Chemistry
Chapter 3:
Section 3.1
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Matter and Property Changes
Properties of Matter p.70
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.
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.
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.
A physical property is a characteristic that can be
observed or measured without changing the sample’s
composition.
a. Examples of physical properties:
i. Color
ii. State at room temperature (25 0C)
iii. Melting point
iv. Boiling point
v. Density
10. Extensive properties are dependent on the amount of
substance present, such as mass, length, or volume.
11. Intensive properties are independent of the amount of
substance present, such as density.
12. The ability of a substance to combine with or change
into one or more other substances is called a
chemical property.
a. Iron forming rust
b. Copper turning green in the air.
13. A substance can change form-an important concept in
chemistry.
14. Chemical properties can change with specific
environment conditions, such as temperature and
pressure.
a. Physical properties:
i. Reddish brown, shiny
ii. Malleable
iii.
iv.
v.
vi.
vii.
Ductile
Good conductor of electricity and heat
Density
Melting point
Boiling point
b. chemical properties:
i. forms green copper carbonate compound when
is contact with moist air.
ii. Forms new substances when combined with
nitric acid and sulfuric acid.
iii. Forms a deep-blue solution when in contact
with ammonia.
Section 3.2
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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 form one
state to another.
Boiling, freezing, melting, and condensing all
describe phase changes in chemistry.
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 describes chemical
changes.
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.
mass reactants = mass products
Section 3.3 Mixtures of Matter
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2.
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4.
p.76
p.80
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.
5.
6.
Types of solution systems:
a. Gas-Gas: air in scuba tank is mixture of
nitrogen, oxygen, and argon gases.
b. Gas-Liquid: oxygen and carbon dioxide are
dissolved in seawater.
c. Liquid-Gas: moist air exhaled by the scuba diver
contains water droplets.
d. Liquid-Liquid: when it is raining, fresh water
mixes with seawater.
e. Solid-Liquid: solid salts are dissolved in
seawater.
f. Solid-Solid: the air tank is made of an alloy-a
mixture of two metals.
Filtration is a technique that uses a porous barrier
to separate a solid from a liquid in a heterogeneous
mixture.
7. Distillation is a separation technique for
homogeneous mixtures that is based on the differences
in boiling points of substances.
8. Crystallization is a separation technique for
homogenous mixtures that results in the formation of
pure solid particles from a solution containing the
dissolved substance.
9. 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.
10. 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.
Section 3.4
Elements and Compounds p.84
1.
An element is a pure substance that cannot be
separated into simpler substances by physical or
chemical means.
2. 92 elements occur naturally on Earth.
3. Each element has a unique name and a one, two, or
three-letter symbol.
4. The periodic table organizes the elements into a grid
of horizontal rows called periods and vertical
columns called groups.
5. A compound is made up of two or more elements
combined chemically.
6. Most of the matter in the universe exists as
compounds.
7. Table salt, NaCl, and water, H2O, are compounds.
8. Elements can never be separated.
9. Compounds can be broken into components by chemical
means.
10. 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.
11. 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
Percent by mass (%) = mass of element x 100
mass of compound
12. 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.
a. Examples
i. H2O2 and H2O
ii. Copper (I) chloride and copper (II) chloride