Matter and Change
Chemistry is…
 …the study of the
composition, structure,
and properties of
matter and the changes
it undergoes
C2H5OH + 3 O2  2 CO2 + 3 H2O + Energy
Reactants

Products
 Matter
 Anything that has mass and occupies space.
 The “stuff” we are made up of.
 Mass
 A measure of the amount of matter.
 How much “stuff” is there.
Atom
 The smallest unit of an element that maintains
 the properties of that element
Element

-A pure substance made of only one kind of atom
 -There are 115 elements on the periodic table.
 -88 occur naturally.
 Compound
 A substance that is made from
the atoms of two or more
elements that are chemically
bonded.
Example -Sucrose – C12H22O11
Sucrose is also known as table
sugar, and is used to make
Gummy Bears!
Properties of Matter
 Extensive Properties - depend on the amount of
matter that is present.
 Examples - Volume, Mass, Energy Content (think
calories!)
 Intensive Properties - Do not depend on the
amount of matter present.
 Examples – Melting point, Boiling Point,Density
Properties of Matter
 Physical Properties – Characteristics that can
change without becoming a different substance
 Examples – odor, color, physical state
 Chemical Properties – its ability to form a new
substance.
 Examples – Wood burning, Rusting of steel,
Digestion of food
Chemical
Change
A change in which one or more substances are converted into different
substances.
This is on an atomic level.
Heat and light are often
evidence of a chemical
change.
Change
A change in a substance that does not involve a change in the identity of
the substance.
Example:
Phase Changes
Mixtures
Anything substance with a variable composition.
EX.
Wood
Soda
Coffee
air
Pure Substance
-contains only a single element or compound
EX.
Gold ring
distilled water
NOT EXAMPLES: water from the tap, soda
Homogeneous Mixtures
-same through out
EX. Sea water, plastic cup
Heterogeneous Mixtures
-has areas with different properties
EX. Wood, bucket of sand and water
Classification of Matter
States of Matter
 Matter can take forms/states
 What are they?
How do solids behave?
 The particles of a
solid are very tightly
packed and move
slightly (vibrate).
 Definite shape
 Definite Volume
How do liquids behave?
 Particles in a liquid
can slide past each
other
 Indefinite shape –
takes shape of
container
 Definite volume
How do gases behave?
 Particles in a gas
can move about
freely
 Indefinite shape
 Indefinite volume
How does plasma behave?
 Particles in plasma
are broken (charged
particles)
 Indefinite shape
 Indefinite volume
 Conduct electricity
Phase
Differences
Solid – definite volume and shape; particles packed in
fixed positions.
Liquid – definite volume but indefinite shape;
particles close together but not in fixed positions
Gas – neither definite volume nor definite shape;
particles are at great distances from one another
Plasma – high temperature, ionized phase of matter as
found on the sun.
Copper Phases - Solid
Copper Phases - Liquid
Copper Phases – Vapor (gas)
States of Matter Graphic Organizer!
For each of the states of Matter complete this
information:
 State
 Definition
 Proximity (how close the particles are to eachother)
 Movement of the particles
 Three examples
Properties of Metals
Metals are good
conductors of heat and
electricity

 Metals are malleable (can
be hammered into thin
sheets)
 Metals are ductile (can be
pulled into wires)
Metals have luster (shiny)
Examples of Metals
Potassium,
K reacts
with water
and must be
stored in
kerosene or
oil
Copper, Cu, is a relatively soft
metal, and a very good
electrical conductor.
Zinc, Zn, is
more stable
than potassium
Mercury, Hg, is the only
metal that exists as a
liquid at room
Properties of Nonmetals
Carbon, the graphite in “pencil lead” is a
great example of a nonmetallic element.
 Nonmetals are poor conductors of heat
and
electricity
 Nonmetals tend to be brittle
 Nonmetals do not have luster
 Many nonmetals are gases at room
temperature
Examples of Nonmetals
Sulfur, S, was
once known as
“brimstone”
Graphite is not the only
pure form of carbon, C.
Diamond is also carbon;
the color comes from
impurities caught within
the crystal structure
Microspheres
of
phosphorus,
P, a reactive
nonmetal
Properties of Metalloids
Metalloids straddle the
border between metals
and nonmetals on the
periodic table.
 They have properties of both metals and
nonmetals.
Metalloids are more brittle than metals,
less brittle than most nonmetallic solids
 Metalloids are semiconductors of
electricity
 Some metalloids possess metallic luster
Silicon, Si – A Metalloid
 Silicon has metallic luster
 Silicon is brittle like a
nonmetal
 Silicon is a semiconductor of
electricity
Other metalloids include:
 Boron, B
 Germanium, Ge
 Arsenic, As
 Antimony, Sb
 Tellurium, Te
Period
Group or Family
The Periodic Table
Group or
family
Period
Describe how to read the periodic
table:
 Every table has:
Describe how to read the periodic
table:
Atomic Symbol:
 One or two letters chosen to represent an element.
 These symbols are used every where in the world
 Usually, abbreviation of the element or the abbreviated
Latin name of the element.
Describe how to read the periodic
table:
Atomic Number
The number of protons in an atom identifies the
element.
Describe how to read the periodic
table:
Atomic Mass:
 The average mass of an element
 Measured in atomic mass units ("amu”)
 Is an average of all the isotopes of an element.
Mass Number:
 protons + neutrons = Mass Number
 Is always a whole number.
What are the 3 major parts of an atom?
 Proton
 Neutron
 Electron
The Nucleus
 The central part of an atom
 Composed of protons and neutrons
 Contains most of an atom's mass
 Discovered by Ernest Rutherford in 1911.
Protons
 Positively charged particles found in the atomic
nucleus.
 Have a mass of 1 AMU
 Are made from other particles called quarks.
Neutrons
 Uncharged particles found in the atomic nucleus
 Have a mass of 1 AMU
 Made from other particles called quarks.
Electron
 Negatively charged particles that surround the atom's
nucleus.
 Have no mass??
 Determine properties of the atom.
 Chemical reactions involve sharing or exchanging
electrons.
Draw a Diagram of an Atom
A diagram showing the location of each
part of the atom.
Atomic Symbols
 Some show the mass number and atomic number
in nuclear symbol form
mass number
23 Na
atomic number
11
Isotopes
Atoms that have the same number
of protons but different numbers of
neutrons
Describe Isotope
Example:
http://education.jlab.org/glossary/isotope.html
Naturally occurring carbon consists of three isotopes,
12C, 13C, and 14C. State the number of protons,
neutrons, and electrons in each of these carbon atoms.
12C
13C
14C
6
6
6
#p+ _______
_______
_______
#no _______
_______
_______
#e- _______
_______
_______
Answers
12C
6
6
13C
6
14C
#p+ 6
6
6
#no 6
7
8
#e- 6
6
6
Some quick questions
An atom has 14 protons and 20 neutrons.
A. Its atomic number is
1) 14
2) 16
3) 34
B. Its mass number is
1) 14
2) 16
C. The element is
1) Si
2) Ca
3) 34
3) Se
D. Another isotope of this element is
1) 34X
2) 34X
3) 36X
16
14
14
IONS
 IONS are atoms or groups of atoms with a
positive or negative charge.
 Taking away an electron from an atom gives a
CATION with a positive charge
 Adding an electron to an atom gives an
ANION with a negative charge.
 To tell the difference between an atom and an
ion, look to see if there is a charge in the
superscript! Examples: Na+ Ca+2 I- O-2
PREDICTING ION CHARGES
In general
 metals (Mg) lose electrons ---> cations
 nonmetals (F) gain electrons ---> anions
Learning Check – Counting
State the number of protons, neutrons, and electrons in
each of these ions.
39 K+
16O -2
41Ca +2
19
#p+ ______
8
______
20
_______
#no ______
______
_______
#e- ______
______
_______