Chemistry, 7e (McMurry/Fay)
Chapter 22 The Main-Group Elements
22.1 Multiple-Choice Questions
1) As one traverses the periodic table from left to right, the effective nuclear charge Zeff increases. As a
result of this the periodic properties of
A) atomic size increases, IE increases, EA increases and electronegativity increases.
B) atomic size decreases, IE increases, EA increases and electronegativity increases.
C) atomic size decreases, IE decreases, EA increases and electronegativity increases.
D) atomic size decreases, IE increases, EA decreases and electronegativity increases.
2) Metallic character for the main group elements generally
A) increases from left to right across a period and increases down a group.
B) increases from left to right across a period and decreases down a group.
C) decreases from left to right across a period and increases down a group.
D) decreases from left to right across a period and decreases down a group.
3) Among the main-group elements the number of semimetals is
A) five.
B) six.
C) seven.
D) eight.
4) Ionization energy of main-group elements generally
A) increases from left to right across a period and increases down a group.
B) increases from left to right across a period and decreases down a group.
C) decreases from left to right across a period and increases down a group.
D) decreases from left to right across a period and decreases down a group.
5) Electronegativity of main-group elements generally
A) increases from left to right across a period and increases down a group.
B) increases from left to right across a period and decreases down a group.
C) decreases from left to right across a period and increases down a group.
D) decreases from left to right across a period and decreases down a group.
6) Atomic radius of main-group elements generally
A) increases from left to right across a period and increases down a group.
B) increases from left to right across a period and decreases down a group.
C) decreases from left to right across a period and increases down a group.
D) decreases from left to right across a period and decreases down a group.
7) Which of the following statements are true about elements with metallic character?
A) Elements with a low ionization energy are more likely to be nonmetallic.
B) Elements with a high electronegativity are more likely to be metallic.
C) Elements with a high electronegativity and low ionization energy are more likely to be metallic.
D) Elements with a low electronegativity, low ionization energy, and malleability are more likely to be
metallic.
8) In general, metallic character
A) increases down a column because the orbitals become more compact.
B) decreases down a column because the orbitals become more compact.
C) increases across a row because the effective nuclear charge increases.
D) increases down a column because the orbitals become more diffuse.
9) Identify a Group 2A element with the smallest radius.
A) Na
B) Ca
C) Sr
D) F
10) Second row elements differ from heavier elements in all of the following ways except
A) atoms of second row elements are smaller.
B) atoms of second row elements have higher electronegativities.
C) heavier elements commonly form multiple bonds while second row elements cannot.
D) heavier elements have electrons in d orbitals while second row elements do not.
11) What is not a true statement?
A) BeO is amphoteric but the oxides of the other group 2A elements are basic.
B) B differs from other elements of group 3A by forming mainly covalent molecular compounds.
C) BF3 is a gaseous molecular halide but AlF3 is a high melting ionic solid.
D) Compounds with C=C double bonds and Si=Si double bonds are quite common.
12) Which of the following are properties not typically associated with second row elements?
A) Ability to form multiple bonds easily.
B) Ability to form good π bond overlap.
C) Ability to form covalent networks.
D) Small sizes of atoms.
13) Hydrogen, H2, has a very low boiling point. What is the force that must be overcome in order to boil
hydrogen?
A) dipole-dipole
B) H—H covalent bonding
C) hydrogen bonding
D) London dispersion
14) What is the Lewis electron dot structure for the hydride ion?
A) H+
B) H: –
C) H ∙
D) H3O+
15) The net ionic reaction of solid CaH2 with water is
A) CaH2(s) + 2 H2O(l) → Ca(OH)2(aq) + 2 H2(g).
B) CaH2(s) + 2 H2O(l) → Ca2+(aq) + 2 OH–(aq) + 2 H2(g).
C) H–(aq) + H2O(l) → OH–(aq) + H2(g).
D) CaH2(s) + H2O(l) → CaO(s) + 2 H2(g).
16) Covalent hydrides of the type MH3 are likely to form with elements of what group?
A) 3A
B) 4A
C) 5A
D) 6A
17) Which is not a chemical reaction of the alkali metal sodium?
A) 4 Na(s) + 2 O2(g) → 2 Na2O(s) + Na2O2(s)
B) 2 Na(s) + 2 NH3(l) → 2 NaNH2(sol) + H2(g)
C) 2 Na(s) + Cl2(g) → 2 NaCl(s)
D) 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g)
18) Which is not a chemical reaction of the alkali metal potassium?
A) K(s) + O2(g) → KO2(s)
B) 2 K(s) + 2 H2O(l) → 2 KOH(aq) + H2(g)
C) 2 K(s) + H2(g) → 2 KH(s)
D) 6 K(s) + N2(g) → 2 K3N(s)
19) Which alkali metal reacts with nitrogen to form a nitride?
A) Li
B) Na
C) K
D) All of these
20) The alkali metals Li and Na are commercially produced by
A) chemical reduction of their molten salts.
B) electrolysis of their molten salts.
C) thermal decomposition of their molten metal halides.
D) thermal decomposition of their molten metal oxides.
21) The alkali metals K, Rb, and Cs are commercially produced by
A) chemical reduction of their molten salts.
B) electrolysis of their molten salts.
C) thermal decomposition of their molten metal halides.
D) thermal decomposition of their molten metal oxides.
22) An incorrect statement about the alkaline earth metals is
A) Melting points generally decrease as one descends the group.
B) Densities are less than those of the corresponding alkali elements of the same period.
C) Ionic radii of the M2+ ion increases as one descends the group.
D) The first ionization energy is less than that of the second ionization energy.
23) Which is not generally considered to be a chemical reaction of the alkaline earth metal calcium?
A) Ca(s) + Cl2(g) → CaCl2(s)
B) 2 Ca(s) + 2 H2O(l) → 2 Ca(OH)2(aq) + H2(g)
C) 6 Ca(s) + 2 N2(g) → 2 Ca3N2(s)
D) Ca(s) + O2(g) → CaO2(s)
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24) Which is not generally considered to be a chemical reaction of the alkaline earth metal magnesium?
A) 2 Mg(g) + O2(g) → 2 MgO(s) at room temperature
B) 3 Mg(s) + N2(g) → Mg3N2(s) at elevated temperatures
C) Mg(s) + 2 H2O(l) → Mg(OH)2(s) + H2(g) at room temperature
D) Mg(s) + F2(g) → MgF2(s) at room temperature
25) Group 2A metals tend to be somewhat less reactive than alkali metals, and the order of their reactivity
is
A) Ba > Sr > Ca > Mg > Be.
B) Be > Mg > Ca > Sr > Ba.
C) Ca > Mg > Be > Ba > Sr.
D) Sr > Ca > Mg > Be > Ba.
26) Calcium, strontium, and barium are all prepared commercially by the same method which is
A) electrolysis of the molten metal oxides.
B) electrolysis of the molten metal halides.
C) chemical reduction of the metal oxides with aluminium.
D) chemical reduction of the metal halides with oxygen.
27) Which of the group 3A elements is the only one to readily form a +1 ion?
A) B
B) Al
C) In
D) Tl
28) What are the common oxidation states of the Group 3A elements Al and Tl?
A) both are +3
B) +3 for Al and +1 for Tl
C) +3 for Al and both +1 and +3 for Tl
D) +3 for Al and +1, +3, and -5 for Tl
29) Of the following elements, which has a melting point slightly above room temperature?
A) B
B) Ga
C) In
D) Tl
30) Which group 3A element has the largest liquid range of any known element?
A) Al
B) Ga
C) In
D) Tl
31) One of the group 3A elements is extremely toxic due to the similarities in chemistry of one of its ions
to alkali metal chemistry. Which element is it?
A) B
B) Ga
C) In
D) Tl
32) The first ionization energy of gallium is greater than that of aluminum and the first ionization energy
of thallium is greater than that of indium. A possible explanation for this is
A) This is the normal trend in ionization energy.
B) Both Ga and Tl prefer to lose three electrons rather than one.
C) Both Ga and Tl follow transition elements which are excellent shielders of nuclear charge.
D) Ga follows a series of transition elements and Tl follows both a series of transition elements and inner
transition elements which are poor shielders of nuclear charge.
33) Which M3+ ion of group 3A elements is the easiest to reduce?
A) B
B) Al
C) Ga
D) In
34) The strongest reducing agent in the group 3A is
A) B.
B) Al.
C) Ga.
D) Tl.
35) What is not an appropriate method for the isolation of elemental boron?
A) refluxing borax with sodium peroxide
B) high temperature reduction of B2O3 with magnesium
C) high temperature reduction of BBr3 with hydrogen over a Ta wire
D) electrolytic reduction of aqueous B(OH)3
36) Which one of the following compounds contains a three–center, two electron (3c-2e) bond?
A) B2H6
B) C2H4
C) N2H4
D) H2O2
37) Which compound contains hydrogen atoms that form two types of bonds?
A) B2H6
B) C2H2
C) C6H6
D) N2H4
38) Compared to the terminal B–H bonds the bridging H–B bonds in B2H6 are
A) longer and stronger.
B) longer and weaker.
C) shorter and stronger.
D) shorter and weaker.
39) What is the hybridization of boron in diborane B2H6?
A) sp
B) sp2
C) sp3
D) None of these
40) Some commercial drain cleaners contain aluminum chips and sodium hydroxide pellets. When water
is added to this mixture a vigorous reaction takes place which is best represented as
A) 2 Al(s) + 6 H+(aq) → 2 Al3+(aq) + 3 H2(g).
B) 2 Al(s) + 2 OH–(aq) + 6 H2O(l) → 2 Al(OH)4–(aq) + 3 H2(g).
C) 2 Al(s) + 6 H2O(l) → 2 Al(OH)3 + 3 H2(g).
D) 2 Al(s) + 3 Cu2+(aq) → 2 Al3+(aq) + 2 Cu(s).
41) What is the ground state valence shell electron configuration of a group 4A element?
A) ns0 np4
B) ns1 np3
C) ns2 np2
D) ns2 np4
42) Which element of group 4A has the highest melting point?
A) C
B) Si
C) Sn
D) Pb
43) Which element of group 4A has the greatest density?
A) C
B) Ge
C) Sn
D) Pb
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44) Which element of group 4A has the greatest electronegativity?
A) C
B) Si
C) Ge
D) Sn
45) Which statement is not consistent with the chemistry of group 4A elements?
A) Elements have the outer valence electron configuration of ns2np2.
B) The most common oxidation state for the elements of the group is +4.
C) The +4 oxidation state compounds are ionic and the +2 oxidation state compounds are covalent.
D) The +2 oxidation state for lead is the most stable.
46) What statement is not consistent with the chemistry of tin?
A) It is abstracted from the mineral cassiterite by reduction of the oxide with carbon.
B) It is an important component of alloys such as bronze, pewter, and some solders.
C) It is a relatively abundant ore within the earth’s crust.
D) It is used as a protective coating over steel in making tin cans.
47) What is the structure of the “gray” allotropic form of tin that is used as a semiconductor?
A) body centered
B) diamond-like
C) graphite-like
D) simple cubic
48) What statement is not consistent with the chemistry of lead?
A) It has the highest density of the group 4A elements.
B) It is commonly used as a fuel additive in gasoline to boost the octane rating.
C) It is obtained from its ore galena (PbS) by roasting in air and then by reduction with carbon monoxide.
D) It is used in making pipes, cables, paint pigments and electrodes for storage batteries.
49) White tin is the high temperature form of the metal. Given that the density of gray tin is 5.769 g/cm3
and that of white tin is 7.28 g/cm3 raising the pressure will favor the
A) more dense allotrope and lower the transition temperature of 13.2°C.
B) more dense allotrope and raise the transition temperature of 13.2°C.
C) less dense allotrope and lower the transition temperature of 13.2°C.
D) less dense allotrope and raise the transition temperature of 13.2°C.
50) What element was one of the “holes” in Mendeleev‘s periodic table?
A) Si
B) Ge
C) Sn
D) Pb
51) What is the molecular structure of germanium that is used in semiconductors?
A) body centered
B) diamond-like
C) graphite-like
D) simple cubic
52) Which allotrope of carbon has the atoms arranged in a spherical array?
A) coke
B) diamond
C) fullerene
D) graphite
53) Carbon is the ________ most abundant element by mass in living organisms.
A) first
B) second
C) third
D) fourth
54) What statement is inconsistent about diamond?
A) A covalent network structure in which each C atom uses sp3 hybrid orbitals.
B) A tetrahedral array of σ bonds with bond lengths of 154 pm.
C) The hardest known substance with the highest melting point for an element.
D) When an electrical potential is applied diamond becomes a valuable semiconductor.
55) What statement is inconsistent about graphite?
A) Carbon sheets are separated by a distance of 335 pm and are held together by weak London dispersion
forces.
B) Electrical conductivity parallel to the planar sheets is 1020 times greater than the conductivity of
diamond.
C) Pi electrons are delocalized and free to move perpendicular to the plane of the hexagonal sheets.
D) A two-dimensional sheetlike structure in which each C atom uses sp2 hybrid orbitals.
56) Electrical conductivity in graphite is maximized
A) parallel to the pi framework and parallel to the planar C atom framework.
B) perpendicular to the pi framework and parallel to the planar C atom framework.
C) parallel to the pi framework and perpendicular to the planar C atom framework.
D) perpendicular to the pi framework and perpendicular to the planar C atom framework.
57) What statement is inconsistent about fullerene?
A) It is an allotrope of carbon and the C60 form has soccer ball shape.
B) The C60 form of fullerene is a good oxidizing agent.
C) The C60 fullerene is a molecular substance.
D) The C60 form of fullerene is soluble in nonpolar organic solvents.
58) Which one of the following is the best electrical conductor?
A) C (diamond)
B) C (graphite)
C) P4
D) S8
59) What statement is inconsistent about carbon monoxide?
A) It is a colorless, odorless and toxic gas.
B) It is formed by burning carbon or hydrocarbon in excess oxygen.
C) One of its main industrial uses is in the synthesis of methanol, CH3OH.
D) Toxicity of CO results from its ability to bond strongly to iron(II) atom in hemoglobin.
60) What is not a reaction commonly associated with carbon dioxide?
A) Oxyhemoglobin + CO2 ⇌ Carboxyhemoglobin + O2
B) C6H12O6(aq) + 6 O2(g) ⇌ 6 CO2(g) + 6 H2O(l)
C) CaCO3(s) + heat → CaO(s) + CO2(g)
D) CO2(g) + H2O(l) ⇌ H+(aq) + HCO3–(aq)
61) What is not a reaction commonly associated with cyanide ion?
A) H+(aq) + CN–(aq) → HCN(aq)
B) Ag+(aq) + CN–(aq) → AgCN(s)
C) 4 Au(s) + 8 CN–(aq) + O2(g) + 2 H2O(l) → 4 Au(CN)2–(aq) + 4 OH–(aq)
D) CN–(aq) + H2(g) → HCN(aq) + H–(aq)
62) Which one of the following is a pseudohalide?
A) CO32-
B) OH–
C) CN–
D) SO42-
63) Which one of the following carbides is not a correct formula?
A) CaC2
B) Fe3C
C) SiC
D) None of these
64) Which statement is most inconsistent with the chemistry of silicon?
A) In nature, it is generally found combined with oxygen in SiO2 and in various silicate minerals.
B) It crystallizes in a diamond-like structure and does not form the graphite-like allotrope.
C) It is a hard, gray, semiconducting solid that melts at 1410°C.
D) It is obtained by oxidation of silica sand with coke.
65) SiO2 can be classified as a(n)
A) amorphous solid.
B) covalent network solid.
C) ionic solid.
D) molecular solid.
66) Which one of the following has a two-dimensional layer structure?
A) silica, SiO2
B) zircon, ZrSiO4
C) talc, Mg3(OH)2(Si4O10)
D) tremolite asbestos, Ca2Mg5(Si4O11)(OH)2
67) What is the charge, n, in the ion Si4O10n that is found in talc?
A) 2 –
B) 4 –
C) 8 –
D) 10 –
68) Mica cleaves into thin sheets because at the molecular level its structure is
A) one dimensional.
B) two dimensional.
C) three dimensional.
D) None of these.
69) Which of the following species has its N atom or atoms in the -1 oxidation state?
A) N2H4
B) NH2OH
C) N2O
D) HONO
70) Which element of group 5A has the highest melting point?
A) nitrogen
B) white phosphorus
C) antimony
D) bismuth
71) Which element of group 5A has the most basic oxide?
A) N
B) P
C) As
D) Bi
72) What statement about nitrogen is not consistent with its chemistry?
A) It is a colorless, odorless, tasteless gas.
B) It makes up 78% of the earth’s atmosphere by volume.
C) It is the most volatile component of liquid air with a boiling point of -196°C.
D) It readily reacts with hydrogen to form NH3 that is used in fertilizers.
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73) In which compound is nitrogen in its highest possible oxidation state?
A) NH3
B) N2H4
C) HNO2
D) HNO3
74) In which compound is nitrogen in its lowest possible oxidation state?
A) NH3
B) N2H4
C) HNO2
D) HNO3
75) What is the Haber process?
A) the isolation of N2 from the atmosphere
B) the synthesis of ammonia, NH3
C) the synthesis of nitric acid, HNO3
D) the synthesis of hydrazine, N2H4
76) What is the chemical equation for the production of hydrazine?
A) N2(g) + 3 H2(g) → 2 NH3(g)
B) 2 NH3(aq) + OCl–(aq) → N2H4(aq) + H2O(l) + Cl–(aq)
C) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l)
D) Au(s) + 3 NO3–(aq) + 6 H+(aq) + 4 Cl–(aq) → AuCl4–(aq) + 3 NO2(g) + H2O(l)
77) What is one method of making “laughing gas”?
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A) NH4NO3(s) + heat → N2O(g) + 2 H2O(l)
B) 3 Cu(s) + 2 NO3–(aq) + 8 H+(aq) → 3 Cu2+(aq) + 2 NO(g) + 4 H2O(l)
C) Cu(s) + 2 NO3–(aq) + 4 H+(aq) → Cu2+(aq) + 2 NO2(g) + 2 H2O(l)
D) 2 NO(g) + O2(g) → 2 NO2(g)
78) If the anhydride of nitrous acid (HNO2) is N2O3 then what is the anhydride of nitric acid (HNO3)?
A) NO2
B) NO3
C) N2O3
D) N2O5
79) What is not a key step in the production of nitric acid by the Ostwald process?
A) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l)
B) 2 NO(g) + O2(g) → 2 NO2(g)
C) 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
D) N2(g) + O2(g) → 2 NO(g)
80) Why does Cu dissolve in concentrated nitric acid but not in concentrated hydrochloric acid?
A) The chloride ion is a stronger oxidizing agent than the nitrate ion.
B) The hydrochloric acid is not as strong as nitric acid.
C) The hydrochloric acid produces insufficient hydronium ion to react with the copper.
D) The nitrate ion is a stronger oxidizing agent than the hydronium ion.
81) What is responsible for the brownish colored gas when copper dissolves in nitric acid?
A) 2 NO(g) + O2(g) → 2 NO2(g)