Multiple Choice (starred * problems are not material covered in class and
will not be on the final)
1. The basic unit of mass in the metric system is
a. liter
b. gram
c. meter
d. yard
2. 1 mile = 1.609 km. The distance between New York and Washington is 250 miles. This is the
same as
a. 600 km
b. 402 km
c. 155 km
d. 200 km
3. The density of ethyl alcohol is 0.789 g/mL. The mass of 2.00 liters of ethyl alcohol is
a. 1.580 g
b. 395 g
c. 2.53 kg
d. 1580 g
4. The law of conservation of energy states that
a. things in nature tend to seek the lowest possible potential energy
b. energy can neither be created nor destroyed
c. potential energy is stored energy
d. it is impossible to convert potential energy to kinetic energy
5. How many calories are required to heat 755 g of iron from 23 degrees C to 175 degrees C if
the specific heat of
iron is 0.11 cal/g deg?
a. 130 cal
b. 13 kcal
c. 56 cal
d. 1430 cal
6. 1 lb = 0.453 kg. If the recommended dosage of a prescribed drug is 2 mg/kg of body weight,
the amount of the drug that should be administered to a 12-pound infant is
a. 11 mg
b. 4 mg
c. 3 mg
d. 22 mg
7. The symbol for the element sodium is
a. K
b. S
c. Na
d. Sc
8. Which is a chemical change?
a. rusting of iron
b. making tea from a tea bag
c. distilling ocean water
d. melting of snow
9. Which elementary particles attract each other?
a. proton and neutron
b. electron and electron
c. proton and electron
d. electron and neutron
10. Which elementary particle has the smallest mass?
a. electron
b. neutron
c. proton
d. they all have the same mass
11. Mercury-202 has how many neutrons in its nucleus?
a. 22
b. 102
c. 122
d. 202
12. An ion with a mass number of 56 that contains 26 protons and 23 electrons is
a. Cr 2+
b. Fe 2+
c. Fe (3+)
d. Sb 2+
13. The ground state electronic configuration of silicon is
a. 1 s2 2 s2 2 p6 3 s2 3 p2
b. 1 s2 2 s2 2 p6 3 s4
c. 1 s2 1 p6 2 s2 2 p2
d. 1 s2 2 s2 3 s2 3 p4 4 s2
14. In the ground state of an atom
a. the energy of the electrons is at a maximum
b. the excited states are all filled
c. all the electrons are in their lowest energy levels
d. the protons and neutrons fill all the available energy states
15. The element strontium is most likely to form which of these ions?
a. Sr +
b. Sr 2+
c. Sr
d.Sr 216. The formula for the compound between potassium and sulfur is
a. KS
b. KS2
c. K2S
d. K2S3
17. A carbon atom forms how many bonds?
a. 2
b. 3
c. 4
d. 5
18. The Lewis structure of the CO2 molecule is
a. O = C = O
b. :: O =C = O::
c. O - C - O
d. :O -C - O:
19. Which of these molecules has a linear shape?
a. HCN
b. H2O
c. NH3
d. CH4
20. The compound iron(III) sulfite has the formula
a. Fe2(SO3)3
b. I2S3
c. FeS
d. Fe2S3
21. The formula weight of Ba(NO3)2 , to the nearest integer, is
a. 199 amu
b. 247 amu
c. 261 amu
d. 398 amu
22. 1.80 moles of CaSO4 weighs
a. 176 g
b. 38.4 g
c. 245 g
d. 245 kg
23. How many molecules are in a cube of dry ice (CO 2 ) that weighs 440 g?
a. 10
b. 1 x 1023
c. 6.02 x 1023
d. 6.02 x 1024
24. For the reaction
2P + 3Cl2 -----> 2PCl3
if 32.5 g of Cl2 reacts completely with excess P, how many g of PCl3 will be produced?
a. 42.0 g
b. 62.9 g
c. 83.9 g
d. 94.4 g
25. In this equation
AgNO3(aq) + NaCl(aq) ----> AgCl (s) + NaNO3(aq)
the spectator ions are
a. Ag+ and Clb.Na+ and Clc.Na+ and NO3 d. Ag+ and NO3 -
26. Which of these ionic compounds is soluble in water?
a. Pb(NO3)2
b. PbS
c. Pb(OH)2
d. PbCO3
27. In the reaction
2Mn2+ + Br2 ---> 2Mn(3+) + 2Br
the species that is oxidized is
a. Mn2+
b. Br2
c. Mn(3+)
d. Br28. A gas occupies 3.0 L at 20 oC and a pressure of 500 torr. What will be the new pressure if the
gas is heated to 100 oC and its volume is decreased to 1.2 L?
a. 1.6 x 103 torr
b. 6.3 x 103 torr
c. 1.2 atm
d. 8.2 atm
29. A gas is under 1.0 atm pressure in a balloon of 50.0 L volume at a temperature of 393 K. If
the gas is heated
to 500 K and the pressure drops to 0.75 atm, what will be the new volume of the balloon?
a. 0.20 mL
b. 8.5 L
c. 9.5 L
d. 85 L
30. Which of these gases will diffuse the fastest?
a. CO
b. CH4
c. H2O
d. CO2
31. The molecules of which of these compounds exhibit hydrogen bonding?
a. CH4
b. NO2
c. NH3
d. CO
32. The solubility of a gas in a liquid mostly
a. increases with increasing temperature
b. increases with decreasing pressure
c. is unaffected by pressure
d. decreases with increasing temperature
33. 20 g of NaBr is dissolved in enough water to make 250 mL of solution. The percent (w/v)
concentration of the
solution is
a. 0.4%
b. 0.8%
c. 2.0%
d. 8.0%
34. When 4.0 g of NaOH is dissolved in 50 mL of aqueous solution the molarity of the solution is
a. 1.0 M
b. 2.0 M
c. 0.10 M
d. 0.20 M
35. Which of these is the least soluble in water?
a. NaCl
b. KI
c. C2 H6
d. CH3OH
36. Fog is an example of a colloidal system in which
a. a liquid is dispersed in a liquid
b. a gas is dispersed in a liquid
c. a liquid is dispersed in a gas
d. a gas is dispersed in a gas
37. Hypertonic solutions cause
a. red blood cells to shrivel
b. red blood cells to burst
c. hemolysis of red blood cells
d. no effect on red blood cells
*38. Activation energy
a. is the energy necessary for a reaction to take place, when molecules collide
b. is the energy of the collision of a molecule with the walls of the container
c. is a concept that applies only to gases
d. is the energy necessary to activate an acid or base
*39. If a reaction takes 8 hours to go to completion at 15 degrees C, approximately how long will it
take at 45 degrees C?
a. 1 hr
b. 2 hr
c. 8 hr
d. 64 hr
*40. When a reaction reaches equilibrium
a. all reaction ceases
b. the rate of the reverse reaction becomes zero
c. the concentration of reactants and products are equal
d. the rate of the forward reaction equals the rate of the reverse reaction
*41. The equilibrium expression for this reaction
2H2O + CH4 < ====> CO2 + 4H2
is
a. K eq = [H2O]2 [CH4] / [CO2][H2]4
b. K eq = [H2O]2 + [CH4] / [CO2] + [H2]4
c. Keq = [CO2][H2]4 / [H2O]2 [CH4]
d. Keq = [CO2] + [H2]4 / [H2O]2 + [CH4]
*42. The following are equilibrium constants for some reactions. In which is formation of products
most favored?
a. 1.0
b. 23.5
c. 0.25
d. 3 x 10-3
43. If, in the reaction S + O2 ---> SO2
the SO2 is constantly removed by allowing it to react with water, the removal of SO 2 will
a. shift the equilibrium to the left
b. shift the equilibrium to the right
c. speed up the rate of the reaction
d. have no effect on the position of equilibrium
*44. The conjugate base of water is
a. OH b.H2 O
c. H+
d. H3O+
45. Which of these is not a strong acid?
a. HCl
b. H2S
c. HNO3
d. H2SO4
*46. Given the ionization constants, which of these is the strongest acid?
a. HCOOH, 1.8 x 10-4
b. HF, 3.5 x 10-4
c. H2 CO3 , 4.3 x 10-7
d. H3BO3 , 7.3 x 10-10
*47. A solution with a [H3O+ ] of 0.0001 M has a pH of
a. 4
b. 5
c. 7
d. 10
*48. If the [OH- ] of a solution is 1 x 10-1 M , the pH of the solution is
a. 1
b. 10
c. 13
d. 14
*49. The pH of an 0.1 M solution of KCl is approximately
a. 1
b. 5
c. 7
d. 9
*50. Which of these, if dissolved in 1.0 L of pure water, will produce a buffer solution?
a. 0.1 mole NaCl + 0.1 mole KCl
b. 0.1 mole HO+ + 0.1 mole OHc. 0.1 mole NaH2PO4 + 0.1 mole Na2HPO4
d. 0.1 mole HCl + 0.1 mole KCl
*51. Which form of radiation penetrates the human skin?
a. radio waves
b. alpha particles
c. gamma rays
d. microwaves
52. An alpha particle is a nucleus of which of these isotopes?
a. hydrogen-1
b. hydrogen-2
c. helium-4
d. carbon-12
53. Po-194 is an alpha emitter. The product is
a. polonium-190
b. lead-194
c. lead-190
d. astatine-194
*54. Tellurium-132 has a half-life of 78 hours. If you have a sample of 184 mg of this isotope, how
much will be left
after 13 days?
a. 11.5 mg
b. 23 mg
c. 46 mg
d. 138 mg
55. A substance that changes color at a certain pH is called
a. a buffer
b. an indicator
c. a conjugate acid
d. a salt
*56. For the reaction
N2 + 3H2 ----> 2NH3
the equilibrium concentrations, in moles/L, were found to be: [N2] = 0.5, [H2] = 1.0, [NH3] = 2.0.
The equilibrium
constant for this reaction is
a. 0.25
b. 4
c. 8
d. 16
57. When sugar is dissolved in water, the sugar is the
a. solute
b. solution
c. solvent
d. colloid
58. The units of the universal gas constant, R = 0.0821 are
a. L atm/ C mole
b. L atm/K mole
c. L torr/K mole
d. mL torr/ C mole
59. When this equation is properly balanced
C H4 + O2 ----> CO2 + H2O
the coefficient of O2 is
a. 2
b. 3
c. 4
d. 5
60. When a solution of H2SO4 is added to a solution of Na2CO3 , the gas CO2 is release
d. A balanced net ionic equation for this process is
a. 2Na+ + SO4 ----> Na2 SO4
b. H2SO4 + Na2CO3 ------> CO2 + Na2SO4 + H2 O
c. 2H+ + CO3 (2-) ------> CO2(g) + H2O (liquid)
d. H+ + CO3(2-) -------> CO2(g) + OH
ANSWER KEY FOR TEST
1. b
2. b
3. d
4. b
5. b
6. a
7. c
8. a
9. c
10. a
11. c
12. c
13. a
14. c
15. b
16. c
17. c
18. b
19. a
20. a
21. c
22. c
23. c
24. a
25. c
26. a
27. a
28. a
29. d
30. b
31. c
32. d
33. d
34. b
35. c
36. c
37. a
38. a
39. a
40. d
41. c
42. b
43. b
44. a
45. b
46. b
47. a
48. c
49. c
50. c
51. c
52. c
53. c
54. a
55. b
56. c
57. a
58. b
59. a
60. c