Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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An element that is a poor conducter of electricity and heat is classified as
a
a. | Nonmetal | c. | Alkali metal | b. | Transition Metal | d. | Alkaline Earth
Metal |
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2.
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Which of the following shows correctly an ion pair and the ionic compound the
two ions form?
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3.
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As a consequence of the discovery of the nucleus by Rutherford, which model of
the atom is thought to be true?
a. | The nucleus is made of electrons and protons. | b. | Electrons are
distributed around the nucleus and occupy almost all the volume of the atom. | c. | The nucleus is made
of protons, electrons, and neutrons. | d. | Protons, electrons, and neutrons are evenly
distributed throughout the volume of the atom. |
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4.
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As you move from left to right across the second period of the periodic table
____.
a. | electronegativity decreases | c. | atomic radii
increase | b. | atomic mass decreases | d. | ionization energy increases |
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5.
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To 225 mL of a 0.80M solution of KI, a student adds enough water to make
1.0 L of a more dilute KI solution. What is the molarity of the new solution?
a. | 2.8M | c. | 180M | b. | 0.18M | d. | 0.35M |
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6.
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If energy is added to a boiling liquid, what happens to the temperature of the
liquid?
a. | It decreases. | c. | It increases. | b. | It does not change. | d. | The change cannot be
determined. |
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7.
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What is ammonia classified as?
a. | Arrhenius acid | c. | Bronsted-Lawry base | b. | Arrhenius base | d. | Bronsted-Lawry
acid |
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8.
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The temperature at which the motion of particles theoretically ceases is
____.
a. | 0 C | c. | –273 K | b. | 0
K | d. | 273 C |
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9.
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Which of the following occurs in an ionic bond?
a. | Oppositely charged ions attract. | b. | Two atoms share more than two
electrons. | c. | Like-charged ions attract. | d. | Two atoms share two
electrons. |
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10.
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Why does the pressure inside a container of gas increase if more gas is added to
the container?
a. | There is an increase in the temperature of the gas. | b. | There is an increase
in the force of the collisions between the particles and the walls of the
container. | c. | There is a decrease in the volume of the gas. | d. | There is an increase
in the number of collisions between particles and the walls of the
container. |
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11.
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Of the elements Fe, Hg, U, and Te, which is a representative element?
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12.
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Density is found by dividing ____.
a. | volume by mass | c. | mass by area | b. | area by mass | d. | mass by volume |
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13.
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What would likely happen if you were to touch the flask in which an endothermic
reaction were occurring?
a. | The flask would probably feel cooler than before the reaction
started. | b. | The flask would feel the same as before the reaction started. | c. | The flask would
probably feel warmer than before the reaction started. | d. | none of the
above |
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14.
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A gas occupies a volume of 2.4 L at 14.1 kPa. What volume will the gas occupy at
84.6 kPa?
a. | 14 L | c. | 2.5 L | b. | 497 L | d. | 0.40 L |
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15.
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A catalyst works by ____.
a. | changing the particle size of the reactants | b. | lowering the
activation energy barrier | c. | shifting the equilibrium position toward the
products | d. | changing the temperature of the reactants |
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16.
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You can classify water that is stored behind a dam as compared to water flowing
through a dam as an example of _______________.
a. | potential energy transformed into kinetic energy | c. | chemical energy transformed into
potential energy | b. | kinetic energy transformed into potential energy | d. | thermal energy transformed into kinetic
energy |
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17.
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What is the volume of 45.6 g of silver if the density of silver is 10.5
g/mL?
a. | 0.23 mL | c. | 4.34 mL | b. | 479 mL | d. | none of the
above |
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18.
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The experimental variable that is graphed on the x-axis is the
__________.
a. | responding variable | c. | dependent variable | b. | controlled variable | d. | manipulated
variable |
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19.
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Which of the following is a property of an acid?
a. | unreactive | c. | nonelectrolyte | b. | strong color | d. | sour taste |
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20.
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Which of the following usually makes a substance dissolve faster in a
solvent?
a. | agitating the solution | b. | decreasing the number of
particles | c. | increasing the particle size of the solute | d. | lowering the
temperature |
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21.
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What is the formula for sodium sulfate?
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22.
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In a chemical reaction, the mass of the products ____.
a. | is less than the mass of the reactants | b. | is equal to the mass of the
reactants | c. | has no relationship to the mass of the reactants | d. | is greater than the
mass of the reactants |
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23.
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At STP, how many liters of oxygen are required to react completely with 3.6
liters of hydrogen to form water? 2H  ( g) +
O  ( g) ® 2H  O( g) a. | 3.6 L | c. | 2.0 L | b. | 1.8 L | d. | 2.4 L |
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24.
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According to VSEPR theory, molecules adjust their shapes to keep which of the
following as far apart as possible?
a. | pairs of valence electrons | c. | mobile
electrons | b. | the electrons closest to the nuclei | d. | inner shell
electrons |
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25.
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The average speed of oxygen molecules in air is about ____.
a. | 170 km/h | c. | 1700 km/h | b. | 0 km/h | d. | 17,000 km/h |
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26.
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The combined gas law relates which of the following?
a. | temperature and pressure only | c. | volume and temperature
only | b. | pressure and volume only | d. | temperature, pressure, and volume |
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27.
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What is the molarity of a solution containing 7.0 moles of solute in 569 mL of
solution?
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28.
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Which is a typical characteristic of an ionic compound?
a. | The ionic compound has a high melting point. | b. | The ionic compound
is described as a molecule. | c. | Electron pairs are shared among
atoms. | d. | The ionic compound has a low solubility in water. |
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29.
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In which of these systems is the entropy decreasing?
a. | snow melting | c. | a liquid cooling | b. | air escaping from a tire | d. | salt dissolving in
water |
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30.
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What happens to the pressure of a gas inside a container if the temperature of
the gas decreases?
a. | The pressure increases. | c. | The pressure does not
change. | b. | The pressure decreases. | d. | The pressure cannot be predicted. |
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31.
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Why does a higher temperature cause a reaction to go faster?
a. | Collisions occur with greater energy only. | b. | There are more
collisions per second or the collisions are of greater energy. | c. | There are more
collisions per second and the collisions are of greater energy. | d. | There are more
collisions per second only. |
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32.
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The variable that is observed during an experiment is called what type of
variable?
a. | independent | c. | controlling | b. | responding | d. | manipulated |
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33.
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Standard conditions when working with gases are defined as ____.
a. | 0 C and 101.3 kPa | c. | 0 K and 101.3
kPa | b. | 0 K and 1 kPa | d. | 0 C and 1 kPa |
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34.
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Compared to the melting points of ionic compounds, the melting points of
molecular solids tend to be ____.
a. | unpredictable | c. | lower | b. | higher | d. | similar |
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35.
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Which expression represents a reaction rate?
a. | number/time | c. | time/mass | b. | energy/time | d. | time/energy |
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36.
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If a balloon is squeezed, what happens to the pressure of the gas inside the
balloon?
a. | It stays the same. | b. | It increases. | c. | The pressure depends
on the type of gas in the balloon. | d. | It decreases. |
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37.
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Consider the reaction N  ( g) 
3H  ( g)  2NH  ( g). What is the effect of decreasing the volume on the contained gases? a. | The system reacts by increasing the number of gas molecules. | b. | The pressure on the
gases decreases momentarily. | c. | Ammonia is consumed in the
reaction. | d. | The reaction shifts toward the product gas. |
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38.
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If the volume of a container of gas is reduced, what will happen to the pressure
inside the container?
a. | The pressure will increase. | b. | The pressure depends on the type of
gas. | c. | The pressure will not change. | d. | The pressure will
decrease. |
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39.
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A neutral atom contans
a. | varying numbers of protons and an equal number of neutrons and
electrons | c. | more electrons than protons | b. | an equal number of protons and
electrons | d. | more protons than
electrons |
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40.
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What is the molar mass of (NH  )  CO  ? a. | 96 g | c. | 78 g | b. | 138 g | d. | 144 g |
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41.
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Which statement is true about electronegativity?
a. | Electronegativity is the ability of an anion to attract another
anion. | b. | Electronegativity generally increases from left to right across a
period. | c. | Electronegativity generally is higher for metals than for
nonmetals. | d. | Electronegativity generally increases as you move from top to bottom within a
group. |
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42.
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An ionic bond is a bond between ____.
a. | valence electrons and cations | c. | a cation and an
anion | b. | the ions of two different nonmetals | d. | the ions of two different
metals |
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43.
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Express the sum of 7.68 m and 5.0 m using the correct number of significant
digits.
a. | 12.68 m | c. | 10 m | b. | 13 m | d. | 12.7 m |
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44.
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Which of the following covalent bonds is the most polar?
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45.
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What happens to the temperature of a gas when it is compressed?
a. | The temperature does not change. | b. | The temperature becomes
unpredictable. | c. | The temperature decreases. | d. | The temperature
increases. |
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46.
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How many moles of glucose, C  H  O  , can be "burned" biologically
when 10.0 mol of oxygen is available? C  H  O  ( s) + 6O  ( g) ® 6CO  ( g) + 6H  O( l) a. | 60.0 mol | c. | 53.3 mol | b. | 1.67 mol | d. | 0.938 mol |
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47.
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What is the molar mass of AuCl3?
a. | 96 g | c. | 130 g | b. | 232.5 g | d. | 303.6 g |
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48.
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Atomic size generally ____.
a. | decreases as you move from left to right across a period | b. | decreases as you
move from top to bottom within a group | c. | increases as you move from left to right across
a period | d. | remains constant within a period |
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49.
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How many moles of aluminum are needed to react completely with 1.2 mol of FeO?
2Al( s) + 3FeO( s) ® 3Fe( s) + Al  O  ( s) a. | 2.4 mol | c. | 1.6 mol | b. | 1.2 mol | d. | 0.8 mol |
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50.
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Which of the following is a heterogeneous mixture?
a. | air | c. | vinegar in water | b. | oil and vinegar | d. | milk |
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51.
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How many liters of NH  , at STP, will react
with 5.3 g O  to form NO  and water? 4NH  ( g) + 7O  ( g)  4NO  + 6H  O( g) a. | 2.12 L | c. | 6.49 L | b. | 0.004 23 L | d. | 3.03 L |
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52.
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What is the density of an object having a mass of 8.0 g and a volume of 25
cm  ? a. | 2.0 g/cm | c. | 0.32 g/cm | b. | 200 g/cm | d. | 3.1
g/cm |
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53.
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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. | 870 g | b. | 450 g | d. | 290 g |
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54.
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Atomic radius of atoms will generally
a. | increase from left to right within a period | c. | decrease from top to bottom within
a group | b. | decrease from left to right within a period | d. | remain constant within a
period |
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55.
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The experimental variable that is graphed on the y-axis is the
__________?
a. | independent variable | c. | dependent variable | b. | controlled variable | d. | secondary
variable |
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56.
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What SI unit is used to measure the number of representative particles in a
substance?
a. | ampere | c. | kilogram | b. | mole | d. | kelvin |
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57.
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What is the electron configuration of potassium?
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58.
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What is the result of adding 2.5  10  and 3.5  10  ?
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59.
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What is the SI unit of pressure?
a. | candela | c. | mole | b. | pascal | d. | newton |
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60.
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Which of the following occurs as temperature increases?
a. | Solubility decreases. | c. | Solubility remains the same. | b. | Solubility
increases. | d. | Molarity
doubles. |
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61.
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What are the missing coefficients for the skeleton equation
below? Cr( s)  Fe(NO  )  ( aq)  Fe( s)  Cr(NO  )  ( aq) a. | 2, 3, 3, 2 | c. | 1, 3, 3, 1 | b. | 4, 6, 6, 2 | d. | 2, 3, 2, 3 |
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62.
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Why is a gas easier to compress than a liquid or a solid?
a. | Its volume increases more under pressure than an equal volume of solid
does. | b. | The volume of a gas’s particles is small compared to the overall volume of the
gas. | c. | The space between gas particles is much less than the space between liquid or solid
particles. | d. | Its volume increases more under pressure than an equal volume of liquid
does. |
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63.
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The volume of a gas is doubled while the temperature is held constant. How does
the gas pressure change?
a. | It is doubled. | b. | It does not change. | c. | It varies depending
on the type of gas. | d. | It is reduced by one
half. |
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64.
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What is the molarity of a solution containing 56 grams of solute in 959 mL of
solution? (molar mass of solute = 26 g/mol)
a. | 2.1M | c. | 2.2M | b. | 0.0022M | d. | 1.5M |
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65.
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What determines that an element is a metal?
a. | its position in the periodic table | c. | the molecules that it
forms | b. | when it is a Group A element | d. | the magnitude of its
charge |
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66.
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What is the formula of the ion formed when potassium achieves noble-gas electron
configuration?
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67.
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What is a property of a base?
a. | watery feel | c. | bitter taste | b. | unreactive | d. | strong color |
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68.
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Which of these is an Arrhenius base?
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69.
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According to the kinetic theory, collisions between molecules in a gas
____.
a. | never occur | c. | are inelastic | b. | cause a loss of total kinetic
energy | d. | are perfectly
elastic |
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70.
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What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide
is dissolved?
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71.
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How many significant figures are in the measurement 811.40 grams?
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72.
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What products will form when sodium hydroxide reacts with hydrochloric
acid?
a. | Sodium hydride and chlorine hydroxide | c. | Sodium hydroxide and hydrochloric
acid | b. | Sodium chloride and water | d. | Sodium chloride, hydrogen gas, and oxygen gas |
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73.
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Which compound can act as both a Brønsted-Lowry acid and a
Brønsted-Lowry base?
a. | sodium hydroxide | c. | ammonia | b. | water | d. | hydrochloric
acid |
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74.
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What element has the electron configuration 1 s 2 s 2 p 3 s 3 p ? a. | silver | c. | nitrogen | b. | silicon | d. | selenium |
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75.
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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. | (l), liters | b. | (aq), dissolved in
water | d. | (s), solid
product |
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76.
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When an acid reacts with a base, what compounds are formed?
a. | a salt and water | c. | metal oxides only | b. | water only | d. | a salt only |
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77.
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Which step in the scientific method requires you to use your senses to obtain
information?
a. | making an observation | c. | designing an experiment | b. | revising a
hypothesis | d. | stating a
theory |
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78.
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What is the number of moles of solute in 250 mL of a 0.4M
solution?
a. | 0.16 mol | c. | 0.62 mol | b. | 0.1 mol | d. | 1.6 mol |
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79.
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What happens to a catalyst in a reaction?
a. | It is unchanged. | c. | It is incorporated into the reactants. | b. | It evaporates
away. | d. | It is incorporated
into the products. |
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80.
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Which of the following measurements (of different masses) is the most
accurate?
a. | 3.1000 g | c. | 3.100 00 g | b. | 3.000 000 g | d. | 3.122 22 g |
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81.
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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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82.
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What is the formula of the ion formed when phosphorus achieves a noble-gas
electron configuration?
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83.
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Which of the following compounds contains the Mn  ion?
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84.
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When potassium hydroxide and barium chloride react, potassium chloride and
barium hydroxide are formed. The balanced equation for this reaction is ____.
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85.
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Which of the following correctly represents an ion pair and the ionic compound
the ions form?
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86.
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What information is needed to calculate the percent composition of a
compound?
a. | the formula of the compound and the atomic mass of its elements | b. | the weight of the
sample to be analyzed and its density | c. | the formula of the compound and its
density | d. | the weight of the sample to be analyzed and its molar
volume |
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87.
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The average kinetic energy of water molecules is greatest in ____.
a. | liquid water at 373 K | c. | steam at 100 C | b. | ice at 0 C | d. | liquid water
at 90 C |
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88.
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Entropy measures ____.
a. | force | c. | energy | b. | disorder | d. | heat
transferred |
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89.
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Which of the following is a heterogeneous mixture?
a. | air | c. | soil | b. | salt water | d. | steel |
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90.
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How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C  H  O? a. | 35  (6.02  10 ) | c. | 35 | b. | 5 | d. | 5  (6.02 
10 ) |
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91.
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What is the formula for potassium sulfide?
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92.
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The average kinetic energy of the particles of a substance ____.
a. | is equal to the total energy absorbed by the substance | b. | is directly
proportional to the temperature of the substance | c. | increases as the temperature of the substance
is lowered | d. | is not affected by the temperature of the substance |
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93.
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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. | 17.1 g | c. | 68.4 g | b. | 34.2 g | d. | 100 g |
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94.
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Express the product of 2.2 mm and 5.00 mm using the correct number of
significant digits.
a. | 11.00 mm | c. | 10 mm | b. | 11.0 mm | d. | 11
mm |
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95.
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A breathing mixture used by deep-sea divers contains helium, oxygen, and carbon
dioxide. What is the partial pressure of oxygen at 101.4 kPa if  = 82.5 kPa
and  = 0.4 kPa? a. | 18.5 kPa | c. | 82.9 kPa | b. | 19.3 kPa | d. | 101.0 kPa |
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96.
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What is pH?
a. | the negative logarithm of the hydroxide ion concentration | b. | the negative
logarithm of the hydrogen ion concentration | c. | the positive logarithm of the hydrogen ion
concentration | d. | the positive logarithm of the hydroxide ion
concentration |
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97.
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What are the missing coefficients for the skeleton equation below?
Al  (SO  )  ( aq) 
KOH( aq) ® Al(OH)  ( aq)  K  SO  ( aq) a. | 4, 6, 2, 3 | c. | 1, 3, 2, 3 | b. | 2, 12, 4, 6 | d. | 1, 6, 2, 3 |
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98.
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In which of the following groups of ions are the charges all shown
correctly?
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99.
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The formula of the hydrogen ion is often written as ____.
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100.
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How many moles of tungsten atoms are in 4.8  10  atoms of tungsten?
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