QUESTION BANK FOR FINALS
1. Written in scientific notation, the measurement 0.000 065 cm is
a. 6. 5 x 10-4 cm.
b. 6. 5 x 10-5 cm.
c. 6. 5 x 10-6 cm
d. 6. 5 x 104 cm.
2. The law that states that mass cannot be created or destroyed in ordinary chemical and physical changes is known as the law of
a. conservation of mass. b. mass action. c. multiple proportions. d. definite composition.
3. The observation that the mass of carbon dioxide formed from the reaction of carbon and oxygen equals the combined masses of the carbon and oxygen that reacted supports the law of
a. conservation of mass. b. mass action. c. multiple proportions. d. definite composition.
4. Which of the following descriptions is not a characteristic of the nucleus of an atom?
a. positively charged b. contains uncharged particles
c. accounts for most of the atom’s volume d. accounts for most of the atom’s mass
5. A neutral atom of 14Si29
a. has an atomic number of 29. b. contains a total of 43 electrons, protons, and neutrons.
c. contains 15 protons and 14 neutrons. d. Both (a) and (c)
6. According to the Bohr model of the atom, which particles are allowed to exist in any one of a number of energy levels.
a. electrons b. protons c. neutrons d. Both (b) and (c)
7. The line-emission spectrum of an atom is caused by the energies released when electrons
a. jump from a lower energy level to a higher energy level.
b. jump from a higher energy level to a lower energy level.
c. jump from the ground state to an excited state.
d. None of the above
8. The electron configuration of 27Al13 is
a. 1s22s22p63s13d2. b. 1s22s22p53s23p2. c. [Ne] 3s23p1. d. [Ne] 3s13p13d1.
9. The atomic mass unit is used to express
a. atomic mass. b. atomic mass number. c. atomic number. d. molar mass.
10. The unit g/mol is the unit of
a. atomic mass. b. molar mass. c. atomic mass number. d. atomic number.
11. The number of atoms in a mole of any element is called
a. its atomic number. b. Avogadro’s number. c. the molar mass number.
d. the gram-atomic number.
12. If samples of two different elements each represent one mole,
a. they are equal in mass. b. they contain the same number of atoms.
c. their molar masses are equal. d. they have the same atomic mass.
13. Using a periodic table, find the identity of the element that has an atomic mass of 40.078 amu.
a. C b. Ca c. Cr d. Cu
14. How many silver atoms are in 1.00 mol Ag?
a. 6.02 x 1023 b. 1.00 x 1023 c. 1.22 x 1026 d. 1.22 x 1028
15. An electron that is found in the outermost shell of an atom and determines the atom’s chemical properties is called a(n)
a. valence electron. b. paired electron. c. p electron. d. octave electron.
16. The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic
a. masses. b. numbers. c. radii. d. structures.
17. Refer to a periodic table. In which period is calcium?
a. Period 2 b. Period 4 c. Period 6 d. Period 8
18. Refer to a periodic table. In which group is calcium?
a. Group 1 b. Group 2 c. Group 17 d. Group 18
19. An element that has the electron configuration [Ne]3s23p5 is in which period?
a. Period 2 b. Period 3 c. Period 5 d. Period 7
20. An element that has the electron configuration [Ne]3s23p5 is in which group?
a. Group 2 b. Group 5 c. Group 7 d. Group 17
21. Elements in the s- or p-blocks of the periodic table are called
a. alloys. b. main-group elements. c. metals. d. transition metals.
22. Nonmetallic elements in Group 17 that react with metals to form salts are
a. alkali-metals. b. halogens. c. lanthanides. d. noble gases.
23. A metal is expected to be a(n)
a. nonconductor. b. insulator. c. conductor. d. fluid at room temperature.
24. Ionization energy is the energy required to remove from an atom of an element.
a. the electron cloud b. all electrons c. one electron d. an ion
25. An octet is equal to
a. 2. b. 4. c. 5. d. 8.
26. How many valence electrons does the element with the electron configuration 1s22s22p63s23s64s1 have?
a. 0 b. 1 c. 9 d. 19
27. Which of the following situations will cause the element with the electron configuration 1s22s22p5 to have an octet configuration?
a. loss of one electron b. gain of one electron c. loss of two electrons
d. gain of three electrons
28. Which of the following situations will cause the element with the electron configuration 1s22s22p63s2 to have an octet configuration?
a. loss of one electron b. gain of one electron c. loss of two electrons
d. gain of three electrons
29. The elements of Group are able to satisfy the octet rule without forming compounds.
a. 1 b. 2 c. 17 d. 18
30. An element with the electron configuration 1s22s22p63s23p5 will ionize to a(n)
a. anion. b. cation. c. noble gas. d. Both (a) and (b)
31. An ion and its parent atom differ in
a. electron configuration. b. number of electrons. c. chemical reactivity. d. All of the above
32. Compounds that have the same number of positive and negative charges are said to be
a. cationic. b. anionic. c. electrically neutral. d. isoelectronic.
33. An ion of bromine with a single negative charge has the symbol and the name
a. Br+, bromide ion. b. Br-, bromide ion. c. Br+, bromium ion. d. Br-, bromium ion.
34. Sodium hydrogen carbonate, NaHCO3
a. contains four different ions. b. contains a polyatomic cation. c. is not a salt.
d. contains only a monatomic cation and a polyatomic anion.
35. What is the formula for the compound formed by aluminum, Al3+ , and the sulfate ion, SO42- _?
a. AlSO4 b. Al3SO4 c. Al2(SO4)3 d. Al(SO4)3
36. A single covalent bond involves the sharing of
a. only one electron. b. two electrons. c. three electrons.
d. a variable number of electrons, which depends on the bonding atoms.
37. The electrons involved in the formation of a covalent bond are
a. transferred from one atom to another. b. found only in the s-orbitals.
c. valence electrons. d. in filled orbitals.
38. As the atomic masses of the elements in the periodic table increase, the number of atoms in 1 mol of each element
a. decreases. b. increases. c. remains the same. d. becomes a negative number.
39. Avogadro’s number is
a. 6.022 x 1023. b. 1.602 x1024 . c. 3.14159. d. 3.0 x108.
40. How many atoms are in two moles of mercury?
a. 1.204 x 1022
b. 1.204 x 1023
c. 6.022 x 1023
d. 1.204 x 1024
41. How many moles of hydrogen are in one mole of C2H6?
a. 2 mol H b. 4 mol H c. 6 mol H d. 8 mol H
42. The molar mass of manganese, Mn, is
a. 25 amu. b. 25 g/mol. c. 54.94 amu. d. 54.94 g/mol.
43. The formation of a gas is evidence of
a. a chemical change. b. a physical change. c. no change in energy.
d. Both (a) and (c).
44. Which of the following may be evidence of a chemical change?
a. release of energy as heat b. production of sound c. reduction in temperature
d. All of the above
45. In the unbalanced formula equation
carbon _hydrogen à methane, the formula CH4 represents
a. one atom of methane. b. five atoms of methane. c. one molecule of methane.
d. one gram of methane
46. In the unbalanced formula equation ?H2 + _?S + _?O2 à ?H2SO4,
how many substances are reactants?
a. two b. three c. four d. unknown
47. From a complete and correctly written chemical equation, you can obtain the
a. chemical formulas of the reactants and products.
b. relative amounts of the reactants and products.
c. physical states of the reactants and products.
d. All of the above
48. In a chemical equation, the formula of a substance in water solution is followed by the symbol
a. (l). b. (s). c. (g). d. (aq).
49. Refer to the following unbalanced formula equation. KBr + _Cl2 à Br2 + _KCl
How many substances are shown in the equation?
a. 2 b. 3 c. 4 d. 8
50. Which statement is true for the balanced formula equation?
a. The coefficients are the same for each substance.
b. There are more reactant elements than product elements.
c. The number of atoms of an element that makes up the reactants is
equal to the number of atoms of that element that makes up the
products.
d. Not enough information is given to balance the equation.
51. According to the law of conservation of mass, the total mass of the reacting substances is
a. always more than the total mass of the products.
b. always less than the total mass of the products.
c. sometimes more and sometimes less than the total mass of the
products.
d. always equal to the total mass of the products.
52. A synthesis reaction is the only type of chemical reaction that
a. has only one reactant. b. can involve the oxidation of organic compounds.
c. results in the formation of a single product. d. Both (b) and (c)
53. Which of the following equations represents a decomposition reaction?
a. 2Sb(s) + 3I2(g) à2SbI3(s) b. 2HgO(s) à 2Hg(l) + O2(g)
c. FeS(s) + 2HCl(aq) àH2S(g) + FeCl2(aq) d. Zn(s) + H2SO4(aq) à ZnSO4(aq) + H2(g)
54. The reaction 2C2H2(g) + 5O2(g) à 4CO2(g) + 2H2O(l) is a
a. combustion reaction. b. synthesis reaction. c. decomposition reaction.
d. double-displacement reaction.
55. The reaction Mg(s) + 2HCl(aq) à H2(g) + MgCl2(aq) is a
a. synthesis reaction. b. decomposition reaction.
c. displacement reaction. d. double-displacement reaction.
56. In the reaction, Zn(s) + H2SO4(aq) à ZnSO4(aq) + H2(g), what element has been displaced?
a. Zn b. H c. S d. O
57. The chemical equation P4O10 + 6H2O à 4H3PO4 can be correctly interpreted as
a. 1 molecule of P4O10 + 6 molecules of H2O form 4 molecules of H3PO4.
b. 1 mol P4O10 + 6 mol H2O reacts to form 4 mol H3PO4.
c. 1 g P4O10 + 6 g H2O produces 4 g H3PO4.
d. Both (a) and (b)
58. Stoichiometry is the branch of chemistry that deals with the between elements and compounds as reactants and products in a chemical reaction.
a. bonding b. energy transfers c. numerical relationship d. physical interactions
59. In the chemical reaction described by the equation , 4Fe(s) + 3O2(g) à 2Fe2O3(s), the mole ratio of iron(III) oxide to iron is
a. 1:1. b. 1:2. c. 2:3. d. 4:1.
60. If, in the reaction A + B à C + D, the quantity of B is insufficient to react with all of A,
a. A is the limiting reactant. b. B is the limiting reactant. c. Both (a) and (b)
d. Neither (a) nor (b)
61. Energy is measured in units of
a. joules. b. kelvins. c. pounds. d. All of the above
62. A sample of matter whose particles are close together and cannot move past each other is
a. a solid. b. a liquid. c. a gas. d. viscous.
63. Fluids are materials that will flow from one place to another. Which of the following is a fluid?
a. solid b. liquid c. gas d. Both (b) and (c)
64. If particles have little attraction for each other and can freely move throughout the container, the particles are part of a
a. solid. b. liquid. c. gas. d. None of the above
65. A liquid becomes a gas during
a. evaporation. b. condensation. c. sublimation. d. deposition.
66. All changes of state are
a. physical changes. b. chemical changes. c. evaporation. d. endothermic.
67. Which of the following processes might occur when an object is heated?
a. condensation b. melting c. deposition d. freezing
68. Much of the volume occupied by a gas is empty space. This explains which characteristic of gases?
a. limited compressibility b. low density c. fixed volume d. ability to dissolve into a liquid
69. What causes a gas to exert pressure?
a. collisions b. density c. temperature d. elevation
70. The SI unit for measuring pressure is
a. newton. b. mm Hg. c. pascal. d. liter.
71. At sea level, the average height of mercury in a barometer is
a. 760 mm. b. 101 325 atmosphere. c. 1.01 325 Pa. d. All of the above
72. The kinetic-molecular theory considers collisions between gas particles to be
a. predictable. b. slow. c. elastic. d. inelastic.
73. Millimeters of mercury (mm Hg) is a measurement of
a. length. b. temperature. c. pressure. d. distance.
78. A pressure of 760.0 mm Hg is equal to .
a. 1.000 atm b. 10.00 atm c. 100.0 atm d. 7.600 atm
79. A pressure of 20 torr is equal to
a. 133.322 Pa. b. 20 Pa. c. 20 mm Hg. d. 1 mm Hg.
80. Which is not a measurable property of gases?
a. odor b. pressure c. temperature d. volume
81. For a fixed amount of gas at a constant temperature, the volume increases as the pressure
a. remains steady. b. increases. c. decreases. d. fluctuates.
82. The direct relationship between temperature and volume is known as
a. Kelvin’s law. b. Charles’s law. c. Boyle’s law. d. Avogadro’s law.
83. Gay-Lussac’s law shows a direct relationship between temperature and
a. volume. b. composition. c. density. d. pressure.
84. The ideal gas law states the relationship between
a. pressure, volume, temperature, the gas constant, and number of moles.
b. pressure, volume, and temperature only.
c. the gas constant and pressure only.
d. the gas constant and volume only.
85. You are measuring the speeds of two particles at the same conditions. The more massive particle will move
a. at a slower speed. b. at a quicker speed.
c. at the same speed as the less massive particle. d. at a changing speed.
86. All organic compounds contain
a. hydrogen. b. water. c. carbon. d. oxygen.
87. Isomers are compounds that have
a. the same molecular formula but different structures.
b. the same molecular formula and the same structure.
c. different molecular formulas and different structures.
d. different molecular formulas but the same structure.
88. An atom or group of atoms responsible for the specific properties of an organic compound is a(n)
a. isomer. b. hydrocarbon. c. substituted hydrocarbon. d. functional group.
89. To what class does an organic compound belong with the formula C3H7OH?
a. alcohols b. alkyl halides c. ethers d. aldehydes
90. In the figure BELOW, what is the structural formula for propyne?
a. A
b. B
c. C
d. none
91. What is the name for the simplest two-carbon alcohol?
a. ethanol b. ethanol c. 2-propanol d. 2-propanal
92. What is the name for the one-carbon alcohol?
a. ethanol b. ethanol c. methanol d. methanol
93 The formula CH3CH2CH2CH2CH=CH2 represents an
a. alkane. b. alkyne. c. alcohol. d. alkene.
1. Written in scientific notation, the measurement 0.000 065 cm is
a. 6. 5 x 10-4 cm.
b. 6. 5 x 10-5 cm.
c. 6. 5 x 10-6 cm
d. 6. 5 x 104 cm.
2. The law that states that mass cannot be created or destroyed in ordinary chemical and physical changes is known as the law of
a. conservation of mass. b. mass action. c. multiple proportions. d. definite composition.
3. The observation that the mass of carbon dioxide formed from the reaction of carbon and oxygen equals the combined masses of the carbon and oxygen that reacted supports the law of
a. conservation of mass. b. mass action. c. multiple proportions. d. definite composition.
4. Which of the following descriptions is not a characteristic of the nucleus of an atom?
a. positively charged b. contains uncharged particles
c. accounts for most of the atom’s volume d. accounts for most of the atom’s mass
5. A neutral atom of 14Si29
a. has an atomic number of 29. b. contains a total of 43 electrons, protons, and neutrons.
c. contains 15 protons and 14 neutrons. d. Both (a) and (c)
6. According to the Bohr model of the atom, which particles are allowed to exist in any one of a number of energy levels.
a. electrons b. protons c. neutrons d. Both (b) and (c)
7. The line-emission spectrum of an atom is caused by the energies released when electrons
a. jump from a lower energy level to a higher energy level.
b. jump from a higher energy level to a lower energy level.
c. jump from the ground state to an excited state.
d. None of the above
8. The electron configuration of 27Al13 is
a. 1s22s22p63s13d2. b. 1s22s22p53s23p2. c. [Ne] 3s23p1. d. [Ne] 3s13p13d1.
9. The atomic mass unit is used to express
a. atomic mass. b. atomic mass number. c. atomic number. d. molar mass.
10. The unit g/mol is the unit of
a. atomic mass. b. molar mass. c. atomic mass number. d. atomic number.
11. The number of atoms in a mole of any element is called
a. its atomic number. b. Avogadro’s number. c. the molar mass number.
d. the gram-atomic number.
12. If samples of two different elements each represent one mole,
a. they are equal in mass. b. they contain the same number of atoms.
c. their molar masses are equal. d. they have the same atomic mass.
13. Using a periodic table, find the identity of the element that has an atomic mass of 40.078 amu.
a. C b. Ca c. Cr d. Cu
14. How many silver atoms are in 1.00 mol Ag?
a. 6.02 x 1023 b. 1.00 x 1023 c. 1.22 x 1026 d. 1.22 x 1028
15. An electron that is found in the outermost shell of an atom and determines the atom’s chemical properties is called a(n)
a. valence electron. b. paired electron. c. p electron. d. octave electron.
16. The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic
a. masses. b. numbers. c. radii. d. structures.
17. Refer to a periodic table. In which period is calcium?
a. Period 2 b. Period 4 c. Period 6 d. Period 8
18. Refer to a periodic table. In which group is calcium?
a. Group 1 b. Group 2 c. Group 17 d. Group 18
19. An element that has the electron configuration [Ne]3s23p5 is in which period?
a. Period 2 b. Period 3 c. Period 5 d. Period 7
20. An element that has the electron configuration [Ne]3s23p5 is in which group?
a. Group 2 b. Group 5 c. Group 7 d. Group 17
21. Elements in the s- or p-blocks of the periodic table are called
a. alloys. b. main-group elements. c. metals. d. transition metals.
22. Nonmetallic elements in Group 17 that react with metals to form salts are
a. alkali-metals. b. halogens. c. lanthanides. d. noble gases.
23. A metal is expected to be a(n)
a. nonconductor. b. insulator. c. conductor. d. fluid at room temperature.
24. Ionization energy is the energy required to remove from an atom of an element.
a. the electron cloud b. all electrons c. one electron d. an ion
25. An octet is equal to
a. 2. b. 4. c. 5. d. 8.
26. How many valence electrons does the element with the electron configuration 1s22s22p63s23s64s1 have?
a. 0 b. 1 c. 9 d. 19
27. Which of the following situations will cause the element with the electron configuration 1s22s22p5 to have an octet configuration?
a. loss of one electron b. gain of one electron c. loss of two electrons
d. gain of three electrons
28. Which of the following situations will cause the element with the electron configuration 1s22s22p63s2 to have an octet configuration?
a. loss of one electron b. gain of one electron c. loss of two electrons
d. gain of three electrons
29. The elements of Group are able to satisfy the octet rule without forming compounds.
a. 1 b. 2 c. 17 d. 18
30. An element with the electron configuration 1s22s22p63s23p5 will ionize to a(n)
a. anion. b. cation. c. noble gas. d. Both (a) and (b)
31. An ion and its parent atom differ in
a. electron configuration. b. number of electrons. c. chemical reactivity. d. All of the above
32. Compounds that have the same number of positive and negative charges are said to be
a. cationic. b. anionic. c. electrically neutral. d. isoelectronic.
33. An ion of bromine with a single negative charge has the symbol and the name
a. Br+, bromide ion. b. Br-, bromide ion. c. Br+, bromium ion. d. Br-, bromium ion.
34. Sodium hydrogen carbonate, NaHCO3
a. contains four different ions. b. contains a polyatomic cation. c. is not a salt.
d. contains only a monatomic cation and a polyatomic anion.
35. What is the formula for the compound formed by aluminum, Al3+ , and the sulfate ion, SO42- _?
a. AlSO4 b. Al3SO4 c. Al2(SO4)3 d. Al(SO4)3
36. A single covalent bond involves the sharing of
a. only one electron. b. two electrons. c. three electrons.
d. a variable number of electrons, which depends on the bonding atoms.
37. The electrons involved in the formation of a covalent bond are
a. transferred from one atom to another. b. found only in the s-orbitals.
c. valence electrons. d. in filled orbitals.
38. As the atomic masses of the elements in the periodic table increase, the number of atoms in 1 mol of each element
a. decreases. b. increases. c. remains the same. d. becomes a negative number.
39. Avogadro’s number is
a. 6.022 x 1023. b. 1.602 x1024 . c. 3.14159. d. 3.0 x108.
40. How many atoms are in two moles of mercury?
a. 1.204 x 1022
b. 1.204 x 1023
c. 6.022 x 1023
d. 1.204 x 1024
41. How many moles of hydrogen are in one mole of C2H6?
a. 2 mol H b. 4 mol H c. 6 mol H d. 8 mol H
42. The molar mass of manganese, Mn, is
a. 25 amu. b. 25 g/mol. c. 54.94 amu. d. 54.94 g/mol.
43. The formation of a gas is evidence of
a. a chemical change. b. a physical change. c. no change in energy.
d. Both (a) and (c).
44. Which of the following may be evidence of a chemical change?
a. release of energy as heat b. production of sound c. reduction in temperature
d. All of the above
45. In the unbalanced formula equation
carbon _hydrogen à methane, the formula CH4 represents
a. one atom of methane. b. five atoms of methane. c. one molecule of methane.
d. one gram of methane
46. In the unbalanced formula equation ?H2 + _?S + _?O2 à ?H2SO4,
how many substances are reactants?
a. two b. three c. four d. unknown
47. From a complete and correctly written chemical equation, you can obtain the
a. chemical formulas of the reactants and products.
b. relative amounts of the reactants and products.
c. physical states of the reactants and products.
d. All of the above
48. In a chemical equation, the formula of a substance in water solution is followed by the symbol
a. (l). b. (s). c. (g). d. (aq).
49. Refer to the following unbalanced formula equation. KBr + _Cl2 à Br2 + _KCl
How many substances are shown in the equation?
a. 2 b. 3 c. 4 d. 8
50. Which statement is true for the balanced formula equation?
a. The coefficients are the same for each substance.
b. There are more reactant elements than product elements.
c. The number of atoms of an element that makes up the reactants is
equal to the number of atoms of that element that makes up the
products.
d. Not enough information is given to balance the equation.
51. According to the law of conservation of mass, the total mass of the reacting substances is
a. always more than the total mass of the products.
b. always less than the total mass of the products.
c. sometimes more and sometimes less than the total mass of the
products.
d. always equal to the total mass of the products.
52. A synthesis reaction is the only type of chemical reaction that
a. has only one reactant. b. can involve the oxidation of organic compounds.
c. results in the formation of a single product. d. Both (b) and (c)
53. Which of the following equations represents a decomposition reaction?
a. 2Sb(s) + 3I2(g) à2SbI3(s) b. 2HgO(s) à 2Hg(l) + O2(g)
c. FeS(s) + 2HCl(aq) àH2S(g) + FeCl2(aq) d. Zn(s) + H2SO4(aq) à ZnSO4(aq) + H2(g)
54. The reaction 2C2H2(g) + 5O2(g) à 4CO2(g) + 2H2O(l) is a
a. combustion reaction. b. synthesis reaction. c. decomposition reaction.
d. double-displacement reaction.
55. The reaction Mg(s) + 2HCl(aq) à H2(g) + MgCl2(aq) is a
a. synthesis reaction. b. decomposition reaction.
c. displacement reaction. d. double-displacement reaction.
56. In the reaction, Zn(s) + H2SO4(aq) à ZnSO4(aq) + H2(g), what element has been displaced?
a. Zn b. H c. S d. O
57. The chemical equation P4O10 + 6H2O à 4H3PO4 can be correctly interpreted as
a. 1 molecule of P4O10 + 6 molecules of H2O form 4 molecules of H3PO4.
b. 1 mol P4O10 + 6 mol H2O reacts to form 4 mol H3PO4.
c. 1 g P4O10 + 6 g H2O produces 4 g H3PO4.
d. Both (a) and (b)
58. Stoichiometry is the branch of chemistry that deals with the between elements and compounds as reactants and products in a chemical reaction.
a. bonding b. energy transfers c. numerical relationship d. physical interactions
59. In the chemical reaction described by the equation , 4Fe(s) + 3O2(g) à 2Fe2O3(s), the mole ratio of iron(III) oxide to iron is
a. 1:1. b. 1:2. c. 2:3. d. 4:1.
60. If, in the reaction A + B à C + D, the quantity of B is insufficient to react with all of A,
a. A is the limiting reactant. b. B is the limiting reactant. c. Both (a) and (b)
d. Neither (a) nor (b)
61. Energy is measured in units of
a. joules. b. kelvins. c. pounds. d. All of the above
62. A sample of matter whose particles are close together and cannot move past each other is
a. a solid. b. a liquid. c. a gas. d. viscous.
63. Fluids are materials that will flow from one place to another. Which of the following is a fluid?
a. solid b. liquid c. gas d. Both (b) and (c)
64. If particles have little attraction for each other and can freely move throughout the container, the particles are part of a
a. solid. b. liquid. c. gas. d. None of the above
65. A liquid becomes a gas during
a. evaporation. b. condensation. c. sublimation. d. deposition.
66. All changes of state are
a. physical changes. b. chemical changes. c. evaporation. d. endothermic.
67. Which of the following processes might occur when an object is heated?
a. condensation b. melting c. deposition d. freezing
68. Much of the volume occupied by a gas is empty space. This explains which characteristic of gases?
a. limited compressibility b. low density c. fixed volume d. ability to dissolve into a liquid
69. What causes a gas to exert pressure?
a. collisions b. density c. temperature d. elevation
70. The SI unit for measuring pressure is
a. newton. b. mm Hg. c. pascal. d. liter.
71. At sea level, the average height of mercury in a barometer is
a. 760 mm. b. 101 325 atmosphere. c. 1.01 325 Pa. d. All of the above
72. The kinetic-molecular theory considers collisions between gas particles to be
a. predictable. b. slow. c. elastic. d. inelastic.
73. Millimeters of mercury (mm Hg) is a measurement of
a. length. b. temperature. c. pressure. d. distance.
78. A pressure of 760.0 mm Hg is equal to .
a. 1.000 atm b. 10.00 atm c. 100.0 atm d. 7.600 atm
79. A pressure of 20 torr is equal to
a. 133.322 Pa. b. 20 Pa. c. 20 mm Hg. d. 1 mm Hg.
80. Which is not a measurable property of gases?
a. odor b. pressure c. temperature d. volume
81. For a fixed amount of gas at a constant temperature, the volume increases as the pressure
a. remains steady. b. increases. c. decreases. d. fluctuates.
82. The direct relationship between temperature and volume is known as
a. Kelvin’s law. b. Charles’s law. c. Boyle’s law. d. Avogadro’s law.
83. Gay-Lussac’s law shows a direct relationship between temperature and
a. volume. b. composition. c. density. d. pressure.
84. The ideal gas law states the relationship between
a. pressure, volume, temperature, the gas constant, and number of moles.
b. pressure, volume, and temperature only.
c. the gas constant and pressure only.
d. the gas constant and volume only.
85. You are measuring the speeds of two particles at the same conditions. The more massive particle will move
a. at a slower speed. b. at a quicker speed.
c. at the same speed as the less massive particle. d. at a changing speed.
86. All organic compounds contain
a. hydrogen. b. water. c. carbon. d. oxygen.
87. Isomers are compounds that have
a. the same molecular formula but different structures.
b. the same molecular formula and the same structure.
c. different molecular formulas and different structures.
d. different molecular formulas but the same structure.
88. An atom or group of atoms responsible for the specific properties of an organic compound is a(n)
a. isomer. b. hydrocarbon. c. substituted hydrocarbon. d. functional group.
89. To what class does an organic compound belong with the formula C3H7OH?
a. alcohols b. alkyl halides c. ethers d. aldehydes
90. In the figure BELOW, what is the structural formula for propyne?
a. A
b. B
c. C
d. none
91. What is the name for the simplest two-carbon alcohol?
a. ethanol b. ethanol c. 2-propanol d. 2-propanal
92. What is the name for the one-carbon alcohol?
a. ethanol b. ethanol c. methanol d. methanol
93 The formula CH3CH2CH2CH2CH=CH2 represents an
a. alkane. b. alkyne. c. alcohol. d. alkene.