Workbook - Oxidation Reduction KEY

Define each

1. Oxidation

2. Reduction

3. Oxidizing agent

4. Reducing agent

- loss of electrons

- gain of electrons

- causes oxidation by undergoing reduction

- causes reduction by undergoing oxidation

Write half reactions for each of the following atoms or ions. Label each as oxidation or

reduction.

Al3+

3e-

5.

Al

----------->

6.

S

+

7.

2O2-

---------->

8.

Ba2+

+ 2e- -----------> Ba

9.

2N3-

---------->

10.

Br2

+

11.

P +

12.

Ca

----------->

13

Ga3+

+ 3e- -----------> Ga

14.

S

+

15.

H2

--------->

16.

2H+

+ 2e- ---------> H2

17.

2F-

---------->

F2

18.

P3-

---------->

P +

2e-

2e3e-

+

O2

N2

reduction

4e-

+

--------->

oxidation

reduction

6e-

oxidation

2Br-

reduction

+

P3-

---------->

2e-

S2-

--------->

Ca2+

reduction

2e-

+

oxidation

reduction

S2-

reduction

+ 2e-

oxidation

--------->

2H+

oxidation

reduction

2e-

+

oxidation

3e-

oxidation

Balance each spontaneous redox equation. Identify the entities reduced and oxidized.

State the reducing agent and the oxidizing agent.

19. Al

&

Zn2+

2Al +

oxidized

reducing agent

3Zn2+

¡ú

reduced

oxidizing agent

2Al3+ +

3Zn

20. F2

&

O2-

2F2

+

reduced

oxidizing agent

21. O2

&

&

4F-

+

O2

Ca

2Ca +

oxidized

reducing agent

22. Al3+

2O2¡ú

oxidized

reducing agent

O2

¡ú

reduced

oxidizing agent

2Ca2+ +

2O2-

+

3Li+

Li

Al3+ +

reduced

oxidizing agent

3Li

¡ú

oxidized

reducing agent

Al

Label the species that is reduced, that is oxidized, the reducing agent and the oxidizing

agent.

Fe2+

23.

+

Co

¡ú

Co2+

+ 2e- oxidation

Co2+

+

Fe

Co

2e-

¡ú

+

¡ú Fe reduction

3 Ag+

24.

Fe2+

+

Ni

¡ú

Ni2+

+ 2e-

oxidation

Ni3+

+

3 Ag

Ni

1e-

¡ú

¡ú Agreduction

Ag+

+

Cu2+

25.

+

Pb

¡ú

Pb2+

+ 2e-

oxidation

Pb2+

+

Cu

Pb

2e-

26.

¡ú

¡ú Cu

reduction

O2

+

2 Sn

¡ú

Sn2+

+ 2e-

oxidation

Cu2+

O2-

+

+

2 Sn2+

+

Sn

¡ú

4e-

¡ú 2O2-

Co2+

27.

O2

reduction

+

2 F-

¡ú

F2

+ 2e-

oxidation

Co

+

F2

2F+ 2e-

¡ú

¡ú Coreduction

28. List the species (formulas from above) that lose electrons:

Co

Ni

Pb

Sn

F-

29. List the species (formulas from above) that gain electrons:

Fe2+

Ag+

Cu2+

O2

Co2+

Co2+

For each of the following reactions, identify:

-The Oxidizing Agent.

-The Reducing Agent.

-The Substance Oxidized.

-The Substance Reduced.

30.

I-

+

Cl2

Substance oxidized

Oxidizing agent

31.

Co

+

Fe3+

Substance oxidized

Oxidizing agent

32.

Cr6+

+

Cl-

---------->

Fe2+

I2

ICl2

Reducing agent

Substance reduced

----------->

Co2+

Co

Fe3+

Fe2+

Cr6+

+

Co

Fe3+

Cr3+

Fe3+

+

Reducing agent

Substance reduced

Redox Half Reactions and Reactions WS #2

1. State the Oxidation Number of each of the elements that is underlined.

a) NH3

c) ZnSO3

e) Na

g) AgNO3

i) SO2

k) Ca(ClO3)2

m) HPO32o) MnO2

q) PbO2

s) K2SO4

u) Na2O2

w) Fe2O3

y) NaIO3

-3

4

0

5

4

5

3

4

4

6

-1

3

5

Fe2+

Reducing agent

Substance reduced

----------->

Substance oxidized

Oxidizing agent

+

b) H2SO4

d) Al(OH)3

f) Cl2

h) ClO4j) K2Cr2O4

l) K2Cr2O7

n) HClO

p) KClO3

r) PbSO4

t) NH4+

v) FeO

x) SiO44z) ClO3-

6

3

0

7

3

6

1

5

2

-3

2

-2

5

Fe2+

Cr6+

ICl2

aa) NO3cc) CaH2

ee) Fe(H2O)63+

5

-1

+3

bb) Cr(OH)4

dd) Pt(H20)5(0H)2+

ff) CH3COOH

4

+3

0

2. What is the oxidation number of carbon in each of the following substances?

a) CO

2

b) C

0

2c) CO2

4

d) CO3

4

e) C2H6

-3

f) CH3OH

-2

3. For each of the following reactions, identify: the oxidizing agent, the reducing agent,

the substance oxidized and the substance reduced.

a) Cu2+ (aq)

Cu2+

+

Zn (s)

-------->

Substance oxidized

Cu (s) +

Zn

b) Cl2 (g)

+

Substance reduced

Cu2+

Oxidizing agent

Zn

2 Na (s) -------->

Substance oxidized

Zn2+ (aq)

Reducing agent

2 Cl- (aq)

2 Na+ (aq)

+

Na

Substance reduced

Cl2

Oxidizing agent

Na

WS # 3

Cl2

Reducing agent

Spontaneous and Non-spontaneous Redox Reactions

Describe each reaction as spontaneous or non-spontaneous.

1. Au+3 + Fe+3

oxidizing agents)

Fe+3

2. Pb

+

3. Cl2

+

4. S2O8-2

5.Cu+2

6. Sn+2

+

+

Fe+2

+

------>

Fe+2

------>

F2

Pb

------>

2SO4-2

2Br-

------>

Cu

Br2

------>

Sn+4

F+

----->

Au

Pb+2

+

+

2Cl+ Pb+2

+ Br2

+ 2Br-

nonspontaneous (two

spontaneous

nonspontaneous

spontaneous

nonspontaneous

spontaneous

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