1) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for
A–?
A) HA (aq) + H2O (l) H2A+ (aq) + OH–(aq)
B) A– (aq) + H3O+ (aq) HA (aq) + H2O (l)
C) HA (aq) + OH– (aq) H2O (l) + H+ (aq)
D) A– (aq) + H2O (l) HA (aq) + OH– (aq)
E) A– (aq) + OH– (aq) HOA2- (aq)
2) Complexes containing metals with which one of the following electron
configurations are usually colorless?
A) d2
B) d1
C) d5
D) d8
E) d10
3) The mass of a proton is 1.00728 amu and that of a neutron is 1.00867 amu. What is
the binding energy (in J) of a Co nucleus? (The mass of a cobalt-60 nucleus is
59.9338 amu.)
A) 2.74 x 10-19
B) 9.12 x 10-28
C) 4.94 x 10-13
D) 8.20 x 10-11
E) 2.74 x 10-16
4) In the smectic A liquid-crystalline phase, ________.
A) the molecules are aligned along their long axes, with no ordering with respect to the
ends of the molecules
B) the molecules are arranged in sheets, with their long axes parallel and their ends
aligned as well
C) the molecules are aligned with their long axes tilted with respect to a line
perpendicular to the plane in which the molecules are stacked
D) disk-shaped molecules are aligned through a stacking of the disks in layers
E) the molecules are oriented in a totally random fashion
5) Under what condition(s) is the enthalpy change of a process equal to the amount of
heat transferred into or out of the system?
(a) temperature is constant
(b) pressure is constant
(c) volume is constant
A) a only
B) b only
C) c only
D) a and b
E) b and c
6) Predict the charge of the most stable ion of aluminum.
A) 3-
B) 1+
C) 2+
D) 1-
E) 3+
7) Sodium bicarbonate is reacted with concentrated hydrochloric acid at 25.0 °C and
1.50 atm. The reaction of 7.75 kg of bicarbonate with excess hydrochloric acid under
these conditions will produce ________ L of CO2.
A) 1.82 x 103
B) 2.85 x 104
C) 1.82 x 104
D) 1.50 x 103
E) 8.70 x 102
8) Electropositivity ________ from left to right within a period and ________ from top
to bottom within a group.
A) decreases, increases
B) increases, increases
C) increases, decreases
D) stays the same, increases
E) increases, stays the same
9) Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction:
2NO2–> 2NO + O2
In a particular experiment at 300 oC, [NO2] drops from 0.0143 to 0.00701 M in 261 s.
The rate of disappearance of NO2 for this period is ________ M/s.
A) 2.79 x 10-5
B) -8.16 x 10-5
C) 5.59 x 10-5
D) 1.40 x 10-5
E) 35,800
10) Element X has three naturally occurring isotopes. The masses (amu) and %
abundances of the isotopes are given in the table below. The average atomic mass of the
element is ________ amu.
A) 41.54
B) 39.68
C) 39.07
D) 38.64
E) 33.33
11) Which one of the following represents an acceptable set of quantum numbers for an
electron in an atom? (arranged as n, l, ml, and ms)
A) 3, 0, 0, -1/2
B) 3, -1, -4, 1/2
C) 3, -3, 1, -1/2
D) 0, 2, 1, 0
E) 3, 3, 4, 3
12) The formula for aluminum hydroxide is ________.
A) AlOH
B) Al3OH
C) Al2(OH)3
D) Al(OH)3
E) Al2O3
13) Molecules with only single bonds do not generally exhibit liquid-crystalline
properties because ________.
A) molecules without multiple bonds lack the rigidity necessary for alignment
B) molecules without multiple bonds are too small to exhibit liquid-crystalline
properties
C) molecules with only single bonds are gases
D) molecules with only single bonds are too big to exhibit liquid-crystalline properties
E) molecules without multiple bonds lack the flexibility necessary for alignment
14) A 1.35 m aqueous solution of compound X had a boiling point of 101.4 oC. Which
one of the following could be compound X? The boiling point elevation constant for
water is 0.52 oC/m.
A) CH3CH2OH
B) C6H12O6
C) Na3PO4
D) KCl
E) CaCl2
15) The process of solute particles being surrounded by solvent particles is known as
________.
A) salutation
B) agglomeration
C) solvation
D) agglutination
E) dehydration
16) What is the charge on the complex ion in Mg2[FeCl6]?
A) 2-
B) 2+
C) 3-
D) 3+
E) 4-
17) The reaction
CH3-NC –> CH3-CN
is a first-order reaction. At 230.3 oC, k = 6.29 x 10-4s-1. If is 1.00 x 10-3
initially, is ________ after 1.000 x 103 s.
A) 5.33 x 10-4
B) 2.34 x 10-4
C) 1.88 x 10-3
D) 4.27 x 10-3
E) 1.00 x 10-6
18) Complexes containing metals with d10 electron configurations are typically
colorless because ________.
A) there is no d electron that can be promoted via the absorption of visible light
B) the empty d orbitals absorb all of the visible wavelengths
C) there are no d electrons to form bonds to ligands
D) a complex must be charged to be colored
E) d electrons must be emitted by the complex in order for it to appear colored