1) As a gaseous element condenses, the atoms become ________ and they have
________ attraction for one another.
A) less separated, more
B) less separated, less
C) more separated, more
D) more separated, less
E) smaller, lesser
2) Of the following substances, only ________ has London dispersion forces as its only
intermolecular force.
A) CCl4
B) SnF3
C) CH3OH
D) HI
E) H2O
3) The value of Keq for the equilibrium
N2 (g) + O2 (g) 2 NO (g)
is 4.2 x 10-31 at 27 oC. What is the value of Keq for the equilibrium below?
4 NO (g) 2 N2 (g) + 2 O2 (g)
A) 5.7 x 1060
B) 8.4 x 10-31
C) 4.2 x 1031
D) 8.4 x 1031
E) none of the above
4) What is the overall order of the reaction?
A) 4
B) 0
C) 1
D) 2
E) 3
5) The value of ΔH° for the reaction below is -186 kJ. Calculate the heat (kJ) released
from the reaction of 25 g of Cl2.
H2 (g) + Cl2 (g) → 2HCl (g)
A) 66 kJ
B) 5.3 x 102 kJ
C) 33 kJ
D) 47 kJ
E) -186 kJ
6) The correct name for HClO3 is ________.
A) hydrochloric acid
B) perchloric acid
C) chloric acid
D) chlorous acid
E) hydrochlorous acid
7) Based on the octet rule, aluminum most likely forms an ________ ion.
A) Al3+
B) Al4+
C) Al4-
D) Al+
E) Al–
8) Given the following table of thermodynamic data,
complete the following sentence. The vaporization of TiCl4 is ________.
A) spontaneous at all temperatures
B) spontaneous at low temperature and nonspontaneous at high temperature
C) nonspontaneous at low temperature and spontaneous at high temperature
D) nonspontaneous at all temperatures
E) not enough information given to draw a conclusion
9) A 100-watt electric incandescent light bulb consumes ________ J of energy in 24
hours. [1 Watt (W) = 1 J/sec]
A) 2.40 x 103
B) 8.64 x 103
C) 4.17
D) 2.10 x 103
E) 8.64 x 106
10) How many hydroxyl groups are in a glycerol molecule?
A) 0
B) 1
C) 2
D) 3
E) 4
11) The element X has three naturally occurring isotopes. The isotopic masses (amu)
and % abundances of the isotopes are given in the table below. The average atomic
mass of the element is ________ amu.
A) 33.33
B) 55.74
C) 56.11
D) 57.23
E) 56.29
12) The molecular geometry of the PF3 molecule is ________, and this molecule is
________.
A) trigonal planar, polar
B) trigonal planar, nonpolar
C) trigonal pyramidal, polar
D) trigonal pyramidal, nonpolar
E) tetrahedral, unipolar
13) Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.152
M in formic acid. The Ka of formic acid is 1.77 x 10-4.
A) 2.74 x 10-5
B) 0.0180
C) 3.44
D) 0.581
E) 8.44
14) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC)
The value of S o for the decomposition of POCl3 into its constituent elements,
2POCl3 (g) –> P2 (g) + O2 (g) + 3Cl2 (g)
is ________ J/K mol.
A) +771.0
B) +442.0
C) -321.0
D) -771.0
E) +321.0
15) Which of the following does not have eight valence electrons?
A) Cl–
B) Xe
C) Ti+4
D) Rb+
E) Sr+
16) ________ is the chemical symbol for elemental sodium.
A) S
B) W
C) So
D) Na
E) Sn
17) The mass of a proton is 1.00728 amu and that of a neutron is 1.00867 amu. What is
the mass defect (in amu) of a 57Ni nucleus? (The mass of a nickel-60 nucleus is 59.9308
amu.)
A) 0.5155 amu
B) 28.76 amu
C) -0.4932 amu
D) 0.5141 amu
E) 1.031 amu
18) Under appropriate conditions, nitrogen and hydrogen undergo a combination
reaction to yield ammonia:
N2 (g) + 3H2 (g) → 2NH3 (g)
A ________ g sample of N2 requires 3.0 g of H2 for complete reaction.
A) 0.51
B) 0.76
C) 1.2
D) 14.0
E) 17.2
19) The volume of HCl gas required to react with excess magnesium metal to produce
6.82 L of hydrogen gas at 2.19 atm and 35.0 °C is ________ L.
A) 6.82
B) 2.19
C) 13.6
D) 4.38
E) 3.41