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1. Which is a list of elements in order of increasing
metallic character?
A. Si, P,
S
B. As, P.
N
C. Sr, Ca,
Mg
D. Br, Se,
As
E. Na, Ne,
F
2. The electron configuration of the oxide ion is most
similar to the electron configuration of the
A. Sulfide
ion
B. Nitride
ion
C. Oxygen
atom
D. Nitrogen
atom
E. Fluorine
atom
3. The value of Plank’s constant is 6.63 * 10-34
J * s. The velocity of light is 3.0 * 108 m * s-1.
Which value is closest to the wave length in nanometers of a quantum of
light with frequency of 8 * 1015 sec-1?
A. 3 * 107
B. 4 * 101
C. 5 * 10-18
D. 2 * 10-25
E. 1 * 10-25
4. What is the number of half-filled orbitals in an atom
of chromium?
A. 0
B. 2
C. 4
D. 6
E. 12
5. What is the number of electrons in an atom of scandium
that have an l quantum number of 1?
A. 1
B. 3
C. 4
D. 6
E. 12
6. The electron configuration of atoms of element X is shown below
[Ar] 4s23d10
Which is the most likely formula for
the compound of this element and oxygen?
A. XO
B. X2O
C. XO2
D. X2O3
E. X2O5
7. Which lists species with the same electron configuration?
A. Mg, Ca,
Sr
B. Mg2+,
Ca2+, Sr2+
C. S2-,
Cl-, K+
D. Fe, Co,
Ni
E. F-,
S2-, As3-
8.One atomic mass unit (amu) is closest to the mass of
A. One proton
B. One electron
C. The oxygen-16
nucleus
D. The carbon-12
nucleus
E. 6.02 *
1023 atoms of hydrogen
9. All of these molecular shapes can be explained by dsp3
hybridization of electrons on the central atom EXCEPT
A. Linear
B. T-shape
C. See-saw
D. Octahedral
E. Trigonal
bipyramidal
10. Which species has a Lewis dot diagram that does not
illustrate the octet rule?
A. NO3-
B. NH3
C. NH4+
D. N2
E. NO2
11. Which substance has the greatest ionic character?
A. Cl2O
B. NCl3
C. PbCl2
D. BaCl2
E. Ch2Cl2
12. The shape of the IO3- ion
is best described as
A. see-saw
B. T-shaped
C. Tetrahedral
D. Trigonal
planer
E. Trigonal
pyramidal
13. Pi bonding is found in all of the following EXCEPT:
A. N2
B. SCN-
C. CO32-
D. AsH3
E. C(graphite)
14. What is the number of sp3 hybrid orbitals associated
with the hydronium ion, H3O+?
A. none
B. two
C. three
D. four
E. six
15. Which change increases the mean free path of molecules
in a sample of gas?
A. increase
in pressure at constant temperature
B. increase
in density at constant temperature
C. increase
in temperature at constant pressure
D. increase
in temperature at constant volume
E. increase
in pressure at constant volume
16. Which occurs when a substance is converted from liquid
to gas at the normal boiling point?
I. Potential energy of the system increases.
II. The distance between molecules increases.
III. The average kinetic energy of the molecules increases.
A. I only
B. II only
C. I and II
only
D. II and
III only
E. I, II,
and III
17. The lattice points of a crystal of hydrogen iodide,
HI, are occupied by
A. HI molecules
B. H atoms
and I atoms
C. H+
cations and I- anions
D. H2I+
cations and I- anions
E. H2
molecules and I2 molecules
18. Which element forms an oxide that is a molecular solid?
A. sodium
B. argon
C. carbon
D. silver
E. iron
19. What is the final concentration of Cl-
ion when 250 mL of 0.20 M CaCl2 solution is mixed with 250 mL
of 0.40 M KCl solution? (Assume additive volumes.)
A. 0.10 M
B. 0.20 M
C. 0.30 M
D. 0.40 M
E. 0.60 M
20. What volume of water should be added to 0.40 L of
6.0 M H2SO4 solution to produce a solution that is
2.0 M H2SO4?
A. 0.40 L
B. 0.80 L
C. 1.2 L
D. 1.6 L
E. 2.4 L
21. What is the percent methanol by mass in a solution
that contains 20 grams of methanol, CH3OH, in 30 grams of water?
A. 20%
B. 33%
C. 40%
D. 60%
E. 67%
22. Compared to water, a 0.20 M solution of NaCl will
have all of the following properties EXCEPT:
A. greater
density
B. lower vapor
pressure
C. lower boiling
point
D. lower freezing
point
E. greater
osmotic pressure
23. In a spontaneous, exothermic dissolving process, which
of these values has a negative sign?
I. /\Gsoln
II. /\Hsoln
III. T
A. I only
B. III only
C. I and II
only
D. II and
III only
E. I, II,
and III
24. Which of these Group 2 oxides has the greatest percent
by mass oxygen?
A. barium
oxide
B. beryllium
oxide
C. calcium
oxide
D. magnesium
oxide
E. strontium
oxide
25. Which oxides of manganese, Mn, have percent by mass of manganese that is greater than 50%.
I. MnO
II. MnO2
III. Mn2O2
A. II only
B. III only
C. I and III
only
D. II and
III only
E. I, II,
and III
26. Which sample contains the greatest number of nitrogen
atoms? (All measurements taken at STP.)
A. 0.20 mol
N2O4(g)
B. 0.40 mol
N2(g)
C. 40. L NO2(g)
D. 40. g NH3(g)
E. 80. g N2O4(g)
27. Al3+ + 3e- -----> Al0
In the
half-reaction shown above, the 3e- represents
A. 3 * 96,
500 electrons
B. 3 * (6.02
* 1023) electrons
C. 3 * (6.02
* 1023) coulombs
D. 3/27 *
96, 500 electrons
E. 3/27 *
(6.02 * 1023) electrons
28. All of the following apply to the reaction A(g)
+ B(g) -----> C(g) as it is carried out at constant
temperature in a rigid container EXCEPT:
A. The total
pressure decreases
B. The rate
of reaction decreases
C. The entropy
of the system decreases
D. The number
of molecules of C decreases
E. The frequency
of collisions between molecule A and B decreases
Rate = k[A]2[B]
At the beginning of one trial
of this reaction, [A] = 4.0 and [B] = 1.0. The observed rate was 0.048
mol C * L-1 * sec-1
29. The value of the rate constant for this reaction is
closest to
A. 3 * 102
B. 4 * 100
C. 8 * 10-1
D. 1 * 10-2
E. 3 * 10-3
30. Which is the label for the rate constant?
A. mol2
* L-2 * sec-1
B. L * mol-2
* sec-1
C. L2
* mol-2 * sec-1
D. L2
* sec * mol-1
E. L2
* sec * mol-2
31. All of the following decrease the rate of a gas phase
reation EXCEPT
A. adding
inert gas
B. removing
the catalyst
C. increasing
the volume
D. lowering
the temperature
E. decreasing
the concentration of one of the reactants
Rate = k[Br-][BrO3-][H+]2
32. The overall order for this reaction is
A. 2
B. 3
C. 4
D. 6
E. 12
33. The pH of a 0.010 M solution of a weak acid is 4.0.
What is the value for the ionization constant, Ka, for this
acid?
A. 10-2
B. 10-4
C. 10-6
D. 10-8
E. 10-10
34. The Ksp for PbCl2 is 1.6 * 10–5.
Which maximum amount of NaCl(s) may be added to 1.0 L of 0.010
Pb(NO3)2 solution without causing precipitate to
occur?
A. 1.6 * 10-5
mol
B. 3.2 * 10-5
mol
C. 1.6 * 10-3
mol
D. 3.2 * 10-3
mol
E. 1.6 * 10-2
mol
35. 2O3(g) <===> 3O2(g) Kp = 2.5 * 1012
Consider a system at equilibrium based on the reaction above. In such a system, the concentration of O2(g) is
A. constant
and equal to the concentration of O3(g)
B. constant
and less than the concentration of O3(g)
C. constant
and greater than the concentration of O3(g)
D. increasing
and the concentration of O3(g) is increasing
E. increasing
and the concentration of O3(g) is decreasing
36. The molar heat of fusion, /\Hfus,
for water is 6.01 kJ / mol. Which expression gives the molar entropy of
fusion, /\Sfus, in kJ / K * mol for ice at its normal
melting point?
A. 6.01 /
273
B. 6.01 /
298
C. 6.01 *
4.18
D. 6.01 *
273
E. 6.01 *
298
37. All of the following reactions illustrate an increase
in entropy EXCEPT:
A. N2O4(g)
-----> 2NO2(g)
B. C6H6(l)
-----> C6H6(g)
C. 2KClO3(s)
-----> 3O2(g) + 2KCl(s)
D. 3Fe(s)
+ 2O2(g) -----> Fe3O4(s)
E. C2H5OH(l)
+ 3O2(g) -----> 2CO2(g) + 3H2O(g)
38. For the burning of propane
C3H8(g) + 5O2(g) -----> 3CO2(g)+4H2O(g)
which of the following is true at any temperature?
I. /\G < 0
II. /\S > 0
III. /\H < 0
A. I only
B. III only
C. I and II
only
D. II and
III only
E. I, II,
and III
39. Which is a polyprotic acid in water?
I. Ca(NO3)2
II. Na2HPO4
III. H3AsO4
A. I only
B. III only
C. II and
III only
D. I and II
only
E. I, II,
and III
40. When solid potassium hydride is dissolved in water,
which of the following is the strongest base in the resulting solution?
A. H+
B. K+
C. O2-
D. KH
E. OH-
41. Which range includes the pH that results when 0.10
mole NaOH is added to 100 mL of 1.0 M HCl solution?
A. between
1 and 4
B. between
4 and 6.5
C. between
6.5 and 7.5
D. between
7.5 and 10
E. between
10 and 14
42. Which range includes the pH that results when 0.10
mole of NaOH is added to 100 mL of 1.0 M H2SO4 solution?
A. between
1 and 4
B. between
4 and 6.5
C. between
6.5 and 7.5
D. between
7.5 and 10
E. between
10 and 14
43. AlCl3 + Cl- -----> AlCl4-
Which description applies to the reaction above?
A. amphotorism
B. anion hydrolysis
C. Arrhenius
neutralization
D. Lewis acid-base
reaction
E. Bronsted-Lowery
proton transfer
Questions 44-45: Balance the
following equation using the electron transfer method. You may wish to
assign oxidation numbers and write the
electronic equations for oxidation and reduction to help balance the overall
reaction.
__ HNO3 + __ P
+ __ H2O ----> __ H3PO4 +
__ NO
44. What is the sum of the coefficients in this balanced
equation?
A. 5
B. 8
C. 10
D. 12
E. 18
45. What is the oxidizing agent in this equation?
A. P
B. H+
C. H2O
D. OH-
E. HNO3
46. Which is the best description of one faraday?
A. 8.31 joules
B. 96,500
amperes
C. one coulomb
/ volt
D. one joule
/ coulomb
E. 6.02 *
1023 electrons
47. H2O + Br2 -----> HOBr + HBr
Which is the best description of the
behavior of bromine in the reaction above?
A. oxidized,
only
B. proton
donor
C. proton
acceptor
D. both oxidized
and reduced
E. neither
oxidized nor reduced
48. Which organic compound is an electrolyte?
A. C2H6
B. CH3Cl
C. HCOOH
D. CH3OH
E. C6H12O6
49. In the complete combustion of butane, the products
are
A. water and
carbon
B. butanone
and water
C. butanoic
acid and water
D. carbon
dioxide and water
E. carbon
dioxide and hydrogen
50. The compound, 2-methyl-2-propanol, is an isomer of
A. butane
B. propane
C. butanol
D. propanoi
E. methanol
51. What is the number of isomers possible for C2H2Cl2?
A. 1
B. 2
C. 3
D. 4
E. 5
52. Which is most likely to be formed in the chemical
reaction that occurs when a gas phase mixture of C4H10
and Cl2 is subjected to ultraviolet light?
A. H2
B. HCl
C. CCl4
D. C4H11Cl
E. C4H10Cl2
53. What is the total number of shared electron pairs
between adjacent carbon atoms in a propyne molecule?
A. 1
B. 2
C. 3
D. 4
E. 5
54. Which general formula applies to hydrocarbons with
one double covalent between adjacent atoms?
A. CnH2n+2
B. CnH2n
C. CnH2n-2
D. CnH2n-4
E. CnH2n-6