CHAPTER 3
Matter – Properties and Change
National Standards for Chapter 3
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UCP.1 Systems, order, and organization
UCP.2 Evidence, models, and explanation
UCP.3 Change, constancy, and measurement
A.1 Abilities necessary to do scientific inquiry
A.2 Understandings about scientific inquiry
B.1 Structure of atoms
B.2 Structure and properties of matter
B.3 Chemical reactions
B.6 Interactions of energy and matter
G.1 Science as a human endeavor
G.2 Nature of scientific knowledge
G.3 Historical perspectives
Vocabulary/Study Guide
• Define each term using the Glossary
• Either write on the handout, or use your own
paper
• This is due on Test Day (tentatively, Monday,
September 23)
Section 1: Properties of Matter
• National Standards:
– UCP.1 Systems, order, and organization
– A.1 Abilities necessary to do scientific inquiry
– B.2 Structure and properties of matter
Objectives – Section 1
•Identify the characteristics of a substance.
•Distinguish between physical and chemical
properties.
•Differentiate among the physical states of
matter.
• REVIEW VOCABULARY:
• density: a ratio that compares the mass of an object to its
volume
New Vocabulary
states of matter
solid
liquid
gas
physical property
extensive property
intensive property
chemical property
vapor
• 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 substance.
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.
States of Matter
• Gases have no definite shape or
volume. They expand to fill their
container.
• Vapor refers to the gaseous state of a
substance that is a solid or liquid at room
temperature.
Properties of
Matter
Physical property:
Extensive properties:
Chemical property:
Intensive properties:
Give examples:
Give examples:
Give examples:
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
• Extensive properties, such as mass, length,
and volume, are dependent on the amount of
substance present.
• Intensive properties, such as density, are
dependent on the what the substance is not
how much there is.
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.
– Iron forming rust
– Copper turning green in the air
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.
Homework, Section 1
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SECTION 1 REVIEW, Page 75
Questions #2, 3
Answer with complete sentences
Finish filling in charts that were handed out in
class: States of Matter and Properties of
Matter
• Due tomorrow
Section 2: Changes in Matter
• National Standards:
– UCP.3 Change, constancy, and measurement
– A.2 Understandings about scientific inquiry
– B.2 Structure and properties of matter
– B.3 Chemical reactions
– B.6 Interactions of energy and matter
– G.1 Science as a human endeavor
– G.2 Nature of scientific knowledge
– G.3 Historical perspectives
Objectives – Section 2
•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.
• Review Vocabulary:
• observation: orderly, direct information gathering about a
phenomenon
New Vocabulary
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physical change
phase change
chemical change
law of conservation of mass
• Matter can undergo physical and chemical
changes.
Physical/Phase
Changes
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.
• Boiling, freezing, melting, and condensing all
describe phase changes in chemistry.
Chemical Changes
• A change that involves one or more
substances turning into new substances is
called a chemical change.
• Decomposing, rusting, exploding, burning, or
oxidizing are all terms that describe chemical
changes.
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
• Practice Problems #5-9 on page 78
Transparency 8: Conservation of Mass
Math Transparency 2: Visualizing the
Conservation of Mass
Homework, Section 2
• SECTION 2 REVIEW, Page 79
• Questions #10-14 – Answer with complete
sentences
• Practice Problems Page 78:5-9 – Write the
problems, then the answers. We will do some
of these in class. Finish them for homework.
• Due tomorrow
Section 3: Mixtures of Matter
• National Standards:
– UCP.1 Systems, order, and organization
– UCP.3 Change, constancy, and measurement
– A.1 Abilities necessary to do scientific inquiry
– B.2 Structure and properties of matter
Objectives – Section 3
•Contrast mixtures and substances.
•Classify mixtures as homogeneous or
heterogeneous.
•List and describe several techniques used to
separate mixtures.
• Review Vocabulary:
• substance: a form of matter that has a uniform and
unchanging composition; also known as a pure substance
New Vocabulary
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mixture
heterogeneous mixture
homogeneous mixture
solution
filtration
distillation
crystallization
sublimation
chromatography
• Most everyday matter occurs as mixtures—
combinations of two or more substances.
Mixtures
• A mixture is a combination of two or more
pure substances in which each pure substance
retains its individual chemical properties.
• A homogenous mixture is a mixture where
the composition is constant throughout.
• Homogeneous mixtures are also called
solutions.
• A heterogeneous mixture is a mixture where
the individual substances remain distinct.
Mixtures
Heterogeneous Mixture
Homogeneous Mixture
• A mixture that does not
blend smoothly throughout
and in which the individual
substances remain distinct.
• Its composition is not
uniform; the substances
remain distinct
• For example: salad
dressing, orange juice
• A mixture that has constant
composition throughout; it
always has a single phase.
• It will contain the same
relative amount of
substances, no matter the
volume of each part.
• For example: silver mercury
amalgam, tea, metal alloys
air
Mixtures
Separating Mixtures
• Filtration is a technique that uses a porous
barrier to separate a solid from a liquid in a
heterogeneous mixture.
• Distillation is a separation technique for
homogeneous mixtures that is based on the
differences in boiling points of substances.
• Crystallization is a separation technique for
homogenous mixtures that results in the
formation of pure solid particles from a solution
containing the dissolved substance.
Separating Mixtures
• 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 technique that separates
the components of a mixture on the basis of
tendency of each to travel across the surface
of another material.
Demo: Separating a Mixture
Mini-Lab: Observe Dye Separation,
page 82
Homework, Section 3
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SECTION 3 REVIEW, Page 83
Questions #15, 17, 18
Answer with complete sentences
Due tomorrow
Section 4: Elements and Compounds
• National Standards:
– UCP.1 Systems, order, and organization
– UCP.2 Evidence, models, and explanation
– A.1 Abilities necessary to do scientific inquiry
– B.1 Structure of atoms
– B.2 Structure and properties of matter
– G.1 Science as a human endeavor
– G.3 Historical perspectives
Objectives – Section 4
• 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.
• REVIEW VOCABULARY:
• proportion: the relation of one part to another or to
the whole with respect to quantity
New Vocabulary
• element
• periodic table
• compound
law of definite proportions
percent by mass
law of multiple proportions
• A compound is a combination of two or more
elements.
Elements
• An element is a pure substance that cannot be
separated into simpler substances by physical
or chemical means.
• 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 elements into
a grid of horizontal rows called periods and
vertical columns called groups.
Elements
• The periodic table organizes the elements into
a grid of horizontal rows called periods and
vertical columns called groups.
• 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.
Compounds
• A compound is a made up of two or more
elements combined chemically.
• 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.
Compounds
• 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.
Compounds
• The properties of a compound are different
from its component elements.
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
Law of Definite Proportions
• The relative amounts are expressed as percent
by mass, the ratio of the mass of each
element to the total mass of the compound
expressed as a percentage.
Law of Definite Proportions
• This table demonstrates that the percentages
of elements in sucrose remain the same
despite differences in sample amount.
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.
Law of Multiple Proportions
Homework, Section 4
• SECTION 4 REVIEW, Page 90
• Questions #25-30 – Answer with complete
sentences
• Practice Problems Page 88:19-23 – Write the
problems, then the answers. We will do some of
these in class. Finish them for homework.
• Due tomorrow
• Chapter 3 Test is tentatively scheduled for
Wednesday, September 25.
– Ch. 3 Vocab/Study Guide is due on Test Day.