Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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All atoms are ____.
a. | positively charged, with the number of protons exceeding the number of
electrons | b. | negatively charged, with the number of electrons exceeding the number of
protons | c. | neutral, with the number of protons equaling the number of
electrons | d. | neutral, with the number of protons equaling the number of electrons, which is equal
to the number of neutrons |
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2.
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Isotopes of the same element have different ____.
a. | positions on the periodic table | c. | atomic numbers | b. | chemical
behavior | d. | mass
numbers |
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3.
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When an electron moves from a lower to a higher energy level, the electron
____.
a. | always doubles its energy | b. | absorbs a continuously variable amount of
energy | c. | absorbs a quantum of energy | d. | moves closer to the
nucleus |
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4.
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Which color of visible light has the shortest wavelength?
a. | yellow | c. | blue | b. | green | d. | violet |
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5.
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What is the name given to the electrons in the highest occupied energy level of
an atom?
a. | orbital electrons | c. | anions | b. | valence electrons | d. | cations |
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6.
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Ionic compounds are normally in which physical state at room temperature?
a. | solid | c. | gas | b. | liquid | d. | plasma |
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7.
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What characteristic of metals makes them good electrical conductors?
a. | They have mobile valence electrons. | b. | They have mobile protons. | c. | They have mobile
cations. | d. | Their crystal structures can be rearranged easily. |
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8.
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Which is a typical characteristic of an ionic compound?
a. | Electron pairs are shared among atoms. | b. | The ionic compound has a low solubility in
water. | c. | The ionic compound is described as a molecule. | d. | The ionic compound
has a high melting point. |
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9.
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Which of these elements does not exist as a diatomic molecule?
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10.
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When naming a transition metal ion that can have more than one common ionic
charge, the numerical value of the charge is indicated by a ____.
a. | prefix | c. | Roman numeral following the name | b. | suffix | d. | superscript after the name |
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11.
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Aluminum is a group 3A metal. Which ion does A1 typically form?
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12.
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The nonmetals in Groups 6A and 7A ____.
a. | lose electrons when they form ions | b. | have a numerical charge that is found by
subtracting 8 from the group number | c. | all have ions with a –1
charge | d. | end in -ate |
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13.
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Which of the following formulas represents an ionic compound?
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14.
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What is the formula for sulfurous acid?
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15.
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Which of the following are produced when a base is dissolved in water?
a. | hydronium ions | c. | hydrogen ions | b. | hydroxide ions | d. | ammonium ions |
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16.
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What does an -ite or -ate ending in a polyatomic ion mean?
a. | Oxygen is in the formula. | c. | Nitrogen is in the
formula. | b. | Sulfur is in the formula. | d. | Bromine is in the formula. |
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17.
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How many moles of CaBr  are in 5.0 grams of
CaBr  ?
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18.
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Which combination of temperature and pressure correctly describes standard
temperature and pressure, STP?
a. | 0 C and 101 kPa | c. | 0 C and 22.4 kPa | b. | 1 C and 0 kPa | d. | 100 C and 100 kPa |
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19.
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If 60.2 grams of Hg combines completely with 24.0 grams of Br to form a
compound, what is the percent composition of Hg in the compound?
a. | 28.5% | c. | 71.5% | b. | 39.9% | d. | 60.1% |
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20.
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What is the percent composition of carbon, in heptane, C  H  ?
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21.
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What is the percent by mass of carbon in acetone, C  H  O? a. | 20.7% | c. | 1.61% | b. | 62.1% | d. | 30.0% |
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22.
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Which of the following is NOT an empirical formula?
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23.
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What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by
weight?
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24.
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Symbols used in equations, together with the explanations of the symbols, are
shown below. Which set is correct?
a. | (g), grams | c. | (aq), dissolved in water | b. | (l),
liters | d. | (s), solid
product |
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25.
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A catalyst is ____.
a. | the product of a combustion reaction | b. | not used up in a reaction | c. | one of the reactants
in single-replacement reactions | d. | a solid product of a
reaction |
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26.
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What is conserved in the reaction shown below? H  ( g) + Cl  ( g) ® 2HCl( g) a. | mass only | c. | mass, moles, and molecules only | b. | mass and moles
only | d. | mass, moles,
molecules, and volume |
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27.
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In a chemical reaction, the mass of the products ____.
a. | is less than the mass of the reactants | b. | is greater than the mass of the
reactants | c. | is equal to the mass of the reactants | d. | has no relationship to the mass of the
reactants |
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28.
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In the reaction 2CO( g) + O  ( g) ® 2CO  ( g), what is the ratio of moles
of oxygen used to moles of CO  produced?
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29.
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Which of the following is an INCORRECT interpretation of the balanced equation
shown below? 2S( s) + 3O  ( g) ® 2SO  ( g) a. | 2 atoms S + 3 molecules O ® 2 molecules SO | b. | 2 g S + 3 g
O ® 2 g
SO | c. | 2 mol S + 3 mol
O ® 2 mol
SO | d. | none of the
above |
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30.
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Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas.
How many grams of aluminum sulfate would be formed if 250 g H  SO  completely reacted with
aluminum?  a. | 0.85 g | c. | 450 g | b. | 290 g | d. | 870 g |
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31.
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When 0.1 mol of calcium reacts with 880 g of water, 2.24 L of hydrogen gas form
(at STP). How would the amount of hydrogen produced change if the volume of water was decreased to
440 mL (440 g)?
a. | Only one half the volume of hydrogen would be produced. | b. | The volume of
hydrogen produced would be the same. | c. | The volume of hydrogen produced would
double. | d. | No hydrogen would be produced. |
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32.
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What is the maximum number of grams of PH  that
can be formed when 6.2 g of phosphorus reacts with 4.0 g of hydrogen to form PH  ? P  ( g) + 6H  ( g)  4PH  ( g) a. | 0.43 g | c. | 270 g | b. | 6.8 g | d. | 45 g |
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33.
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Which statement is true if 12 mol CO and 12 mol Fe  O  are allowed to react? 3CO( g)
+ Fe  O  ( s)  2Fe( s) +
3CO  ( g) a. | The limiting reagent is CO and 8.0 mol Fe will be formed. | b. | The limiting reagent
is CO and 3.0 mol CO will be formed. | c. | The limiting reagent
is Fe O and 24
mol Fe will be formed. | d. | The limiting reagent is Fe O and 36 mol CO will be
formed. |
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34.
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Which of the following statements is NOT true, according to the kinetic
theory?
a. | There is no attraction between particles of a gas. | b. | Only particles of
matter in the gaseous state are in constant motion. | c. | The particles of a gas collide with each other
and with other objects. | d. | All of the statements are
true. |
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35.
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What is one standard atmosphere of pressure in kilopascals?
a. | 0 kPa | c. | 101.3 kPa | b. | 760 kPa | d. | 1 kPa |
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36.
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As the temperature of the gas in a balloon decreases, which of the following
occurs?
a. | The volume of the balloon increases. | b. | The average kinetic energy of the gas
decreases. | c. | The gas pressure inside the balloon increases. | d. | all of the
above |
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37.
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When the Kelvin temperature of an enclosed gas doubles, the particles of the gas
____.
a. | move faster | b. | strike the walls of the container with less
force | c. | decrease in average kinetic energy | d. | decrease in
volume |
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38.
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In which of the following is the solution concentration expressed in terms of
molarity?
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39.
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What is the number of moles of solute in 250 mL of a 0.4M
solution?
a. | 0.1 mol | c. | 0.62 mol | b. | 0.16 mol | d. | 1.6 mol |
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40.
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What mass of sucrose, C  H  O  , is needed to make 500.0 mL of a
0.200 M solution? a. | 34.2 g | c. | 17.1 g | b. | 100 g | d. | 68.4 g |
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41.
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What mass of Na  SO  is
needed to make 2.5 L of 2.0 M solution? (Na = 23 g; S = 32 g; O = 16 g) a. | 178 g | c. | 356 g | b. | 284 g | d. | 710 g |
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42.
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How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of
0.50M NaBr?
a. | 25 mL | c. | 100 mL | b. | 50 mL | d. | 150 mL |
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43.
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A piece of candy has 5 Calories (or 5000 calories). If it could be burned,
leaving nothing but carbon dioxide and water, how much heat would it give off?
a. | 500 calories | c. | 5000 joules | b. | 5 kilocalories | d. | Not enough information is
given. |
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44.
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How can you describe the specific heat of olive oil if it takes approximately
420 J of heat to raise the temperature of 7 g of olive oil by 30  C? a. | greater than the specific heat of water | c. | equal to the specific heat of
water | b. | less than the specific heat of water | d. | Not enough information is
given. |
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45.
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Why does a higher concentration make a reaction faster?
a. | There are more collisions per second only. | b. | Collisions occur
with greater energy only. | c. | There are more collisions per second and the
collisions are of greater energy. | d. | There are more collisions per second or the
collisions are of greater energy. |
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46.
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Why does a catalyst cause a reaction to proceed faster?
a. | There are more collisions per second only. | b. | The collisions occur
with greater energy only. | c. | The activation energy is lowered
only. | d. | There are more collisions per second and the collisions are of greater
energy. |
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47.
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What is the formula for phosphoric acid?
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48.
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What is a property of a base?
a. | bitter taste | c. | strong color | b. | watery feel | d. | unreactive |
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49.
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If the hydrogen ion concentration of a solution is 10  M, is
the solution acidic, alkaline, or neutral? a. | acidic | c. | neutral | b. | alkaline | d. | The answer cannot be
determined. |
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50.
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In a neutral solution, the [H  ] is ____. a. | 10 M | c. | 1  10 M | b. | zero | d. | equal to [OH ] |
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51.
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Which of these solutions is the most basic?
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52.
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Which of the following pairs consists of a weak acid and a strong base?
a. | sulfuric acid, sodium hydroxide | c. | acetic acid, sodium
hydroxide | b. | acetic acid, ammonia | d. | nitric acid, calcium hydroxide |
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