Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of
sulfur dioxide, SO2.
A.The electron-pair geometry is trigonal-planar, the molecular geometry is
trigonal-planar.
B.The electron-pair geometry is trigonal-planar, the molecular geometry is bent.
C.The electron-pair geometry is tetrahedral, the molecular geometry is bent.
D.The electron-pair geometry is tetrahedral, the molecular geometry is linear.
E.The electron-pair geometry is trigonal-bipyramidal, the molecular geometry is linear.
Ammonia gas is synthesized according to the balanced equation below.
N2(g) + 3 H2(g) 2 NH3(g)
If 1.55 L N2 react with 4.92 L H2, what is the theoretical yield (in liters) of NH3?
Assume that the volumes of reactants and products are measured at the same
temperature and pressure.
A.1.55 L
B.3.10 L
C.3.28 L
D.4.93 L
E.6.42 L
Excited sodium atoms emit light in the infrared at 589 nm. What is the energy of a
single photon with this wavelength?
A.5.09 1014 J
B.1.12 10“27 J
C.3.37 10“19 J
D.3.37 10“28 J
E.1.30 10“-19 J
The layer of the atmosphere closest to the Earth’s surface is the ________.
A.thermosphere
B.stratosphere
C.stratopause
D.troposphere
E.mesosphere
Which of the following molecules or ions will have a Lewis structure most like that of
sulfur dioxide, SO2?
A.NO2
+
B.CO2
C.O3
D.SCN“
E.ClO2
“
Which of the following compounds is a common oxide for phosphorus?
A.PO
B.P2O3
C.PO3
D.PO5
E.P4O10
Diagram 9-1
The molecular orbital diagram below may be used for the following problem(s). For
oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However,
the diagram will still yield correct bond order and magnetic behavior for these
molecules.
Energy ________ s*2p
________ ________ p*2p
________ s2p
________ ________ p2p
________ s*2s
________ s2s
________ s*1s
________ s1s
Refer to Diagram 9-1. According to molecular orbital theory, which of the following
species has the highest bond order?
A.F2
B.F2
2+
C.C2
2″
D.Li2
E.B2
2+
Most copper minerals are mined as ________.
A.fluorides
B.sulfides
C.oxides
D.nitrates
E.silicates
What is the correct Lewis structure for IF3?
A.
B.
C.
D.
E.
If a radio wave has a frequency of 17.0 MHz, what is the wavelength of this radiation?
A.5.10 1015 m
B.5.67 10“2 m
C.5.88 10“2 m
D.1.76 101 m
E.1.76 106 m
If 15.0 g N2 and 2.00 g H2 react to produce 1.38 g NH3, what is the percent yield of the
reaction?
N2(g) + 3 H2(g) 2 NH3(g)
A.7.57%
B.12.2%
C.8.12%
D.15.1%
E.8.17%
Which of the following molecules or ions are likely to be free radicals: N2O, NO, and
NO2?
A.N2O only
B.NO only
C.NO2 only
D.N2O and NO
E.NO and NO2
Which is the best colored indicator to use in the titration of 0.1 M CH3CO2H(aq) with
NaOH(aq)? Why? (Ka of CH3CO2H = 1.8 10“5, Kb of CH3CO2
“ = 5.6 10“10)
Indicator pKa
Bromcresol Green 4.8
Bromthymol Blue 6.8
Phenolphthalein 9.2
A.Bromcresol Green. The equivalence point for a weak acid titration occurs at low pH.
B.Bromthymol Blue. The pH at the equivalence point is 7.0.
C.Bromcresol Green. The pKa of CH3CO2H and the pKa of the indicator are similar.
D.Phenolphthalein. The pKa of CH3CO2
“ and the pKb of the indicator are similar.
E.Phenolphthalein. The pH at the equivalence point is near the pKa of the indicator.
The reaction A B follows first-order kinetics with a half-life of 21.7 hours. If the
concentration of A is 0.023 M after 48.0 hours, what is the initial concentration of A?
A.0.0050 M
B.0.051 M
C.0.51 M
D.0.11 M
E.2.0 102 M
To form a molecule with an octahedral electron geometry, what set of pure atomic
orbitals must be mixed?
A.one s and three p
B.one s, three p, and one d
C.one s, three p, and two d
D.two s, six p, and two d
E.two s, six p, and four d
Which of the following statements concerning solubility is/are CORRECT?
1/ Ionic compounds composed of Group 1A metal ions and halide ions, such as NaCl,
are insoluble in nonpolar solvents.
2/ The solubility of the halogens (Cl2, Br2, and I2) in polar solvents is greater than their
solubility in nonpolar solvents.
3/ The solubility of polar molecules, such as sugar, in polar solvents is generally greater
than their solubility in nonpolar solvents.
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
What element is in the fourth period in Group 3A?
A.Sb
B.Ga
C.In
D.Si
E.Tl
Diagram 9-1
The molecular orbital diagram below may be used for the following problem(s). For
oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However,
the diagram will still yield correct bond order and magnetic behavior for these
molecules.
Energy ________ s*2p
________ ________ p*2p
________ s2p
________ ________ p2p
________ s*2s
________ s2s
________ s*1s
________ s1s
Refer to Diagram 9-1. Consider the molecules B2, C2, N2 and F2. Which two molecules
have the same bond order?
A.B2 and C2
B.B2 and F2
C.C2 and N2
D.C2 and F2
E.N2 and F2
Which of the following relationships is/are CORRECT for gases?
1/ The amount of a gas (in moles) is inversely proportional to its volume (at constant
temperature and pressure).
2/ The volume of a gas is directly proportional to its temperature in kelvin (at constant
pressure and moles).
3/ The pressure of a gas is inversely proportional to its temperature in kelvin (at
constant volume and moles).
A.1 only
B.2 only
C.3 only
D.1 and 2
E.2 and 3
Diagram 9-1
The molecular orbital diagram below may be used for the following problem(s). For
oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However,
the diagram will still yield correct bond order and magnetic behavior for these
molecules.
Energy ________ s*2p
________ ________ p*2p
________ s2p
________ ________ p2p
________ s*2s
________ s2s
________ s*1s
________ s1s
Refer to Diagram 9-1. Use molecular orbital theory to predict which ion is
paramagnetic.
A.F2
2+
B.O2
2″
C.O2
2+
D.N2
2+
E.B2
2″
Which of the following statements is INCORRECT?
A.H3PO4 is a stronger acid than H2PO4
–.
B.HClO3 is a stronger acid than HClO2.
C.HNO3 is a stronger acid than HNO2.
D.[Fe(H2O)6]2+ is a stronger acid than [Fe(H2O)6]3+.
E.HOCl is stronger acid than HOBr.
44.0 g of ice at “20.0 C is mixed with 325 g of water at 32.1 C. Calculate the final
temperature of the mixture. Assume that no energy in the form of heat is transferred to
the environment. (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/gK,
liquid water = 4.184 J/gK)
A.”0.6 C
B.5.5 C
C.12.1 C
D.17.6 C
E.38.9 C
The standard molar enthalpy of formation of NH3(g) is “45.9 kJ/mol. What is the
enthalpy change if 9.51 g N2(g) and 1.96 g H2(g) react to produce NH3(g)?
A.”10.3 kJ/mol-rxn
B.”20.7 kJ/mol-rxn
C.”29.8 kJ/mol-rxn
D.”43.7 kJ/mol-rxn
E.”65.6 kJ/mol-rxn
What is the effect of adding NaOH(aq) to an aqueous solution of ammonia?
1/ The pH of the solution will increase.
2/ The concentration of NH4
+(aq) will decrease.
3/ The concentration of NH3(aq) will increase.
A.1 only
B.2 only
C.3 only
D.2 and 3
E.1, 2, and 3
Approximately 300 billion liters of hydrogen is produced annually. The majority of the
hydrogen is used in the production of ____.
A.ammonia
B.hydrogen chloride
C.methane
D.sulfuric acid
E.water
What is the atomic symbol for an element that has 30 neutrons and a mass number of
55?
A.At
B.Zn
C.Co
D.Mn
E.Cs
At constant temperature, 7.72 L of Cl2 at 458 mm Hg is compressed to 3.75 L. What is
the final pressure of Cl2?
A.0.485 mm Hg
B.0.00106 mm Hg
C.222 mm Hg
D.943 mm Hg
E.1820 mm Hg
According to the Arrhenius definition, a base is a substance that when dissolved in
water increases the concentration of
A.hydroxide ion.
B.hydronium ion.
C.protons.
D.electrolytes.
E.cations.
Methane gas, CH4, effuses through a barrier at a rate of 0.568 mL/minute. If an
unknown gas effuses through the same barrier at a rate of 0.343 mL/minute, what is the
molar mass of the gas?
A.20.8 g/mol
B.28.0 g/mol
C.32.0 g/mol
D.44.0 g/mol
E.64.0 g/mol
For which of the following molecules or ions does the central atom have sp
hybridization: N3
“, O3, and I3
“?
A.N3
“ only
B.O3 only
C.I3
“ only
D.O3 and I3
“
E.I3
“ and N3
“
According to the Brnsted-Lowry definition, a base
A.is a weak electrolyte.
B.increases the OH“ concentration in an aqueous solution.
C.is an electron-pair donor.
D.increases the pH of a solution.
E.is a proton acceptor.
If 1.00 g of an unknown molecular compound contains 8.35 1021 molecules, what is its
molar mass?
A.44.0 g/mol
B.66.4 g/mol
C.72.1 g/mol
D.98.1 g/mol
E.132 g/mol
Which of the following reactions is an example of electron capture?
A.
B.
C.
D.
E.
Which of the following equations is the solubility product for Cu(II) hydroxide,
Cu(OH)2?
A.
B.
C.
D.
E.
The boiling points of some group 7A hydrides are tabulated below.
gas b.p. (C)
NH3 “33
PH3 “88
AsH3 “62
Which intermolecular force or bond is responsible for the high boiling point of NH3
relative to PH3 and AsH3?
A.hydrogen bonding
B.dipole/induced dipole force
C.induced dipole/induced dipole force
D.covalent bonding
E.dipole-dipole force