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Chemistry Reference Table Review
1. According to Table N, which pair of isotopes spontaneously decays?
(1) C-12 and N-14
(2) C-12 and N-16
(3) C-14 and N-14
(4) C-14 and N-16
2. Which substance has the lowest vapor pressure at 75°C?
(1) water
(2) ethanoic acid
(3) propanone
(4) ethanol
3. In which shell are the valence electrons of the elements in Period 2 found?
(1) 1
(2) 2
(3) 3
(4) 4
4. Which halogen is a solid at STP?
(1) Br2
(2) F2
(3) Cl2
(4) I2
5. Which trends are observed when the elements in Period 3 on the Periodic Table are
considered in order of increasing atomic number?
(1) the atomic radius decreases, and the first ionization energy generally increases
(2) the atomic radius decreases, and the first ionization energy generally decreases
(3) the atomic radius increases, and the first ionization energy generally increases
(4) the atomic radius increases, and the first ionization energy generally decreases
6. Which of the following Group 15 elements has the greatest metallic character?
(1) nitrogen
(2) phosphorus
(3) antimony
(4) bismuth
7. What amount of heat is required to completely melt a 29.95 g sample of H2O (s) at 0°C?
(1) 334 J
(2) 2260 J
(3) 1.00 x 103 J
(4) 1.00 x 104 J
8. Which symbol represents a particle that has the same total number of electrons as S -2?
(1) O-2
(2) Si
(3) Se-2
(4) Ar
9. The percent by mass of calcium in the compound CaSO4 is approximately
(1) 15%
(2) 29%
(3) 34%
(4) 47%
10. A saturated solution of NaNO3 is prepared at 60°C using 100 grams of water. As this
solution is cooled to 10°C, NaNO3 precipitates (settles) out of the solution. The resulting
solution is saturated. Approximately how many grams of NaNO3 settled out?
(1) 46 g
(2) 61 g
(3) 85 g
(4) 126 g
11. 2,000 mL can be expressed as
(1) 20 dL
(2) 2 L
(3) 2 kL
(4) 20 kL
12. Which compound contains both ionic and covalent bonds?
(1) HCl (g)
(2) NaCl (s)
(3) NH4Cl (s)
(4) CCl4 (g)
13. Which metal is more active than Ni and less active than Zn?
(1) Cu
(2) Mg
(3) Cr
(4) Pb
14. In the reaction 239Np  239Pu + X, what does X represent?
(1) a neutron
(2) a proton
(3) an alpha particle
(4) a beta particle
15. According to Table S, which sequence correctly places the elements in order of
increasing ionization energy?
(1) H  Li  Na  K
(2) I  Br  Cl  F
(3) O  S  Se  Te
(4) H  Be  Al  Ga
16. As the temperature of a gas increases at constant pressure, the volume of the gas
(1) decreases
(2) increases
(3) remains the same
17. The half-life of 131I is 8.021 days. What fraction of a sample remains after 24.063 days?
(1) 1/2
(2) 1/4
(3) 1/8
(4) 1/16
18. The mass of an unknown solid is 10.04 g and the volume is 8.21 cm3. What is the
density to the correct significant figures?
(1) 1.2 g/cm3
(2) 1.22 g/cm3
(3) 1.222 g/cm3
(4) 0.82 g/cm3
19. Which change of phase is exothermic?
(1) solid to liquid
(2) gas to liquid
(3) solid to gas
(4) liquid to gas
20. According to Table F, which of these salts is least soluble in water?
(1) LiCl
(2) RbCl
(3) FeCl2
(4) PbCl2
21. Which two radioisotopes have the same decay mode?
(1) 37Ca & 53Fe
(2) 220Fr & 60Co
(3) 37K & 42K
(4) 99Tc & 19Ne
22. Under standard conditions, which metal will react with 0.1 M HCl to liberate H2 gas?
(1) Ag
(2) Au
(3) Cu
(4) Mg
23. What is the concentration of a solution in parts per million, if 0.089 grams of NaCl is
dissolved in 250 g of water?
(1) 0.03 ppm
(2) 0.27 ppm
(3) 35.6 ppm
(4) 356 ppm
24. The degree of polarity of a chemical bond in a molecule of a compound can be
predicted by determining the difference in the
(1) melting points of the elements in the compound
(2) densities of the elements in the compound
(3) electronegativities of the bonded atoms in a molecule of the compound
(4) atomic masses of the bonded atoms in a molecule of the compound
25. A student intended to make a salt solution with a concentration of 10.0 grams of solute
per liter of solution. When the student’s solution was analyzed, it was found to contain
8.90 grams of solute per liter of solution. What was the percent error?
(1) 1.10%
(2) 8.90%
(3) 11.0%
(4) 18.9%
26. Which element has atoms with the greatest attraction for electrons in a bond?
(1) beryllium
(2) fluorine
(3) lithium
(4) oxygen
27. Which electron configuration could represent a strontium atom in an excited state?
(1) 2-8-18-7-1
(2) 2-8-18-7-3
(3) 2-8-18-8-1
(4) 2-8-18-8-2
28. Which Celsius temperature is equal to 298 K?
(1) 25
(2) 273
(3) 298
(4) 571
29. Which type of radioactive emission has a positive charge and weak penetrating power?
(1) alpha particle
(2) beta particle
(3) gamma ray
(4) neutron
30. As the elements in Group 17 are considered in order of increasing atomic number, the
chemical reactivity of each successive element
(1) decreases
(2) increases
(3) remains the same
31. Which product of nuclear decay has mass but no charge?
(1) alpha particle
(2) neutron
(3) gamma ray
(4) positrons
32. What determines the order of placement of the elements on the modern Periodic Table?
(1) atomic number
(2) atomic mass
(3) the number of neutrons, only
(4) the number of neutrons and protons
33. Which compound when stirred in water will not pass through filter paper?
(1) NaCl
(2) (NH4)2S
(3) Mg(OH)2
(4) LiCl
34. The modern model of the atom shows that electrons are
(1) orbiting the nucleus in fixed paths
(2) found in regions called orbitals
(3) combined with neutrons in the nucleus
(4) located in a solid sphere
35. Which element is a liquid at room temperature (293 K)?
(1) Br
(2) Cd
(3) Ar
(4) K
36. Which metal reacts spontaneously with a solution containing zinc ions?
(1) strontium
(2) nickel
(3) copper
(4) silver
37. A 3.0 M HCl (aq) solution contains a total of
(1) 3.0 grams of HCl per liter of water
(2) 3.0 grams of HCl per mole of solution
(3) 3.0 moles of HCl per liter of solution
(4) 3.0 moles of HCl per mole of water
38. Which list consists of elements that have the most similar chemical properties?
(1) Mg, Al, Si
(2) Mg, Ca, Ba
(3) K, Al, Ni
(4) K, Ca, Ga
39. Which formula represents an ionic compound?
(1) NaCl
(2) N2O
(3) HCl
(4) H2O
40. How many moles are there in 222.3 grams of Ca(OH)2?
(1) 1.5 mol
(2) 3.0 mol
(3) 5.5 mol
(4) 22.3 mol
41. As the pressure of a given sample of a gas decreases at constant temperature, the
volume of the gas
(1) decreases
(2) increases
(3) remains the same
42. Which list of elements is arranged in order of increasing atomic radii?
(1) Li, Be, B, C
(2) Sr, Ca, Mg, Be
(3) Sc, Ti, V, Cr
(4) F, Cl, Br, I
43. The temperature of a sample of water changes from 10°C to 20°C when the water
absorbs 418 joules of heat. What is the mass of the sample?
(1) 1 g
(2) 10 g
(3) 100 g
(4) 1,000 g
44. According to Table H, what is the vapor pressure of propanone at 45°C?
(1) 22 kPa
(2) 33 kPa
(3) 70 kPa
(4) 98 kPa
45. The element in Period 4 and Group 1 of the Periodic Table would be classified as a
(1) metal
(2) metalloid
(3) nonmetal
(4) noble gas
46. Based on Table G, what is the maximum number of grams of KCl(s) that will dissolve
in 200 grams of water at 50°C to produce a saturated solution?
(1) 38 g
(2) 42 g
(3) 58 g
(4) 84 g
47. Which quantity is equivalent to 50 kilocalories?
(1) 5,000 cal
(2) 0.05 cal
(3) 5 x 103 cal
(4) 5 x 104 cal
48. Which of the following represents the nucleus of an atom of 27Al?
(1) 14 n, 27 p
(2) 14 n, 13 p
(3) 27 n, 13 p
(4) 40 n, 13 p
49. Which of these elements has an atom with the most stable outer electron configuration?
(1) Ne
(2) Cl
(3) Ca
(4) Na
50. Which element in Group 1 has the greatest tendency to lose an electron?
(1) cesium
(2) rubidium
(3) potassium
(4) sodium
51. How many electrons are contained in an Au+3 ion?
(1) 76
(2) 79
(3) 82
(4) 197
52. Which element has both metallic and nonmetallic properties?
(1) Rb
(2) Rn
(3) Si
(4) Sr
53. Which element is malleable and can conduct electricity in the solid phase?
(1) iodine
(2) phosphorus
(3) sulfur
(4) tin
54. Which changes occur as a cadmium atom, Cd, becomes a cadmium ion, Cd +2?
(1) the Cd atom gains two electrons and its radius decreases
(2) the Cd atom gains two electrons and its radius increases
(3) the Cd atom loses two electrons and its radius decreases
(4) the Cd atom loses two electrons and its radius increases
55. The atomic number of an atom is always equal to the number of its
(1) protons, only
(2) neutrons, only
(3) protons plus neutrons
(4) protons plus electrons
56. Which particle has the same electron configuration as a potassium ion?
(1) fluoride ion
(2) sodium ion
(3) neon atom
(4) argon atom
57. A sample of gas occupies a volume of 50.0 mL. The pressure of the sample is 0.90
atmosphere and the temperature is 298 K. What is the volume of the gas at STP?
(1) 41 mL
(2) 49 mL
(3) 51 mL
(4) 55 mL
58. What is the molarity of a solution containing 20 g of NaOH in 500 mL of solution?
(1) 1 M
(2) 2 M
(3) 0.04 M
(4) 0.5 M
59. Element X is a solid that is brittle, lacks luster, and has six valence electrons. In which
group on the Periodic Table would element X be found?
(1) 1
(2) 2
(3) 15
(4) 16
60. Which element has the greatest density at STP?
(1) calcium
(2) carbon
(3) chlorine
(4) copper
61. Which reaction is an example of a natural transmutation?
(1) 239Pu  235U + 4He
(2) 27Al + 4He  30P + 1n
(3) 238U + 1n  239Pu + 2 0e
(4) 239Pu + 1n  147Ba + 90Sr + 3 1n
62. What is the chemical formula for sodium sulfate?
(1) Na2SO3
(2) Na2SO4
(3) NaSO3
(4) NaSO4
63. Given the reaction: CH4 (g) + 2 O2 (g)  2 H2O () + CO2 (g) + heat, which statement is
true about energy in this reaction?
(1) the reaction is exothermic because it releases heat
(2) the reaction is exothermic because it absorbs heat
(3) the reaction is endothermic because it releases heat
(4) the reaction is endothermic because it absorbs heat
64. A student observed the following reaction:
NaCl (aq) + AgNO3 (aq)  NaNO3 (aq) + AgCl (s)
After the products were filtered, which substance remained on the filter paper?
(1) NaCl
(2) AgNO3
(3) NaNO3
(4) AgCl
65. What is the half-life and decay mode of Rn-222?
(1) 1.912 days and alpha decay
(2) 1.912 days and beta decay
(3) 3.823 days and alpha decay
(4) 3.823 days and beta decay
66. Which notation represents an atom of sodium with an atomic number of 11 and a mass
number of 24?
(1) 24Na
(2) 11Na
(3) 13Na
(4) 35Na
67. What is the structure of a krypton-85 atom?
(1) 49 electrons, 49 protons, and 85 neutrons (2) 49 electrons, 49 protons, and 49 neutrons
(3) 36 electrons, 36 protons, and 85 neutrons (4) 36 electrons, 36 protons, and 49 neutrons
68. Compared to the radius of a chlorine atom, the radius of a chloride ion is
(1) larger because Cl loses an electron
(2) larger because Cl gains an electron
(3) smaller because Cl loses an electron
(4) smaller because Cl gains an electron
69. What is the half-life of sodium-25 if 1.00 gram of a 16.00-gram sample of sodium-25
remains unchanged after 237 seconds?
(1) 47.4 s
(2) 59.3 s
(3) 79.0 s
(4) 118 s
70. How much energy is required to vaporize 10.00 grams of water at its boiling point?
(1) 100 J
(2) 260 J
(3) 2,260 J
(4) 22,600 J
71. Which element is an alkali metal?
(1) hydrogen
(2) calcium
(3) sodium
(4) zinc
72. During a flame test, ions of a specific metal are heated in the flame of a gas burner. A
characteristic color of light is emitted by these ions in the flame when the electrons
(1) gain energy as they return to lower energy levels
(2) gain energy as they move to higher energy levels
(3) emit energy as they return to lower energy levels
(4) emit energy as they move to higher energy levels
73. What is the mass of 5.2 moles of NO3?
(1) 62 g
(2) 322.4 g
(3) 11.9 g
(4) 161.2 g
74. Which of these particles has the greatest mass?
(1) alpha
(2) beta
(3) neutron
(4) positron
75. What is the total charge of the nucleus of a carbon atom?
(1) -6
(2) 0
(3) +6
(4) +12
76. Which pair of atoms is held together by a covalent bond?
(1) HCl
(2) LiCl
(3) NaCl
(4) KCl
77. Which two solutions, when mixed together, will undergo a double replacement
reaction and form a white, solid substance?
(1) NaCl (aq) and LiNO3 (aq)
(2) KCl (aq) and AgNO3 (aq)
(3) KCl (aq) and LiCl (aq)
(4) NaNO3 (aq) and AgNO3 (aq)
78. The number of moles in 24 grams of MgBr2 is
(1) 24/104 mole
(2) 24/184 mole
(3) 104/184 mole
(4) 184/24 mole
79. What is the boiling point of propanone if the pressure on its surface is 48 kilopascals?
(1) 25°C
(2) 30°C
(3) 35°C
(4) 40°C
80. Which substance is correctly paired with its type of bonding?
(1) NaBr – nonpolar covalent
(2) HCl – nonpolar covalent
(3) NH3 – polar covalent
(4) Br2 – polar covalent
81. During an experiment to determine the percent by mass of water in a hydrated crystal,
a student found the mass of the hydrated crystal to be 4.10 grams. After heating to
constant mass, the mass was 3.70 grams. What is the percent by mass of water?
(1) 90%
(2) 11%
(3) 9.8%
(4) 0.40%
82. The volume of a gas is 4.00 liters at 293 K and constant pressure. For the volume of the
gas to become 3.00 liters, the Kelvin temperature must be equal to
(1) 3.00 x 293 / 4.00
(2) 4.00 x 293 / 3.00
(3) 3.00 x 4.00 / 293
(4) 293 / 3.00 x 4.00
83. What are two properties of most nonmetals?
(1) high ionization energy and poor electrical conductivity
(2) high ionization energy and good electrical conductivity
(3) low ionization energy and poor electrical conductivity
(4) low ionization energy and good electrical conductivity
84. Based on Table G, a solution of NaNO3 that contains 120 grams of solute dissolved in
100 grams of H2O at 50°C is best described as
(1) saturated and dilute
(2) saturated and concentrated
(3) supersaturated and dilute
(4) supersaturated and concentrated
85. A student calculated the percent by mass of water in a sample of BaCl2 •2 H2O to be
16.4%, but the accepted value is 14.8%. What was the student’s percent error?
(1) 14.8/16.4 x 100
(2) 16.4/14.8 x 100 (3) 1.6/14.8 x 100
(4) 14.8/1.6 x 100
86. Atoms of the same element that have different numbers of neutrons are called
(1) ions
(2) allotropes
(3) isomers
(4) isotopes
87. The freezing point of bromine on the Kelvin temperature scale is
(1) 332
(2) 266
(3) 490
(4) 958
88. Which of these formulas contains the most polar bond?
(1) HBr
(2) HCl
(3) HF
(4) HI
89. What is the total number of moles of solute in 250 mL of a 1.0 M solution of NaCl?
(1) 1.0 mole
(2) 0.25 mole
(3) 0.50 mole
(4) 42 moles
90. Which formula represents a nonpolar molecule containing polar covalent bonds?
(1) H2O
(2) CCl4
(3) NH3
(4) H2
91. Which equation represents a fusion reaction?
(1) 2H + 2 H  4He
(2) 14C  0e + 14N
(3) 238U + 4He  241Pu + 1n
(4) 1n + 27Al  24Na + 4He
92. Which Kelvin temperature is equal to 56˚C?
(1) – 329 K
(2) – 217 K
(3) 217 K
93. Which formula represents lead (II) phosphate?
(1) PbPO4
(2) Pb4PO4
(3) Pb3(PO4)2
(4) 329 K
(4) Pb2(PO4)3
94. As the temperature of a liquid increases, its vapor pressure
(1) decreases
(2) increases
(3) remains the same
95. Under which conditions does a real gas behave most like an ideal gas?
(1) at low temperatures and high pressures (2) at low temperatures and low pressures
(3) at high temperatures and high pressures (4) at high temperatures and low pressures
96. At STP, an element that is a brittle solid and a poor conductor of heat and electricity
could have an atomic number of
(1) 12
(2) 13
(3) 16
(4) 17
97. A sample of helium gas has a volume of 900 mL and a pressure of 2.50 atm at 298 K.
What is the new pressure when the temperature is changed to 336 K and the volume is
decreased to 450 mL?
(1) 0.177 atm
(2) 4.43 atm
(3) 5.64 atm
(4) 14.1 atm
98. Which equation represents the radioactive decay of 226Ra?
(1) 226Ra  222Rn + 4He
(2) 226Ra  222Ac + 0e
(3) 226Ra  222Fr + 0e
(4) 226Ra  225Ra + 1n
99. The average kinetic energy of water molecules increases when
(1) H2O (s) changes to H2O() at 0˚C
(2) H2O () changes to H2O(s) at 0˚C
(3) H2O () at 10˚C changes to H2O() at 20˚C
(4) H2O () at 20˚C changes to H2O() at 10˚C
100. The average kinetic energy of water molecules is greatest in which of these samples?
(1) 10 g of water at 35°C
(2) 10 g of water at 55°C
(3) 100 g of water at 25°C
(4) 100 g of water at 45°C