1) Air containing 4% H2 can be explosive.
2) The wavelength of radio waves can be longer than a football field.
3) In some molecules and polyatomic ions, the sum of the valence electrons is odd and
as a result the octet rule fails.
4) The formula for chromium (II) iodide is CrI2.
5) The instantaneous rate of a reaction can be read directly from the graph of molarity
versus time at any point on the graph.
6) The chelate effect must always occur with positive enthalpy change.
7) The effect of a catalyst on a chemical reaction is to react with product, effectively
removing it and shifting the equilibrium to the right.
8) Gold has a density of 0.01932 kg/cm3. What volume (in cm3) would be occupied by
a 22.2 g sample of gold?
A) 0.429
B) 0.870
C) 0.000429
D) 16.81
E) 1.15
9) The order of MO energies in B2, C2, and N2 (σ2p > π2p), is different from the order in
O2, F2, and Ne2 (σ2p > π2p). This is due to ________.
A) less effective overlap of p orbitals in O2, F2, and Ne2
B) the more metallic character of boron, carbon and nitrogen as compared to oxygen,
fluorine, and neon
C) greater 2s-2p interaction in O2, F2, and Ne2
D) greater 2s-2p interaction in B2, C2,and N2
E) less effective overlap of p orbitals in B2, C2, and N2
10) Which of the following correctly lists the five atoms in order of increasing size
(smallest to largest)?
A) Ge < Si < S < O < Ne
B) Ne < O < S < Si < Ge
C) Ne < S < O < Si < Ge
D) Ne < Si < O < S < Ge
E) Ne < Ge < Si < S < O
11) A sample of He gas (3.0 L) at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas
at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the
flask was ________ atm. Assume the initial pressure in the flask was 0.00 atm and the
temperature upon mixing was 25 °C.
A) 2.6
B) 9.2
C) 1.0
D) 3.7
E) 24
12) Which two bonds are most similar in polarity?
A) O-F and Cl-F
B) B-F and Cl-F
C) Al-Cl and I-Br
D) I-Br and Si-Cl
E) C-Cl and Be-Cl
13) An electron in a ________ subshell experiences the greatest effective nuclear
charge in a many-electron atom.
A) 3f
B) 3p
C) 3d
D) 3s
E) 4s
14) What is the pOH of an aqueous solution at 25.0 oC in which [H+] is 0.0050 M?
A) 8.70
B) 11.70
C) -11.70
D) -8.70
E) none of the above
15) What is the mass in grams of 9.76 x 1012 atoms of naturally occurring potassium?
A) 2.41 x 1012
B) 2.50 x 1011
C) 6.34 x 10-10
D) 1.62 x 10-11
E) 3.82 x 1014
16) The symbol for the element sodium is ________.
A) Me
B) Hg
C) Sn
D) Na
E) Pb
17) How many chiral atoms does the open-chain form of glucose have?
A) 1
B) 2
C) 3
D) 4
E) 5
18) Which of the following complexes has a coordination number of 6?
A) [Co(en)2Cl2]+
B) [Pt(NH3)2Cl2]
C) [Cu(NH3)4]2+
D) [Ag(NH3)2]+
E) None of these complexes has coordination number 6.
19) The reaction below is exothermic:
2SO2 (g) + O2 (g) 2SO3 (g)
Le Ch¢telier’s Principle predicts that ________ will result in an increase in the number
of moles of SO3 (g) in the reaction container.
A) increasing the amount of SO2
B) decreasing the pressure
C) increasing the temperature
D) removing some oxygen
E) increasing the volume of the container
20) Lead ions can be precipitated from aqueous solutions by the addition of aqueous
iodide:
Pb2+ (aq) + 2I– (aq) → PbI2 (s)
Lead iodide is virtually insoluble in water so that the reaction appears to go to
completion. How many milliliters of 3.550 M HI(aq) must be added to a solution
containing 0.600 mol of Pb(NO3)2 (aq) to completely precipitate the lead?
A) 2.96 x 10-3
B) 338
C) 169
D) 0.169
E) 0.338
21) Calculate G o for the autoionization of water at 25 oC. Kw = 1.0 x 10-14
22) What are the three bond angles in the trigonal bipyramidal structure?
23) Clean rainwater is acidic mainly due to the presence of ________.
24) The three most concentrated ions in seawater are ________.
25) 1.035 X 10-4 L = ________ mL
26) Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF) and 0.180
M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 x 10-4.
27) Write the balanced equation for the reaction of potassium with water.
28) The electrical conductivity of ________ is low in the dark, but increases on
exposure to light.
29) Which noble gas has the lowest first ionization energy?