Multiple Choice
Identify the choice that best completes the statement or answers the question.
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1.
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A molecule of water (H2O) is made from _____ combining two hydrogen atoms and one oxygen atom.
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a.
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physically |
c.
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thermally |
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b.
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ionically |
d.
|
chemically |
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2.
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You put 1 spoonful of salt into 1 liter of water and stir. The resulting liquid is an example of a(n)
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a.
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pure substance. |
c.
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heterogeneous mixture. |
|
b.
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homogeneous mixture. |
d.
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immiscible mixture. |
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3.
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A material that can be represented by a chemical formula is
|
a.
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an element. |
c.
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a homogeneous solution. |
|
b.
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a mixture. |
d.
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a pure substance. |
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4.
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Lead has a density of 11.3 g/cm3 and a mass of 282.5 g. What is its volume?
|
a.
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2.5 cm3 |
c.
|
250 cm3 |
|
b.
|
25 cm3 |
d.
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2500 cm3 |
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5.
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Which of the following is not a potential sign of chemical change?
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a.
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release of gas |
c.
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change of color |
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b.
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evaporation of water |
d.
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production of gas |
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6.
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Solids, liquids, and gases are three forms of matter that
|
a.
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take up space. |
c.
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are made of atoms. |
|
b.
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have mass. |
d.
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All of the above |
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7.
|
How many atoms are in a single molecule of Fe2O3?
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8.
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What is the density of a sample of liquid that has a volume of 125 mL and a mass of 200 g?
|
a.
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75 g/mL |
c.
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1.6 g/mL |
|
b.
|
16 g/mL |
d.
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0.625 g/mL |
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9.
|
Helium is used in balloons because it is
|
a.
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reactive with rubber. |
c.
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flammable. |
|
b.
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lighter than air. |
d.
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a colored gas. |
|
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10.
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A chemical property of copper is its
|
a.
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density. |
c.
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color. |
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b.
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reactivity. |
d.
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melting point. |
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11.
|
Which of the following is not a physical property of iron?
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a.
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melting point |
c.
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color |
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b.
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ability to rust |
d.
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conductivity |
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12.
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Which property of a substance is not affected by physical changes?
|
a.
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reactivity |
c.
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shape |
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b.
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size |
d.
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position |
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13.
|
Which of the following is not a potential sign of chemical change?
|
a.
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change in odor |
c.
|
change in color |
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b.
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fizzing |
d.
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boiling |
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14.
|
Which of the following causes a chemical change?
|
a.
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moving |
c.
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burning |
|
b.
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shattering |
d.
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melting |
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15.
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A chemical change occurs whenever
|
a.
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substances are mixed. |
c.
|
hot objects melt. |
|
b.
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objects change shape. |
d.
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new substances form. |
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16.
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Which of the following is a physical change?
|
a.
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dissolving |
c.
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bending |
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b.
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evaporating |
d.
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All of the above |
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17.
|
The chemical symbol for sulfuric acid is H2SO4. How many atoms are contained in each molecule of sulfuric acid?
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18.
|
Which of the following is an example of a gas-liquid mixture?
|
a.
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the air we breathe |
c.
|
a carbonated drink |
|
b.
|
a helium balloon |
d.
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ice cubes |
|
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19.
|
A substance has a mass of 360 g and a volume of 7.5 mL. What is its density?
|
a.
|
2,700 g/mL |
c.
|
270 g/mL |
|
b.
|
480 g/mL |
d.
|
48 g/mL |
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20.
|
Which of the following is an example of a chemical change?
|
a.
|
ice melting |
c.
|
paint fading |
|
b.
|
pounding gold into a coin |
d.
|
a puddle of water evaporating |
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21.
|
Digesting food is an example of
|
a.
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physical change. |
c.
|
change of state. |
|
b.
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chemical change. |
d.
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buoyancy. |
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22.
|
The science of what matter is made of and how it changes is called
|
a.
|
chemistry. |
c.
|
kinetics. |
|
b.
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physics. |
d.
|
engineering. |
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23.
|
The chemical formula for table sugar is C12H22O11. How many oxygen atoms are in each sugar molecule?
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24.
|
Knowing the chemical properties of a substance will tell you how the substance
|
a.
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looks. |
c.
|
smells. |
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b.
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can be broken down into atoms. |
d.
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reacts with other substances. |
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25.
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Temperature is a measure of the average _____ energy of the particles in the object.
|
a.
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thermal |
c.
|
potential |
|
b.
|
kinetic |
d.
|
chemical |
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26.
|
Which state of matter will hold its shape without a container?
|
a.
|
solid |
c.
|
gas |
|
b.
|
liquid |
d.
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plasma |
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27.
|
The kinetic theory states that the higher the temperature, the faster the
|
a.
|
particles that make up a substance move. |
|
b.
|
bonds between atoms break down. |
|
c.
|
molecules of gas rush together. |
|
d.
|
lighter particles within a substance clump together. |
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28.
|
The law of conservation of mass states that mass cannot be
|
a.
|
burned. |
c.
|
created or destroyed. |
|
b.
|
changed in form. |
d.
|
heated or cooled. |
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29.
|
Boyle’s law relates the pressure of a gas to its
|
a.
|
container. |
c.
|
molecular composition. |
|
b.
|
volume. |
d.
|
temperature. |
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30.
|
When a fixed sample of gas increases in volume, it must also
|
a.
|
decrease in pressure. |
c.
|
Either (a) or (b) |
|
b.
|
increase in temperature. |
d.
|
Both (a) and (b) |
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31.
|
Gay-Lussac’s law relates the temperature of a gas to its
|
a.
|
container. |
c.
|
molecular composition. |
|
b.
|
volume. |
d.
|
pressure. |
|
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32.
|
As the temperature of a fixed amount of gas at constant volume decreases, its pressure
|
a.
|
decreases. |
c.
|
increases. |
|
b.
|
stays the same. |
d.
|
None of the above |
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33.
|
As the volume of a fixed amount of gas at constant temperature decreases, its pressure
|
a.
|
decreases. |
|
b.
|
stays the same. |
|
c.
|
increases. |
|
d.
|
Insufficient data to answer question |
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34.
|
What happens to the particles of a substance when it condenses?
|
a.
|
Particles speed up and spread out. |
|
b.
|
Particles slow down and clump together. |
|
c.
|
Particles stick together and stop moving. |
|
d.
|
Particles vibrate as they lose energy. |
|
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35.
|
Gases are unique in comparison to solids and liquids because they
|
a.
|
obey Bernoulli’s principle. |
c.
|
are fluids. |
|
b.
|
have no definite shape. |
d.
|
are easily compressible. |
|
|
36.
|
Which of these properties is shared by solids, liquids, and gases?
|
a.
|
They expand to fill their containers. |
|
b.
|
Their particles are in constant motion. |
|
c.
|
They are easily compressible. |
|
d.
|
They are fluids. |
|
|
37.
|
Why does the volume of a gas decrease when the pressure increases?
|
a.
|
Gas particles slow down when the pressure is increased. |
|
b.
|
Gas particles bond when the pressure is increased. |
|
c.
|
Gas particles are pushed together when the pressure is increased. |
|
d.
|
Gas particles become smaller when the pressure is increased. |
|
|
38.
|
When a fixed sample of gas increases in temperature, it must also
|
a.
|
increase in pressure. |
c.
|
decrease in pressure. |
|
b.
|
increase in volume. |
d.
|
increase in mass. |
|
|
39.
|
Atoms have no electric charge because they
|
a.
|
have an equal number of charged and noncharged particles. |
|
b.
|
have neutrons in their nuclei. |
|
c.
|
have an equal number of electrons and protons. |
|
d.
|
have an equal number of neutrons and protons. |
|
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40.
|
Valence electrons determine an atom’s
|
a.
|
mass. |
c.
|
electric charge. |
|
b.
|
chemical properties. |
d.
|
period. |
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|
41.
|
A mole is an SI base unit that describes the
|
a.
|
mass of a substance. |
c.
|
volume of a substance. |
|
b.
|
amount of a substance. |
d.
|
electric charge of a substance. |
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42.
|
If the atomic mass of carbon is 12 u, 1 mole of pure carbon will have a mass of
|
a.
|
6 g. |
c.
|
12 g. |
|
b.
|
6 mol. |
d.
|
12 mol. |
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43.
|
You have 85.5 g of fluorine, which has a molar mass of approximately 19 g/mol. How many moles of fluorine do you have?
|
a.
|
4.5 mol |
c.
|
45 mol |
|
b.
|
19 mol |
d.
|
85 mol |
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44.
|
A subatomic particle that has a negative charge is called a(n)
|
a.
|
molecule. |
c.
|
element. |
|
b.
|
electron. |
d.
|
compound. |
|
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45.
|
Which of the following statements not true?
|
a.
|
Protons have a positive charge. |
|
b.
|
A nucleus has a positive charge. |
|
c.
|
Neutrons have no charge. |
|
d.
|
Neutrons have a negative charge. |
|
|
46.
|
What is an atom’s nucleus made of?
|
a.
|
protons and neutrons |
c.
|
only neutrons |
|
b.
|
only protons |
d.
|
anodes |
|
|
47.
|
Avogadro’s number is useful for
|
a.
|
counting atoms. |
c.
|
locating an atom’s electrons. |
|
b.
|
counting large objects. |
d.
|
None of the above |
|
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48.
|
The charge of an atom is
|
a.
|
positive. |
c.
|
negative. |
|
b.
|
neutral. |
d.
|
unbalanced. |
|
|
49.
|
An iron atom has an atomic mass of 56. Its atomic number is 26. How many neutrons does the iron atom have?
|
|
50.
|
How much effect do commonly found isotopes have on the average atomic mass of an element?
|
a.
|
less than rarely found isotopes |
c.
|
same as rarely found isotopes |
|
b.
|
no effect on atomic mass |
d.
|
more than rarely found isotopes |
|
|
51.
|
An element’s atomic number is equal to its number of
|
a.
|
protons. |
c.
|
valence electrons |
|
b.
|
neutrons. |
d.
|
protons and neutrons. |
|
|
52.
|
Two different isotopes of an element have different
|
a.
|
numbers of neutrons. |
c.
|
atomic numbers. |
|
b.
|
numbers of protons. |
d.
|
numbers of electrons. |
|
|
53.
|
A sodium atom, which has 11 electrons, has _____ electron(s) in its third energy level.
|
|
54.
|
Which statement about the atom’s nucleus is correct?
|
a.
|
The nucleus is made of protons and neutrons and has a negative charge. |
|
b.
|
The nucleus is made of protons and neutrons and has a positive charge. |
|
c.
|
The nucleus is made of electrons and has a positive charge. |
|
d.
|
The nucleus is made of electrons and has a negative charge. |
|
|
55.
|
Oxygen’s atomic number is 8. This means that an oxygen atom has
|
a.
|
eight neutrons in its nucleus. |
|
b.
|
a total of eight protons and neutrons. |
|
c.
|
eight protons in its nucleus. |
|
d.
|
a total of eight neutrons and electrons. |
|
|
56.
|
Which statement about an element’s average atomic mass is correct?
|
a.
|
It is determined by counting the number of isotopes in a sample of the element. |
|
b.
|
It is equal to one-twelfth the mass of the most common isotope. |
|
c.
|
It is a weighted average, so common isotopes have a greater effect than uncommon ones. |
|
d.
|
It is based on an isotope’s charge, so negatively charged isotopes have a greater effect than positive ones. |
|
|
57.
|
An atom’s mass number equals the number of
|
a.
|
protons plus the number of electrons. |
|
b.
|
protons plus the number of neutrons. |
|
c.
|
protons. |
|
d.
|
neutrons. |
|
|
58.
|
A unified atomic mass unit is equal to
|
a.
|
one-half the mass of a hydrogen atom. |
|
b.
|
one-fourth the mass of a lithium atom. |
|
c.
|
one-twelfth the mass of a carbon-12 atom. |
|
d.
|
one-fifteenth the mass of a nitrogen-15 atom. |
|
|
59.
|
Avogadro’s number is defined as the number of particles in
|
a.
|
one mole of a substance. |
c.
|
one gram of a substance. |
|
b.
|
one liter of a substance. |
d.
|
one kilogram of a substance. |
|
|
60.
|
The order of elements in the periodic table is based on
|
a.
|
the number of protons in the nucleus. |
|
b.
|
the electric charge of the nucleus. |
|
c.
|
the number of neutrons in the nucleus. |
|
d.
|
atomic mass. |
|
|
61.
|
Atoms of elements that are in the same group have the same number of
|
a.
|
protons. |
c.
|
valence electrons. |
|
b.
|
neutrons. |
d.
|
protons and neutrons. |
|
|
62.
|
Which of the following elements is an alkali metal?
|
a.
|
calcium |
c.
|
mercury |
|
b.
|
magnesium |
d.
|
sodium |
|
|
63.
|
In Mendeleev’s periodic table, elements in each column had similar
|
a.
|
atomic masses. |
c.
|
atomic numbers |
|
b.
|
properties. |
d.
|
symbols. |
|
|
64.
|
Magnesium (Mg) is located to the right of sodium (Na) because Mg has
|
a.
|
fewer protons. |
c.
|
no protons. |
|
b.
|
no neutrons. |
d.
|
more protons. |
|
|
65.
|
As you move from left to right across the periodic table, elements
|
a.
|
become less metallic. |
c.
|
have a lower atomic weight. |
|
b.
|
have a lower atomic number. |
d.
|
become more metallic. |
|
|
66.
|
How was Mendeleev’s periodic table arranged?
|
a.
|
by increasing atomic mass |
c.
|
by increasing atomic number |
|
b.
|
by decreasing atomic mass |
d.
|
by decreasing atomic number |
|
|
67.
|
What is Mendeleev is known for?
|
a.
|
creating today’s atomic model |
c.
|
publishing the first periodic table |
|
b.
|
discovering protons |
d.
|
discovering Mendelevium |
|
|
68.
|
Mendeleev left gaps in his periodic table because
|
a.
|
the table was too small. |
c.
|
the table was too full. |
|
b.
|
protons belonged there. |
d.
|
no known elements fit there. |
|
|
69.
|
Each column of the periodic table is
|
a.
|
an element. |
c.
|
an isotope. |
|
b.
|
a group. |
d.
|
a period. |
|
|
70.
|
The periodic law states that elements that have similar properties appear
|
a.
|
to the left of each other. |
c.
|
at every tenth element. |
|
b.
|
to the right of each other. |
d.
|
at regular intervals. |
|
|
71.
|
As you move from up to down in a column of the periodic table, elements have
|
a.
|
fewer protons. |
c.
|
a higher atomic number. |
|
b.
|
a lower atomic number. |
d.
|
a higher group number. |
|
|
72.
|
Elements that belong to the same group have the same number of
|
a.
|
valence electrons. |
c.
|
inner electrons. |
|
b.
|
neutral electrons. |
d.
|
total electrons. |
|
|
73.
|
Because they differ in numbers of protons in their nuclei and in numbers of electrons in their filled inner energy levels, elements in a group
|
a.
|
have different charges. |
c.
|
are very interactive. |
|
b.
|
are not exactly the same. |
d.
|
are inert. |
|
|
74.
|
Atoms that gain or lose electrons are called
|
a.
|
metals. |
c.
|
ions. |
|
b.
|
nonmetals. |
d.
|
isotopes. |
|
|
75.
|
Elements that have one valence electron tend to
|
a.
|
be highly reactive. |
c.
|
become charged. |
|
b.
|
form ions. |
d.
|
All of the above |
|
|
76.
|
The three main groups of elements are metals, nonmetals, and
|
a.
|
inert gases. |
c.
|
radioactive isotopes. |
|
b.
|
alkali metals. |
d.
|
semiconductors. |
|
|
77.
|
Most elements on the left side of the periodic table are
|
a.
|
semiconductors. |
c.
|
nonmetals. |
|
b.
|
metals. |
d.
|
metalloids. |
|
|
78.
|
Most nonmetals are
|
a.
|
brittle. |
c.
|
metalloids. |
|
b.
|
good conductors. |
d.
|
shiny. |
|
|
79.
|
Each element in an element family shares the same
|
a.
|
average atomic mass. |
c.
|
number of valence electrons. |
|
b.
|
number of protons. |
d.
|
atomic number |
|
|
80.
|
Elements in an element family have similar
|
a.
|
atomic symbols. |
c.
|
atomic weights. |
|
b.
|
atomic sizes. |
d.
|
chemical properties. |
|
|
81.
|
How do you know that potassium, an alkali metal, is highly reactive?
|
a.
|
It conducts heat. |
c.
|
It is a soft and shiny metal. |
|
b.
|
It conducts electricity. |
d.
|
It has one valence electron. |
|
|
82.
|
Which of the following is not true of noble gases?
|
a.
|
They are highly reactive. |
c.
|
They belong to Group 18. |
|
b.
|
They exist as single atoms. |
d.
|
They are nonmetals. |
|
|
83.
|
Elements that share properties of both metals and nonmetals are called
|
a.
|
ions. |
c.
|
semiconductors. |
|
b.
|
periods. |
d.
|
valences. |
|
|
84.
|
Which statement about the alkali metals is correct?
|
a.
|
They are located in the left-most column of the periodic table. |
|
b.
|
They are extremely nonreactive. |
|
c.
|
They are usually gases. |
|
d.
|
They form negative ions with a 1– charge. |
|
|
85.
|
Which statement about noble gases is correct?
|
a.
|
They form compounds with very bright colors. |
|
b.
|
They exist as single atoms rather than as molecules. |
|
c.
|
They are highly reactive with both metals and nonmetals. |
|
d.
|
They are extremely rare in nature. |
|
|
86.
|
Group 18 noble gases are relatively inert because
|
a.
|
they readily form positive ions. |
|
b.
|
they can have either a positive or a negative charge. |
|
c.
|
their outermost energy level is missing one electron. |
|
d.
|
their s and p orbitals are filled. |
|
|
87.
|
Mendeleev studied the properties of the elements and looked for
|
a.
|
electrons. |
c.
|
patterns. |
|
b.
|
ions. |
d.
|
protons. |
|
|
88.
|
Which is not a family of the periodic table?
|
a.
|
alkaline-earth metals |
c.
|
halogens |
|
b.
|
anions |
d.
|
noble gases |
|
|
89.
|
A release of energy is a sign that
|
a.
|
a chemical change is taking place. |
c.
|
oxygen is present. |
|
b.
|
a physical change has just occurred. |
d.
|
organic chemicals are present. |
|
|
90.
|
When methane reacts with abundant amounts of oxygen, the products are
|
a.
|
carbon dioxide and water. |
c.
|
soot and water. |
|
b.
|
carbon monoxide and water. |
d.
|
simple sugar and oxygen. |
|
|
91.
|
If you start with 5 mol of O2 in the reaction 2Mg + O2 ® 2MgO, how many moles of Mg will you need?
|
a.
|
4 mol |
c.
|
8 mol |
|
b.
|
5 mol |
d.
|
10 mol |
|
|
92.
|
Which of these is not a sign of a chemical reaction?
|
a.
|
A gas is given off. |
c.
|
Heat is released. |
|
b.
|
The material dissolves. |
d.
|
A color change occurs. |
|
|
93.
|
Which of the following occurs in an endothermic reaction but not in an exothermic reaction?
|
a.
|
Chemical bonds are broken. |
c.
|
Molecules are formed. |
|
b.
|
Energy is absorbed. |
d.
|
Atoms are rearranged. |
|
|
94.
|
In the reaction 3CuCl2 + 2Al ® 2AlCl3 + 3Cu, how many moles of Al react with 3 moles of CuCl2?
|
a.
|
1 mol |
c.
|
3 mol |
|
b.
|
2 mol |
d.
|
4 mol |
|
|
95.
|
In the electrolysis of water, 2H2O ® 2H2 + O2, if the volume of oxygen produced was 8 mL, what would be the volume of hydrogen produced?
|
a.
|
4 mL |
c.
|
16 mL |
|
b.
|
8 mL |
d.
|
24 mL |
|
|
96.
|
If you use 3 mol of O2 in the reaction 2Mg + O2 ® 2MgO, how many moles of Mg are needed?
|
a.
|
1 mol |
c.
|
4 mol |
|
b.
|
2 mol |
d.
|
6 mol |
|
|
97.
|
Give the mole ratio for the following equation:
Zn + 2HCl ® ZnCl2 + H2.
|
a.
|
1:1:1 |
c.
|
1:2:1:1 |
|
b.
|
1:2:1 |
d.
|
1:2:2:2 |
|
|
98.
|
In the reaction 2H2O ® 2H2 + O2, if you start with 4 mol of water, how many moles of hydrogen gas are formed?
|
a.
|
2 mol |
c.
|
6 mol |
|
b.
|
4 mol |
d.
|
8 mol |
|
|
99.
|
The decomposition of water can be brought about by
|
a.
|
combustion. |
c.
|
synthesis reactions. |
|
b.
|
electrolysis. |
d.
|
oxidation. |
|
|
100.
|
A synthesis reaction between magnesium (Mg) and oxygen (O2) might produce
|
a.
|
Mg2. |
c.
|
MgO. |
|
b.
|
O4. |
d.
|
MgCO2. |
|
|
101.
|
All of these are likely to speed up the rate of a reaction except
|
a.
|
decreasing the surface area. |
c.
|
increasing the temperature. |
|
b.
|
increasing the pressure. |
d.
|
adding a catalyst. |
|
|
102.
|
A substance that undergoes a change in a chemical reaction is
|
a.
|
a product. |
c.
|
a reactant. |
|
b.
|
a chemical. |
d.
|
an enzyme. |
|
|
103.
|
The energy source in photosynthesis is
|
a.
|
light energy. |
c.
|
heat energy. |
|
b.
|
chemical energy. |
d.
|
kinetic energy. |
|
|
104.
|
A chemical equation is balanced by changing or adding
|
a.
|
chemical symbols. |
c.
|
coefficients. |
|
b.
|
subscripts. |
d.
|
reactants. |
|
|
105.
|
In the reaction H2S + 2O2 ® H2SO4, the law of definite proportions predicts that for every mole of H2S you will need how many moles of O2?
|
a.
|
1 mol |
c.
|
3 mol |
|
b.
|
2 mol |
d.
|
4 mol |
|
|
106.
|
In a balanced chemical reaction, the total mass of the products always equals the
|
a.
|
molar mass of the reactants. |
c.
|
total mass of the reactants. |
|
b.
|
atomic mass of the reactants. |
d.
|
proportional masses of the reactants. |
|
|
107.
|
What happens in a chemical reaction?
|
a.
|
Atoms are destroyed. |
c.
|
Atoms are heated and cooled. |
|
b.
|
Atoms are created. |
d.
|
Atoms are rearranged. |
|
|
108.
|
Which of the following is an example of a decomposition reaction?
|
a.
|
photosynthesis |
|
b.
|
digestion |
|
c.
|
respiration |
|
d.
|
exchange of ions between two compounds |
|