1) What is the coefficient of NO2 when the following disproportionation reaction is
balanced?
NO2 (g) + H2O (l) –> H+ (aq) + NO3
– (aq) + NO (g)
A) 1
B) 2
C) 3
D) 5
E) 4
2) An example of a form of pure carbon that contains only sp3 hybridized carbon atoms
is ________.
A) diamond
B) charcoal
C) graphite
D) carbon black
E) carborundum
3) What decimal power does the abbreviation nano represent?
A) 1 X 106
B) 1 X 109
C) 1 X 10-1
D) 1 X 10-9
E) 1 X 10-12
4) A typical double bond consists of ________.
A) three sigma bonds
B) three pi bonds
C) one sigma and two pi bonds
D) one sigma and one pi bond
E) three ionic bonds
5) The reaction of 100 mL of Cl2 gas with 100 mL of CH4 gas via the equation:
Cl2 (g) + CH4 (g) → HCl (g) + CH3Cl (g)
will produce a total of ________ mL of products if pressure and temperature are kept
constant.
A) 100
B) 50
C) 200
D) 150
E) 250
6) Which one of the following compounds is copper(I) chloride?
A) CuCl
B) CuCl2
C) Cu2Cl
D) Cu2Cl3
E) Cu3Cl2
7) The mass % of F in the binary compound KrF2 is ________.
A) 18.48
B) 45.38
C) 68.80
D) 81.52
E) 31.20
8) Ethanol (C2H5OH) melts at -114 oC. The enthalpy of fusion is 5.02 kJ/mol. The
specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively.
How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -135 oC to liquid
ethanol at -60 oC?
A) 207.3
B) -13.3
C) 6.34
D) 3617
E) 8.63
9) The base-dissociation constant of ethylamine (C2H5NH2) is 6.4 x 10-4 at 25.0 oC.
The [H+] in a
1.4 x 10-2 M solution of ethylamine is ________ M.
A) 3.7 x 4.9 x 10-12
B) 2.7 x 10-3
C) 3.3 x 10-12
D) 3.0 x 10-3
E) 11.43
10) Based on the octet rule, iodine most likely forms an ________ ion.
A) I2+
B) I4+
C) I4-
D) I+
E) I–
11) The ground-state electron configuration for Zn is ________.
A) [Kr]4s23d10
B) [Ar]4s23d10
C) [Ar]4s13d10
D) [Ar]3s23d10
E) [Kr]3s23d10
12) The net ionic equation for formation of an aqueous solution of NiI2 accompanied by
evolution of CO2 gas via mixing solid NiCO3 and aqueous hydriodic acid is ________.
A) 2NiCO3 (s) + HI (aq) → 2H2O (l) + CO2 (g) + 2Ni2+ (aq)
B) NiCO3 (s) + I– (aq) → 2H2O (l) + CO2 (g) + Ni2+ (aq) + HI (aq)
C) NiCO3 (s) + 2H+ (aq) → H2O (l) + CO2 (g) + Ni2+ (aq)
D) NiCO3 (s) + 2HI (aq) → 2H2O (l) + CO2 (g) + NiI2 (aq)
E) NiCO3 (s) + 2HI (aq) → H2O (l) + CO2 (g) + Ni2+ (aq) + 2I– (aq)
13) The molecular geometry of the CHF3 molecule is ________, and the molecule is
________.
A) trigonal pyramidal, polar
B) tetrahedral, nonpolar
C) seesaw, nonpolar
D) tetrahedral, polar
E) seesaw, polar
14) The mole fraction of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g
of C2H6O is ________. The density of the solution is 0.79 g/mL.
A) 0.027
B) 0.034
C) 0.028
D) 0.035
E) 0.151
15) Sodium is much more apt to exist as a cation than is chlorine. This is because
________.
A) chlorine is a gas and sodium is a solid
B) chlorine has a greater electron affinity than sodium does
C) chlorine is bigger than sodium
D) chlorine has a greater ionization energy than sodium does
E) chlorine is more metallic than sodium
16) Which compound has the strongest intermolecular forces?
A) CBr4
B) C12H26
C) CI4
D) N2
E) O2