1) What type of reaction is known as a thermonuclear reaction?
A) fission
B) fusion
C) transmutation
D) beta emission
E) neutron emission
2) In a px orbital, the subscript x denotes the ________.
A) energy of the electron
B) spin of the electrons
C) probability of the shell
D) size of the orbital
E) axis along which the orbital is aligned
3) The order of the reaction in B is ________.
A) 1
B) 2
C) 3
D) 4
E) 0
4) Which halogen forms an oxyacid with the formula HXO2?
A) bromine
B) fluorine
C) chlorine
D) iodine
E) astatine
5) In a solution, when the concentrations of a weak acid and its conjugate base are
equal, ________.
A) the system is not at equilibrium
B) the buffering capacity is significantly decreased
C) the -log of the [H+] and the -log of the Ka are equal
D) All of the above are true.
6) Which choice is not one of the Ionic Constituents of seawater typically present in
concentrations greater than 1 ppm?
A) ClO4
–
B) Sr2+
C) Na+
D) H3Bo3
E) Cl–
7) Which of these metals is the least easily oxidized?
Na
Au
Fe
Ca
Ag
A) Na
B) Au
C) Fe
D) Ca
E) Ag
8) The element that has a valence configuration of 2s1 is ________.
A) Li
B) Na
C) K
D) Rb
E) Cs
9) Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide:
PbCO3 (s) → PbO (s) + CO2 (g)
How many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of
lead (II) carbonate?
A) 0.41
B) 2.50
C) 0.00936
D) 2.09
E) 2.61
10) A metal complex absorbs light mainly at 420 nm. What is the color of the complex?
A) green
B) yellow
C) red
D) orange
E) purple
11) A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight =
101 g/mol) in enough water to make 1.00 L of solution. The osmotic pressure of the
solution is 1.25 atm at 25.0 oC. What is the van’t Hoff factor (i) for the unknown solute?
A) 0
B) 0.99
C) 1.98
D) 2.98
E) 0.630
12) The type of compound that is most likely to contain a covalent bond is ________.
A) one that is composed of a metal from the far left of the periodic table and a nonmetal
from the far right of the periodic table
B) a solid metal
C) one that is composed of only nonmetals
D) held together by the electrostatic forces between oppositely charged ions
E) There is no general rule to predict covalency in bonds.
13) The white allotropic form of ________ bursts into flame when exposed to air.
A) phosphorus
B) carbon
C) sulfur
D) selenium
E) oxygen
14) This element is more reactive than lithium and magnesium but less reactive than
potassium. This element is ________.
A) Na
B) Rb
C) Ca
D) Be
E) Fr
15) How many equivalent resonance forms can be drawn for CO3
2-? (Carbon is the
central atom.)
A) 1
B) 2
C) 3
D) 4
E) 0
16) The charge on the copper ion in the salt CuO is ________.
A) +1
B) +2
C) +4
D) +3
E) +5