2. Chapter 3: Main Ideas
Chapter 3: Main Ideas
Most common substances exist as solids,
Most common substances exist as solids,
liquids, and gases, which have diverse physical
liquids, and gases, which have diverse physical
and chemical properties.
and chemical properties.
Matter can undergo physical and chemical
Matter can undergo physical and chemical
changes.
changes.
Most everyday matter occurs as mixtures—
Most everyday matter occurs as mixtures—
combinations of two or more substances.
combinations of two or more substances.
A compound is a combination of two or more
A compound is a combination of two or more
elements.
elements.
3. 3-1 Properties of Matter
3-1 Properties of Matter
Objectives:
Objectives:
Identify
Identify the characteristics of a
the characteristics of a
substance.
substance.
Distinguish
Distinguish between physical and
between physical and
chemical properties
chemical properties
Differentiate
Differentiate among physical states of
among physical states of
matter.
matter.
4. States of Matter
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.
• 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.
5. Physical Properties of
Physical Properties of
Matter
Matter
• A physical property is a characteristic that
can be observed or measured without
changing the sample’s composition.
6. Physical Properties of
Physical Properties of
Matter
Matter
• Extensive properties are dependent
on the amount of substance present.
• mass, length, or volume.
• Intensive properties are independent
of the amount of substance present.
• Density,
7. Chemical Properties of
Chemical Properties of
Matter
Matter
• The ability of a substance to
combine with or change into one
or more other substances is
called a chemical property.
Examples:
• Iron forming rust
• Copper turning green in the air
10. Question?
Question?
What defines a gas?
A. Gases have a definite volume and shape.
B. Gases have a definite volume but take the
shape of their container.
C. Gases have no definite volume or shape.
D. Gases have a definite shape but no definite
volume.
11. 3-2 Changes in Matter
3-2 Changes in Matter
Objectives
Objectives
Define
Define physical change and list several
physical change and list several
common physical changes.
common physical changes.
Define
Define chemical change and list several
chemical change and list several
indications that a chemical change has
indications that a chemical change has
taken place.
taken place.
Apply
Apply the law of conservation of mass to
the law of conservation of mass to
chemical reactions.
chemical reactions.
12. 3-2 Changes in Matter
3-2 Changes in Matter
• 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.
• Dependent on temperature and pressure.
• Examples: Boiling, freezing, melting, and
condensing all describe phase changes in
13. Chemical Changes
Chemical Changes
• A change that involves one or more
substances turning into new substances
is called a chemical change.
Examples: Decomposing, rusting,
exploding, burning, or oxidizing are all
terms that describe chemical changes.
14. Conservation of Mass
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
15. When one substances turns into
another, what kind of change has taken
place?
A. chemical reaction
B. physical reaction
C. extensive reaction
D. nuclear reaction
Question?
Question?
16. Question?
Question?
The law of conservation of mass states
that:
A. Matter can be created and destroyed.
B. Matter can be created but not destroyed.
C. The products of a reaction always
have a greater mass than the reactants.
D. The products of a reaction must
have the same mass as the
reactants.
17. 3-3 Mixtures of Matter
3-3 Mixtures of Matter
Objectives
Objectives
Contrast
Contrast mixtures and substances
mixtures and substances
Classify
Classify mixtures as homogeneous or
mixtures as homogeneous or
heterogeneous.
heterogeneous.
List and describe
List and describe several techniques
several techniques
used to separate mixtures.
used to separate mixtures.
18. Mixtures
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.
• Also called a solution.
21. Separation of Mixtures
Separation of 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.
22. Separation of Mixtures
Separation of 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.
23. Question?
Question?
Which is NOT a technique for
separating a homogenous mixture?
A. crystallization
B. distillation
C. filtration
D. chromatography
24. Question?
Question?
Which of the following is a
heterogeneous mixture?
A. seawater
B. silver mercury amalgam
C. atmosphere
D. salad dressing
25. 3-4 Elements and
3-4 Elements and
Compounds
Compounds
Objective
Objective
Distinguish
Distinguish between elements and
between elements and
compounds.
compounds.
Describe
Describe the organization of elements in
the organization of elements in
the periodic table.
the periodic table.
Explain
Explain how all compounds obey the laws
how all compounds obey the laws
of definite and multiple proportions.
of definite and multiple proportions.
26. 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.
27. Compounds
Compounds
• A compound is pure substance made up
of two or more elements combined
chemically.
• Compounds can be separated into
components by chemical means.
• Electricity or heat
28. Compounds
Compounds
• Have properties different than that of
their components.
• Most of the matter in the universe exists
as compounds
• Example: Table salt, NaCl, and water,
H2
O, are compounds.
29. Compounds vs. Elements
Compounds vs. Elements
• Elements can never be separated.
• Compounds can be broken into
components by chemical means.
32. Law of Definite
Law of Definite
Proportions
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.
• Water is always 2 parts H and 1 part O
• CO is always 1 part C and 1 part O
33. Percent by Mass
Percent by Mass
• 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.
34. Law of Multiple
Law of Multiple
Proportions
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.
• H2O2 and H2O
• CO and CO2
35. Section 3-4
Section 3-4
What is a period on the periodic table of
the elements?
A. a vertical columns
B. even numbered elements only
C. horizontal rows
D. the last vertical column only
36. Question?
Question?
An element is a substance that cannot
be
A. divided into simpler substances.
B. combined to form a mixture.
C. combined to form an element.
D. different phases.
37. Study Guide
Study Guide
• 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.
38. Study Guide
Study Guide
• 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.
39. Study Guide
Study Guide
• 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.
40. Study Guide
Study Guide
• Elements cannot be broken down into
simpler substances.
• 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.
41. Study Guide
Study Guide
• 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.
42. Question?
Question?
Which of the following is NOT a physical
property of water?
A. Ice melts at 0°C.
B. Water boils at 100.
C. Water reacts violently with
pure sodium.
D. Water is a liquid at room
temperature.
43. Question?
Question?
28.0 grams of nitrogen gas reacts
completely with 6.0 grams of hydrogen to
form 34.0 grams of ammonia. What does
this demonstrate?
A. the law of conservation of energy
B. sublimation
C. distillation
D. the law of conservation of mass
44. Question?
Question?
What is the best way to separate salt
dissolved in water?
A. sublimation
B. crystallization
C. freezing
D. filtration
45. Question?
Question?
Two or more elements chemically
joined form what?
A. substance
B. heterogeneous mixture
C. homogenous solution
D. compound
47. Question?
Question?
Which is NOT a chemical reaction?
A. a car rusting
B. dissolving sugar in water
C. wood burning
D. a banana ripening
48. Question?
Question?
Which describes a substance that is in
the liquid state?
A. It has a definite shape.
B. It has no definite volume.
C. It can be compressed into a
smaller volume.
D. It has a definite volume.
49. Question?
Question?
Elements in the same period are
likely to have similar ____.
A. physical properties
B. densities
C. chemical properties
D. melting points
51. Question?
Question?
Compounds can be broken into their
component elements by which of the
following?
A. crystallization
B. distillation
C. filtration
D. chemical reaction
62. CIM
CIM
4 Three Common States of Matter
10 Conservation of Mass
3 Types of Solution Systems
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