1) Which compound would produce an acidic aqueous solution?
A) HF
B) MgH2
C) C2H2
D) KH
E) H2
2) Ka for HF is 7.0 x 10-4. Kb for the fluoride ion is ________.
A) 2.0 x 10-8
B) 1.4 x 10-11
C) 7.0 x 10-18
D) 7.0 x 10-4
E) 1.4 x 103
3) An aqueous solution of ________ will produce an acidic solution.
A) NH4I
B) KBr
C) Sr(ClO4)2
D) K2CO3
E) NaNO3
4) Lattice energy is ________.
A) the energy required to convert a mole of ionic solid into its constituent ions in the
gas phase
B) the energy given off when gaseous ions combine to form one mole of an ionic solid
C) the energy required to produce one mole of an ionic compound from its constituent
elements in their standard states
D) the sum of ionization energies of the components in an ionic solid
E) the sum of electron affinities of the components in an ionic solid
5) The atomic mass unit is presently based on assigning an exact integral mass (in amu)
to an isotope of ________.
A) hydrogen
B) oxygen
C) sodium
D) carbon
E) helium
6) The primary commercial use of oxygen is ________.
A) for the treatment of respiratory distress
B) in oxyacetylene welding
C) as a household bleach
D) as an oxidizing agent
E) to charge oxygen-containing cylinders used by deep-sea divers
7) The addition of hydrochloric acid and ________ to water produces a buffer solution.
A) HC6H5O
B) NaOH
C) NaCl
D) C2H5NH2
E) none of the above
8) ________ hybrid orbitals are used for bonding by Xe in the XeF4 molecule.
A) sp2
B) sp3
C) sp3d
D) sp3d2
E) sp
9) What is the pOH of an aqueous solution at 25.0 oC in which [OH–] is 0.0010 M?
A) 11.00
B) -3.00
C) 3.00
D) -11.00
E) 6.91
10) A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M
NaOH solution. The titration curve above was obtained. The unknown compound is
________.
A) a strong acid
B) a strong base
C) a weak acid
D) a weak base
E) neither an acid nor a base
11) A 255 mL round-bottom flask is weighed and found to have a mass of 114.85 g. A
few milliliters of an easily vaporized liquid are added to the flask and the flask is
immersed in a boiling water bath. All of the liquid vaporizes at the boiling temperature
of water, filling the flask with vapor. When all of the liquid has vaporized, the flask is
removed from the bath, cooled, dried, and reweighed. The new mass of the flask and
the condensed vapor is 115.23 g. Which of the following compounds could the liquid
be? (Assume the ambient pressure is 1 atm.)
A) C4H10
B) C3H7OH
C) C2H6
D) C2H5OH
E) C4H9OH
12) The lime-soda process is used for large-scale water-softening operations. CaO is
added to ________.
A) oxidize Fe2+ to insoluble Fe2O3
B) cause precipitation of magnesium as Mg(OH)2
C) remove most Al3+ as solid Al(OH)3
D) cause precipitation of iron and magnesium as Fe2MgO4
E) reduce the pH to 3-4
13) Of the following, ________ contains the greatest number of electrons.
A) P3+
B) P
C) P2-
D) P3-
E) P2+
14) Which electron configuration represents a violation of Hund’s rule for an atom in its
ground state?
A)
B)
C)
D)
E)
15) What color of visible light has the longest wavelength?
A) blue
B) violet
C) red
D) yellow
E) green
16) One million argon atoms is ________ mol (rounded to two significant figures) of
argon atoms.
A) 3.0
B) 1.7 x 10-18
C) 6.0 x 1023
D) 1.0 x 10-6
E) 1.0 x 106
17) Which electron configuration represents a violation of the Pauli exclusion
principle?
A)
B)
C)
D)
E)
18) The wavelength of light that has a frequency of 1.20 X 1013 s-1 is ________ m.
A) 25.0
B) 2.50 X 10-5
C) 0.0400
D) 12.0
E) 2.5
19) Which ions are spectator ions in the formation of a precipitate of AgCl via
combining aqueous solutions of CoCl2 and AgNO3?
A) Co2+ and NO3
–
B) NO3
– and Cl–
C) Co2+ and Ag+
D) Cl–
E) NO3
–
20) How many quantum numbers are necessary to designate a particular electron in an
atom?
A) 3
B) 4
C) 2
D) 1
E) 5