1) The relationship between the concentrations of reactants and products of a system at
equilibrium is given by the law of mass action.
2) Possible shapes of AB3 molecules are linear, trigonal planar, and T-shaped.
3) The bond energy of oxygen is higher than that of nitrogen.
4) The overall polarity of organic molecules is high.
5) The value of the boiling-point-elevation constant (Kb) depends on the identity of the
solvent.
6) The solubility of slightly soluble salts containing basic anions is proportional to the
pH of the solution.
7) Oxides can react with water to form acids or bases.
8) Bond enthalpy can be positive or negative.
9) Of the following, only ________ is a valid unit for reaction rate.
A) M/s
B) mmol/mL
C) mol/g
D) g/L
E) atm/g
10) The concentration of fluoride ions in a saturated solution of barium fluoride is
________ M. The solubility product constant of BaF2 is 1.7 x 10-6.
A) 3.8 x 10-4
B) 3.0 x 10-3
C) 1.5 x 10-2
D) 7.5 x 10-3
E) 1.4 x 10-4
11) Using the data in the table, which of the conjugate bases below is the strongest
base?
A) OAc–
B) CHO2
–
C) ClO–
D) F–
E) OAc– and CHO2
–
12) Which of the following has the largest second ionization energy?
A) Si
B) Mg
C) Al
D) Na
E) P
13) How much energy (in J) is produced when 0.067 g of matter is converted to energy?
A) 6.0 x 1018
B) 6.0 x 1012
C) 2.0 x 104
D) 6.0 x 1015
E) 2.0 x 107
14) There are ________ unpaired electrons in a ground state fluorine atom.
A) 0
B) 1
C) 2
D) 3
E) 4
15) Crystalline solids ________.
A) have their particles arranged randomly
B) have highly ordered structures
C) are usually very soft
D) exist only at high temperatures
E) exist only at very low temperatures
16) An electron cannot have the quantum numbers n = ________, l = ________, ml =
________.
A) 2, 0, 0
B) 2, 1, -1
C) 3, 1, -1
D) 1, 1, 1
E) 3, 2, 1
17) Cathode rays are ________.
A) neutrons
B) X-rays
C) electrons
D) protons
E) atoms
18) The alpha decay of what isotope of what element produces lead-206?
A) polonium-210
B) radon-222
C) mercury-202
D) bismuth-208
E) thallium-204
19) When gases are treated as real, via use of the van der Waals equation, the actual
volume occupied by gas molecules ________ the pressure exerted and the attractive
forces between gas molecules ________ the pressure exerted, as compared to an ideal
gas.
A) decreases, increases
B) increases, increases
C) increases, decreases
D) does not affect, decreases
E) does not affect, increases
20) A chemical reaction that absorbs heat from the surroundings is said to be ________
and has a ________ ΔH at constant pressure.
A) endothermic, positive
B) endothermic, negative
C) exothermic, negative
D) exothermic, positive
E) exothermic, neutral
21) Cl2 (g) + H2O (l) → ________
A) HCl (aq) + HOCl (aq)
B) 2Cl– (aq) + H2O (l)
C) 2HCl (aq) + O2 (g)
D) 2HCl (aq) + O2
– (g)
E) Cl2 (aq) + H2O (l)
22) Predict the charge of the most stable ion of selenium.
A) 3+
B) 1-
C) 2+
D) 2-
E) 1+
23) The correct formula of iron (III) bromide is ________.
A) FeBr2
B) FeBr3
C) FeBr
D) Fe3Br3
E) Fe3Br
24) Calculate the work (kJ) done during a reaction in which the internal volume
contracts from 83 L to
13 L against an outside pressure of 4.4 atm.
A) 31 kJ
B) 43 kJ
C) -31 kJ
D) -43 kJ
E) 0 kJ; No work is done.
25) Calculate the kinetic energy in joules of an 80.0 g bullet traveling at 300.0 m/s.
A) 3.60 x 106 J
B) 1.20 x 104 J
C) 3.60 x 103 J
D) 12.0 J
E) 80.0 J
26) In the presence of oxygen, the nitrogen present in biodegradable material ends up
mainly as ________.
A) NO3
–
B) NO2
C) N2O
D) NH3
E) NH4
+
27) Calculate the mole fraction of HCl in a 9.45% (by mass) aqueous solution.
A) 0.0491
B) 0.0516
C) 0.0981
D) 0.0245
E) The density of the solution is needed to solve the problem.
28) In compounds of ________ and ________, the octet rule is violated due to the
presence of fewer than eight valence electrons.
29) Low levels of arsenic consumption can lead to ________ or bladder cancer.
30) The deviation from ideal behavior of a gas is most evident at ________ and/or low
temperature.
31) Given the equation
H2O (l) → H2O (g) ΔHrxn = 40.7 kJ at 100 °C
Calculate the mass of liquid water (in grams) at 100 °C that can converted to vapor by
absorbing 2400 J of heat.
32) The average pH of the oceans is ________ and is maintained by the buffering
capacity of ________.
33) The 1s hydrogen orbital overlaps with the ________ iodine orbital in HI.
34) 1 milligram = ________ micrograms
35) The most important acidic and basic functional groups in all amino acids are the
________ and the ________ groups, respectively.
36) A chemical bond rupture resulting from the absorption of a photon is called
________.