Oxidation reduction reactions
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Oxidation-Reduction Reactions. Oxidation-reduction (redox) reactions are those in which one or more electrons are transferred. Remember that the sum of the oxidation states in a neutral compound must equal zero and must be equal to the overall charge in an ionic compound .

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Oxidation-Reduction Reactions

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Oxidation reduction reactions

Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions are those in which one or more electrons are transferred.

Remember that the sum of the oxidation states in a neutral compound mustequal zero and must be equal to the overall charge in an ionic compound.

Assign oxidation states to each of the atoms in the following compounds:

a. FeF2b. H2O c. KMnO4

d. C2H6e. ICl5 f. SO42-

K = +1, Mn = +7, O = -2

Fe = +2, F = -1

H = +1, O = -2

1(+2)

2(-1)

2(+1)

1(-2)

1(+1)

+7

4(-2)

I = +5, Cl = -1

C = -3, H = +1

S = +6, O = -2

2(-3)

6(+1)

+5

5(-1)

+6

4(-2) +2

Assign oxidation states to each atom in the equation.

Fe2O3 + 2 Al  Al2O3 + 2 Fe

Fe gains electrons. It has been REDUCED

+3

-2

0

+3

-2

0

Al lost electrons. It has been OXIDIZED


Oxidation reduction reactions

Remember LEO GER:LOSE ELECTRONS OXIDATION

GAIN ELECTRONS REDUCTION

Something that is reduced is called an oxidizing agent.

Something that is oxidized is called a reducing agent.

For each reaction, identify that atoms that undergo reduction, or oxidation.

  • 2 H2(g) + O2(g) 2 H2O (g)

  • Zn (s) + Cu2+(aq) Zn2+(aq) + Cu (s)

  • 2 AgCl(s) + H2(g) 2 H+(aq) + 2 Ag (s) + 2 Cl-(aq)

    d. 2 MnO4-(aq) + 16 H+(aq) + 5 C2O42-(aq) 2 Mn2+(aq) + 10 CO2(g) + 8 H2O(l)

oxidized: hydrogen (0 to +1)

reduced: oxygen (0 to -2)

0

0

+1

-2

oxidized: zinc (0 to +2)

reduced: copper (+2 to 0)

0

+2

+2

0

+1

-1

0

+1

0

-1

oxidized: hydrogen (0 to +1)

reduced: silver (+1 to 0)

+7

-2

+1

+3

-2

+2

+4

-2

+1

-2

oxidized: carbon (+3 to +4)

reduced: manganese (+7 to +2)


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