Chemistry: The Central Science, 12e (Brown et al.)
Chapter 22 Chemistry of the Nonmetals
22.1 Multiple–Choice
1) How many oxygen atoms are bonded to each silicon atom in SiO2?
A) 1
B) 2
C) 3
D) 4
E) none
2) Of the following, the most nonmetallic element is __________.
A) carbon
B) selenium
C) iodine
D) fluorine
E) phosphorus
3) The least electronegative of the elements below is __________.
A) I
B) Cl
C) H
D) F
E) Br
4) In the following chemical equation
Na3P + 3H2O →
the products (when the equation is balanced) are
A) H2PO3 + 3NaH
B) NaOH + 3PH
C) 3NaH + POH3
D) 3NaO + PH6
E) 3NaOH + PH3
5) Of the atoms below, __________ is the most effective in forming π bonds.
A) C
B) P
C) N
D) Si
E) Ge
6) Which one of the following is false concerning tritium?
A) It is radioactive, emitting alpha particles with a half-life of 12.3 yr.
B) It can be produced by neutron bombardment of lithium-6.
C) It is formed continuously in the upper atmosphere.
D) It has the same chemical properties as protium but reacts more slowly.
E) The atomic number of tritium is 1.
7) What method is used to produce the most hydrogen gas in the United States?
A) electrolysis of water
B) reaction of zinc with acid
C) reaction of methane with steam
D) reaction of coke (carbon) with steam
E) reaction of metallic sodium with water
8) Water gas is ________.
A) H2O and H2
B) CO2 and O2
C) H2O and CO2
D) H2O and CO
E) H2 and CO
9) What is the primary commercial use of hydrogen in the United States?
A) as a rocket fuel, especially on the space shuttle
B) hydrogenation of vegetable oils
C) manufacture of methanol
D) manufacture of ammonia by the Haber process
E) as an automobile fuel
10) Which of the following is a molecular hydride?
A) CaH2
B) TiH2
C) NaH
D) SrH2
E) CH4
11) Of the following, which is an ionic hydride?
A) BaH2
B) LiH
C) CaH2
D) SrH2
E) all of the above
12) Which compound would produce an acidic aqueous solution?
A) KH
B) CaH2
C) H2S
D) NH3
E) H2O
13) Which compound would produce a basic aqueous solution?
A) MgH2
B) H2S
C) HCl
D) HI
E) CH3OH
14) Isotopes of hydrogen
A) have the same atomic number and different mass numbers.
B) have the same atomic number and the same mass number.
C) have different atomic numbers and different mass numbers.
D) have different atomic numbers and the same mass number.
E) are exactly alike.
15) Which of the following would produce a basic solution?
A) CO and CO2
B) Na2O and MgO
C) Na2O, MgO, and BeH2
D) BeH2 only
E) CO, CO2, and BeH2
16) Which of the following would produce an acidic solution?
A) Na2O and MgO
B) Na2O, MgO, and BeH2
C) CO2 only
D) BeH2 only
E) CO, CO2, and BeH2
17) How are the oxygen-containing compounds of xenon made?
A) by direct combination of the elements
B) by reaction of xenon with peroxide
C) by thermal decomposition of the xenon hydroxide
D) by reaction of the corresponding xenon fluoride with water
E) Xenon is inert and does not form compounds with oxygen.
18) Of the following compounds, which is the most stable?
A) XeF6
B) XeOF4
C) XeO3
D) XeO2F2
E) XeF2
19) What is the F Xe F bond angle in XeF2?
A) 90°
B) 109°
C) 180°
D) 120°
E) 60°
20) Consider the following xenon compounds:
(i) XeF2 (ii) XeF4 (iii) XeO4 (iv) XeOF4 (v) XeO3
Which of the compounds is(are) polar?
A) (i) only
B) (ii) and (iii)
C) (iv) only
D) (iii) and (iv)
E) (iv) and (v)
21) The heavier noble gases are more reactive than the lighter ones because
A) the lighter noble gases exist as diatomic molecules.
B) the lighter noble gases have complete octets.
C) the heavier noble gases are more abundant.
D) the heavier noble gases have low ionization energies relative to the lighter ones.
E) the heavier noble gases have greater electron affinities.
22) Which noble gas is known to form a variety of binary compounds?
A) Xe
B) He
C) Ne
D) Ar
E) Kr
23) The oxidation number of xenon in XeO2F2 is ________.
A) +2
B) +4
C) +6
D) +8
E) +10
24) Interhalogen compounds __________.
A) are exceedingly reactive
B) contain halogens in both positive and negative oxidation states
C) are powerful oxidizing agents
D) that contain fluorine are very active fluorinating agents
E) all of the above
25) Which elemental halogen(s) can be used to prepare I2 from NaI?
A) F2only
B) Cl2 only
C) Br2 only
D) both Cl2 and Br2, but not F2
E) F2, Cl2, and Br2
26) Which halogen is the most easily oxidized?
A) F
B) Cl
C) Br
D) I
27) Which equation correctly represents the reaction between elemental fluorine and sodium iodide?
A) F + NaI → I + NaF
B) F– + NaI → I– + NaF
C) F2 + 2NaI → I2 + 2NaF
D) F + NaI → 1/2I2 + NaF
E) F2 + NaI → NaF2 + I–
28) Which equation correctly represents the reaction between silica and hydrofluoric acid?
A) SiCl4 + 4HF → SiF4 + 4HCl
B) SiO2 + 6HF → H2SiF6 + 2H2O
C) SiCl2 + 2HF → SiF2 + 2HCl
D) SiH4 + 4HF → SiF4 + 4H2
E) none of the above
29) The interhalogen compound ICl3 can form but BrCl3 cannot form. This is because
A) iodine is large enough to accommodate three chlorine atoms around itself
B) bromine is not electronegative enough to react with chlorine.
C) bromine is too electronegative to react with chlorine.
D) iodine can have a positive oxidation state but bromine cannot.
E) iodine can have a negative oxidation state but bromine cannot.
30) Chlorine can have a positive oxidation state
A) if it combines with bromine or iodine.
B) if it combines with oxygen or fluorine.
C) if it combines with hydrogen.
D) if it combines with an alkali metal.
E) in its elemental form.
31) The oxidation state of fluorine in its compounds is
A) positive unless it combines with another halogen.
B) negative unless it combines with another halogen.
C) negative unless it combines with oxygen.
D) negative unless it combines with an active metal.
E) always negative.
32) The most stable allotrope of oxygen is __________.
A) H2O
B) O3
C) O2
D) HClO
E) O
33) Which of the following react with oxygen to form superoxides?
A) Ca
B) Na
C) K
D) Sr
E) Ba
34) Nearly all commercial oxygen is obtained __________.
A) from air
B) by electrolysis of water
C) by thermal decomposition of potassium chlorate
D) by thermal cracking of petroleum
E) as a byproduct of the preparation of aluminum in the Hall process
35) Which of the following statements is false?
A) Ozone is a better reducing agent than O2 (g).
B) Ozone is produced by passing electricity through dry O2 (g).
C) Ozone oxidizes all of the common metals except gold and platinum.
D) Ozone decomposes to O2 and O.
E) Ozone is an allotrope of oxygen.
36) Which one of the following compounds is peroxide?
A) Li2O
B) H2O
C) Na2O2
D) CsO2
E) both Na2O2 and CsO2
37) A disproportionation reaction is one in which
A) a single element is both oxidized and reduced.
B) a compound is separated into its constituent elements.
C) the ratio of combination of two elements in a compound changes.
D) aqueous ions combine to form an insoluble salt.
E) an insoluble salt separates into ions.
38) The oxidation state of oxygen in O2F2 is
A) 0
B) +2
C) +1
D) -1
E) -2
39) The oxidation state of oxygen in OF2 is
A) +1
B) +2
C) 0
D) -1
E) -2
40) Metal oxides are typically __________ while nonmetal oxides are typically __________.
A) basic, amphoteric
B) basic, acidic
C) amphoteric, basic
D) acidic, basic
E) amphoteric, acidic
41) Amphoteric oxides are also known as __________.
A) basic oxides
B) basic anhydrides
C) acidic oxides
D) acidic anhydrides
E) none of the above
42) Which element in group 6A is not found as the central atom in compounds with an expanded
valence shell?
A) oxygen
B) selenium
C) tellurium
D) polonium
E) sulfur
43) Which group 6A element is not commonly found in a positive oxidation state?
A) sulfur
B) selenium
C) oxygen
D) tellurium
E) polonium
44) What sulfur compound is used to sterilize wine?
A) H2SO4
B) H2S
C) Na2SO3
D) SO2
E) Na2S
45) What is the major commercial source of elemental sulfur?
A) sulfide minerals
B) sulfate minerals
C) underground deposits of elemental sulfur
D) seawater
E) coal and petroleum
46) Which form of elemental sulfur is the most stable at room temperature?
A) rhombic sulfur
B) monoclinic
C) hexagonal
D) triclinic
E) tetraclinic
47) The molecular shape of the SF6 molecule is __________.
A) tetrahedral
B) trigonal bipyramidal
C) octahedral
D) trigonal pyramidal
E) T-shaped
48) The prefix thio- denotes
A) replacement of an oxygen atom by a sulfur atom.
B) a sulfur sulfur double bond.
C) sulfur in a negative oxidation state.
D) a sulfur oxygen double bond.
E) an allotropic form of sulfur.
49) The oxidation numbers of sulfur in the sulfate ion, sulfite ion, sulfur trioxide, and hydrogen sulfide
are __________, __________, __________, and __________, respectively.
A) +4, -2, +4, +6
B) +6, +2, +4, +6
C) +6, +4, +6, -2
D) +4, +6, +4, -2
E) -2, +6, -2, 0
50) Which one of the following is sodium thiosulfate?
A) Na2SO4
B) Na2SO3
C) Na2S2O3
D) Na2S4O6
E) Na2S
51) Which one of the following is false concerning pure hydrazine?
A) It is an oily, colorless liquid.
B) It can be made by reaction of hypochlorite and ammonia.
C) It is used as a rocket fuel.
D) Hydrazine is quite poisonous.
E) It is a clear, red liquid that is highly viscous.
52) The careful, thermal decomposition of solid ammonium nitrate will yield __________.
A) N2O
B) NO
C) NO2
D) N2O3
E) N2O5
53) The oxidation number of N in NO2 is __________.
A) +1
B) +2
C) +3
D) +4
E) +5
54) The oxidation number of N in HNO3 is __________.
A) +1
B) +2
C) +3
D) +4
E) +5
55) The oxidation number of N in HNO2 is __________.
A) +1
B) +2
C) +3
D) +4
E) +5
56) The oxidation number of As in HAsO4-2 is __________.
A) +1
B) +2
C) +3
D) +4
E) +5
57) The oxidation number of As in H2AsO3– is __________.
A) +1
B) +2
C) +3
D) +4
E) +5
58) The oxidation number of B in NaBH4 is __________.
A) +1
B) +2
C) +3
D) +4
E) +5
59) Which of the following is the nitride ion?
A) N3-
B) N3–
C) NO3–
D) NO2–
E) N–
60) Which of the following equations correctly represents the combustion of hydrazine?
A) N2H4 (l) + O2 (g) → NH3 (g) + HNO2 (g)
B) N2H4 (l) + 2O2 (g) → 2NO2 (g) + 2H2 (g)
C) N2H4 (l) + O2 (g) → 2H2NO (g)
D) N2H4 (l) + O2 (g) → N2 (g) + 2H2O (g)
E) N2H4 (l) + O2 (g) → N2 (g) + 2H2 (g) + O2 (g)
61) Which pair of formula/name is incorrect?
A) NO / nitric oxide
B) N2O / nitrous oxide
C) NO2 / nitrogen dioxide
D) N2O4 / dinitrogen trioxide
E) N2O5 / dinitrogen pentoxide
62) The oxidation numbers of nitrogen in the nitride ion, hydrazine, ammonium cation, and nitrate ion
are __________, __________, __________, and __________, respectively.
A) -3, -2, -3, +5
B) +3, -2, -3, +5
C) +3, -2, +1, +3
D) -3, +2, +1, +5
E) -3, +2, -3, +3
63) Which equation correctly represents what happens when NO2 dissolves in water?
A) NO2 (g) + H2O (l) → 2H+ (aq) + NO3– (aq)
B) 3NO2 (g) + H2O (l) → 2H+ (aq) + 2NO3– (aq) + NO (g)
C) NO2 (g) + H2O (l) → H2O2 (aq) + NO (g)
D) 2NO2 (g) + H2O (l) → 2H+ (aq) + NO42- (aq) + NO (g)
E) 2NO2 (g) + 2H2O (l) → 2 HNO2 (aq) + O2 (g) + H2 (g)
64) The reaction between nitrogen dioxide and water is a
A) decomposition
B) combustion
C) disproportionation
D) neutralization
E) replacement
65) Of the following substances, __________ is both a very strong acid and a powerful oxidizing agent.
A) HNO3
B) H2SO4
C) HCl
D) H3PO4
E) HF
66) In the reaction of phosphorus with chlorine to form a phosphorus chloride, whether PCl3 or PCl5
forms depends on
A) which allotropic form of phosphorus is used.
B) the amount of chlorine present.
C) whether the reaction is carried out in the gas phase or in solution.
D) whether the chlorine used is molecular or atomic.
E) the amount of moisture present.
67) What are the products of the reaction of PF3 (g) and water?
A) phosphorous acid and hydrofluoric acid
B) elemental phosphorus and hydrofluoric acid
C) phosphoric acid and fluorine gas
D) elemental phosphorus and fluorine gas
E) phosphoric acid and phosphorous acid
68) What are the products of the reaction of PCl5 (g) and water?
A) phosphoric acid and phosphorous acid
B) elemental phosphorus and hydrochloric acid
C) phosphoric acid and chlorine gas
D) elemental phosphorus and chlorine gas
E) phosphoric acid and hydrochloric acid
69) Which one of the following is false concerning buckminsterfullerene?
A) It is the most recently discovered crystalline allotrope of carbon.
B) It consists of individual molecules like C60 and C70.
C) It is a molecular form of carbon.
D) It is made up of Cl2 molecules.
E) It is made up of molecules that resemble soccer balls.
70) Of the following, which is most likely to form interstitial carbides?
A) active metals
B) transition metals
C) boron and silicon
D) alkaline earth metals
E) alkali metals
71) Which of the following would produce the most strongly acidic aqueous solution?
A) HCO3–
B) CO
C) CO2
D) CO32-
E) CaCO3
72) How many pairs of unpaired electrons are there in one molecule of carbon monoxide?
A) 0
B) 1
C) 2
D) 3
E) 4
73) What gas has the odor of bitter almonds?
A) H2S
B) NO2
C) CO
D) HCN
E) Cl2
74) Which of the following is not an allotropic form of carbon?
A) graphite
B) diamond
C) carbide
D) buckminsterfullerene
E) All of the above are allotropic forms of carbon.
75) A carbonyl compound contains
A) a carbon-oxygen double bond
B) a carbon-oxygen triple bond
C) a carbon atom with a lone pair of electrons
D) a carbon-carbon triple bond
E) a carbon-carbon double bond
76) Carbon dioxide is produced
A) in blast furnaces when metal oxides are reduced with CO.
B) by combustion of carbon-containing substances in an excess of oxygen.
C) when carbonates are heated.
D) by fermentation of sugar during the production of ethanol.
E) by all of the above processes.
77) Which of the following would produce the most strongly basic aqueous solution?
A) CO
B) CO32-
C) CO2
D) HCO3–
E) NaHCO3
78) Which equation correctly represents the reaction between carbon dioxide and water?
A) CO2 (aq) + H2O (l) → H2CO3 (aq)
B) CO2 (aq) + H2O (l) → H2 (g) + CO (g) + O2 (g)
C) CO2 (aq) + H2O (l) → H2O2 (aq) + CO (g)
D) CO2 (aq) + 2H2O (l) → CH4 (g) + 2O2 (aq)
E) CO2 (aq) + H2O (l) → H2CO (aq) + O2 (g)
79) What is the function of the carbon fibers in a composite?
A) to provide a structure to help the epoxy resin solidify in the desired shape
B) to transmit loads evenly in all directions
C) to provide resistance to oxidation
D) to provide ultraviolet protection
E) to “spread out” the epoxy so that it remains more flexible
80) The arrangement of oxygen atoms around a silicon atom in SiO44- is
A) square planar
B) octahedral
C) linear
D) tetrahedral
E) trigonal pyramidal
81) Addition of B2O3 to soda-lime glass
A) imparts a greater ability to withstand temperature change.
B) imparts a deep blue color.
C) results in a denser glass with a higher refractive index.
D) results in a glass with a lower melting point.
E) results in opaque glass.
82) Replacement of Na2O by K2O in soda-lime glass results in
A) opaque glass.
B) a softer glass with a lower melting point.
C) glass with a deep blue color.
D) denser glass with a high refractive index.
E) a harder glass with a higher melting point.
83) Replacement of CaO by PbO in soda-lime glass results in
A) denser glass with a higher refractive index.
B) glass with a deep blue color.
C) opaque glass.
D) a softer glass with a lower melting point.
E) a harder glass with a higher melting point.
84) Soda-lime glass contains
A) SiO2 and aluminum
B) SiO2, CaO, and Na2O
C) SiO2, CO2, and citric acid
D) SiO2, CO2, Na2O
E) pure SiO2