67) Choose the INCORRECT statement.
A) Amphoteric means useful in photography.
B) Tin disease, tin pest, or tin plague is actually just a second form of tin.
C) A solder is a low melting alloy used to join wires or pieces of metal.
D) Roasting an ore is heating that ore in air.
E) Pewter is an alloy made mainly of tin.
68) Write an equation for the roasting of PbS.
A) 2 PbS(s) + 2 O2(g) → 2 PbO2(s) + S2(s)
B) 2 PbS(s) + 3 O2(g) → 2 PbO(s) + 2 SO2(s)
C) 8 PbS(s) + 4 O2(g) → 8 PbO(s) + S8(s)
D) 2 PbS(s) + O2(g) → 2 PbO(s) + 2 S(s)
E) There is no reaction.
69) Which of the following elements forms a +4 oxidation state that is more stable than its +2 oxidation
state, and is also found as a significant component of commercial bronze, pewter, red brass, and most
solders?
A) zinc
B) tin
C) magnesium
D) lead
E) carbon
70) Choose the molecular shape for BCl3.
A) trigonal planar
B) tetrahedral
C) bent
D) linear
E) trigonal pyramidal
71) Choose the INCORRECT statement.
A) Diborane is B2H6.
B) B(OH)3 boric acid is a monoprotic acid.
C) Being electron deficient makes boron compounds strong Lewis acids.
D) The B-H-B three-center bond has only two electrons.
E) Boron is one of several nonmetals in group 13.
72) Choose the INCORRECT statement about boron.
A) Boron is the only nonmetal in group 13 (3A).
B) Many boron compounds are electron deficient.
C) Borax actually contains no boron.
D) Diborane B2H6 has three center-two atom bonds.
E) The best formula for boric acid is B(OH)3.
73) Choose the INCORRECT statement.
A) The strong C-C and C-H bonds are very important in organic chemistry.
B) At standard temperature and pressure graphite is more stable than diamond.
C) Graphite changes spontaneously but very slowly to diamond.
D) Pencil lead is a graphite and clay mixture.
E) No harder substance than diamond is known.
74) Choose the INCORRECT statement about carbon.
A) In addition to diamonds and graphite, fullerenes and nanotubes are allotropes.
B) The finely divided soot from an incomplete combustion of natural gas is called carbon black.
C) Coke is the result of heating coal in the absence of air.
D) Charcoal is the result of heating wood in the absence of air.
E) Diamond is an excellent conductor.
75) Choose the INCORRECT equation.
A) CaO + 3 C CaC2 + CO
B) CaC2 + 2 H2O → Ca(OH)2 + C2H2
C) CH4 + 4 S → CS2 + 2 H2S
D) (CN)2 + 2 OH– → 2 HOCN
E) CH4 + 4 Cl2 → CCl4 + 4 HCl
76) Choose the INCORRECT statement about silicon.
A) Silicon forms on stable oxide.
B) Silicon exhibits more catenation than carbon.
C) Sand and quartz are SiO2.
D) The central feature of silicates is the SiO44- tetrahedron.
E) A silicone is a compound with an alternating silicon and oxygen chain as a backbone with carbon
containing groups as sidechains.
77) Choose the INCORRECT statement about carbon.
A) Carbon does not form multiple bonds.
B) There are two very common allotropes: diamond and graphite.
C) There is a strong tendency for catenation.
D) Carbon can be hybridized into sp, sp2 and sp3 orbitals.
E) Carbon primarily forms two gaseous oxides: CO and CO2.
78) Choose the INCORRECT statement.
A) Elemental silicon is produced by reduction of SiO2 with coke.
B) In silica each silicon atom is bonded directly to four other silicon atoms.
C) Coke is made by heating coal in the absence of air.
D) Charcoal is made by heating wood in the absence of air.
E) Allotropes of carbon include diamond, graphite, fullerenes and nanotubes.
79) Choose the INCORRECT statement.
A) A glass is an amorphous solid.
B) An amorphous solid has order over relatively short distances.
C) A sol is a colloidal dispersion of particles in a liquid.
D) Silicones are materials consisting of molecules with long silicon-oxygen chains.
E) Silicates are silicon-hydrogen containing compounds.
80) Graphite and diamond are:
A) allotropes
B) amorphous substances
C) bivalent
D) elastomers
E) very unstable
81) Choose the INCORRECT statement.
A) Graphite and diamond are two allotropes of carbon.
B) Graphite can be used as a lubricant because sheets of graphite slide over other sheets of graphite.
C) Carbon black is finely divided soot used in tires, inks and pigments.
D) All carbon containing compounds are the subject of inorganic chemistry.
E) Certain groupings of atoms which have the characteristics of a halogen atom are called
psuedohalogens.
82) Predict the shape of cyanogen, (CN)2.
A) linear
B) bent
C) tetrahedral
D) trigonal pyramidal
E) square planar
19
83) Which of the following metals is refined by some means other than electrolysis?
A) Na
B) Mg
C) Sn
D) Al
E) Zn
84) Which of the following has more than one allotrope?
A) Pb
B) Cd
C) Sn
D) Mg
E) Al
85) Quartz and mica are examples of:
A) silanols
B) silanes
C) silicones
D) silicates
E) isomers
86) Write the equation for the electrolysis of molten NaCl.
A) 2 NaCl(s) → 2 Na(s) + Cl2(g)
B) 2 NaCl(l) → 2 Na(l) + Cl2(g)
C) 2 NaCl(l) → Na2Cl2(s)
D) 2 NaCl(l) → Na(s) + NaCl2(s)
E) There is no reaction.
87) Write the equation for the production of potassium metal from potassium chloride.
A) KCl(s) + Na(s) NaCl(s) + K(s)
B) KCl(s) + Na(s) KNaCl(s)
C) KCl(l) + Na(l) NaCl(l) + K(g)
D) KCl(l) + Na(g) NaCl(s) + K(s)
E) There is no reaction.
88) Write the chemical equation for the reaction of potassium superoxide with carbon dioxide to produce
oxygen.
A) KO(s) + CO2(g) → O2(g) + K(s) + CO(g)
B) K2O(s) + CO2(g) → O2(g) + K(s) + KCO(s)
C) KO2 + CO2(g) → 2 O2(g) + KC(s)
D) 2 KO2(s) + 2 CO2(g) → K2CO3(s) + O2(g)
E) There is no reaction.
89) What mass of potassium superoxide could be prepared from 15.6 g of potassium metal and excess
oxygen?
A) 37.6 g
B) 15.6 g
C) 22.0 g
D) 28.4 g
E) 0.399 g
90) What volume of oxygen gas, measured at STP, would be required for the preparation of 39.0 g of
sodium peroxide from sufficient sodium metal?
A) 11.2 L
B) 9.6 L
C) 7.4 L
D) 5.6 L
E) 2.2 L
21
91) An analysis of a Solvay plant show that for every 4.30 tons of NaCl consumed, 4.75 tons of NaHCO3
is obtained. What is the % efficiency of this process for converting NaCl to NaHCO3?
A) 76.8%
B) 61.8%
C) 63.0%
D) 158%
E) 90.5%
92) What is the pH of a solution labeled “0.020 M Potassium Hypochlorite”? [Ka for hypochlorous acid is
2.9 × 10-8]
A) 1.70
B) 4.62
C) 8.16
D) 9.92
E) 12.30
93) What potential would be expected from a galvanic cell using a solid magnesium/0.20 M Mg2+(aq)
half-cell with a solid thallium/0.010 M Tl+(aq) half-cell [for Mg2+(aq) + 2 e– = Mg(s), E° = –2.36 V; for
Tl+(aq) + e– = Tl(s), E° = -0.34 V]?
A) 3.04 V
B) 1.92 V
C) 1.68 V
D) 2.70 V
E) 2.02 V
94) A sample of water has hardness expressed as 1.6 × 102 ppm Ca2+(aq). The sample is passed through
an ion exchange column and the Ca2+(aq) ions are replaced by H+(aq) ions. What is the pH of the water
after it has been treated? (1 ppm = 1 g solute/106 g solution)
A) 2.09
B) -0.80
C) 1.10
D) 7.00
E) 2.40
Answer: A
Diff: 3 Type: BI Var: 1
Reference: Section 21-3
22
95) A sample of water has hardness expressed as 81 ppm Ca2+(aq). The sample is passed through an ion
exchange column and the Ca2+(aq) ions are replaced by H+(aq) ions. What is the pH of the water after it
has been treated? (1 ppm = 1 g solute/106 g solution)
A) 2.50 ppm
B) 1.10 ppm
C) 0.79 ppm
D) 2.39 ppm
E) 2.70 ppm
96) A sample of water has hardness expressed as 160 ppm Ca2+(aq). The sample is passed through an ion
exchange column and the Ca2+(aq) ions are replaced by Na+(aq) ions. What is the [Na+] in ppm of the
water after it has been treated? (1 ppm = 1 g solute/106 g solution)
A) 46.0 ppm
B) 92 ppm
C) 184 ppm
D) 320 ppm
E) 80.0 ppm
97) A sample of water has hardness expressed as 185 ppm Ca2+(aq). The sample is passed through an ion
exchange column and the Ca2+(aq) ions are replaced by Na+(aq) ions. What is the [Na+] in ppm of the
water after it has been treated? (1 ppm = 1 g solute/106 g solution)
A) 104 ppm
B) 212 ppm
C) 370 ppm
D) 92.5 ppm
E) 52.0 ppm
98) Calculate the number of grams of aluminum produced in the electrolytic process when 2.5 × 105
coulombs are provided to the reaction. Assume 100% efficiency.
A) 23 g
B) 7.7 g
C) 70 g
D) 3.5 g
E) 11 g
23
99) What average current is required to form 5.7 grams of aluminum per hour by the electrolytic reaction?
A) 1.9 A
B) 5.7 A
C) 17 A
D) 0.024 A
E) 7.9 × 10-3 A
100) At the start of 1980, the average lead content in blood had dropped to about 10 μg/dL blood. How
many mg is that in 2.0 gallons of blood? (1 gallon = 3.7854 L)
A) 760 mg
B) 0.80 mg
C) 0.76 mg
D) 0.20 mg
E) 80 mg
101) How much tin is needed to make a bronze piece that will contain 475 g of copper? Bronze is 90% Cu
and 10% Sn by mass.
A) 4.3 × 103 g
B) 890 g
C) 48 g
D) 52.8 g
E) 430 g
102) Complete the reaction:
SiO2 + 2 C
A) SiO + C2O
B) SiC + CO2
C) Si + 2 CO
D) SiCO + CO
E) SiC2O2
103) The molecular geometry for HCN is ________.
A) trigonal planar
B) trigonal bipyramid
C) bent
D) linear
E) trigonal pyramidal
104) The molecular geometry for CO2 is ________.
A) trigonal planar
B) trigonal bipyramid
C) bent
D) linear
E) trigonal pyramidal
105) Bronze is 90% Cu and 10% Sn by mass. What is the density of bronze if the density of Cu
is 8.95 g/cm3 and the density of Sn is 5.77 g/cm3?
A) 7.36
B) 6.07
C) 8.06
D) 14.72
E) 8.63
106) Complete the following reaction:
B(OH)3(aq) + 2 H2O(l) →
A) B ∙ H2O + O2 + H3O+
B) HBO32- + 2 H3O+
C) B + H2 + 5 OH–
D) H3O+ + B(OH)4–
E) 2 H3O+ + HBO3
107) The Ka for boric acid is 5.6 × 10–10. What is the pH for 0.10 M sodium borate?
A) 8.87
B) 5.13
C) 5.75
D) 2.87
E) 11.13
108) The production of lead is a two step process:
2 PbS(s) + 3 O2(g) 2 PbO(s) + 2 SO2(g)
2 PbO(s) + C(s) 2 Pb(l) + CO2(g)
How much ore that is 5.2% PbS is necessary to produce 12.0 kg of Pb?
A) 0.721 kg
B) 200 kg
C) 2.67 kg
D) 133 kg
E) 267 kg
109) An aqueous solution of boric acid can be represented by the equilibrium system:
B(OH)3(aq) + 2 H2O(l) ⇌ H3O+(aq) + B(OH)4–(aq) (Ka = 5.6 × 10–10)
What is the pH of an eyewash solution which is 0.0018 M in boric acid?
A) 3.75
B) 4.75
C) 6.00
D) 7.49
E) 9.25
110) If in a lead storage battery the reaction at the cathode is:
PbO2(s) + 4 H+(aq) + SO4(aq) + 2 e– → PbSO4(s) + 2 H2O(l)
How many grams of lead sulfate are formed on one plate if 20. A average current occurs for 2.0 minutes?
Assume 100% efficiency.
A) 0.063 g
B) 0.13 g
C) 3.8 g
D) 7.5 g
E) requires additional information
111) How much tin is required to make a pewter dish if the dish is 85% Sn and weighs 185 g?
A) 157 g
B) 218 g
C) 185 g
D) 1.59 g
E) 27.8 g
112) What weight of lead sulfate is produced during discharge of a lead storage battery over a 3.0 hour
period at an average current of 0.50 A? [Hint: Consider both electrode processes.]
A) 8.6 g
B) 17 g
C) 26 g
D) 53 g
E) 61 g
113) What average current must be maintained for a tin plating operation forming 2.4 kg of tin per hour
from a solution of a tin(IV) complex, at an electrode efficiency of 90.0%?
A) 750 A
B) 1,000 A
C) 1,600 A
D) 2,400 A
E) 3,000 A
114) What mass of borax [Na2B4O7(H2O)10] could be prepared from 25 kg of colemanite ore
[Ca2B6O11(H2O)5] by a process that is 95% efficient, assuming that no other boron-containing product is
formed?
A) 47 kg
B) 42 kg
C) 33 kg
D) 31 kg
E) 20 kg
115) Complete and balance the following equation.
CaC2(s) + H2O(l) →
Please include states.
116) The acidity of the group 3 oxides ________ (increases, decreases, does not change) moving down the
group.