1) The gold foil experiment performed in Rutherford’s lab ________.
A) confirmed the plum-pudding model of the atom
B) led to the discovery of the atomic nucleus
C) was the basis for Thomson’s model of the atom
D) utilized the deflection of beta particles by gold foil
E) proved the law of multiple proportions
2) Which hydroxides are strong bases?
Sr(OH)2
KOH
NaOH
Ba(OH)2
A) KOH, Ba(OH)2
B) KOH, NaOH
C) KOH, NaOH, Ba(OH)2
D) Sr(OH)2, KOH, NaOH, Ba(OH)2
E) None of these is a strong base.
3) A 22.9 g sample of iron absorbs 155 J of heat, upon which the temperature of the
sample increases from 23.9 °C to 38.9 °C. What is the specific heat of iron?
A) 0.451 J/g-K
B) -0.451 J/g-K
C) 237 J/g-K
D) 102 J/g-K
E) 53,200 J/g-K
4) The net ionic equation for the reaction between aqueous solutions of HF and KOH is
________.
A) HF + KOH → H2O + K+ + F–
B) HF + OH– → H2O + F–
C) HF + K+ + OH– → H2O + KF
D) H+ + OH– → H2O
E) H+ + F– + K+ + OH– → H2O + K+ + F–
5) Isooctane is assigned an octane number of 100, whereas ________ is assigned an
octane number of 0.
A) methane
B) propane
C) benzene
D) heptane
E) nitrous oxide
6) What are the products of the reaction of PF3 (g) and water?
A) phosphorous acid and hydrofluoric acid
B) elemental phosphorus and hydrofluoric acid
C) phosphoric acid and fluorine gas
D) elemental phosphorus and fluorine gas
E) phosphoric acid and phosphorous acid
7) By what process does thorium-230 decay to radium-226?
A) gamma emission
B) alpha emission
C) beta emission
D) electron capture
E) positron emission
8) A tank containing both HF and HBr gases developed a leak. The ratio of the rate of
effusion of HF to the rate of effusion of HBr is ________.
A) 4.04
B) 0.247
C) 2.01
D) 0.497
E) 16.3
9) An iron mine produces 1.67 X 104 tons of raw ore per day. If the ore is 26.39%
elemental iron, the mine produces ________ pounds of elemental iron per year.
(Assume the mine operates 365 days per year.)
A) 1.221 X 1010
B) 8.814 X 106
C) 3.217 X 109
D) 1.611 X 106
E) 3.66 X 1011
10) An object measuring 77 milliliters will have a volume of ________ liters.
A) 0.077
B) 77000
C) 13
D) 7700
E) 770
11) What is the maximum mass in grams of NH3 that can be produced by the reaction
of 1.0 g of N2 with 3.0 g of H2 via the equation below?
N2 (g) + H2 (g) → NH3 (g) (not balanced)
A) 2.0
B) 1.2
C) 0.61
D) 17
E) 4.0
12) Which one of the following compounds is peroxide?
A) Li2O2
B) Li2O
C) LiO2
D) both Li2O2 and LiO2
E) H2O
13) In which set of elements would all members be expected to have very similar
chemical properties?
A) P, Se, I
B) Cl, Br, Na
C) Si, As, Te
D) Ne, Na, Mg
E) Br, I, At
14) Transition metals within a period differ mainly in the number of ________
electrons.
A) s
B) p
C) d
D) f
E) all of the above
15) What is the pOH 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
16) Compounds found in fossil fuels that contain ________ are primarily responsible
for acid rain.
A) sulfur
B) carbon
C) hydrogen
D) phosphorus
E) neon
17) Which ion shown has empty 4d orbitals?
A) Y3+
B) Zr2+
C) Nb+
D) Mo3+
E) Zr3+
18) The balanced net ionic equation for precipitation of CaCO3 when aqueous solutions
of Na2CO3 and CaCl2 are mixed is ________.
A) 2Na+ (aq) + CO3
2- (aq) → Na2CO3 (aq)
B) 2Na+ (aq) + 2Cl– (aq) → 2NaCl (aq)
C) Na+ (aq) + Cl– (aq) → NaCl (aq)
D) Ca+(aq) + CO3
2- (aq) → CaCO3 (s)
E) Na2CO3 (aq) + CaCl2 (aq) → 2NaCl (aq) + CaCO3 (s)
19) The pressure exerted by a column of liquid is equal to the product of the height of
the column times the gravitational constant times the density of the liquid, P = ghd.
How high a column of methanol
(d = 0.79 g/mL) would be supported by a pressure that supports a 713 mm column of
mercury
(d = 13.6 g/mL)?
A) 713 mm
B) 41 mm
C) 1.2 x 104 mm
D) 9.7 x 103 mm
E) 17 mm
20) The oxidation state of As in the As2O3 molecule is ________.
A) 3
B) 2
C) 4
D) -3
E) 0