2. An analytical balance is capable of measuring mass to the nearest 0.1 mg. Which
measurement correctly reflects the precision which can be obtained when using this
(A) 2.06 g
(B) 2.060 g
(C) 2.0600 g
(D) 2.06000 g
3. A sample of gallium has an atomic weight of approximately 69.8. If the sample
consists of two isotopes of masses 69.0 and 71.0 respectively, what is the approximate
percentage of the lighter isotope in the sample?
(A) 80.0 %
(B) 60.0 %
(C) 40.0 %
(D) 20.0 %
4. One basic assumption in the Bohr theory of the structure of the hydrogen atom was
(A) the electron could have any of a continuous range of energies.
(B) the electron could exist in any one of a set of discrete energy levels.
(C) the electron could move from a higher to a lower energy orbit by absorbing a quantum
(D) electromagnetic radiation would be given off as the electron moved in orbit around the
5. Which experiment led to the belief that the atom contained an extremely small,
positively charged nucleus?
(A) Millikan's oil drop experiment
(B) Rutherford's scattering experiment
(C) Thomson's cathode ray tube experiment
(D) Moseley's experiment on X-ray emission by metals
6. According to the Heisenberg Uncertainty Principle, as the wavelength of light used
to locate an electron decreases,
(A) the error in determining its position increases and the error in determining its
momentum increases also.
(B) the error in determining its position decreases and the error in determining its
momentum decreases also.
(C) the error in determining its position increases and the error in determining its
(D) the error in determining its position decreases and the error in determining its
7. Relative atomic and molar masses are determined with a mass spectrometer utilizing
the fact that
(A) the velocity of the paritcles can be accurately determined.
(B) a definite fraction of the particles is formed in a charged state.
(C) all particles with the same charge to mass ratio follow the same curved path.
(D) the force with which the accelerated particles strike a target can be measured.
8. If a neutral atom has an atomic number of 29 and a mass number of 61, then the atom
11. What is the energy of a photon with a wavelength of 6400 nm?
(A) 4.2 x 10¯40 J
(B) 4.2 x 10¯31 J
(C) 3.1 x 10¯19 J
(D) 3.1 x 10¯17 J
12. The attraction that nonpolar molecules have for each other is primarily caused by
the presence of
(B) hydrogen bonding.
(C) van der Waals' forces.
(D) permanent dipole-dipole interactions.
13. The geometries of the molecules BF3 and NF3 are trigonal
planar and trigonal pyramidal respectively. Which statement best accounts for the
(A) N is more elctronegative than B.
(B) BF3 is ionic, which NF3is covalent.
(C) B utilizes sp hybridization, while N does not.
(D) N has a non-bonding pair of valence electrons, while B does not.
14. The best example of a nonpolar molecule containing polar bonds is
15. Which molecule utilizes sp3 hybridization according to Valence Bond
16. How many oxygen molecules are contained in a 3.25 L flask at 25.0 °C and a
pressure of 725 torr (mm of Hg)? Assume ideal behavior.
(A) 7.63 x 1019
(B) 7.63 x 1022
(C) 9.90 x 1023
(D) 5.80 x 1025
17. Which statement best explains why real gases sometimes exhibit a measured volume
greater than that which is calculated from the Ideal Equation of State?
(A) Molecules have a finite size.
(B) Collisions between molecules are not elastic.
(C) Significant intermolecular attractions exist between molecules.
(D) High temperatures result in a significant decrease in pressures.
18. A gas which will diffuse twice as fast as SO2 (MW = 64) is
(A) He (MW = 4)
(B) CH4 (MW = 16)
(C) O2 (MW = 32)
(D) HI (MW = 128)
19. An ideal gas occupies a volume of 31.6 Liters at a pressure of 735 torr (mm of Hg)
and a temperature of 25.0 °C. Which expression correctly calculates the volume of the gas
at a pressure of 765 torr (mm of Hg) and a temperature of 50.0 °C?
20. The density of an unknown gas at 65.0 °C and a pressure of 730 torr (mm of Hg) is
2.14 g L¯1. The density of oxygen gas at the same conditions is 1.11 g L¯1.
What is the molar mass of the unknown gas?
(A) 16.6 g mol¯1
(B) 47.9 g mol¯1
(C) 61.7 g mol¯1
(D) 76.0 g mol¯1
21. A white solid has these properties:
1. The solid is soluble in water.
2. The solid is soluble in chloroform, CHCl3.
3. The pure solid does not conduct electricity.
4. An aqueous solution of the solid conducts electricity.
5. When the solid is melted, the resulting liquid does not conduct electricity.
Based upon this information, this solid would most likely be classified as
35. A reaction for which DH < 0 and DS
< 0 is most likely to have which of these thermodynamic properties?
(A) The reaction cannot be spontaneous at any temperature.
(B) The reaction will tend to be spontaneous at low temperatures.
(C) The reaction will tend to be spontaneous at high temperatures.
(D) The spontaneity of the reaction will be independent of temperature.
36. For the reaction X(g) + Y(g) ---> Z(g) this kinetic data was
Initial [X], M
Initial [Y], M
Initial rate M min¯1
6.20 x 10¯3
2.48 x 10¯2
1.24 x 10¯2
Calculate the initial rate of the reaction in Exp. #4.
(A) 4.36 x 10¯3
(B) 5.81 x 10¯3
(C) 7.27 x 10¯3
(D) 9.69 x 10¯3
37. Below is a potential energy graph for a simple one-step reaction, A ---> B.
What is the value of the activation energy for the reaction B ---> A?
(A) -30 kJ
(B) +20 kJ
(C) +30 kJ
(D) +50 kJ
38. A small increase in temperature often produces a large increases in the rate of a
chemical reaction because it
(A) decreases the activation energy of the reaction.
(B) increases the effectiveness of the collisions between the reactant molecules.
(C) decreases the number of collisions per second between the reactant molecules.
(D) decreases the volume of the solution, altering the concentrations of the reactants.
39. Calculate the pH of a solution made by mixing 150 cm3 of 0.10 M NaC2H3O2
and 250 cm3 of 0.10 M HC2H3O2. Ka
of HC2H3O2 = 1.8 x 10¯5
40. Consider the equilibrium reaction
4 NH3(g) + 3 O2(g) <===> 2 N2(g)
+ 6 H2O(g)
DH = -1268 kJ
Which change will cause the reaction to shift to the right?
(A) Increase the temperature
(B) Decrease the volume of the container.
(C) Add a catalyst to speed up the reaction.
(D) Remove the gaseous water by allowing it to react and be absorbed by KOH.
41. The solubility product constant, Ksp, of Ag3PO4 is
1.8 x10¯18. What is the molar solubility of Ag3PO4 in
water? Neglect any hydrolysis.
(A) 1.6 x 10¯5
(B) 8.4 x10¯7
(C) 1.3 x 10¯9
(D) 4.5 x 10¯19
42. The reaction
2 A(g) + B(g) <===> 3 C(g) + D(g)
is begun with the concentrations of A and B both at an initial value of 1.00 M. When
equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The
value for the equilibrium constant for this reaction is given by the expression
(A) Sn4+ is the oxidizing agent and Fe2+ is the reducing agent.
(B) Sn4+ is the reducing agent and Fe2+ is the oxidizing agent.
(C) Sn4+ is the reducing agent and Fe3+ is the oxidizing agent.
(D) Fe3+ is the oxidizing agent and Sn2+ is the reducing agent.
45. Given the standard reduction potentials
Cu2+ + 2e¯ <===> Cu(s)
E° = +0.34 Volt
Al3+ + 3e¯ <===> Al(s)
E° = -1.66 Volt
Calculate the standard voltage for the reaction
2 Al(s) + 3 Cu2+ ---> 2 Al3+ + 3 Cu(s)
(A) -1.22 Volt
(B) +2.00 Volt
(C) +4.34 Volt
(D) +5.86 Volt
46. The half-life of 214Bi is 19.7 min. Starting with 1.00 x 10¯3
grams of 214Bi, how many grams remain after 59.1 min?
(A) 1.25 x 10¯4
(B) 2.50 x 10¯4
(C) 3.33 x 10¯4
(D) 5.00 x 10¯4
When properly balanced with the simplest set of whole number coefficients, the sum of
the coefficients in the balanced equation is
48. An isotope of uranium undergoes a fission reaction when bombarded with neutrons.
What is the mass number of the uranium isotope used?
49. Which acid can be considered to be an organic acid?
50. An amber-colored, crystalline element burns in air with blue flame, producing an
irritating gas. The gas turns moist litmus paper red. The element exists in more than one
amorphous form, one of which is a caramel-colored gummy substance. The element is
51. A white compound is produced by precipitating it from an aqueous solution. There is
a possibility that the compound may be contaminated by Cu2+. To test for the
contamination, the compound is subsequently dissolved in aqueous ammonia. If Cu2+
were present in the precipitate, the solution produced would be expected to exhibit what
52. Compounds which exhibit color are
(A) Cr2O3 and Fe(OH)3
(B) NaNO3 and KCl
(C) Mg(NO3)2 and BaCl2
(D) AlCl3 and Zn(NO3)2
53. Which series is ranked in order of increasing electronegativity?
(A) O, S, Se, Te
(B) Cl, S, P, Si
(C) In, Sn, N, O
(D) C, Si, P, Se
54. Atom T has 3 valence electrons and atom S has 6 valence electrons. The formula
expected for an ionic compound of T and S is
55. Which gaseous atom has the highest 2nd ionization energy?
56. A 5.00 gram sample of BaCl2 contaminated with an inert substance is
dissolved in 200 mL of water and reacted with an excess of AgNO3 solution,
precipitating AgCl. If 3.23 grams of AgCl are precipitated, what was the percentage by
mass of BaCl2 in the original sample?
57. A student heats 3.000 g of crystalline CuSO4. 5H2O
until it is converted into anhydrous CuSO4. She reports the anhydrous compound
to have a measured mass of 2.000 g. What is the student's approximate percent error in the
mass of the anhydrous compound, assuming the molar masses of the hydrate and the anhydrous
compound to be 249.7 mol¯1 and 159.6 g mol¯1 respectively?
58. When performing an acid-base titration, which procedure would NOT introduce an
error into the experimental results
(A) adding an unmeasured amount of water to the carefully measured acid sample which is
(B) failing to rinse the burettes with the appropriate reactants after cleaning and
rinsing with water.
(C) failing to remove bubbles of air from the tips of the burettes before beginning the
(D) using an indicator that changes color at a pH considerably removed from the pH at the
equivalence point of the titration.
59. For the reaction
2 C2H5OH(l) + 6 O2(l) ---> 4 CO2(g)
+ 6 H2O(l)
for which DH° = -2733.6 kJ, calculate the standard enthalpy
(heat) of formation of C2H5OH(l), in kJ mol¯1, given
that the standard enthalpies of formation of CO2(g) and H2O(l) are
-393.1 and -285.5 kJ mol-1 respectively.
60. Which represents a valid method for dissolving a precipitate of silver chloride?
61. Which species is paramagnetic in the gaseous state?
62. Which kind(s) of isomerism may be exhibited by the molecule
(A) optical only
(B) geometrical only
(C) both geometrical and optical
(D) neither geometrical nor optical
63. An ionic solid has a unit cell consisting of A ions at the corners of a cube and B
ions on the centers of the faces of the cube. The empirical formula for this solid would
64. 1.05 kg of frozen organic solvent (already at its normal freezing temperature) is
place in 10.0 kg of water, originally at 50.0 °C. The enthalpy of fusion of the organic
solvent is 127 kJ kg¯1. The specific heat of water is 4.18 J g¯1
°C¯1. The water temperature when the organic solvent has just finished
melting is approximately
(A) 50 °C
(B) 47 °C
(C) 24 °C
(D) 0 °C
65. A 0.100 m aqueous solution of a weak electroyte, HY, freezes at -0.214 °C.
What is the approximate percent ionization of HY? The freezing poing depression constant
for water is 1.86 °C / m.
66. If a substance has a molar heat of vaporization of 3.05 x 104 J mol¯1
and a normal boiling temperature of 80.0 °C, what is the value of its molar entropy of
vaporization, DSvap, in J K¯1 mol¯1?
(D) 1.08 x 107
67. The Gibbs Free Energy change at 25.0 °C for the reaction
Ag+(aq) + I¯(aq) ---> AgI(s)
is -91.9 kJ mol¯1. The equilibrium constant for the reaction as written is
(A) 7.78 x 10¯17
(B) 1.29 x 1016
(C) 1.24 x 1037
68. The reaction
A + B ---> AB
is 1st order with respect to A and zero order with respect to B. The reaction is begun
with the initial concentration of both reactants at 0.100 M. After 1.5 hours the
concentration of B has dropped to 0.060 M. What is the approximate value of the specific
rate (reaction rate) constant for this reaction?
(A) 0.15 hr¯1
(B) 0.34 hr¯1
(C) 0.61 hr¯1
(D) the specific rate constant cannot be determined unless the mechanism of the reaction
69. 25.0 cm3 of a 0.050 M solution of formic acid, HCOOH, was neutralized
with 25.0 cm3 of a 0.050 M solution of sodium hydroxide, NaOH. What is the pH
of the resulting solution? Ka for HCOOH = 2.1 x 10¯4
70. The standard reduction potentials for Al3+ and Zn2+ are -1.66
Volt and -0.76 Volt respectively. Calculate the free energy change for this reaction as
2 Al(s) + 3 Zn2+(aq) ---> 2 Al3+(aq) + Zn(s)
(A) -5.2 x 105 J
(B) -6.0 x 105 J
(C) +9.0 x 105 J
(D) +1.4 x 106 J