CHEMISTRY
Matter and Change
Chapter 3: Matter—Properties and
Changes
CHAPTER
3
Table Of Contents
Section 3.1
Properties of Matter
Section 3.2
Changes in Matter
Section 3.3
Mixtures of Matter
Section 3.4
Elements and Compounds
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SECTION
3.1
Properties of Matter
• Identify the characteristics of a substance.
• Distinguish between physical and chemical
properties.
• Differentiate among the physical states of matter.
density: a ratio that compares the mass of an
object to its volume
SECTION
Properties of Matter
3.1
states of matter
physical property
solid
extensive property
liquid
intensive property
gas
chemical property
vapor
Most common substances exist as solids,
liquids, and gases, which have diverse
physical and chemical properties.
SECTION
Properties of Matter
3.1
Substances
• Matter is anything that has mass and takes up
space.
• Matter is everything around us.
• Matter with a uniform and unchanging
composition is a substance.
SECTION
3.1
Properties of Matter
States of Matter
• The physical forms of matter, either solid, liquid,
or gas, are called the states of matter.
• Solids are a form of matter that
have their own definite shape and
volume.
• Liquids are a form of matter that
have a definite volume but take the
shape of the container.
SECTION
3.1
Properties of Matter
States of Matter (cont.)
• Gases have no definite shape or
volume. They expand to fill their
container.
• Vapor refers to the *
SECTION
3.1
Properties of Matter
Physical Properties of Matter
• A physical property is a *
SECTION
3.1
Properties of Matter
Physical Properties of Matter (cont.)
• Extensive properties, such as mass,
length, and volume, are *
• Intensive properties, such as density, are
dependent * .
SECTION
3.1
Properties of Matter
Chemical Properties of Matter
• * is called a chemical property.
– Iron forming rust
– Copper turning green in the air
SECTION
3.1
Properties of Matter
Observing Properties of Matter
• A substance can change form–an important
concept in chemistry.
• Both physical and chemical properties can
change with specific environmental conditions,
such as temperature and pressure.
SECTION
3.2
Changes in Matter
• Define physical change and list several common
physical changes.
• Define chemical change and list several indications
that a chemical change has taken place.
• Apply the law of conservation of mass to chemical
reactions.
observation: orderly, direct information gathering about a
phenomenon
SECTION
Changes in Matter
3.2
physical change
phase change
chemical change
law of conservation of mass
Matter can undergo physical and chemical
changes.
SECTION
3.2
Changes in Matter
Physical Changes
• * is known as a physical change.
• A phase change is a transition of matter from
one state to another.
• Boiling, freezing, melting, and condensing all
describe phase changes in chemistry.
SECTION
3.2
Changes in Matter
Chemical Changes
• * is called a chemical change.
• Decomposing, rusting, exploding, burning, or
oxidizing are all terms that describe chemical
changes.
SECTION
3.2
Changes in Matter
Conservation of Mass
• The law of conservation of mass states that
*.
• The mass of the reactants equals the mass of
the products.
massreactants = massproducts
SECTION
3.3
Mixtures of Matter
• Contrast mixtures and substances.
• Classify mixtures as homogeneous or
heterogeneous.
• List and describe several techniques used to
separate mixtures.
substance: a form of matter that has a uniform and
unchanging composition; also known as a pure
substance
SECTION
3.3
Mixtures of Matter
mixture
distillation
heterogeneous mixture
crystallization
homogeneous mixture
sublimation
solution
chromatography
filtration
Most everyday matter occurs as
mixtures—combinations of two or more
substances.
SECTION
Mixtures of Matter
3.3
Mixtures
• A mixture is a *.
• A homogenous mixture is a mixture where
the *.
SECTION
Mixtures of Matter
3.3
Mixtures (cont.)
• Homogeneous mixtures are also called
solutions.
• A heterogeneous mixture is a mixture where
the individual substances remain distinct.
SECTION
3.3
Mixtures (cont.)
Mixtures of Matter
SECTION
3.3
Mixtures of Matter
Separating Mixtures
• Filtration is a technique that *
• Distillation is a separation technique *
• Crystallization is a separation technique for *
SECTION
3.3
Mixtures of Matter
Separating Mixtures (cont.)
• Sublimation is the process of a solid changing
directly to a gas, which can be used to separate
mixtures of solids when one sublimates and the
other does not.
• Chromatography is a *
SECTION
3.4
Elements and Compounds
• Distinguish between elements and compounds.
• Describe the organization of elements in the periodic
table.
• Explain how all compounds obey the laws of definite
and multiple proportions.
proportion: the relation of one part to another or to the
whole with respect to quantity
SECTION
Elements and Compounds
3.4
element
law of definite proportions
periodic table
percent by mass
compound
law of multiple proportions
A compound is a combination of two or
more elements.
SECTION
Elements and Compounds
3.4
Elements
• An element is a *
• 92 elements occur naturally on Earth.
• Each element has a unique name and a one,
two, or three-letter symbol.
• The periodic table organizes the *
SECTION
3.4
Elements and Compounds
Elements (cont.)
• The periodic table organizes *
• Elements in the same group have similar
chemical and physical properties.
• The table is called periodic because the pattern
of similar properties repeats from period to
period.
SECTION
3.4
Elements and Compounds
Compounds (cont.)
• A compound is a *.
• Most of the matter in the universe exists as
compounds.
• Table salt, NaCl, and water, H2O, are
compounds.
• Unlike elements, compounds can be broken
into smaller components by chemical means.
SECTION
3.4
Elements and Compounds
Compounds (cont.)
• Separating a
compounds into its
elements often requires
external energy, such
as heat or electricity.
• This figure shows
electrolysis of water to
form hydrogen and
oxygen gas.
SECTION
3.4
Elements and Compounds
Compounds (cont.)
• The properties of a compound are different
from its component elements.
SECTION
3.4
Elements and Compounds
Law of Definite Proportions
• The law of definite proportions states
that a compound is always composed of
the same elements in the same proportion
by mass, no matter how large or small the
sample.
–Ex. Water is always composed of 2 Hydrogen to
1 Oxygen
SECTION
3.4
Elements and Compounds
Law of Definite Proportions (cont.)
• The relative amounts are expressed as
percent by mass, the *.
SECTION
3.4
Elements and Compounds
Law of Definite Proportions (cont.)
• This table demonstrates that the percentages of
elements in sucrose remain the same despite
differences in sample amount.
SECTION
3.4
Elements and Compounds
Law of Multiple Proportions
• The law of multiple proportions states that
when different compounds are formed by a
combination of the same elements, different
masses of one element combine with the same
relative mass of the other element in whole
number ratios.
– Ex. Peroxide, H2O2, and water, H2O.
– Different compounds formed from the same elements.
– Hydrogen mass the same in both compounds but oxygen
mass is a 2:1 ratio in peroxide to water.
SECTION
3.4
Elements and Compounds
Law of Multiple Proportions (cont.)
SECTION
Properties of Matter
3.1
Study Guide
Key Concepts
• The three common states of matter are solid, liquid,
and gas.
• Physical properties can be observed without altering a
substance’s composition.
• Chemical properties describe a substance’s ability to
combine with or change into one or more new
substances.
• External conditions can affect both physical and
chemical properties.
SECTION
Changes in Matter
3.2
Study Guide
Key Concepts
• A physical change alters the physical properties of a
substance without changing its composition.
• A chemical change, also known as a chemical reaction,
involves a change in a substance’s composition.
• In a chemical reaction, reactants form products.
• The law of conservation of mass states that mass is
neither created nor destroyed during a chemical reaction;
it is conserved.
massreactants = massproducts
SECTION
Mixtures of Matter
3.3
Study Guide
Key Concepts
• A mixture is a physical blend of two or more pure
substances in any proportion.
• Solutions are homogeneous mixtures.
• Mixtures can be separated by physical means.
Common separation techniques include filtration,
distillation, crystallization, sublimation, and
chromatography.
SECTION
Elements and Compounds
3.4
Study Guide
Key Concepts
• Elements cannot be broken down into simpler
substances by physical or chemical means.
• Elements are organized in the periodic table of the
elements.
• Compounds are chemical combinations of two or more
elements and their properties differ from the properties
of their component elements.
SECTION
Elements and Compounds
3.4
Study Guide
Key Concepts
• The law of definite proportions states that a
compound is always composed of the same
elements in the same proportions.
• The law of multiple proportions states that if elements
form more than one compound, those compounds will
have compositions that are whole-number multiples of
each other.