Electrochemistry

Question 1

Oxidation

Answer 1

loss of an electron
gain of oxygen
increase in oxidation number
loss of a hydrogen

Question 2

Reduction

Answer 2

Gain of an electron
decrease in oxidation number
loss of an oxygen
gain of a hydrogen

Question 3

Oxidant

Answer 3

Causes another species in reaction to be oxidised

Question 4

reductant

Answer 4

causes other species in reaction to be reduced

Question 5

Oxidation rule 1

Answer 5

The sum of all the oxidation numbers in any substance is equal to the total charge. This means that the elemental form will always have an oxidation number of zero.

Question 6

Oxidation rule 2

Answer 6

Fluorine has an oxidation number of -1 in compounds.​

Question 7

Oxidation rule 3

Answer 7

Group 1 metals are +1 in compounds, while Group 2 metals are +2 in compounds.​

Question 8

Oxidation rule 4

Answer 8

When H is bonded to non-metals it has an oxidation number of +1.​

When H is bonded to a metal it has an oxidation number of -1 (Hydride ion = H-).​

Question 9

Oxidation rule 5

Answer 9

Oxygen usually has an oxidation number of -2 in compounds. However, in peroxides, it has an oxidation number of -1.​