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
(+) Positive Protons (0) Neutral Neutrons Nucleus
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.DemocritusFirst Atomos - Indivisible 2. John
DaltonAtomic Theory 3. J.J. ThomsonElectrons - Plum Pudding 4.
Ernest Rutherford+ Charged Nucleus Gold Foil 5. Niels BohrElectrons
Specific NRG Levels 6. James ChadwickNeutrons (Jimmy Neutron) 7.
Erwin SchrodingerElectron Cloud Wave
Slide 11
Way to Remember the Order of the Scientists for the Atomic
Theory Democritus Discovered Dalton Tiny Thomson Round Rutherford
Circular Chadwick Ball-like Bohr Spheres Schrodinger
Slide 12
IndivisibleElectronNucleusOrbitElectron Cloud Greek X Dalton X
Thomson X Rutherford X X Bohr X X X Wave X X X
Slide 13
Dont 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? Lets check it out
http://www.micro.magnet.fsu.edu/primer/jav
a/scienceopticsu/powersof10http://www.micro.magnet.fsu.edu/primer/jav
a/scienceopticsu/powersof10 http://www.cellsalive.com/howbig.htm
http://www.strangematterexhibit.com/struc
ture.htmlhttp://www.strangematterexhibit.com/struc ture.html
http://learn.genetics.utah.edu/content/begin
/cells/scale/http://learn.genetics.utah.edu/content/begin
/cells/scale/ http://www.azonano.com/Details.asp?Article
ID=1780http://www.azonano.com/Details.asp?Article ID=1780
Slide 16
Whats the Matter? Matter
Slide 17
Whats the Matter? Matter Has Mass= The Amount of Matter in an
Object Stuff that Everything is made of! Made of Atoms 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 Element Pure Substance Made of 1 kind of atom
Compound Molecules containing atoms of different elements Molecule
2 or more atoms joined tightly together Smallest part of
compound
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 H 2 O O HH =
Hydrogens Electron = Oxygens Electrons
Slide 32
Ionic Bonding = give or take e- Ionic Bond= giving or taking of
electrons that occurs between metals and non-metals Ex) Salt NaCl
Na give outer e- to Cl Na Cl Na 1+ Cl 1-
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 (cont) 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. monatomic
ionpolyatomic ionoxygencarbonatesulfateoxyanions 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. HSO
Slide 35
Elements in the Earth & Air Element Symbol Use 1.Oxygen O
Breathing 2.Silicon Si Glass/Rocks 3.Aluminum Al Foil/Cans 4.Iron
Fe Steel 5.Calcium Ca Bones/Teeth 6.Potassium K Bones/Muscles
7.Sodium Na Salt
Slide 36
Elements In Our Bodies O 65% C 17.5% H 10.2% N 2.4% Ca 1.6%
Other 3.3%
Slide 37
Nucleus P+ & N O 1 st = 2 e- 2 nd = 8 e- 3 rd = 18 e-
Slide 38
Periodic Table Atomic # = # of p+ = # of e- # of n 0 = 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+ & N O 1 st = 2 e- 2 nd = 8 e- 3 rd = 18 e-
Slide 41
Nucleus P+ & N O 1 st = 2 e- 2 nd = 8 e- 3 rd = 18 e-
Acting Out Bohr Models!
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
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 wasnt 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 Atomic Number 8 Atomic Symbol O Atomic
Weight 16.00 Oxygen 8 16.00 O
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. (Dont 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 On the _______
of the staircase/zig-zag (except for hydrogen) Most are shiny,
hard, and dense. 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 aluminum foil. left high
Slide 64
Metalloids 7 elements _____ the staircase/zig-zag 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. on both
Slide 65
Non-Metals To the _______ of the staircase/zig-zag Most have
low melting points Are dull and brittle if solid. Most are _______
conductors of heat and electricity. Ex) Sulfur is a non-metal. It
is often used to make fertilizer. right poor
Slide 66
II. 7 Periods/Rows The Period # = the # of Electron
Shells/Orbitals/Energy Levels 1.This period contains the two
__________ 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 ____________,
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 in this period. lightest atmosphere 3
Slide 67
4. The elements in this period have 4 electron shells. This
period includes the element iron (Fe), a commonly used _____. 5.
The elements in this period have 5 electron shells. Silver (___) is
found in this period 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 elements. Many are
________________ - some so unstable that they fall apart almost
instantly. Uranium (U) is found in this period metal Ag heavier
radioactive
Slide 68
III. 18 Columns/Groups/Families 1.Alkali Metals 2.Alkaline
Earth Metals 3.Transition Metals 4.BCNO Family 5.Halogens 6.Noble
Gases 7.Lanthanides 8.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
________________. All have 1 __________ in their outer shells. They
are all soft and very reactive. Their reactivity ___ as we read
down the table. 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. Hydrogen will _______
____ upon any contact with flames. The metals are so reactive they
will _______ the skin if touched. reactivity electron blow up
burn
Slide 70
1. Alkali Metals (cont) They tarnish rapidly and react
violently with __________. They easily form _______ with the
halogens. They are _______ found in their pure forms in nature,
only found as compounds The metals in this family are easy to
identify because they give off a different _________ when burned:
Lithium = crimson, Sodium = yellow, Potassium = violet, Rubidium =
reddish-violet, Cesium = blue, and Francium = Rare Little is Known
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. water salts never colors Uses
Slide 71
2. The Alkaline Earth Metals Group 2 6 metals: Berylium,
Magnesium, Calcium, Strontium, Barium, and Radium. Are _______ and
bright silvery-white in color. Have high melting points and _______
densities. All have ___ electrons in their outer shells. Are all
reactive and react with water. Are __________ reactive than the
alkali metals. Have reactivity that ___ as we read down the table.
Will oxidize or tarnish in air, but can be handled by __________.
Are __________ found in nature in their pure forms. soft high 2
less humans never
Slide 72
2. Alkaline Earth (cont) Are good conductors of electricity
Burn in different colors: Magnesium = Bright White, Calcium =
Orange-Red, Strontium = Bright Red, Barium = Yellowish-Green, and
Radium = Crimson Used in ____________ because of their bright
colors Beryllium is often added to other metals to make hard 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 __________.
fireworks alloys cancer
Slide 73
3. The Transition Metals Groups 3-12 The __________ family on
the Periodic Table with 40 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. Most of them have very _______ melting points and boiling
points. ____________ is one exception- it is a liquid at room
temperature. Most are good ____________ of heat and electricity.
Most will dissolve in an acid, however, __________ resists acids.
Most can bond to _________ in more ways than one, making different
compounds. largest metals high Mercury conductors gold oxygen
Slide 74
3. Transition Metals (cont) Most can be pounded into sheets or
shapes (____________) or drawn into a wire (____________) 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, bicycles, cooking utensils, paints, cleaners, etc. malleable
ductile strong
Slide 75
4. The BCNO Family Groups 13-16 Large family with ___ members
Some of the more common members of this family include carbon,
nitrogen, oxygen, aluminum, silicon, sulfur, arsenic, tin, and
lead. This family is sometimes __________ into two or four separate
families. Most __________ family of elements. Name is from the
____________ of the elements in each column- Boron, Carbon,
Nitrogen, and Oxygen. There are metals, nonmetals, and metalloids
in this family Some members are _______ at room temp like nitrogen
and oxygen, but most are __________. 25 divided diverse lightest
gases solids
Slide 76
4. The BCNO Family (cont) They are reactive, but selective with
which elements they will __________. Most will bond with oxygen
& oxygen will 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 electronics, nonmetals are used
as ____________ on wires, poisons, fertilizers, in scuba gear,
soap, glass-making, solder, aircraft, weapons, drink cans, foil,
pots, and pans. bond itself bond insulators
Slide 77
5. The Halogens Group 17 All have seven electrons in their
outer shells and are ____________ non-metals. Most reactive of all
nonmetals, but are poor conductors of ____________ Their reactivity
decreases as we read __________ the table. Very small family
consisting of only ___ elements- fluorine, chlorine, bromine,
iodine, and astatine At _______ temperature fluorine and chlorine
are gases, bromine is a liquid, and iodine and astatine are solids
______ reactive and never found in their pure forms in nature.
Combine with alkali metals to form a family of chemical compounds -
__________. poisonous electricity 5 down room Very salts
Slide 78
5. The Halogens (cont) Fluorine is added to toothpaste and
water to prevent 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 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 water supplies. Astatine is very rare, very radioactive, and has
___ uses. nuclear Bromine no
Slide 79
6. The Noble Gases - Group 18 They are very non-reactive
because they have _____ outer shellsinert. These are some of the
__________ and heaviest elements. Six gases- helium, neon, argon,
krypton, xenon, and radon __________, 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 _____ combine with other elements Xenon, krypton,
and radon will combine with other elements, but difficult process.
full Colorless rarest not
Slide 80
6. The Noble Gases (cont) When an electrical current is passed
through one of these gases it will glow in a characteristic
__________ ex) neon has a characteristic orange- red glow Helium is
lighter than _____ and is used in balloons and blimps Ne, Ar, Kr,
& Xe are used in lights b/c of the colors they make in light
bulbs because they ___ ___ react with the metal (tungsten) that
makes the filament. __________ is radioactive and is used in the
treatment of cancer. Argon is the most abundant Noble Gas, making
up one percent of the atmosphere. color air do not Radon
Slide 81
7. Lanthanides 1st of the 2 rows at the bottom of the table 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 rare
Slide 82
7. Lanthanides (cont) Similar to transition metals _______ for
poor conductors React in similar manner because they are found
together 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 of colors are Europium = red and Terbium =
_______ except nature spark green
Slide 83
8. Actinides 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 be synthetic or __________, but found small amounts in nature.
_____ other members are synthetic bottom manmade All
Slide 84
8. Actinides (cont) 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. ____________ is used in smoke detectors. small
Americium
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.Who was the first to develop the Periodic
Table? a.Henry Mosely b.Niels Bohr c.Dmitri Mendeleev 2.The modern
Periodic Table is designed according to increasing a.Atomic Mass
b.Atomic Number c.Atomic Theory 3.Most of the elements are a.Solids
b.Liquids c.Gases 4.The Periodic Table is divided into which of the
following 3 properties? a.Metals, Nonmetals, and Metalloids
b.Metals, Solids, and Liquids c.Metals, Nonmetals, and Gases
5.Where on the Periodic Table are the Metalloids located? a.To the
Left of the Staircase/Zig-Zag b.On the Staircase/Zig-Zag c.To the
Right of the Staircase/Zig-Zag
Slide 87
6. What are the horizontal rows on the periodic table called?
a.Periods b.Groups c.Families 7. How many rows are there? a.7 b.12
c.18 8. What are the vertical columns on the periodic table called?
a.Rows b.Periods c.Families 9. How many columns are there? a.7 b.12
c.18 10. As you move across the Periodic Table from left to right,
what happens to the reactivity of the elements? a.Increases
b.Decreases c.Stays the Same
118 Elements 1 st created by Dmitri Mendeleev 1 st 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
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
Nucleus with Protons & Neutrons Electron
Shells/Orbitals/Levels Electrons = approx. size of P & N 2, 8,
18 Periodic Table Rows = # of Shells 7 Shell Max Periodic Table
Columns = # of Valence e- Electron Cloud Wave Model
Slide 97
Elements
Slide 98
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
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
Reactants = Start With Products = End With Reactants Products 4
Types of Chemical Reactions: 1.Synthesis 2.Decomposition 3.Single
Displacement 4.Double Displacement
Slide 103
Matter
Slide 104
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
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 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
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