1) Carbon-11 decays by ________.
A) alpha emission
B) beta emission
C) positron emission
D) photon emission
E) neutron capture
2) Standard temperature and pressure (STP), in the context of gases, refers to
________.
A) 298.15 K and 1 atm
B) 273.15 K and 1 atm
C) 298.15 K and 1 torr
D) 273.15 K and 1 pascal
E) 273.15 K and 1 torr
3) Consider the following reaction at equilibrium:
C (s) + H2O (g) CO (g) + H2 (g)
Which of the following conditions will decrease the partial pressure of CO?
A) decreasing the volume of the reaction vessel
B) increasing the volume of the reaction vessel
C) decreasing the amount of carbon in the system
D) decreasing the pressure of the reaction vessel
E) adding a catalyst to the reaction system
4) Iron and chlorine form an ionic compound whose formula is FeCl3. The name of this
compound is ________.
A) iron chlorine
B) iron (III) chloride
C) moniron trichloride
D) iron (III) trichloride
E) ferric trichloride
5) Which element would be expected to have chemical and physical properties closest
to those of rubidium?
A) Cu
B) Fe
C) S
D) Ca
E) K
6) The density of silver is 10.5 g/ cm3. A piece of silver that occupies a volume of 9.60
cm3 would have a mass of ________ g.
A) 101
B) .445
C) 2.25
D) 112
E) 23.6
7) Calculate the energy (J) change associated with an electron transition from n = 2 to n
= 5 in a Bohr hydrogen atom.
A) 6.5 X 10-19 J
B) 5.5 X 10-19 J
C) 8.7 X 10-20 J
D) 4.9 X 10-19 J
E) 5.8 X 10-53 J
8) The number 0.0101 has ________ significant figures.
A) 2
B) 3
C) 5
D) 4
E) 6
9) At 400 K, the equilibrium constant for the reaction
Br2 (g) + Cl2 (g) 2BrCl (g)
is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2(g), 1.00 atm of
Cl2 (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is
true.
A) The equilibrium partial pressures of Br2, Cl2, and BrCl will be the same as the initial
values.
B) The equilibrium partial pressure of Br2 will be greater than 1.00 atm.
C) At equilibrium, the total pressure in the vessel will be less than the initial total
pressure.
D) The equilibrium partial pressure of BrCl (g) will be greater than 2.00 atm.
E) The reaction will go to completion since there are equal amounts of Br2 and Cl2.
10) Which of the following has the same number of significant figures as the number
1.00310?
A) 1 X 106
B) 199.791
C) 8.66
D) 5.119
E) 100
11) The molecular shape of the SF2 molecule is ________.
A) bent
B) tetrahedral
C) linear
D) trigonal planar
E) trigonal pyramidal
12) The element(s) ________ could be used to produce a red or crimson color in
fireworks.
A) Mg or Ba
B) Sr
C) Ca, Sr, or Li
D) Ba
E) Na or K
13) The kinetic-molecular theory predicts that pressure rises as the temperature of a gas
increases because ________.
A) the average kinetic energy of the gas molecules decreases
B) the gas molecules collide more frequently with the wall
C) the gas molecules collide less frequently with the wall
D) the gas molecules collide more energetically with the wall
E) both the gas molecules collide more frequently with the wall and the gas molecules
collide more energetically with the wall
14) Which equation correctly represents the first ionization of phosphorous?
A) P(g) → P+(g) + e–
B) P+(g) → P2+(g) + e–
C) P(g) → P–(g) + e–
D) P+(g) + e– → P(g)
E) P2+(g) → P3+(g) + e–
15) Which of the following will display optical isomerism?
A) square-planar [Rh(CO)2Cl2]–
B) square-planar [Pt(H2NC2H4NH2)2]2+
C) octahedral [Co(NH3)6]3+
D) octahedral [Co(NH3)5Cl]2+
E) octahedral [Co(H2NC2H4NH2)3]3+
16) [Kr]5s2 is the electron configuration for ________.
17) Which of the following has the bonds correctly arranged in order of increasing
polarity?
18) How does an elevated body temperature deprive some bacteria in the body of iron?
19) Of the 20 amino acids found in our bodies, ________ of them must be ingested
because our bodies cannot synthesize sufficient quantities of them.
20) What anion containing Cl is used as a rocket fuel?
21) Myoglobin has ________ heme group(s) that bind(s) ________.
22) The formula for potassium sulfide is ________.
23) The condensation reaction of a carboxyl group of one amino acid and the amino
group of a second amino acid results in the formation of a(n) ________.
24) The initial discovery of a liquid crystal resulted from studies on what compound?
25) If 588 grams of FeS2 is allowed to react with 352 grams of O2 according to the
following equation, how many grams of Fe2O3 are produced?
FeS2 + O2 → Fe2O3 + SO2