1) According to MO theory, overlap of two s atomic orbitals produces ________.
A) one bonding molecular orbital and one hybrid orbital
B) two bonding molecular orbitals
C) two bonding molecular orbitals and two antibonding molecular orbitals
D) two bonding molecular orbitals and one antibonding molecular orbital
E) one bonding molecular orbital and one antibonding molecular orbital
2) What decimal power does the abbreviation d represent?
A) 1 X 10-2
B) 10
C) 1 X 10-9
D) 1 X 10-1
E) 1 X 103
3) The normal boiling point of water is 100.0 oC and its molar enthalpy of vaporization
is 40.67 kJ/mol. What is the change in entropy in the system in J/K when 24.7 grams of
steam at 1 atm condenses to a liquid at the normal boiling point?
A) 88.8
B) -88.8
C) -150
D) 373
E) -40.7
4) Which one of the following is not true concerning automotive air bags?
A) They are inflated as a result of a decomposition reaction.
B) They are loaded with sodium azide initially.
C) The gas used for inflating them is oxygen.
D) The two products of the decomposition reaction are sodium and nitrogen.
E) A gas is produced when the air bag activates.
5) How many moles of gas are there in a 53.7 L container at 24.6 °C and 845.9 torr?
A) 2.45
B) 29.6
C) 0.409
D) 0.0241
E) 1860
6) In the symbol below, x is ________.
C
A) the number of neutrons
B) the atomic number
C) the mass number
D) the isotope number
E) the elemental symbol
7) When a metal and a nonmetal react, the ________ tends to lose electrons and the
________ tends to gain electrons.
A) metal, metal
B) nonmetal, nonmetal
C) metal, nonmetal
D) nonmetal, metal
E) None of the above; these elements share electrons.
8) The SI unit of temperature is ________.
A) K
B) °C
C) °F
D) t
E) T
9) Nitrogen fixation is a difficult process because ________.
A) there is so little nitrogen in the atmosphere
B) nitrogen exists in the atmosphere primarily as its oxides which are very unreactive
C) nitrogen is very unreactive, largely due to its triple bond
D) of the extreme toxicity of nitrogen
E) of the high polarity of nitrogen molecules preventing them from dissolving in
biological fluids, such as those inside cells
10) Of the following substances, ________ has the highest boiling point.
A) H2O
B) SiH4
C) Ar
D) Cl2
E) BF3
11) Determine the pH of a 0.15 M aqueous solution of KF. For hydrofluoric acid, Ka =
7.0 x 10-4.
A) 0.82
B) 5.83
C) 8.17
D) 5.01
E) 1.17
12) Which one of the following substances is the product of this combination reaction?
Al (s) + I2 (s) → ________
A) AlI2
B) AlI
C) AlI3
D) Al2I3
E) Al3I2
13) A compound contains 38.7% K, 13.9% N, and 47.4% O by mass. What is the
empirical formula of the compound?
A) KNO3
B) K2N2O3
C) KNO2
D) K2NO3
E) K4NO5
14) The angular momentum quantum number is 3 in ________ orbitals.
A) s
B) p
C) d
D) f
E) a
15) What is the mass in grams of 2.00 x 105 atoms of naturally occurring neon?
A) 6.07 x 1019
B) 9910
C) 797
D) 3.32 x 10-19
E) 4040000
16) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC)
The value of G o at 25 oC for the formation of phosphorous trichloride from its
constituent elements,
P2 (g) + 3Cl2 (g) –> 2PCl3 (g)
is ________ kJ/mol.
A) -539.2
B) +539.2
C) -642.9
D) +642.9
E) -373.3
17) The belt of nuclear stability ends with the element ________.
A) lead
B) polonium
C) radon
D) astatine
E) bismuth
18) Calculate the pOH of 0.606 M anilinium hydrochloride (C6H5NH3Cl) solution in
water, given that Kb for aniline is 3.83 x 10-4.
A) 1.82
B) 12.18
C) 5.40
D) 8.60
E) 12.42
19) In balancing the nuclear reaction U –> E + He, the identity of element E is
________.
A) Pu
B) Np
C) U
D) Pa
E) Th
20) ________ are particularly polarizable.
A) Small nonpolar molecules
B) Small polar molecules
C) Large nonpolar molecules
D) Large polar molecules
E) Large molecules, regardless of their polarity,