Download Chemistry (B) Final Exam Study Guide 3

Chemistry (B) Final Exam Study Guide 3
Matching
Match each item with the correct statement below.
a. product
d. balanced equation
b. reactant
e. skeleton equation
c. chemical equation
____
____
____
____
____
1.
2.
3.
4.
5.
a chemical equation that does not indicate relative amounts of reactants and products
a new substance formed in a chemical reaction
a starting substance in a chemical reaction
a concise representation of a chemical reaction
an equation in which each side has the same number of atoms of each element
Match each item with the correct statement below.
a. activity series of metals
c. combustion reaction
b. single-replacement reaction
d. decomposition reaction
____
____
____
____
6.
7.
8.
9.
a reaction in which a single compound is broken down into simpler substances
a reaction in which oxygen reacts with another substance, often producing heat or light
a reaction in which the atoms of one element replace the atoms of a second element in a compound
a list of metals in order of decreasing reactivity
Match each item with the correct statement below.
a. melting point
d. evaporation
b. boiling point
e. vaporization
c. sublimation
f. normal boiling point
____
____
____
____
____
____
10.
11.
12.
13.
14.
15.
vaporization at the surface of a liquid that is not boiling
the conversion of a liquid to a gas below the boiling point
the temperature at which the vapor pressure of a liquid is equal to the external pressure
the temperature at which the vapor pressure of a liquid is equal to 1 atmosphere
the temperature at which a solid changes into a liquid
the change of a solid directly to a vapor
Match each item with the correct statement below.
a. kinetic theory
d. barometer
b. atmospheric pressure
e. kinetic energy
c. vapor pressure
____
____
____
____
____
16.
17.
18.
19.
20.
All matter consists of tiny particles that are in constant motion.
the energy an object has due to its motion
a device used to measure atmospheric pressure
the pressure resulting from the collision of atoms and molecules with objects
a measure of the force exerted by a gas above a liquid
Match each item with the correct statement below.
a. substituent
e. asymmetric carbon
b. structural isomers
f. trans configuration
c. geometric isomers
g. cis configuration
d. stereoisomers
____
____
____
____
____
____
____
21.
22.
23.
24.
25.
26.
27.
atom or group of atoms that can take the place of a hydrogen in a parent hydrocarbon molecule
compounds that have the same molecular formula, but the atoms are joined in a different order
arrangement in which substituted groups are on the same side of a double bond
molecules in which atoms are joined in the same order but differ in the arrangements of their atoms in space
arrangement in which substituted groups are on opposite sides of a double bond
compounds that differ in the orientation of groups around a double bond
carbon atom to which four different atoms or groups are attached
Match each item with the correct statement below.
a. positron
d. transuranium element
b. alpha particle
e. gamma radiation
c. beta particle
f. transmutation
____
____
____
____
____
____
28.
29.
30.
31.
32.
33.
element with atomic number greater than 92
emitted helium nucleus
energetic electron from decomposed neutron
high-energy photons emitted by a radioisotope
particle of charge +1 and mass equal to that of an electron
conversion of an atom of one element to an atom of another element
Match each item with the correct statement below.
a. fission
e. scintillation counter
b. fusion
f. neutron absorption
c. Geiger counter
g. neutron moderation
d. radioisotope
____
____
____
____
____
____
____
34.
35.
36.
37.
38.
39.
40.
element with unstable nucleus
combination of two nuclei to form a nucleus of greater mass
process that decreases the number of slow-moving neutrons
splitting of nucleus into smaller fragments
process that slows down neutrons so a reactor fuel can capture them to continue a chain reaction
radiation detector that makes use of a phosphor-coated surface
radiation detector that makes use of a gas-filled metal tube
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 41. Chemical reactions ____.
a. occur only in living organisms
b. create and destroy atoms
____ 42. Everyday equations describe ____.
a. thermonuclear reactions
b. everyday processes
c. only occur outside living organisms
d. produce new substances
c. chemical reactions
d. biological chemistry
____ 43. What does the symbol in a chemical equation mean?
a. Heat is supplied to the reaction.
c. yields
b. A catalyst is needed.
d. precipitate
____ 44. Chemical equations ____.
a. describe chemical reactions
b. show how to write chemical formulas
c. give directions for naming chemical compounds
d. describe only biological changes
____ 45. A skeleton equation does NOT show which of the following?
a. the correct formulas of the reactants and products
b. the reactants on the left, the products on the right
c. an arrow connecting the reactants to the products
d. the relative amounts of reactants and products
____ 46. 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
____ 47. 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
____ 48. Which of the following is the correct skeleton equation for the reaction that takes place when solid
phosphorus combines with oxygen gas to form diphosphorus pentoxide?
a. P(s) O (g)  PO (g)
c. P(s) O2(g)  P O (s)
b. P(s) O(g)  P O (g)
d. P O (s)  P (s) O (g)
____ 49. If you rewrite the following word equation as a balanced chemical equation, what will the coefficient and
symbol for fluorine be?
nitrogen trifluoride
nitrogen fluorine
a. 6F
c. 6F
b. F
d. 3F
____ 50. What are the coefficients that will balance the skeleton equation below?
AlCl + NaOH
Al(OH)
NaCl
a. 1, 3, 1, 3
c. 1, 1, 1, 3
b. 3, 1, 3, 1
d. 1, 3, 3, 1
____ 51. What are the coefficients that will balance the skeleton equation below?
N +H
NH
a. 1, 1, 2
c. 3, 1, 2
b. 1, 3, 3
d. 1, 3, 2
____ 52. When the equation Fe Cl
FeCl is balanced, what is the coefficient for Cl ?
a. 1
c. 3
b. 2
d. 4
____ 53. When the following equation is balanced, what is the coefficient for HCl?
Mg(s) HCl(aq)
MgCl (aq) H (g)
a. 6
c. 1
b. 3
d. 2
____ 54. Which of the following statements is NOT true about what happens in all chemical reactions?
a. The ways in which atoms are joined together are changed.
b. New atoms are formed as products.
c. The starting substances are called reactants.
d. The bonds of the reactants are broken and new bonds of the products are formed.
____ 55. Chemical equations must be balanced to satisfy ____.
a. the law of definite proportions
c. the law of conservation of mass
b. the law of multiple proportions
d. Avogadro’s principle
____ 56. When the equation KClO (s)
KCl(s) + O (g) is balanced, the coefficient of KClO3 is ____.
a. 1
c. 3
b. 2
d. 4
____ 57. What are the missing coefficients for the skeleton equation below?
Cr(s) Fe(NO ) (aq)
Fe(s) Cr(NO ) (aq)
a. 4, 6, 6, 2
c. 2, 3, 3, 2
b. 2, 3, 2, 3
d. 1, 3, 3, 1
____ 58. What are the missing coefficients for the skeleton equation below?
Al (SO ) (aq) KOH(aq)  Al(OH) (aq) K SO (aq)
a. 1, 3, 2, 3
c. 4, 6, 2, 3
b. 2, 12, 4, 6
d. 1, 6, 2, 3
____ 59. The product of a combination reaction is Ba(OH) . If one of the reactants is H O, what is the other reactant?
a. Ba O
c. BaH
b. BaO
d. BaO
____ 60. In order to predict whether or not a single-replacement reaction takes place, you need to consult a chart that
shows the ____.
a. periodic table
b. activity series of metals
c. common polyatomic ions
d. ionic charges of representative elements
____ 61. In order for the reaction 2Al 6HCl
2AlCl
3H to occur, which of the following must be true?
a. Al must be above Cl on the activity series.
b. Al must be above H on the activity series.
c. Heat must be supplied for the reaction.
d. A precipitate must be formed.
____ 62. In a combustion reaction, one of the reactants is ____.
a. hydrogen
c. oxygen
b. nitrogen
d. a metal
____ 63. The products of a combustion reaction do NOT include ____.
a. water
c. carbon monoxide
b. carbon dioxide
d. hydrogen
____ 64. In a double-replacement reaction, the ____.
a. products are always molecular
b. reactants are two ionic compounds
c. reactants are two elements
d. products are a new element and a new compound
____ 65. Which of the following statements is NOT correct?
a. The only way to determine the products of a reaction is to carry out the reaction.
b. All chemical reactions can be classified as one of five general types.
c. Complete combustion has occurred when all the carbon in the product is in the form of
carbon dioxide.
d. A single reactant is the identifying characteristic of a decomposition reaction.
____ 66. Which of the following is a balanced equation representing the decomposition of lead(IV) oxide?
a. PbO
c. Pb O
Pb 2O
2Pb O
b. PbO
d. PbO
Pb O
Pb O
____ 67. What are the correct formulas and coefficients for the products of the following double-replacement reaction?
RbOH H PO

a. Rb(PO ) H O
c. Rb PO
3H O
b. RbPO
d. H Rb PO OH
2H O
____ 68. Which of the following statements is NOT true about the decomposition of a simple binary compound?
a. The products are unpredictable.
b. The products are the constituent elements.
c. The reactant is a single substance.
d. The reactant could be an ionic or a molecular compound.
____ 69. Which of the following statements is true about single-replacement reactions?
a. They are restricted to metals.
c. Two reactants produce two products.
b. They involve a single product.
d. Any metal replaces any other metal.
____ 70. In the activity series of metals, which metal(s) will displace hydrogen from an acid?
a. only metals above hydrogen
c. any metal
b. only metals below hydrogen
d. only metals from Li to Na
____ 71. Use the activity series of metals to complete a balanced chemical equation for the following single
replacement reaction.
Ag(s) KNO (aq) 
a. AgNO
K
b. AgK NO
c. AgKNO
d. No reaction takes place because silver is less reactive than potassium.
____ 72. Which of the following statements is NOT true about double-replacement reactions?
a. The product may precipitate from solution.
b. The product may be a gas.
c. The product may be a molecular compound.
d. The reactant may be a solid metal.
____ 73. In a double-replacement reaction, ____.
a. the reactants are usually a metal and a nonmetal
b. one of the reactants is often water
c. the reactants are generally two ionic compounds in aqueous solution
d. energy in the form of heat or light is often produced
____ 74. A double-replacement reaction takes place when aqueous Na CO reacts with aqueous Sn(NO ) . You
would expect one of the products of this reaction to be ____.
a. NaNO
c. Sn(CO )
b. NaSn
d. CNO
____ 75. The complete combustion of which of the following substances produces carbon dioxide and water?
a. C H
c. CaHCO
b. K CO
d. NO
____ 76. Which of the following is the correctly balanced equation for the incomplete combustion of heptene, C H ?
a. C H
c. 2C H
14O
7CO 7H O
21O
14CO
14H O
b. C H
d. C H
7O
7CO 7H O
O
C O
7H
____ 77. The reaction 2Fe 3Cl
2FeCl is an example of which type of reaction?
a. combustion reaction
c. combination reaction
b. single-replacement reaction
d. decomposition reaction
____ 78. The equation Mg(s) 2HCl(aq)
MgCl (aq) H g is an example of which type of reaction?
a. combination reaction
c. decomposition reaction
b. single-replacement reaction
d. double-replacement reaction
____ 79. The equation H PO
3KOH
K PO
3H O is an example of which type of reaction?
a. double-replacement reaction
c. decomposition reaction
b. combination reaction
d. single-replacement reaction
____ 80. The equation 2C H OH 9O
6CO
8H O is an example of which type of reaction?
a. combustion reaction
c. double-replacement reaction
b. single-replacement reaction
d. decomposition reaction
____ 81. A double-replacement reaction takes place when aqueous cobalt(III) chloride reacts with aqueous lithium
hydroxide. One of the products of this reaction is ____.
a. Co(OH)
c. LiCo
b. Co(OH)
d. LiCl
____ 82. What is the balanced chemical equation for the reaction that takes place between bromine and sodium iodide?
a. Br
c. Br NaI
NaI
NaBr
I
NaBrI
b. Br
d. Br NaI
2NaI
2NaBr I
NaBr I
____ 83. What is the driving force in the following reaction?
Ni(NO ) (aq) K S(aq)
NiSs 2KNO (aq)
a. A gas is formed.
c. Ionic compounds are reactants.
b. A precipitate is formed.
d. Ionic compounds are products.
____ 84. According to the kinetic theory, collisions between molecules in a gas ____.
a. are perfectly elastic
c. never occur
b. are inelastic
d. cause a loss of total kinetic energy
____ 85. Which of the following statements is part of the kinetic theory?
a. The particles of a gas move independently of each other.
b. The particles in a gas move rapidly.
c. The particles in a gas are relatively far apart.
d. all of the above
____ 86. 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.
____ 87. Particles in a gas are best described as ____.
a. slow-moving, kinetic, hard spheres
b. spheres that are in fixed positions when trapped in a container
c. small, hard spheres with insignificant volumes
d. hard spheres influenced by repulsive forces from other spheres
____ 88. Which of the following statements is NOT true about the movement of particles in a gas?
a. Particles travel in straight-line paths until they collide with other objects.
b. Particles usually travel uninterrupted indefinitely.
c. Particles fill their containers regardless of the shape or volume of the container.
d. The aimless path taken by particles is known as a random walk.
____ 89. What instrument is normally used to measure atmospheric pressure?
a. thermometer
c. vacuum
b. barometer
d. manometer
____ 90. What is the SI unit of pressure?
a. candela
c. pascal
b. mole
d. newton
____ 91. What is one standard atmosphere of pressure in kilopascals?
a. 0 kPa
c. 101.3 kPa
b. 760 kPa
d. 1 kPa
____ 92. Standard conditions when working with gases are defined as ____.
a. 0 K and 101.3 kPa
c. 0 C and 101.3 kPa
b. 0 K and 1 kPa
d. 0 C and 1 kPa
____ 93. How does the atmospheric pressure at altitudes below sea level compare with atmospheric pressure at sea
level?
a. The atmospheric pressure below sea level is higher.
b. The atmospheric pressure below sea level is lower.
c. The pressures are the same.
d. Differences in pressures cannot be determined.
____ 94. What causes gas pressure in a container such as a helium balloon?
a. the walls of the container
b. the vacuum maintained in the container
c. the simultaneous collisions of fast-moving particles in the container
d. atmospheric pressure acting on the outside walls of the container
____ 95. The pressure of a gas in a container is 152 mm Hg. This is equivalent to ____.
a. 0.2 atm
c. 0.3 atm
b. 2 atm
d. 0.4 atm
____ 96. What happens to the average kinetic energy of the particles in a sample of matter as the temperature of the
sample is increased?
a. The average kinetic energy decreases.
b. The average kinetic energy increases.
c. The average kinetic energy does not change.
d. The change in average kinetic energy cannot be determined.
____ 97. With which temperature scale is temperature directly proportional to average kinetic energy?
a. Celsius
c. Kelvin
b. Fahrenheit
d. centigrade
____ 98. What happens to the range of energies of the particles in matter when the temperature is increased?
a. The range of energies becomes narrower.
b. The range of energies becomes broader.
c. The range of energies does not change.
d. The range of energies cannot be determined.
____ 99. The average kinetic energy of the particles of a substance ____.
a. is not affected by the temperature of the substance
b. increases as the temperature of the substance is lowered
c. is directly proportional to the temperature of the substance
d. is equal to the total energy absorbed by the substance
____ 100. When a gas is heated, ____.
a. all of the absorbed energy is converted to kinetic energy
b. some of the absorbed energy is converted to potential energy, and some is converted to
kinetic energy
c. all of the absorbed energy is converted to potential energy
d. none of the energy is converted to kinetic energy
____ 101. Consider an iron cube and an aluminum cube. If the two cubes were at the same temperature, how would the
average kinetic energy of the particles in iron compare with the average kinetic energy of the particles in
aluminum?
a. The average kinetic energy of the iron particles would be greater.
b. The average kinetic energy of the aluminum particles would be greater.
c. There would be no difference in the average kinetic energies.
d. No determination can be made based on the information given.
____ 102. The average kinetic energy of water molecules is greatest in ____.
a. steam at 100 C
c. liquid water at 373 K
b. liquid water at 90 C
d. ice at 0 C
____ 103. What is the key difference between a liquid and a gas?
a. intermolecular attractions
c. average kinetic energy
b. the ability to flow
d. the motion of their particles
____ 104. Which states of matter can flow?
a. gases only
c. gases and liquids only
b. liquids only
d. gases, liquids, and solids
____ 105. What happens to the temperature of a liquid as it evaporates?
a. It increases.
c. It does not change.
b. It decreases.
d. The change cannot be determined.
____ 106. Which are the first particles to evaporate from a liquid?
a. particles with the lowest kinetic energy
b. particles with the highest kinetic energy
c. particles below the surface of the liquid
d. All particles evaporate at the same rate.
____ 107. What happens to the rate of evaporation of a liquid as the liquid is cooled?
a. It increases.
c. It does not change.
b. It decreases.
d. The change cannot be determined.
____ 108. Why does a liquid's rate of evaporation increase when the liquid is heated?
a. More molecules have enough energy to overcome the attractive forces holding them in the
liquid.
b. The average kinetic energy of the liquid decreases.
c. The surface area of the liquid is reduced.
d. The potential energy of the liquid increases.
____ 109. Which of the following will evaporate the fastest?
a. water at 0 C
b. water at 20 C
c. water at 40 C
d. All samples will evaporate at the same rate.
____ 110. In a dynamic equilibrium between the liquid state and the gas state, what is true about the rate of evaporation?
a. It is greater than the rate of condensation.
b. It is less than the rate of condensation.
c. It is equal to the rate of condensation.
d. The rate of evaporation cannot be determined.
____ 111. If a liquid is sealed in a container and kept at constant temperature, how does its vapor pressure change over
time?
a. It continues to steadily increase.
b. It increases at first, then remains constant.
c. It increases at first, then decreases.
d. It continues to steadily decrease.
____ 112. An increase in the temperature of a contained liquid ____.
a. has no effect on the kinetic energy of the liquid
b. causes the vapor pressure above the liquid to decrease
c. causes fewer particles to escape from the surface of the liquid
d. causes the vapor pressure above the liquid to increase
____ 113. If energy is added to a boiling liquid, what happens to the temperature of the liquid?
a. It increases.
c. It does not change.
b. It decreases.
d. The change cannot be determined.
____ 114. What is the pressure when a liquid is boiling at its normal boiling point?
a. 0 kPa
c. 202 kPa
b. 101.3 kPa
d. 505 kPa
____ 115. Water could be made to boil at 105 C instead of 100 C by ____.
a. adding a lot of energy to the water
c. decreasing the external pressure
b. increasing the external pressure
d. taking the sample to a higher altitude
____ 116. When the external pressure is 505 kPa, what is the vapor pressure of water at its boiling point?
a. 0 kPa
c. 505 kPa
b. 101.3 kPa
d. 1010 kPa
____ 117. The normal boiling point of chloroform, which has a higher vapor pressure than water at 100 C, is ____.
a. higher than the normal boiling point of water
b. lower than the normal boiling point of water
c. the same as the normal boiling point of water
d. unable to be measured
____ 118. Which of the following best describes the motion of the particles in a piece of steel?
a. None are moving.
c. All are moving.
b. A few are moving.
d. Most are moving.
____ 119. Most solids ____.
a. are dense and difficult to compress
c. are amorphous
b. are able to flow
d. have a disorderly structure
____ 120. Crystals are classified into how many different crystal systems?
a. 4
c. 6
b. 5
d. 7
____ 121. Crystals are characterized by particular patterns that repeat in how many dimensions?
a. one dimension only
c. three dimensions only
b. two dimensions only
d. The patterns do not repeat.
____ 122. How do crystal systems differ?
a. in the angles between faces only
b. in the number of edges of equal length only
c. in the angles between faces and the number of edges of equal length
d. Crystal systems do not differ.
____ 123. Which of the following elements has the ability to undergo sublimation?
a. oxygen
c. sodium
b. carbon
d. iodine
____ 124. Which of the following is an example of a phase?
a. pressure
c. temperature
b. water vapor
d. triple point
____ 125. How are conditions of pressure and temperature, at which two phases coexist in equilibrium, shown on a
phase diagram?
a. by a line separating the phases
b. by the endpoints of the line segment separating the phases
c. by the planar regions between lines in the diagram
d. by a triple point on the diagram
____ 126. 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 liquid does.
b. Its volume increases more under pressure than an equal volume of solid does.
c. The space between gas particles is much less than the space between liquid or solid
particles.
d. The volume of a gas’s particles is small compared to the overall volume of the gas.
____ 127. 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 number of collisions between particles and the walls of the
container.
b. There is an increase in the temperature of the gas.
c. There is a decrease in the volume of the gas.
d. There is an increase in the force of the collisions between the particles and the walls of the
container.
____ 128. How does the gas propellant move when an aerosol can is used?
a. from a region of high pressure to a region of lower pressure
b. from a region of high pressure to a region of equally high pressure
c. from a region of low pressure to a region of higher pressure
d. from a region of low pressure to a region of equally low pressure
____ 129. 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 will not change.
c. The pressure will decrease.
d. The pressure depends on the type of gas.
____ 130. If a balloon is squeezed, what happens to the pressure of the gas inside the balloon?
a. It increases.
b. It stays the same.
c. It decreases.
d. The pressure depends on the type of gas in the balloon.
____ 131. What happens to the temperature of a gas when it is compressed?
a. The temperature increases.
b. The temperature does not change.
c. The temperature decreases.
d. The temperature becomes unpredictable.
____ 132. 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
____ 133. 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 decreases.
b. The pressure does not change.
d. The pressure cannot be predicted.
____ 134. If 4 moles of gas are added to a container that already holds 1 mole of gas, how will the pressure change
inside the container?
a. The pressure will be five times higher.
b. The pressure will double.
c. The pressure will be four times higher.
d. The pressure will not change.
____ 135. Why does air escape from a tire when the tire valve is opened?
a. The pressure outside the tire is lower than the pressure inside the tire.
b. The pressure outside the tire is greater than the pressure inside the tire.
c. The temperature is higher outside the tire than inside the tire.
d. There are more particles of air outside the tire than inside the tire.
____ 136. Which of these changes would NOT cause an increase in the pressure of a contained gas?
a. The volume of the container is increased.
b. More of the gas is added to the container.
c. The temperature is increased.
d. The average kinetic energy of the gas in increased.
____ 137. 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
____ 138. The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change?
a. It is reduced by one half.
b. It does not change.
c. It is doubled.
d. It varies depending on the type of gas.
____ 139. The volume of a gas is reduced from 4 L to 0.5 L while the temperature is held constant. How does the gas
pressure change?
a. It increases by a factor of four.
c. It increases by a factor of eight.
b. It decreases by a factor of eight.
d. It increases by a factor of two.
____ 140. When the temperature and number of particles of a gas are constant, which of the following is also constant?
a. the sum of the pressure and volume
b. the difference of the pressure and volume
c. the product of the pressure and volume
d. the ratio of the pressure and volume
____ 141. If a balloon is heated, what happens to the volume of the air in the balloon if the pressure is constant?
a. It increases.
c. It decreases.
b. It stays the same.
d. The change cannot be predicted.
____ 142. When the pressure and number of particles of a gas are constant, which of the following is also constant?
a. the sum of the volume and temperature in kelvins
b. the difference of the volume and temperature in kelvins
c. the product of the volume and temperature in kelvins
d. the ratio of the volume and temperature in kelvins
____ 143. If a balloon is heated, what happens to the pressure of the air inside the balloon if the volume remains
constant?
a. It increases.
c. It decreases.
b. It stays the same.
d. The change cannot be predicted.
____ 144. When the volume and number of particles of a gas are constant, which of the following is also constant?
a. the sum of the pressure and temperature in kelvins
b. the difference of the pressure and temperature in kelvins
c. the product of the pressure and temperature in kelvins
d. the ratio of the pressure and temperature in kelvins
____ 145. If a sealed syringe is plunged into cold water, in which direction will the syringe piston slide?
a. in
c. No movement will occur.
b. out
d. The direction cannot be predicted.
____ 146. What happens when a piston is used to decrease the volume of a contained gas?
a. Fewer gas particles exert a force on the piston.
b. The piston’s pressure on the gas becomes greater than the pressure exerted by the gas on
the piston.
c. Gas particles become compressed.
d. Gas particles leak out of the container.
____ 147. If a sealed syringe is heated, in which direction will the syringe plunger move?
a. out
c. The plunger will not move.
b. in
d. The direction cannot be predicted.
____ 148. In general, for a gas at a constant volume, ____.
a. the pressure of the gas is inversely proportional to its temperature in kelvins
b. the volume of the gas is inversely proportional to its temperature in kelvins
c. the volume of the gas is directly proportional to its temperature in kelvins
d. the pressure of the gas is directly proportional to its temperature in kelvins
____ 149. The combined gas law relates which of the following?
a. pressure and volume only
c. volume and temperature only
b. temperature and pressure only
d. temperature, pressure, and volume
____ 150. What does the ideal gas law allow a scientist to calculate that the other gas laws do not?
a. number of moles
c. volume
b. pressure
d. temperature
____ 151. At a certain temperature and pressure, 0.20 mol of carbon dioxide has a volume of 3.1 L. A 3.1-L sample of
hydrogen at the same temperature and pressure ____.
a. has the same mass
b. contains the same number of atoms
c. has a higher density
d. contains the same number of molecules
____ 152. How is the ideal gas law usually written?
a.
=R
b.
= nR
c. PV = nRT
d.
P=
____ 153. Which law can be used to calculate the number of moles of a contained gas?
a. Boyle’s law
c. ideal gas law
b. combined gas law
d. Charles’s law
____ 154. Which of the following is constant for 1 mole of any ideal gas?
a. PVT
c.
b.
d.
____ 155. At high pressures, how does the volume of a real gas compare with the volume of an ideal gas under the same
conditions?
a. It is much greater.
c. There is no difference.
b. It is much less.
d. It depends on the type of gas.
____ 156. At low temperatures and pressures, how does the volume of a real gas compare with the volume of an ideal
gas under the same conditions?
a. It is greater.
c. There is no difference.
b. It is less.
d. It depends on the type of gas.
____ 157. An ideal gas CANNOT be ____.
a. condensed
c. heated
b. cooled
d. compressed
____ 158. Under what conditions of temperature and pressure is the behavior of real gases most like that of ideal gases?
a. low temperature and low pressure
c. high temperature and low pressure
b. low temperature and high pressure
d. high temperature and high pressure
____ 159. If the atmospheric pressure on Mt. Everest is one-third the atmospheric pressure at sea level, the partial
pressure of oxygen on Everest is ____.
a. one-sixth its pressure at sea level
c. one-half its pressure at sea level
b. one-third its pressure at sea level
d. equal to its pressure at sea level
____ 160. What happens to the partial pressure of oxygen in a sample of air if the temperature is increased?
a. It increases.
c. It decreases.
b. It stays the same.
d. The change cannot be determined.
____ 161. If oxygen is removed from a sample of air as iron rusts, what happens to the partial pressure of oxygen in the
air?
a. It increases.
c. It decreases.
b. It stays the same.
d. The change cannot be determined.
____ 162. If oxygen is removed from a sample of air as iron rusts, what happens to the total pressure of the air?
a. It increases.
c. It decreases.
b. It stays the same.
d. The change cannot be determined.
____ 163. A box with a volume of 22.4 L contains 1.0 mol of nitrogen and 2.0 mol of hydrogen at 0 C. Which of the
following statements is true?
a. The total pressure in the box is 101 kPa.
b. The partial pressures of N and H are equal.
c. The total pressure is 202 kPa
d. The partial pressure of N is 101 kPa.
____ 164. If the volume of a container of air is reduced by one-half, what happens to the partial pressure of oxygen
within the container?
a. It is reduced by one-half.
c. It is doubled.
b. It does not change.
d. It is reduced by one-fourth.
____ 165. Which of the following gases will effuse the most rapidly?
a. bromine
c. ammonia
b. chlorine
d. hydrogen
____ 166. Which of the following atoms would have the greatest velocity if each atom had the same kinetic energy?
a. bromine
c. ammonia
b. chlorine
d. hydrogen
____ 167. Which of the following gases is the best choice for inflating a balloon that must remain inflated for a long
period of time?
a. argon
c. hydrogen
b. oxygen
d. neon
____ 168. How many valence electrons does a carbon atom have?
a. 1
c. 3
b. 2
d. 4
____ 169. How many covalent bonds can each carbon atom form?
a. 1
c. 3
b. 2
d. 4
____ 170. How many double covalent bonds are in an alkane?
a. 0
c. 2
b. 1
d. 3
____ 171. Alkanes are hydrocarbons that contain what type of bonds?
a. single covalent bonds only
c. at least one triple bond
b. at least one double bond
d. ionic bonds
____ 172. What is the simplest alkane?
a. butane
c. methane
b. ethane
d. pentane
____ 173. How many carbons are in a molecule of hexane?
a. 3
c. 5
b. 4
d. 6
____ 174. What is the name of the alkane having five carbons?
a. propane
c. octane
b. methane
d. pentane
____ 175. What is the simplest straight-chain alkane?
a. graphite
c. methane
b. ammonia
d. ethane
____ 176. Which of the following is a condensed structural formula for propane?
a. C H
c. CH CH CH
b. CH CH CH
d. CH CH CH CH
____ 177. The name for an alkyl group that contains two carbon atoms is ____.
a. diphenyl
c. dimethyl
b. ethyl
d. propyl
____ 178. What is the physical state of the smallest alkanes at room temperature?
a. gas
c. solid
b. liquid
d. gas or liquid
____ 179. What is the general formula for a straight-chain alkane?
a. C H
c. C H
b. C H
d. C H
____ 180. What is the increment of change in a series of straight-chain alkanes?
a. CH
c. CH
b. CH
d. CH
____ 181. What is the condensed structural formula for 2,2-dimethylbutane?
a. CH (CH ) CH
c. (CH ) CCH CH
b. CH CH CH CH CH
d. C H (CH )
____ 182. What is the name of the compound CH CH(CH )C(CH ) ?
a. 2,2,3-trimethylbutane
c. 1,1,1,2-tetramethylpropane
b. tetramethylpropane
d. isoheptane
____ 183. The condensed structural formula for 2,2,3-trimethylbutane is ____.
a. CH CH (CH )CH(CH )
c. CH C(CH ) CH(CH )
b. CH C(CH ) C(CH )
d. CH CH CH(CH )C(CH )
____ 184. In which of the following liquids is hexane most likely to dissolve?
a. aqueous ammonium hydroxide
c. rubbing alcohol
b. vinegar
d. octane
____ 185. Why are the molecules of hydrocarbons nonpolar?
a. The intermolecular attractions are strong.
b. All the bonds are single covalent bonds.
c. The electron pair is shared almost equally in all the bonds.
d. Van der Waals forces overcome polarity.
____ 186. Which of the following compounds is an unsaturated hydrocarbon?
a. methane
c. nonane
b. propyne
d. methyl
____ 187. In which of the following compounds does rotation occur around all covalent bonds between carbons?
a. octene
c. octane
b. octyne
d. all of the above
____ 188. A saturated straight-chain hydrocarbon with two carbons is ____.
a. ethene
c. propane
b. decane
d. ethane
____ 189. Which of these compounds is an alkene?
a. methane
c. butyne
b. nonene
d. propanone
____ 190. What is the name of the smallest alkyne?
a. butyne
c. methyne
b. ethyne
d. propyne
____ 191. An organic compound that contains only carbon and hydrogen and at least one carbon-carbon triple bond is
classified as an ____.
a. alkane
c. alkyne
b. alkene
d. arene
____ 192. How are hydrogen atoms arranged in ethene?
a. in the same plane, separated by angles of 120
b. in different planes, separated by angles of 120
c. in the same plane, separated by angles of 180
d. in different planes, separated by angles of 180
____ 193. Which of the following compounds is a structural isomer of butane?
a. 2-methylbutane
c. 2-methylpropane
b. 2,2-dimethylbutane
d. 2,2-diethylpropane
____ 194. Which of the following is true about structural isomers?
a. Structural isomers have the same molecular formula.
b. Structural isomers have different physical and chemical properties.
c. Structural isomers have the same elemental composition.
d. all of the above
____ 195. A structural isomer of hexane is ____.
a. 2,2-dimethylbutane
c. benzene
b. cyclohexane
d. 2-methylpentene
____ 196. Alkanes do not have geometric isomers because the carbon atoms in their carbon-carbon bonds are ____.
a. double bonds
c. free to rotate
b. quite polar
d. asymmetric
____ 197. How many different atoms or groups are attached to an asymmetric carbon?
a. 2
c. 6
b. 4
d. 8
____ 198. Which hydrocarbon rings are most common in nature?
a. rings with 3 or 4 carbon atoms
c. rings with 5 or 6 carbon atoms
b. rings with 4 or 5 carbon atoms
d. rings with 6 or 7 carbon atoms
____ 199. In a cyclic hydrocarbon with only carbon-carbon single bonds and n number of carbon atoms, how many
hydrogen atoms are there in terms of n?
a. 2 – n
c. 2 + n
b. 2
d. 2n
____ 200. What compound is the simplest aromatic compound?
a. methane
c. ethyne
b. ethene
d. benzene
____ 201. Which of the following molecules does NOT display resonance?
a. benzene
c. m-xylene
b. phenylethane
d. cyclohexane
____ 202. Which of the following is NOT an important fossil fuel?
a. petroleum
c. natural gas
b. hydrogen
d. coal
____ 203. What is the first stage in the formation of coal?
a. lignite
c. peat
b. anthracite coal
d. bituminous coal
____ 204. What is the main hydrocarbon component of natural gas?
a. benzene
c. ethene
b. ethane
d. methane
____ 205. Which type of coal has the highest carbon content?
a. anthracite
c. lignite
b. bituminous
d. peat
____ 206. What is the first step in the refining of petroleum?
a. cracking
c. cooling
b. drilling
d. distillation
____ 207. Which of the following is NOT a fraction obtained from crude oil?
a. ammonia
c. gasoline
b. natural gas
d. kerosene
____ 208. Which of the following is NOT a product obtained from the distillation of coal tar?
a. benzene
c. coke
b. phenol
d. toluene
____ 209. An unstable nucleus ____.
a. increases its nuclear mass by fission
c. emits energy when it decays
b. increases its half-life
d. expels all of its protons
____ 210. Which is the most susceptible to damage from ionizing radiation?
a. soft tissue
c. wood
b. paper
d. lead
____ 211. What particle is emitted in alpha radiation?
a. electron
c. helium nucleus
b. photon
d. hydrogen nucleus
____ 212. A beta particle is a(n) ____.
a. photon
c. helium nucleus
b. electron
d. hydrogen nucleus
____ 213. What is the change in atomic mass when an atom emits a beta particle?
a. decreases by 2
c. remains the same
b. decreases by 1
d. increases by 1
____ 214. What is the change in atomic mass when an atom emits gamma radiation?
a. decreases by 2
c. remains the same
b. decreases by 1
d. increases by 1
____ 215. What is the change in the atomic number when an atom emits an alpha particle?
a. decreases by 2
c. increases by 1
b. decreases by 1
d. increases by 2
____ 216. What is the change in atomic number when an atom emits a beta particle?
a. decreases by 2
c. increases by 2
b. decreases by 1
d. increases by 1
____ 217. What is the change in atomic number caused by the emission of gamma radiation?
a. decreases by 2
c. remains the same
b. decreases by 1
d. increases by 1
____ 218. Which symbol is used for an alpha particle?
a. He
c. He
b. He
d. He
____ 219. Which of the following materials is necessary to stop an alpha particle?
a. three feet of concrete
c. single sheet of aluminum foil
b. three inches of lead
d. single sheet of paper
____ 220. What particle decomposes to produce the electron of beta radiation?
a. proton
c. electron
b. neutron
d. positron
____ 221. What symbol is used for beta radiation?
a. e
c.
e
b.
d.
e
e
____ 222. Which of the following materials is necessary to stop a beta particle?
a. three feet of concrete
c. thin pieces of wood
b. three inches of lead
d. single sheet of paper
____ 223. Which of the following materials is most effective for stopping gamma radiation?
a. several cm of lead
c. single sheet of aluminum foil
b. one cm of water
d. single sheet of paper
____ 224. Which type of ionizing radiation can be blocked by clothing?
a. beta radiation
c. gamma radiation
b. X radiation
d. alpha radiation
____ 225. What is the change in atomic mass number when an atom emits an alpha particle?
a. decreases by 2
c. increases by 2
b. decreases by 4
d. increases by 4
____ 226. What does the band of stability for atomic nuclei refer to?
a. the ratio of protons to neutrons
b. the ratio of neutrons to protons
c. the ratio of beta particles to neutrinos
d. the ratio of alpha particles to beta particles
____ 227. If an isotope decays by the process of beta emission, ____.
a. the mass number changes
b. the atomic number changes
c. protons are given off
d. the number of neutrons remains the same
____ 228. What particle is needed to complete this nuclear reaction?
Rn
Po + _____
a. He
c. H
b.
e
d.
n
____ 229. How does an atom with too many neutrons relative to protons undergo radioactive decay?
a. by emitting an alpha particle
c. by emitting gamma radiation
b. by emitting a beta particle
d. by emitting X radiation
____ 230. What particle does argon-39 (atomic number 18) emit when it decays to potassium-39 (atomic number 19)?
a. neutron
c. proton
b. electron
d. alpha particle
____ 231. What particle is needed to complete the following nuclear equation?
Mn
____ + e
a.
c.
Co
Fe
b.
Mn
d.
Cr
____ 232. What particle is needed to complete the following equation?
N + ____
C+ H
a. n
c. He
b.
e
d.
e
____ 233. To what element does polonium-208 (atomic number 84) decay when it emits an alpha particle?
a.
c.
Pb
Pb
b.
Po
d.
Rn
____ 234. What is the approximate half-life of uranium-238?
a. hundreds of years
c. millions of years
b. thousands of years
d. billions of years
____ 235. Which of the following naturally occurring radioisotopes would be most useful in dating objects thought to be
millions of years old?
a. carbon-14; t
= 5.73 10 years
b. potassium-40; t
= 1.28 10 years
c. thorium-234; t
= 25 days
d. radon-222; t
= 3.8 days
____ 236. The production of carbon-14 ____.
a. takes place in the upper atmosphere
b. is mostly due to fallout from nuclear explosions
c. occurs to a large extent in nuclear reactors
d. is caused by photosynthesis in plants
____ 237. What happens in a chain reaction?
a. Products that start a new reaction are released.
b. Reactants that have two parts split.
c. Products that are radioactive are lost.
d. Radioactive reactants are deposited on control rods.
____ 238. Controlled nuclear chain reactions ____.
a. take place in nuclear reactors
b. are always fusion reactions
c. never produce radioactive by-products
d. are characteristic of atomic bombs
____ 239. Which type of coolant(s) usually is (are) used to remove heat from a nuclear reactor core?
a. water only
c. liquid sodium or water
b. liquid sodium only
d. CFCs
____ 240. Nuclear fusion ____.
a. takes place in the sun
c. can be controlled in the laboratory
b. occurs at low temperatures
d. is used in medicine
____ 241. What does neutron absorption accomplish in a nuclear reactor?
a. It slows down the reaction.
b. It speeds up the reaction.
c. It increases the rate of heat absorption.
d. It recycles the fuel.
____ 242. Control rods made of ____.
a. carbon
c. plutonium
b. liquid sodium
d. cadmium
____ 243. What substances are used as moderators in a nuclear reactor?
a. carbon and water
c. plutonium and neptunium
b. liquid sodium and water
d. cadmium or other metal
____ 244. Which of the following statements is correct?
a. Water is used to moderate (slow down) neutrons in a nuclear reactor.
b. Carbon control rods are used to absorb neutrons in a nuclear fission reaction.
c. A very high temperature is required to initiate a nuclear fission reaction.
d. The energy released from the sun is the result of a nuclear fission reaction.
____ 245. What type of radiation is best detected by a scintillation counter?
a. alpha radiation only
c. alpha and beta radiation only
b. gamma radiation only
d. all types of radiation
____ 246. What instrument is used routinely to check a person's exposure to radiation?
a. Geiger counter
c. film badge
b. scintillation counter
d. moderating rod
____ 247. What is the main detector of a Geiger counter?
a. ionizable gas in a metal tube
c. plates of ionizable plastic
b. phosphor-covered surface
d. potassium metal surface
____ 248. What is the main detector of a scintillation counter?
a. ionizable gas in a metal tube
c. plates of ionizable plastic
b. phosphor-covered surface
d. potassium metal surface
____ 249. Radiation therapy is used to ____.
a. study reaction mechanisms
c. treat cancer
b. detect elements
d. initiate neutron activation analysis
____ 250. Radioisotopes taken internally for medical reasons ____.
a. must be eliminated from the body slowly
b. should be fissionable isotopes
c. are usually deposited in fat tissue
d. should have a short half-life