Chapter 19

Question 1

• often called “redox” reactions
• involves transfer of e- between reactants (oxidation numbers change)

Answer 1

Oxidation-Reduction Reactions

Question 2

loss of e-

Answer 2

oxidation

Question 3

gain of e-

Answer 3

reduction

Question 4

species that accepts e-

Answer 4

oxidizing agent (gets reduced)

Question 5

species that donates e-

Answer 5

reducing agent (gets oxidized)

Question 6

occurs because different elements gave different tendencies to gain or lose e-

Answer 6

redox reactions

Question 7

charge on an atom if e- were transferred completely
- another way that allows us to keep track of electrons

Answer 7

Oxidation numbers (oxidation state)

Question 8

• early work by Micheal Faraday (1830’s)
• amount of chemical change during electrolysis is directly proportional to amount of electrical charge that is passed thru wire

Answer 8

Stoichiometric Relationships in Electrolysis

Question 9

the use of electrical energy to drive non spontaneous chemical reaction is called

Answer 9

electrolysis

Question 10

the cell used to carry out electrolysis

Answer 10

electrolytic cell

Question 11

• have a reduction potential associated with it
• natural tendency to proceed as reduction

Answer 11

Each half reaction in a redox reaction can be considered to

Question 12

reduction potential for half reaction under standard conditions

Answer 12

standard reduction potential

Question 13

difference in electrical potential between anode and cathode

Answer 13

cell potential

Question 14

• electrical current flows from anode to cathode
• an electrical potential anergy difference between two electrodes
• analogous to flow of water down hill due to difference in gradational potential energy

Answer 14

standard reduction potentials

Question 15

device that use a chemical reaction to generate electricity and is a spontaneous reaction

Answer 15

Galvanic Cells (Voltaic Cells)