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.
a. | physically | c. | thermally | b. | 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)
a. | pure substance. | c. | heterogeneous mixture. | b. | homogeneous
mixture. | d. | immiscible
mixture. |
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3.
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A material that can be represented by a chemical formula is
a. | an element. | c. | a homogeneous solution. | b. | a
mixture. | d. | 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. | 2.5 cm3 | c. | 250 cm3 | b. | 25 cm3 | d. | 2500
cm3 |
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5.
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Which of the following is not a potential sign of chemical change?
a. | release of gas | c. | change of color | b. | evaporation of water | d. | production of
gas |
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6.
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Solids, liquids, and gases are three forms of matter that
a. | take up space. | c. | are made of atoms. | b. | have mass. | d. | All of the
above |
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7.
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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. | 75 g/mL | c. | 1.6 g/mL | b. | 16 g/mL | d. | 0.625 g/mL |
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9.
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Helium is used in balloons because it is
a. | reactive with rubber. | c. | flammable. | b. | lighter than air. | d. | a colored gas. |
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10.
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A chemical property of copper is its
a. | density. | c. | color. | b. | reactivity. | d. | melting point. |
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11.
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Which of the following is not a physical property of iron?
a. | melting point | c. | color | b. | ability to rust | d. | conductivity |
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12.
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Which property of a substance is not affected by physical changes?
a. | reactivity | c. | shape | b. | size | d. | position |
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13.
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Which of the following is not a potential sign of chemical change?
a. | change in odor | c. | change in color | b. | fizzing | d. | boiling |
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14.
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Which of the following causes a chemical change?
a. | moving | c. | burning | b. | shattering | d. | melting |
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15.
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A chemical change occurs whenever
a. | substances are mixed. | c. | hot objects melt. | b. | objects change shape. | d. | new substances
form. |
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16.
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Which of the following is a physical change?
a. | dissolving | c. | bending | b. | evaporating | d. | All of the
above |
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17.
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The chemical symbol for sulfuric acid is H2SO4. How many
atoms are contained in each molecule of sulfuric acid?
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18.
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Which of the following is an example of a gas-liquid mixture?
a. | the air we breathe | c. | a carbonated drink | b. | a helium balloon | d. | ice cubes |
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19.
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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.
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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.
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Digesting food is an example of
a. | physical change. | c. | change of state. | b. | chemical change. | d. | buoyancy. |
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22.
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The science of what matter is made of and how it changes is called
a. | chemistry. | c. | kinetics. | b. | physics. | d. | engineering. |
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23.
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The chemical formula for table sugar is
C12H22O11. How many oxygen atoms are in each sugar molecule?
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24.
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Knowing the chemical properties of a substance will tell you how the
substance
a. | looks. | c. | smells. | b. | can be broken down into
atoms. | d. | 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. | thermal | c. | potential | b. | kinetic | d. | chemical |
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26.
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Which state of matter will hold its shape without a container?
a. | solid | c. | gas | b. | liquid | d. | plasma |
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27.
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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.
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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.
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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.
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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.
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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.
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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.
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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.
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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.
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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. |
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36.
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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. |
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37.
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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. |
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38.
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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. |
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39.
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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.
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Valence electrons determine an atom’s
a. | mass. | c. | electric charge. | b. | chemical properties. | d. | period. |
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41.
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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.
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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.
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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.
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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.
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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. |
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46.
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What is an atom’s nucleus made of?
a. | protons and neutrons | c. | only neutrons | b. | only protons | d. | anodes |
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47.
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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.
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The charge of an atom is
a. | positive. | c. | negative. | b. | neutral. | d. | unbalanced. |
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49.
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An iron atom has an atomic mass of 56. Its atomic number is 26. How many
neutrons does the iron atom have?
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50.
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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 |
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51.
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An element’s atomic number is equal to its number of
a. | protons. | c. | valence electrons | b. | neutrons. | d. | protons and
neutrons. |
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52.
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Two different isotopes of an element have different
a. | numbers of neutrons. | c. | atomic numbers. | b. | numbers of protons. | d. | numbers of
electrons. |
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53.
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A sodium atom, which has 11 electrons, has _____ electron(s) in its third energy
level.
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54.
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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. |
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55.
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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. |
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56.
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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. |
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57.
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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. |
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58.
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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. |
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59.
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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. |
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60.
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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. |
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61.
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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. |
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62.
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Which of the following elements is an alkali metal?
a. | calcium | c. | mercury | b. | magnesium | d. | sodium |
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63.
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In Mendeleev’s periodic table,
elements in each column had similar
a. | atomic masses. | c. | atomic numbers | b. | properties. | d. | symbols. |
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64.
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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. |
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65.
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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. |
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66.
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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 |
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67.
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What is Mendeleev is known for?
a. | creating today’s atomic model | c. | publishing the first periodic
table | b. | discovering protons | d. | discovering Mendelevium |
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68.
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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. |
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69.
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Each column of the periodic table is
a. | an element. | c. | an isotope. | b. | a group. | d. | a period. |
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70.
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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. |
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71.
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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. |
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72.
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Elements that belong to the same group have the same number of
a. | valence electrons. | c. | inner electrons. | b. | neutral electrons. | d. | total
electrons. |
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73.
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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. |
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74.
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Atoms that gain or lose electrons are called
a. | metals. | c. | ions. | b. | nonmetals. | d. | isotopes. |
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75.
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Elements that have one valence electron tend to
a. | be highly reactive. | c. | become charged. | b. | form ions. | d. | All of the
above |
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76.
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The three main groups of elements are metals, nonmetals, and
a. | inert gases. | c. | radioactive isotopes. | b. | alkali
metals. | d. | semiconductors. |
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77.
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Most elements on the left side of the periodic table are
a. | semiconductors. | c. | nonmetals. | b. | metals. | d. | metalloids. |
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78.
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Most nonmetals are
a. | brittle. | c. | metalloids. | b. | good conductors. | d. | shiny. |
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79.
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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 |
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80.
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Elements in an element family have similar
a. | atomic symbols. | c. | atomic weights. | b. | atomic sizes. | d. | chemical
properties. |
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81.
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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. |
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82.
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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. |
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83.
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Elements that share properties of both metals and nonmetals are called
a. | ions. | c. | semiconductors. | b. | periods. | d. | valences. |
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84.
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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. |
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85.
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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. |
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86.
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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. |
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87.
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Mendeleev studied the properties of the elements and looked for
a. | electrons. | c. | patterns. | b. | ions. | d. | protons. |
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88.
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Which is not a family of the periodic table?
a. | alkaline-earth metals | c. | halogens | b. | anions | d. | noble gases |
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89.
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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. |
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90.
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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. |
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91.
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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 |
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92.
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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. |
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93.
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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. |
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94.
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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 |
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95.
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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 |
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96.
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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 |
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97.
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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 |
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98.
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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 |
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99.
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The decomposition of water can be brought about by
a. | combustion. | c. | synthesis reactions. | b. | electrolysis. | d. | oxidation. |
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100.
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A synthesis reaction between magnesium (Mg) and oxygen (O2) might
produce
a. | Mg2. | c. | MgO. | b. | O4. | d. | MgCO2. |
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101.
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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. |
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102.
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A substance that undergoes a change in a chemical reaction is
a. | a product. | c. | a reactant. | b. | a chemical. | d. | an enzyme. |
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103.
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The energy source in photosynthesis is
a. | light energy. | c. | heat energy. | b. | chemical energy. | d. | kinetic energy. |
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104.
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A chemical equation is balanced by changing or adding
a. | chemical symbols. | c. | coefficients. | b. | subscripts. | d. | reactants. |
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105.
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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 |
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106.
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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. |
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107.
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What happens in a chemical reaction?
a. | Atoms are destroyed. | c. | Atoms are heated and cooled. | b. | Atoms are
created. | d. | Atoms are
rearranged. |
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108.
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Which of the following is an example of a decomposition reaction?
a. | photosynthesis | b. | digestion | c. | respiration | d. | exchange of ions between two
compounds |
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