1) How many protons does the Br– ion possess?
A) 34
B) 36
C) 6
D) 8
E) 35
2) CO2 from hydrocarbon combustion creates a major environmental problem that is
described as ________.
A) the greenhouse effect
B) photochemical smog
C) acid rain
D) stratospheric ozone depletion
E) all of the above
3) Which of the following generalizations cannot be made with regard to reactions of
alkali metals? (The symbol M represents any one of the alkali metals.)
A) M (s) + O2 (g) → MO2 (s)
B) 2M (s) + 2H2O (l) → 2MOH (aq) + H2 (g)
C) 2M (s) + H2 (g) → 2MH (s)
D) 2M (s) + Cl2 (g) → 2MCl (s)
E) 2M (s) + S (s) → M2S (s)
4) The value of ΔE for a system that performs 19 kJ of work on its surroundings and
loses 9kJ of heat is ________ kJ.
A) -28
B) 28
C) 171
D) 10
E) -10
5) The molecular weight of a gas is ________ g/mol if 6.7 g of the gas occupies 6.3 L at
STP.
A) 24
B) 3.6 x 103
C) 27
D) 3.0 x 102
E) 1.8 x 10-2
6) Based on the figure above, the boiling point of ethyl alcohol under an external
pressure of 0.658 atm is ________ oC.
A) 20
B) 40
C) 60
D) 80
E) 70
7) When the following equation is balanced, the coefficient of Al is ________.
Al (s) + H2O (l) → Al(OH)3 (s) + H2 (g)
A) 1
B) 2
C) 3
D) 5
E) 4
8) Which one of the following is true concerning the Haber process?
A) It is a process used for shifting equilibrium positions to the right for more
economical chemical synthesis of a variety of substances.
B) It is a process used for the synthesis of ammonia.
C) It is another way of stating Le Ch¢telier’s principle.
D) It is an industrial synthesis of sodium chloride that was discovered by Karl Haber.
E) It is a process for the synthesis of elemental chlorine.
9) Which of the following is not a chelating agent?
A) water
B) ethylenediamine
C) ortho-phenanthroline
D) carbonate ion
E) triphosphate ion
10) What is the pH of an aqueous solution at 25.0 oC that contains 3.98 x 10-9 M hydro
xide ion?
A) 8.40
B) 5.60
C) 9.00
D) 3.98
E) 7.00
11) The energy (J) required for an electronic transition in a Bohr hydrogen atom from n
= 1 to n = 3 is ________ J.
A) -8.90 X 10-1
B) 3.00 X 10-19
C) -3.00 X 10-19
D) 1.94 X 10-18
E) 8.90 X 10-1
12) THMs are ________.
A) non-toxic
B) natural
C) used in green chemistry
D) suspected carcinogens
E) atmospheric pollutants
13) Does either or both cis- or trans-[Mn(en)2Br2] have optical isomers?
A) cis only
B) trans only
C) both cis and trans
D) neither cis nor trans
E) [Mn(en)2Br2] does not exhibit cis-trans isomerism.
14) There is/are ________ hybridized s atomic orbital(s) in an sp-hybridized carbon
atom.
A) 4
B) 0
C) 3
D) 1
E) 2
15) Different isotopes of a particular element contain the same number of ________.
A) protons
B) neutrons
C) protons and neutrons
D) protons, neutrons, and electrons
E) subatomic particles
16) B2O3 is the anhydride of ________.
A) borous acid
B) diborane
C) tetraboric acid
D) boric acid
E) borax
17) What is the atomic number of a neutron?
A) 3
B) 1
C) 2
D) 0
E) 4
18) Which one of the following ions cannot form both a high spin and a low spin
octahedral complex ion?
A) Fe3+
B) Co2+
C) Cr3+
D) Mn3+
E) Cr2+
19) When the following equation is balanced, the coefficient of H2SO4 is ________.
H2SO4 (aq) + NaOH (aq) → Na2SO4 (aq) + H2O (l)
A) 1
B) 2
C) 3
D) 4
E) 0.5
20) Classify the following compounds as weak acids (W) or strong acids (S):
benzoic acid
nitric acid
acetic acid
A) W W W
B) S S S
C) S W W
D) W S S
E) W S W