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What is the oxidation number of each atom in sodium hydrogen carbonate, NaHCO3?
A.Na = +1, H = "1, C = +6, O = "2
B.Na = +1, H = +1, C = +4, O = "2
C.Na = +1, H = "1, C = +2, O = "2
D.Na = "1, H = +1, C = 0, O = "2
E.Na = 0, H = 0, C = 0, O = 0
Round 0.00680483 to 3 significant figures.
A.0.00
B.0.007
C.0.00680
D.0.006804
E.0.006805
Calcium carbonate, or limestone, is relatively insoluble in water. At 25 C, only 5.8 mg
will dissolve in 1.0 liter of water. What volume of water is needed to dissolve 5.0 g of
calcium carbonate?
A.4.6 10"3 L
B.3.0 10"2 L
C.1.4 102 L
D.3.4 102 L
E.8.6 102 L
Which of the following statements is/are CORRECT?
1/ Naturally occurring isotopes account for only a small fraction of known radioactive
isotopes.
2/ A few radioactive isotopes with long half-lives, such as U-235 and U-238, are found
in nature.
3/ Trace quantities of some short-lived radioactive isotopes, such as C-14, are found in
nature because they are formed continuously by nuclear reactions.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
What is the correct answer to the following expression: (205.18 " 197.3) 6.226? Carry
out the subtraction operation first.
A.1
B.1.3
C.1.27
D.1.266
E.1.2657
Which of the following chemical equations depicts a halogenation reaction with
benzene?
A.C6H6( ) + 3 Br2(g) 3 C2H2Br2(g)
B.C6H6( ) + Cl2(g) C6H5Cl( ) + HCl(g)
C.C6H6( ) + CH3I(g) C6H5CH3( ) + HI(g)
D.C6H6( ) + Cl2(g) C6H4Cl2( ) + H2(g)
E.C6H6( ) + 3 Br2(g) 6 C6H6Br6(g)
A 50.0 mL sample of 0.155 M HNO2(aq) is titrated with 0.100 M NaOH(aq). What is
the pH of a solution after the addition of 25.0 mL of NaOH? (Ka of HNO2 = 4.5 10"4)
A.3.02
B.3.22
C.3.67
D.3.86
E.4.05
For the zero-order reaction below, a graph of ____ versus time will generate a straight
line.
A B + C rate = k[A]0
A.[A]t
B.
C.ln[A]t
D.
E.
What is the O-C-N bond angle in OCN"?
A.90
B.107
C.109.5
D.120
E.180
According to the Brnsted-Lowry definition, an acid
A.increases the H3O+ concentration in an aqueous solution.
B.is a strong electrolyte.
C.is a proton acceptor.
D.increases the pH of a solution.
E.is a proton donor.
Use VSEPR theory to predict the molecular geometry of BrO3
".
A.trigonal-pyramidal
B.trigonal-planar
C.bent
D.T-shaped
E.linear
Complete the following fusion reaction.
A.
B.
C.
D.
E.
The nitrogen atom in cyanide ion, CN", is surrounded by
A.one single bond and three lone pairs of electrons.
B.one double bond and one lone pair of electrons.
C.one double bond and two lone pairs of electrons.
D.one triple bond and one lone pair of electrons.
E.one triple bond and no lone pairs of electrons.
How long will it take 10.0 mL of Ne gas to effuse through a porous barrier if it has been
observed that 125 minutes are required for 10.0 mL of Ar gas to effuse through the
same barrier?
A.1.41 min.
B.31.9 min.
C.63.1 min.
D.88.8 min.
E.176 min.
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. Assuming that the molecular orbital energy diagram for a
homonuclear diatomic molecule applies to a heteronuclear diatomic molecule,
determine which of the following species is paramagnetic.
A.NO+
B.CO
C.CN"
D.OF"
E.NO
The molar nuclear mass of fluorine-19 is 18.99840 g/mol. The molar mass of a proton
is 1.007825 g/mol. The molar mass of a neutron is 1.008665 g/mol. Calculate the
binding energy (in J/mol) of F-19. (c = 2.998 108 m/s)
A.6.753 1012 J/mol
B.7.131 1012 J/mol
C.1.426 1013 J/mol
D.8.609 1014 J/mol
E.8.538 1014 J/mol
If an aqueous solution of ____ is added to a mixture of Pb2+ and Ba2+, the lead ion will
precipitate, but the barium ion will remain in solution.
A.NaOH
B.Na2SO4
C.K3PO4
D.KCO3
E.Ca(CH3CO2)2
What is the mass number of an argon atom with 22 neutrons?
A.2
B.18
C.22
D.40
E.39.95
In which of the following equilibrium systems will an increase in the pressure have no
effect on the concentrations of products and reactants?
A.H2(g) + F2(g) 2 HF(g)
B.N2(g) + 3 H2(g) 2 NH3(g)
C.CaCO3(s) CaO(s) + CO2(g)
D.2 NOBr(g) 2 NO(g) + Br2(g)
E.2 H2O(g) + O2(g) 2 H2O2(g)
Which of the following species is the strongest acid in an aqueous solution?
A.CH3CH2CO2H
B.CH2ClCO2H
C.CH3CO2H
D.CCl3CO2H
E.CHCl2CO2H
Rhodium (atomic mass 102.9 g/mol) crystallizes in a face-centered cubic unit cell. In
addition, rhodium has an atomic radius of 135 pm. What is the density (in g/cm3) of
rhodium?
A.1.53 g/cm3
B.6.14 g/cm3
C.17.4 g/cm3
D.12.3 g/cm3
E.27.8 g/cm3
What is a possible set of quantum numbers for an unpaired electron in the orbital box
diagram below?
A.n = 1, = 1, = "1, ms = +1/2
B.n = 4, = 2, = "1, ms = "1/2
C.n = 5, = 2, = "2, ms = +1/2
D.n = 5, = 0, = 0, ms = "1/2
E.n = 5, = 1, = "1, ms = +1/2
In metals, there are not enough electrons to fill all of the electronic energy levels. At 0
K, the highest energy level filled is referred to as the ________.
A.valence band
B.conduction band
C.free energy
D.Fermi level
E.band gap
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. Assume that the molecular orbital energy diagram for a
homonuclear diatomic molecule applies to a heteronuclear diatomic molecule. What is
the molecular orbital configuration of CO?
A.[core electrons] (s2s)2 (s*2s)2 (p2p)4 (s2p)2
B.[core electrons] (s2s)2 (s*2s)2 (p2p)2 (s2p)2 (p*2p)2
C.[core electrons] (s2s)2 (s*2s)2 (p2p)2 (s2p)4
D.[core electrons] (s2s)2 (s*2s)2 (p2p)6
E.[core electrons] (s2s)2 (s*2s)2 (p2p)3 (s2p)3
Which of the following chemical equations corresponds to the acid ionization constant,
Ka, for benzoic acid (C6H5CO2H)?
A.C6H5CO2
-(aq) + H3O+(aq) C6H5CO2H(aq) + H2O( )
B.C6H5CO2H(aq) + H2O( ) C6H5CO2
-(aq) + H3O+(aq)
C.C6H5CO2H(aq) + OH"(aq) C6H5CO2
-(aq) + H2O( )
D.C6H5CO2H(aq) + H3O+(aq) C6H5CO2H2
+(aq) + H2O( )
E.C6H5CO2
-(aq) + H2O( ) C6H5CO2H(aq) + OH"(aq)
Use your knowledge of group properties to predict the chemical formula for selenic
acid.
A.HSeO2
B.H2SeO3
C.H2SeO4
D.H3SeO3
E.H3SeO4
For a chemical reaction, the activation energy for the forward reaction is +181 kJ and
the activation energy for the backward reaction is +62 kJ. What is the overall energy
change for the forward reaction?
A."119 kJ
B."62 kJ
C.+119 kJ
D.+181 kJ
E.+243 kJ
Determine the enthalpy change for the decomposition of calcium carbonate
CaCO3(s) CaO(s) + CO2(g)
given the thermochemical equations below.
Ca(OH)2(s) CaO(s) + H2O( ) DrH = 65.2 kJ/mol-rxn
Ca(OH)2(s) + CO2(g) CaCO3(s) + H2O( ) DrH = -113.8 kJ/mol-rxn
C(s) + O2(g) CO2(g) DrH = -393.5 kJ/mol-rxn
2 Ca(s) + O2(g) 2 CaO(s) DrH = -1270.2 kJ/mol-rxn
A.+48.6 kJ/mol-rxn
B.+179.0 kJ/mol-rxn
C.+345.5 kJ/mol-rxn
D.+441.0 kJ/mol-rxn
E.+1711.7 kJ/mol-rxn
Use the standard reduction potentials below to determine which element or ion is the
best oxidizing agent.
O2(g) + 4 H+(aq) + 4 e" 2 H2O( ) E = +1.229 V
Hg2
2+(aq) + 2 e" 2 Hg( ) E = +0.789 V
I2(s) + 2 e" 2 I"(aq) E = +0.535 V
A.I2(s)
B.O2(g)
C.I"(aq)
D.Hg2
2+(aq)
E.H2O( )
If a cordless phone operates at a frequency of 9.00 108 s"1. What is the wavelength of
this radiation?
A.0.333 m
B.1.99 10"25 m
C.3.33 10"9 m
D.3.71 10"18 m
E.2.70 1017 m
Which element from the first transition series does NOT react with hydrochloric acid?
A.titanium
B.chromium
C.cobalt
D.nickel
E.copper
