1) To convert from one resonance structure to another, ________.
A) only atoms can be moved
B) electrons and atoms can both be moved
C) only electrons can be moved
D) neither electrons nor atoms can be moved
E) electrons must be added
2) Oxygen is a ________ and nitrogen is a ________.
A) metal, metalloid
B) nonmetal, metal
C) metalloid, metalloid
D) nonmetal, nonmetal
E) nonmetal, metalloid
3) The equilibrium constant for the gas phase reaction
N2 (g) + 3H2 (g) 2NH3 (g)
is Keq = 4.34 x 10-3 at 300 oC. At equilibrium, ________.
A) products predominate
B) reactants predominate
C) roughly equal amounts of products and reactants are present
D) only products are present
E) only reactants are present
4) How many sulfur dioxide molecules are there in 0.180 mol of sulfur dioxide?
A) 1.80 x 1023
B) 6.02 x 1024
C) 6.02 x 1023
D) 1.08 x 1024
E) 1.08 x 1023
5) Elements from opposite sides of the periodic table tend to form ________.
A) covalent compounds
B) ionic compounds
C) compounds that are gaseous at room temperature
D) homonuclear diatomic compounds
E) covalent compounds that are gaseous at room temperature
6) The element that has a valence configuration of 2s2 is ________.
A) Be
B) Mg
C) Ca
D) Sr
E) Ba
7) When argon is placed in a container of neon, the argon spontaneously disperses
throughout the neon because ________.
A) of the large attractive forces between argon and neon atoms
B) of hydrogen bonding
C) a decrease in energy occurs when the two mix
D) the dispersion of argon atoms produces an increase in disorder
E) of solvent-solute interactions
8) The hydride ion, H–, is a stronger base than the hydro xide ion, OH–. The product(s)
of the reaction of hydride ion with water is/are ________.
A) H3O+ (aq)
B) OH– (aq) + H2 (g)
C) OH– (aq) + 2H+ (aq)
D) no reaction occurs
E) H2O2 (aq)
9) What is the missing product from this reaction?
P –> S + _____
A) He
B) e
C) ³
D) e
E) p
10) There are ________ molecules of methane in 0.123 mol of methane (CH4).
A) 5
B) 2.46 x 10-2
C) 2.04 x 10-25
D) 7.40 x 1022
E) 0.615
11) The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ) released
to the surroundings when 10.0 g of CO (g) reacts completely.
2CO (g) + O2 (g) → 2CO2 (g)
A) 2410 kJ
B) 172 kJ
C) 86.0 kJ
D) 482 kJ
E) -482 kJ