1) Classify the following compounds as weak bases (W) or strong bases (S):
ammonia
fluoride ion
sodium hydro xide
A) W W S
B) S S S
C) S W W
D) W S S
E) W S W
2) The structure of 2,3-dimethylheptane is ________.
A)
B)
C)
D)
E)
3) Based on molecular orbital theory, the bond orders of the H-H bonds in H2, H2
+, and
H2
– are ________, respectively
A) 1, 0, and 0
B) 1, 1/2, and 0
C) 1, 0, and 1/2
D) 1, 1/2, and 1/2
E) 1, 2, and 0
4) Calculate the pH of a solution prepared by dissolving 0.850 mol of NH3 and 0.300
mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77
x 10-5.
A) 5.204
B) 4.300
C) 9.700
D) 8.781
E) 8.796
5) The law of constant composition says ________.
A) that the composition of a compound is always the same
B) that all substances have the same composition
C) that the composition of an element is always the same
D) that the composition of a homogeneous mixture is always the same
E) that the composition of a heterogeneous mixture is always the same
6) The expression of Keq for the following reaction will not include ________.
A(g) + B (g) C (l) + D (g)
A) [C]
B) [A]
C) [B]
D) [D]
E) none of the above
7) Methane and ethane are both made up of carbon and hydrogen. In methane, there are
12.0 g of carbon for every 4.00 g of hydrogen, a ratio of 3:1 by mass. In ethane, there
are 24.0 g of carbon for every 6.00 g of hydrogen, a ratio of 4:1 by mass. This is an
illustration of the law of ________.
A) constant composition
B) multiple proportions
C) conservation of matter
D) conservation of mass
E) octaves
8) What is the empirical formula of a compound that is 66.6% C, 11.2% H, and 22.2%
O by mass?
A) C4HO
B) C6HO2
C) C8H16O2
D) C6H11O
E) C4H8O
9) Which one of the following substances would be the least soluble in CCl4?
A) Na2SO4
B) C4H10
C) F2
D) HCl
E) CH3CH2CH2CH2OH
10) Based on the octet rule, phosphorus most likely forms a ________ ion.
A) P3+
B) P3-
C) P5+
D) P5-
E) P+
11) The oxidation state of phosphorous in the PF5 molecule is ________.
A) +5
B) +4
C) -5
D) +6
E) 0
12) The primary source of the specificity of enzymes is ________.
A) their polarity, which matches that of their specific substrate
B) their delocalized electron cloud
C) their bonded transition metal, which is specific to the target substrate
D) their locations within the cell
E) their shape, which relates to the lock-and-key model
13) A volatile liquid is one that ________.
A) is highly flammable
B) is highly viscous
C) is highly hydrogen-bonded
D) is highly cohesive
E) readily evaporates
14) Which one of the following orbitals can hold two electrons?
A) 2px
B) 3s
C) 4dxy
D) all of the above
E) none of the above
15) Of the hydrogen halides, only ________ is a weak acid.
A) HCl (aq)
B) HBr (aq)
C) HF (aq)
D) HI (aq)
E) They are all weak acids.
16) Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.00
mol of neon gas at is ________ atm. (a = 0.211 L2-atm/mol2, b = 0.0171 L/mol)
A) 0.730
B) 1.00
C) 1.21
D) 1.37
E) 0.367
17) Sn is the symbol for the element ________.
18) What is the osmotic pressure (in atm) of a 0.040 M solution of a non-electrolyte at
30.0 oC?
19) In the equation below, what is the meaning of the asterisk?
O + O2–> O3*
20) [Xe]6s2 is the electron configuration for ________.
21) What is an acetylide?
a carbide containing the C2
22) KNO3 and NaNO3 are also known as ________.
23) Approximately 90% of the earth’s ozone is in the ________.
24) A compound that can occupy two coordination sites is a (an) ________.
25) Draw a diagram of the short-hand ground state electron configuration of zinc.
26) The standard enthalpy change of a reaction is the enthalpy change when all
reactants and products are at ________ pressure and a specific temperature.