PRACTICE CPCHEM FINAL
NAME__________________________
6/3/14
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question. Enter your
response on the scantron at the appropriate number
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1. Which of the following categories includes the majority of the elements?
a. metalloids
c. metals
b. liquids
d. nonmetals
2. Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a. Pt
c. Li
b. V
d. Kr
3. Which of the following elements is a transition metal?
a. cesium
c. tellurium
b. copper
d. tin
4. Which of the following groupings contains only representative elements?
a. Cu, Co, Cd
c. Al, Mg, Li
b. Ni, Fe, Zn
d. Hg, Cr, Ag
5. What are the Group 1A and Group 7A elements examples of?
a. representative elements
c. noble gases
b. transition elements
d. nonmetallic elements
6. How does atomic radius change from top to bottom in a group in the periodic table?
a. It tends to decrease.
c. It first increases, then decreases.
b. It tends to increase.
d. It first decreases, then increases.
7. What element in the second period has the largest atomic radius?
a. carbon
c. potassium
b. lithium
d. neon
8. What is the charge of a cation?
a. a positive charge
b. no charge
c. a negative charge
d. The charge depends on the size of the nucleus.
9. Which of the following statements is true about ions?
a. Cations form when an atom gains electrons.
b. Cations form when an atom loses electrons.
c. Anions form when an atom gains protons.
d. Anions form when an atom loses protons.
10. The metals in Groups 1A, 2A, and 3A ____.
a. gain electrons when they form ions c. all have ions with a 1 charge
b. all form ions with a negative charge d. lose electrons when they form ions
____ 11. In which of the following sets are the charges given correctly for all the ions?
a. Na , Mg , Al
b. K , Sr , O
c. Rb , Ba , P
d. N , O , F
____ 12. What is the element with the lowest electronegativity value?
a. cesium
c. calcium
b. helium
d. fluorine
____ 13. What is the element with the highest electronegativity value?
a. cesium
c. calcium
b. helium
d. fluorine
____ 14. Which of the following elements has the smallest ionic radius?
a. Li
c. O
b. K
d. S
____ 15. Which statement is true about electronegativity?
a. Electronegativity is the ability of an anion to attract another anion.
b. Electronegativity generally increases as you move from top to bottom within a
group.
c. Electronegativity generally is higher for metals than for nonmetals.
d. Electronegativity generally increases from left to right across a period.
____ 16. Which of the following statements correctly compares the relative size of an ion to its neutral
atom?
a. The radius of an anion is greater than the radius of its neutral atom.
b. The radius of an anion is identical to the radius of its neutral atom.
c. The radius of a cation is greater than the radius of its neutral atom.
d. The radius of a cation is identical to the radius of its neutral atom.
____ 17. How many valence electrons are in a silicon atom?
a. 2
c. 6
b. 4
d. 8
____ 18. What is the name given to the electrons in the highest occupied energy level of an atom?
a. orbital electrons
c. anions
b. valence electrons
d. cations
____ 19. How does calcium obey the octet rule when reacting to form compounds?
a. It gains electrons.
b. It gives up electrons.
c. It does not change its number of electrons.
d. Calcium does not obey the octet rule.
____ 20. Which of the following elements does NOT form an ion with a charge of 1 ?
a. fluorine
c. potassium
b. hydrogen
d. sodium
____ 21. How does oxygen obey the octet rule when reacting to form compounds?
a. It gains electrons.
b. It gives up electrons.
c. It does not change its number of electrons.
d. Oxygen does not obey the octet rule.
____ 22. Which of the following occurs in an ionic bond?
a. Oppositely charged ions attract.
b. Two atoms share two electrons.
c. Two atoms share more than two electrons.
d. Like-charged ions attract.
____ 23. Which of the following is true about an ionic compound?
a. It is a salt.
c. It is composed of anions and cations.
b. It is held together by ionic bonds.
d. all of the above
____ 24. What is the name of the ionic compound formed from lithium and bromine?
a. lithium bromine
c. lithium bromium
b. lithium bromide
d. lithium bromate
____ 25. What is the formula for sodium sulfate?
a. NaSO
c. Na(SO )
b. Na SO
d. Na (SO )
____ 26. Which of the following pairs of elements is most likely to form an ionic compound?
a. magnesium and fluorine
c. oxygen and chlorine
b. nitrogen and sulfur
d. sodium and aluminum
____ 27. Ionic compounds are normally in which physical state at room temperature?
a. solid
c. gas
b. liquid
d. plasma
____ 28. What is shown by the structural formula of a molecule or polyatomic ion?
a. the arrangement of bonded atoms
c. the number of inner shell electrons
b. the number of ionic bonds
d. the number of protons
____ 29. Which of these elements does not exist as a diatomic molecule?
a. Ne
c. H
b. F
d. I
____ 30. Why do atoms share electrons in covalent bonds?
a. to become ions and attract each other
b. to attain a noble-gas electron configuration
c. to become more polar
d. to increase their atomic numbers
____ 31. Which of the following elements can form diatomic molecules held together by triple covalent
bonds?
a. carbon
c. fluorine
b. oxygen
d. nitrogen
____ 32. Which noble gas has the same electron configuration as the oxygen in a water molecule?
a. helium
c. argon
b. neon
d. xenon
____ 33. Which elements can form diatomic molecules joined by a single covalent bond?
a. hydrogen only
b. halogens only
c. halogens and members of the oxygen group only
d. hydrogen and the halogens only
____ 34. Which of the following is the name given to the pairs of valence electrons that do not
participate in bonding in diatomic oxygen molecules?
a. unvalenced pair
c. inner pair
b. outer pair
d. nonbonding pair
____ 35. Which of the following diatomic molecules is joined by a double covalent bond?
a.
c.
b.
d.
____ 36. A molecule with a single covalent bond is ____.
a. CO
c. CO
b. Cl
d. N
____ 37. 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. inner shell electrons
d. the electrons closest to the nuclei
____ 38. What causes water molecules to have a bent shape, according to VSEPR theory?
a. repulsive forces between unshared pairs of electrons
b. interaction between inner shell electrons and unshared pairs of electrons
c. ionic attraction and repulsion
d. the unusual location of the free electrons
____ 39. What is the shape of a molecule with a triple bond?
a. tetrahedral
c. bent
b. pyramidal
d. linear
____ 40. Which of the following atoms forms the most polar covalent bond with hydrogen?
a. C
c. O
b. Na
d. S
____ 41. When Group 2A elements form ions, they ____.
a. lose two protons
c. lose two electrons
b. gain two protons
d. gain two electrons
____ 42. What is the correct name for the N ion?
a. nitrate ion
c. nitride ion
b. nitrogen ion
d. nitrite ion
____ 43. When naming a transition metal ion that can have more than one common ionic charge, the
numerical value of the charge is indicated by a ____.
a. prefix
c. Roman numeral following the name
b. suffix
d. superscript after the name
____ 44. Which of the following correctly provides the name of the element, the symbol for the ion, and
the name of the ion?
a. fluorine, F , fluoride ion
c. copper, Cu , cuprous ion
b. zinc, Zn , zincate ion
d. sulfur, S , sulfurous ion
____ 45. What determines that an element is a metal?
a. the magnitude of its charge
c. when it is a Group A element
b. the molecules that it forms
d. its position in the periodic table
____ 46. Which of the following is true about the composition of ionic compounds?
a. They are composed of anions and cations.
b. They are composed of anions only.
c. They are composed of cations only.
d. They are formed from two or more nonmetallic elements.
____ 47. Which element, when combined with fluorine, would most likely form an ionic compound?
a. lithium
c. phosphorus
b. carbon
d. chlorine
____ 48. Which of the following shows correctly an ion pair and the ionic compound the two ions form?
a. Sn , N ; Sn N
c. Cr , I ; CrI
b. Cu , O ; Cu O
d. Fe , O ; Fe O
____ 49. Which of the following compounds contains the lead(II) ion?
a. PbO
c. Pb2O
b. PbCl4
d. Pb2
____ 50. What type of compound is CuSO ?
a. monoatomic ionic
b. polyatomic covalent
c. polyatomic ionic
d. binary molecular
____ 51. Sulfur hexafluoride is an example of a ____.
a. monatomic ion
c. binary compound
b. polyatomic ion
d. ternary compound
____ 52. Molecular (covalent) compounds are usually ____.
a. composed of two or more transition elements
b. composed of positive and negative ions
c. composed of two or more nonmetallic elements
d. exceptions to the law of definite proportions
____ 53. Which of the following correctly shows a prefix used in naming binary molecular compounds
with its corresponding number?
a. deca-, 7
c. hexa-, 8
b. nona-, 9
d. octa-, 4
____ 54. Which of the following is a binary covalent compound?
a. BeHCO
c. AgI
b. PCl
d. MgS
____ 55. Select the correct formula for sulfur hexafluoride.
a. S F
c. F S
b. F SO
d. SF
____ 56. What is the correct name for the compound CoCl ?
a. cobalt(I) chlorate
c. cobalt(II) chlorate
b. cobalt(I) chloride
d. cobalt(II) chloride
____ 57. What SI unit is used to measure the number of representative particles in a substance?
a. kilogram
c. kelvin
b. ampere
d. mole
____ 58. How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C3H8O?
a. 8 (6.02 10 )
c. 40
b. 8
d. 40 (6.02 10 )
____ 59. Which of the following elements exists as a diatomic molecule?
a. neon
c. nitrogen
b. lithium
d. sulfur
____ 60. How many atoms are in 0.075 mol of titanium?
a. 1.2 10-25
c. 6.4 10
b. 2.2 10
d. 4.5 10
____ 61. How many molecules are in 2.10 mol CO ?
a. 2.53 10 molecules
c. 3.49 10 molecules
b. 3.79 10 molecules
d. 1.26 10 molecules
____ 62. How many atoms total are in one molecule of Prussian blue Fe7(CN)18
a. 25 b. 43 c. 9 d. 18
____ 63. What is the molar mass of AuCl3?
a. 96 g
c. 232.5 g
b. 130 g
d. 303.6 g
____ 64. What is the mass in grams of 5.90 mol C H ?
a. 0.0512 g
c. 389 g
b. 19.4 g
d. 673 g
____ 65. What is the number of moles of beryllium in 36 g of Be?
a. 0.25 mol
c. 45.0 mol
b. 4.0 mol
d. 320 mol
____ 66. Which one of the following diagrams is correct for the electron dot of N2?
a.
b.
c.
d.
____ 67. Which combination of temperature and pressure correctly describes standard temperature
and pressure, STP?
a. 0 C and 1.0 atm
c. 0 C and 22.4 atm
b. 1 C and 0 atm
d. 100 C and 100 atm
____ 68. What is the number of moles in 500 L of He gas at STP?
a. 0.05 mol
c. 22 mol
b. 0.2 mol
d. 90 mol
____ 69. The molar mass of a certain gas is 49 g. What is the density of the gas in g/L at STP?
a. 3.6 10
c. 2.2 g/L
g/L
b. 0.46 g/L
d. 71 g/L
____ 70. Which of the following gas samples would have the largest number of particles at STP?
a. 12.0 L He
c. 0.10 L Xe
b. 7.0 L O
d. 0.007 L SO
____ 71. Given 1.00 mole of each of the following gases at STP, which gas would have the greatest
volume?
a. He
c. SO
b. O
d. All would have the same volume.
____ 72. If 20.0 grams of Ca combines completely with 16.0 grams of S to form a compound, what is the
percent composition of Ca in the compound?
a. 1.25%
c. 44.4%
b. 20.0%
d. 55.6%
____ 73. What is the percent composition of carbon, in heptane, C H ?
a. 12%
c. 68%
b. 19%
d. 84%
____ 74. Which expression represents the percent by mass of nitrogen in NH4NO3?
a. 14 g N/80 g NH NO
c. 80 g NH NO /14 g N 100%
100%
b. 28 g N/80 g NH NO
d. 80 g NH NO /28 g N 100%
100%
____ 75. Which of the following compounds has the highest percent gold content by weight?
a. AuOH
c. AuCl
b. Au(OH)
d. AuI
____ 76. Chemical reactions ____.
a. occur only in living organisms
c. only occur outside living organisms
b. create and destroy atoms
d. produce new substances
____ 77. 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
____ 78. 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
____ 79. When the equation Fe Cl
FeCl is balanced, what is the coefficient for Cl ?
a. 1
c. 3
b. 2
d. 4
____ 80. 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.
____ 81. 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
____ 82. When the equation KClO (s)
KCl(s) + O (g) is balanced, the coefficient of KClO3 is ____.
a. 1
c. 3
b. 2
d. 4
____ 83. 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
____ 84. What are the correct formulas and coefficients for the products of the following doublereplacement reaction?
RbOH H PO
a. Rb(PO )
c. Rb PO
H O
3H O
b. RbPO
d. H Rb PO OH
2H O
____ 85. 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
____ 86. 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. SnCO
b. NaSn
d. CNO
____ 87. The reaction 2Fe 3Cl
2FeCl is an example of which type of reaction?
a. double displacement reaction
c. synthesis reaction
b. single-replacement reaction
d. decomposition reaction
____ 88. The equation Mg(s) 2HCl(aq)
MgCl (aq) H2(g) is an example of which type of
reaction?
a. synthesis reaction
b. single-replacement reaction
c. decomposition reaction
d. double-replacement reaction
____ 89. A double-replacement reaction takes place when aqueous cobalt (III) chloride reacts with
aqueous lithium hydroxide. The product of this reaction is ____.
a. Co(OH)
c. LiCo
b. Co(OH)
d. LiCl
____ 90. 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
2NaI
2NaBr
I
d. Br
NaI
NaBr
I
____ 91. What is conserved in the reaction shown below?
H (g) + Cl (g)  2HCl(g)
a. mass only
c. mass, moles, and molecules only
b. mass and moles only
d. mass, moles, molecules, and volume
____ 92. What is the net ionic equation for the following double replacement reaction?
CuCl2(aq) + H2S(g) → CuS(s) +
HCl(aq)
a. Cu+2 + S-2  CuS(s)
b. Cu+ + S-2  CuS(s)
c. H+ + Cl-  HCl(aq)
d. H- + Cl+  HCl(aq)
_ ___93. In any chemical reaction, the quantities that are preserved are ____.
a. the number of moles and the volumes
b. the number of molecules and the volumes
c. mass and number of atoms
d. mass and moles
____ 94. The first step in most stoichiometry problems is to ____.
a. add the coefficients of the reagents c. convert given quantities to volumes
b. convert given quantities to moles
d. convert given quantities to masses
____ 95. In the reaction 2CO(g) + O (g)  2CO (g), what is the ratio of moles of oxygen used to moles
of CO produced?
a. 1:1
c. 1:2
b. 2:1
d. 2:2
____ 96. Which of the following is true about the total number of reactants and the total number of
products in the reaction shown below?
C H (l) + 8O (g)  5CO (g) + 6H O(g)
a. 9 moles of reactants chemically change into 11 moles of product.
b. 9 grams of reactants chemically change into 11 grams of product.
c. 9 liters of reactants chemically change into 11 liters of product.
d. 9 atoms of reactants chemically change into 11 atoms of product.
____ 97. 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. 1.2 mol b. 0.8 mol
c. 1.6 mol
d. 2.4 mol
____ 98. Calculate the number of moles of Al O that are produced when 0.60 mol of Fe is produced in
the following reaction.
2Al(s) + 3FeO(s)
3Fe(s) + Al O (s)
a. 0.20 mol
c. 0.60 mol
b. 0.40 mol
d. 0.90 mol
____ 99. 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. 1.8 L
c. 2.0 L
b. 3.6 L
d. 2.4 L
100. Which one of the following is insoluble in water?
a. NH4CH3COO b. RbNO3 c. AgBr d. ZnCl2