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Matter—Properties and Change
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 3.1 Properties of Matter (cont.)
states of matter
physical property
solid
extensive property
liquid
intensive property
gas
chemical property
Vapor
Plasma
Most common substances exist as
solids, liquids, and gases, which have
diverse physical and chemical
properties.
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 pure substance.
• Particles of matter are always in motion.
• The kinetic energy (speed) of these particles
increases as temperature increases.
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. Very Low Kinetic Energy
• Liquids are a form of matter that
have a definite volume but take the
shape of the container. Low Kinetic
Energy
States of Matter (cont.)
• Gases have no definite shape or
volume. They expand to fill their
container. Very High Kinetic
Energy
• Vapor refers to the gaseous state of a
substance that is normally a solid or liquid at
room temperature.
• Plasma very high kinetic energy- particles
collide with enough energy to break into
charged particles (+/-).
• gas-like, variable shape & volume
Physical Properties of Matter
• A physical property is a characteristic that
can be observed or measured without
changing the sample’s composition.
Physical Properties of Matter (cont.)
• Extensive properties are dependent on
the amount of substance present, such
as…
• Intensive properties are independent of the
amount of substance present, such as…
Extensive vs. Intensive
• Examples:
– boiling point
intensive
– volume
extensive
– mass
extensive
– density
intensive
– conductivity
intensive
Chemical Properties of Matter
• The ability of a substance to combine with
or change into one or more other
substances is called a chemical property.
• describes the ability of a substance to
undergo changes in identity
– Examples:
Observing Properties of Matter
• A substance can change
• Chemical properties can change with specific
environmental conditions, such as temperature
and pressure.
Physical vs. Chemical
• Examples:
– melting point
physical
– flammable
chemical
– density
physical
– magnetic
physical
– tarnishes in air
chemical
Section 3.1 Assessment
Density is what kind of property?
A. atomic
B. intensive
C. extensive
D
C
A
0%
B
D. dependent
A. A
B. B
C. C
0%
0%
0%
D. D
Section 3.1 Assessment
What defines a gas?
A. Gases have a definite volume
and shape.
0%
A
D. Gases have a definite shape
but no definite volume.
0%
B
C. Gases have no definite volume or
shape.
A
B
C
D
0%
0%
D
A.
B.
C.
D.
C
B. Gases have a definite volume
but take the shape of their container.
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 3.2 Changes in Matter (cont.)
physical change
phase change
chemical change
law of conservation of mass
Matter can undergo physical and
chemical changes.
Physical Changes
• A change that alters a substance without
changing its composition is known as a
physical change.
• A phase change is a transition of matter
from one state to another.
• Examples:
Chemical Changes
• A change that involves one or more
substances turning into new substances is
called a chemical change.
• changes the identity of a substance
• products have different properties
• Examples:
• Signs of a Chemical Change
– change in color or odor
– formation of a gas
– formation of a precipitate (solid)
– change in light or heat
http://www.youtube.com/watch?v=QL7V3
L3dfDM
Physical vs. Chemical
• Examples:
– rusting iron
chemical
– dissolving in water
physical
– burning a log
chemical
– melting ice
physical
– grinding spices
physical
• Reaction occurs when one or more
substances are changed into new
substances.
• Reactants- stuff you start with; elements or
compounds
• Products- What you make
products have NEW PROPERTIES
• Yields Arrow separates reactants and
products
Conservation of Mass
• The law of conservation of mass states
that mass is neither created nor destroyed
in a chemical reaction, it is conserved.
• The mass of the reactants equals the mass of
the products.
massreactants = massproducts
Section 3.2 Assessment
When one substances turns into another,
what kind of change has taken place?
A. chemical reaction
B. physical reaction
D
A
0%
C
D. nuclear reaction
A. A
B. B
C. C
0%
0%
0%
D. D
B
C. extensive reaction
Section 3.2 Assessment
The law of conservation of mass states
that:
A. Matter can be created and destroyed.
B. Matter can be created but not destroyed.
0%
0%
D
0%
A
B
C
D
C
0%
A
D. The products of a reaction must
have the same mass as the
reactants.
A.
B.
C.
D.
B
C. The products of a reaction always
have a greater mass than the
reactants.