Self Quiz

NOTE: Use an SOP list with the quiz.

1. Which of the following chemicals can be oxidized most easily?

a. Na
b. Mg
c. Cl₂
d. F^-
e. Al³⁺

2. Which of the following is/are oxidation-reduction reactions?

a. Mg + 2H⁺ = Mg²⁺ + H₂
b. N₂ + O₂ = 2NO
c. NaCl + AgNO₃ = AgCl + NaNO₃
d. (a) and (b)
e. (a), (b) and (c)

3. Oxidation and reduction must take place at the same time because electrons are:

a. gained.
b. lost.
c. transferred.

4. What voltage could a cell generate (under ideal conditions) using the following reaction?

3 Mg + 2 AlCl₃ 3 MgCl₂ + 2 Al

a. -4.03 v
b. -0.71 v
c. +0.71 v
d. +3.79 v
e. +4.03 v

5. Electrolytic cells:

1. can be used to force reactions that do not occur spontaneously.

2. need an external source of electricity.

3. can be used for electroplating.

a. only one of these
b. 1 and 2
c. 1 and 3
d. 2 and 3
e. all of these

6. Which of the following combinations will react in a spontaneous oxidation-reduction reaction?

a. Zn + Zn²⁺
b. Cr + Fe
c. Cd + Ni²⁺
d. Sn + Fe²⁺
e. Ag⁺ + Br₂

7. The gain of electrons is called:

a. oxidation.
b. oxidation-reduction.
c. redox.
d. reduction.
e. none of the above.

8. If two copper electrodes are put into a silver nitrate solution and a current is run through the cell, what will happen at the anode?

a. Copper will plate out.
b. Silver will plate out.
c. Copper will go into solution.
d. Silver will go into solution.

9. In what kind of cell would this reaction occur?

2 Al + 3 CuCl₂ 2 AlCl₃ + 3 Cu

a. anodic
b. cathodic
c. electrolytic
d. hypnotic
e. voltaic

10. Diagram a voltaic cell using this reaction:  Ni + Pb²⁺ Pb + Ni²⁺.

Indicate the placement of the chemicals, the location of the electron flow, and the half reaction occurring at each electrode.