[PDF] Chemistry 30 Unit 6: Redox Reactions and Electrochemistry Answers





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Jun 28 2010 · Chapter 20 Worksheet: Redox ANSWERS I Determine what is oxidized and what is reduced in each reaction Identify the oxidizing agent and the reducing agent also 1 2Sr + O2 2SrO Sr 0 to Sr2+; oxidized/reducing agent O0 to O2-; reduced/ox ag 2 2Li + S Li2S Li 0 to Li1+; oxidized/red ag S0 to S2-; reduced/ox ag 3

What is the difference between redox and electrochemistry?

    Electrochemistry is the study of how chemical reactions produce electrical energy and in turn how electrical energy causes chemical reactions. These chemical reactions involve transfer of electrons. A redox reaction is one in which reduction and oxidation processes occur simultaneously. Redox reactions involve electron gain and electron loss.

What are redox reactions?

    Any such reaction involves both a reduction process and a complementary oxidation process, two key concepts involved with electron transfer processes. Redox reactions include all chemical reactions in which atoms have their oxidation state changed; in general, redox reactions involve the transfer of electrons between chemical species.

How do you balance a redox reaction?

    There are two ways of balancing the redox reaction. One method is by using the change in oxidation number of oxidizing agent and the reducing agent, and the other method is based on dividing the redox reaction into two half reactions-one of reduction and another of oxidation.

What is the difference between a cathode and anode redox reaction?

    Each half-reaction that makes up a redox reaction has a standard electrode potential. This potential equals the voltage produced by an electrochemical cell in which the cathode reaction is the half-reaction considered, whereas the anode is a standard hydrogen electrode.

Chemistry 30

Unit 6: Redox Reactions and Electrochemistry Answers Practice Set 1: Oxidation Numbers and Redox Reactions

1. Determine the oxidation number of each element in the following compounds.

Rules: 1. Pure elements have an oxidation number of 0

2. If the compound is an ionic compound, the oxidation number for each element is the ion's

charge

3. The oxidation number of hydrogen in a compound is +1

4. The oxidation number of oxygen in most compounds is -2

(peroxides are the exception; in peroxides oxygen has an oxidation number of -1)

5. The sum of the oxidation numbers in a compound is zero.

6. The sum of the oxidation numbers in a polyatomic ion is equal to the ion charge.

Hint

Oxidation Numbers for each Element

a. SnCl 4

Rule 2

Sn +4 Cl -1

b. Ca 3 P 2

Rule 2

Ca +2 P -3

c. SnO

Rules 4, 5

Sn +2 O -2

d. Ag 2 S

Rule 2

Ag +1 S -2

e. HI

Rule 3, 5

H +1 I -1

f. N 2 H 4

Rule 3, 5

N -2 H +1 watch the sign for N!

g. Al 2 O 3

Rule 4, 5

Al +3 O -2

h. S 8

Rule 1

S 0 i. HNO 2

Rules 3, 4, 5

H +1 N +3 O -2

j. O 2

Rule 1

O 0 pure element!

k. H 3 O

Rules 3, 4, 6

H +1 O -2 surprised?

l. ClO 3

Rules 4, 6

Cl +5 O -2

m. S 2 O 3 2-

Rules 4, 6

S +2 O -2

n. KMnO 4

Rules 4, 5, 6

K +1 Mn +7 O -2

o. (NH 4 2 SO 4

Rules 4, 5, 6

N -3 H +1 S +6 O -2

Unit 6: Redox & Electrochemistry Practice Set 1 Page 1 of 2 Unit 6: Redox & Electrochemistry Practice Set 1 Page 2 of 2

Extra help for KMnO

4 & (NH 4 2 SO 4 You will need to recognize polyatomic ions. It will simplify determining oxidation numbers to break molecules with polyatomic ions into two separate ions, then find oxidation numbers for each part separately. KMnO 4 K

Oxidation Number = +1

MnO 4 oxygen's oxidation number = -2 4 oxygens total = -8 sum of ox. nos. for MnO 4 -1 therefore oxidation number of Mn +7 (NH 4 2 SO 4 NH 4 Hydrogen's oxidation number = +1 4 hydrogens total = +4 charge of ammonium ion +1 therefore oxidation number of N -3

Note - there are two NH

4 ions, but the oxidation numbers in both will be the same! SO 4 2- oxygen's oxidation number = -2 4 oxygens total = -8 charge of sulfate ion -2 therefore oxidation number of S +6

2. Determine the oxidation number of carbon in each of the following compounds:

a. methane, CH4 b. formaldehyde, CH 2 O

C = -4 C = 0

element Ox.

No. No.

Atoms

Total element

Ox.

No. No.

Atoms Total

H +1 4 +4 H +1 2 +2

C -4 1 -4 O -2 1 -2

SUM 0 C 0 1 0

SUM 0

c. carbon monoxide, CO d. carbon dioxide, CO 2

C = +2 C = +4

element Ox.

No. No.

Atoms

Total element

Ox.

No. No.

Atoms Total

O -2 1 -2 O -2 2 -4

C +2 1 +2 C +4 1 +4

SUM 0 SUM 0

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