REDOX

Question 1

Oxidation number for elements by itself

Answer 1

0

Question 2

For monatomic ions:

Answer 2

Their oxidation number is equal to their charge

Question 3

All group 1 atoms (alkali metals) have an oxidation number of

Answer 3

+1

Question 4

Group 2 atoms (alkali earth metals) in compounds have an oxidation number of

Answer 4

+2

Question 5

Halogens in compounds have an oxidation number of

Answer 5

-1

Question 6

Aluminum has an oxidation number of

Answer 6

+3

Question 7

Hydrogen’s oxidation number is usually

Answer 7

+1

Question 8

Exception for oxidation # for hydrogen

Answer 8

When combined with a metal it is -1

Question 9

Oxidation number for oxygen

Answer 9

-2

Question 10

All atoms are neutral so oxidation #s must add to

Answer 10

0

Question 11

Trick to remember oxidation and reduction

Answer 11

O - oxidation
I - is
L - losing electrons

R - reduction
I - is
G - gaining electrons

Question 12

Oxidizing agent

Answer 12

Allows element to be oxidized

-BEING REDUCED

Question 13

Reducing agent

Answer 13

Allows an element to be reduced

-BEING OXIDIZED

Question 14

Metals (and non metals) that are more active will

Answer 14

Replace those that are below them on the table, in the compound
Thus, reaction occurs (its spontaneous)

Question 15

Oxidation half reaction:

Answer 15

Electrons lost must be shown on product side of equation

Question 16

Reduction half reaction:

Answer 16

Electrons gained must be shown on reactant side of equation

Question 17

Electrodes

Answer 17

Metal bars

Question 18

Salt Bridge

Answer 18

Keeps solutions neutral

Question 19

Half Cells

Answer 19

Have solutions of dissolved ions

Question 20

Voltaic Cells

Answer 20

• Spontaneous Reaction
• Electrons flow from the anode to the cathode
• Uses chemical energy to create electrical energy (batteries!)

Question 21

Anode

Answer 21

• Negatively charged electrode
• More active metal
• Metal atoms are oxidized (lose electrons)
• The electrode loses mass as atoms become ions and dissolve into the solution

Question 22

Cathode

Answer 22

• Positively charged electrode
• Less reactive metal
• Metal ions from the solution get reduced (gain electrons)
• The electrode gains mass as ions from the solution become atoms attached to the electrode

Question 23

Metals on Table J

Answer 23

• Higher up → more easily oxidized

- Lower down → least easily oxidized

Question 24

Non-metals on Table J

Answer 24

• Higher up → most easily reduced

- Lower down → least easily reduced

Question 25

Electrolytic Cell

Answer 25

• Nonspontaneous
• Uses a battery or source of energy (electrical energy is converted to chemical energy.) to force the reaction
• Anode becomes (+), cathode becomes (-) electrode

Question 26

Electrolysis

Answer 26

Negative ions (anions) migrate to the (+) anode

Positive ions (cations) migrate to the (-) cathode

Question 27

Which statement describes a benefit of using fission reactions?

Answer 27

Large amounts of energy are produced per mole of reactant

Question 28

Which information is sufficient to differentiate a sample of sodium from a sample of silver?

Answer 28

the reactivity of each sample with water