properties vs. Chemical Properties
of Matter p.14
Does not change the identity of
the matter
Observed with your senses
Color
Odor
Mass
Volume
Conduction of Heat
State of Matter – Solid, Liquid,
Gas
Change of State – Melting,
Freezing, Boiling
Malleability
Ductility
Solubility
Density
• Changes into a new
substance with different
properties
• Not as easy to observe as
physical properties.
• Flammability
• Reactivity
• Chemical Changes always
include Physical Changes
• You can observe chemical
properties only in situations
in which the identity of the
substance could change!
1) How would you classify copper
(Cu)?
a)
b)
c)
Element
Compound
Mixture
2) How would you classify a
cheeseburger?
a)
b)
c)
Element
Compound
Mixture
3) How would you classify
salt (NaCl)?
a)
b)
c)
Element
Compound
Mixture
4) How would you classify
Jell-O, Mayonnaise, & Fog?
a)
b)
c)
Solution
Suspension
Colloid
5) How would you classify Salt
Water, Kool-Aid, & Coffee?
a)
b)
c)
Solution
Suspension
Colloid
6) How would you classify Italian Salad
Dressing, Snow Globe, or Muddy Water?
a)
b)
c)
Solution
Suspension
Colloid
7) A pizza is what type of
mixture?
a)
b)
Homogenous
Heterogeneous
8) Milk is what type of mixture?
a)
b)
Homogenous
Heterogeneous
9) Flammability and Reactivity
are what type of properties?
a)
b)
Physical Property
Chemical Property
10) Color, Odor, Change of State are
what type of properties?
a)
b)
Physical Property
Chemical Property
11) Cutting grass, breaking glass, mixing
cake batter, freezing water, are all what
types of changes?
a)
b)
Physical Change
Chemical Change
12) Fizzing alka-seltzer, burning a
candle, rusting nail, are all what types
of changes?
a)
b)
Physical Change
Chemical Change
Answer Key
1)
2)
3)
4)
5)
6)
7)
8)
9)
10)
A
C
B
C
A
B
B
A
B
A
# Wrong = Grade
0-100 1-95 2-90 3-85 4-80 5-75 6-70 7-65 8-60 9-55 10-50
11-45 12-40 13-35 14-30 15-25 16-20 17-15 18-10 19-5 20-0
11) A
12) B
13) B
14) A
15) A
16) D
17) B
18) C
19) C
20) A
SOLID
LIQUID
1) Have a definite
volume
2) Maintain Shape
1) Have a definite
volume
2) Take the shape of
their container
3) Does not compress 3) Flow instead of
break
4) Break instead of
4) Does not compress
flow
5) May be molded or 5) Allow solids to pass
drawn
through
6) Become liquid when
heated
6) Become gas when
heated
pH Scale p.27
Tomatoes 4
Soda 3
0
1
2
Seawater 8
Milk 6.5
Blood 7.4
Vinegar 5.6
3
4
5
6
Detergent 10
7
8
Pure Water 7
9
10
11
Oven Cleaner 14
12
13
14
pH Scale p. 27 con’t
Acids
H+ > OHTurns Litmus Red
Taste Sour
Doesn’t Feel Slippery
React with Metals
Neutralized by Bases
Neutral
H+ = OH-
Bases
H+ < OHTurns Litmus Blue
Taste Bitter
Feels Slippery
Don’t React with Metals
Neutralized by Acids
Both conduct Electricity because they form ions & are electrolytes!
Ex)
Ex)
BrainPOP- pH Scale
1. The term _________ refers to the chemical potential of hydrogen.
2. The pH _________ measures how _________ or basic a substance on a scale of 1 to
14.
_______ measure from 1 to 7, while the _________ or alkaline side measures from 7
to 14.
3. Identify each as an acid (A) or a base (B).
____ Lemon juice ____ Soap ____ Battery acid ____ Hydrochloric acid
____ Toothpaste ____ Vinegar ____ Baking soda ____ Floor cleaner
4. Really strong acids and bases are found at the ____________ of the scale, while
those near the ______________ are weaker. Right in the middle at exactly 7, or pH
______________, you have pure water.
5. Acids contain ________________ ions (H+), while bases contain _______________
(OH-) ions. Ions are atoms that have either lost or gained ___________. In bases
you find hydroxyl ions, which have ______________ electrons. Hydrogen ions
found in acids are ___________ that have had an electron knocked off, which is
why these ions are always trying to get the lost electrons back. When you put a
metal in acid, the metal starts to ___________________.
6. Bases have the power to _______________ acids. The hydroxyl ion ___________ its
electron with the hydrogen ion. The H+ from the hydrogen ion and the OH- from
the hydroxyl ion bond together to form H2O, which is ____________ with pH
neutral. Different types of ___________ are formed depending on the types of
acids and bases involved in the reaction.
7. When Moby poured the baking soda (a base) into the vinegar (an acid), a reaction
occurred. Salt, water, and ___________ _____________ were produced by the
reaction.
8. _____________ are substances that can block changes in their pH for period of
time. You can find them on buffered aspirin, which keeps your ____________
___________ from dissolving the medicine too quickly.
Buffers are made by combining ___________ acids and bases. Buffers also are found in
our body to keep our the pH of our ___________ at or around 7.4.
9. Most science labs have pH paper, which is paper that has been soaked in a special
chemical __________________. They turn _________ in an acid and __________
in a base. By comparing the color of the pH paper to a chart, you can determine
how ______________ an acid or base is.
10. Constant reactions between acids and bases keep our _________________ from
being too acidic or too alkaline.
http://www.miamisci.org/ph/phpanel.html
Acids
•Lemon Juice
•Aspirin
•Lemon Soap
•Vinegar
•Tonic Water
Neutral
•Water
Bases
•Baking Soda
•Ammonia
•Milk of
Magnesia
•Lava Soap
•Borax
•Liquid Plumber
Acids
• B = pH~1 Hydrochloric Acid (HCl)
• C = pH~2 Lemon Juice
• D = pH~3 Vinegar
• F = ~4 Boric Acid
Neutrals
• E = pH~6 Distilled Water
• I = pH~7 Tap Water
• O = pH~8 Salt Water
•
Bases
V = pH~9 Baking Soda
(Bicarbonate/Sodium Hydrogen Carbonate)
• W = pH~10 Borax (Soap)
• X = pH~11 Washing Soda/Sodium Carbonate
• Y = pH~12 Ammonia
• Z = pH~13-14 Sodium Hydroxide
•
•
•
•
•
•
•
•
•
•
•
•
B = Hydrochloric Acid (HCl) pH~1
C = Lemon Juice pH~2
D = Vinegar pH~3
F = Boric Acid~4
E = Distilled Water pH~6
I = Tap Water pH~7
O = Salt Water pH~8
V = Baking Soda pH~9
(Bicarbonate/Sodium Hydrogen Carbonate)
W = Borax (Soap) pH~10
X = Washing Soda/Sodium Carbonate pH~11
Y = Ammonia pH~12
Z = Sodium Hydroxide pH~13-14
Mixtures
A mixture is a
combination of two or
more substances where
there is no chemical
combination or reaction.
Mixtures combine
physically in no specific
proportions.
They just mix.
Solids, liquids and gases
can be combined to create
a mixture.
You make a mixture by adding
at least one material to
another. When you add
material to a gas or liquid, the
material you add is called the
solute and the material you
are adding to is called the
solvent.
When you create a mixture,
there are no new
substances formed.
Each part of a mixture
keeps its own properties.
Mixtures can be
heterogeneous or
homogeneous.
Heterogeneous mixtures are
those where the substances
are not distributed evenly.
They usually involve a
mixture of a solid in a solid.
A mixture of stones in soil is
an example of a
heterogeneous mixture.
Homogeneous mixtures are
those where the materials
are evenly distributed
throughout.
Homogenized milk is an
example.
Mixtures can be classified
into 3 types: suspension,
colloidal and solution.
Some liquid mixtures are
solutions.
Suspension mixtures have
larger particles and are
heterogeneous.
They are cloudy
with at least 2 substances
visible –
1 that settles out.
Most mixtures are suspension
mixtures.
Italian salad dressing is a good
example.
Colloidal mixtures fall
between suspension and
solution mixtures. The
ingredients in colloidal
mixtures are smaller and
usually homogeneous. JellO and fog are examples.
They are cloudy,
uniform, and light is
dispersed.
Solutions are
homogeneous mixtures
that consist of microscopic
particles and evenly spread
out molecules. Sugar or
salt dissolved in water are
examples.
They are clear,
transparent,
and light passes
through them.
You can separate a simple
mixture by physical means.
No chemical reaction is
needed.
Homogeneous
or Heterogeneous?
Gasoline
Homogeneous
Trail Mix
Heterogeneous
Granite
Heterogeneous
Margarine
Homogeneous
Salad
Heterogeneous
Guess the Mixture
Which of the
following is a
Solution, Colloid, or a Suspension?
Kool-Aid
Solution
Fog
Colloid
Paint
Colloid
Salad Dressing
Suspension
Salt Water
Solution
Blood
Colloid
Milk
Colloid
Sand in Water
Suspension
Lemonade
Solution
Glue
Colloid
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
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
Example
• Name – Oxygen
• Atomic Number – 8
• Atomic Symbol – O
• Atomic Weight – 16.00
Oxygen
8
O
16.00
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.
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)
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.
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.
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.
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.
The gray area represents the metals.
The yellow area represents the semiconductors.
The blue area represents the nonmetals.
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.
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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
Atomic Structure
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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
Elements
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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
Matter
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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
States of Matter
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
Physical vs. Chemical Changes
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,
Mixtures
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