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Chemistry / Chemical Reactions / Redox Reaction

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Redox Reaction

Oxidation Reaction:

It can be defined as:

The process in which oxygen is added to a substance.

The process in which a substance loses electron(s).

e.g. $(i);2Cu+O_{2}overset{Heat}{rightarrow}2CuO$

Copper + Oxygen $rightarrow$ Copper oxide

$(ii);2H_{2}S+O_{2}rightarrow 2S+2H_{2}O$

Hydrogen + Oxygen $rightarrow$ Suphur + Hydrogen oxide

Sulphide

$(iii);Znrightarrow Zn^{2+}+2e^{-}$

Zinc

Reduction Reaction:

It is defined as:

The process in which oxygen is removed from a substance.

The process in which hydrogen is added to a substance.

The process in which a substance gains electron(s).

e.g. $(i);2KClO_{3}(s)overset{Delta }{rightarrow}2KCl(s)+3O_{2}(g)$

Potassium $rightarrow$ Potassium Oxygen

Chlorate chloride

$(ii);2Na+H_{2}rightarrow 2NaH$

Sodium + Hydrogen $rightarrow$ Sodium hydride

$(iii);Zn^{2+}+2e^{-}rightarrow Zn$

Zinc

Some Facts:

If a substance gains oxygen during a reaction, it is said to be oxidised. If a substance loses oxygen during a reaction, it is said to be reduced.

Redox Reactions

Those reactions in which oxidation and reduction take place simultaneously, are called redox reactions.

e.g.

(i) In the following reaction, the copper (II) oxide is losing oxygen and is being reduced. Whereas, oxygen is added to hydrogen and is being oxidised.

$CuO+H_{2}overset{Heat}{rightarrow}Cu+H_{2}O$

Copper oxide + Hydrogen $rightarrow$ Copper + Water

(ii) In the following reaction HCl is oxidised to $Cl_{2}$ whereas, $MnO_{2}$ is reduced to $MnCl_{2}.$

$MnO_{2}(s)+4HClrightarrow MnCl_{2}(aq)+Cl_{2}(g)+2H_{2}O$

(Conc.)

Oxidizing Agent

The substance which oxidizes elements or compound is known as an oxidizing agent.

(i) Oxygen is an oxidizing agent. It oxidises iron (Fe) to ferric oxide $(Fe_{2}O_{3}).$

$4Fe+3O_{2}rightarrow 2Fe_{2}O_{3}$

(ii) Potassium permanganate solution is an oxidizing agent. It oxidizes ferrous suphate to ferric sulphate.

Reducing Agent

The substance which reduces compounds is known as a reducing agent.

(i) Hydrogen is a reducing agent. It reduces cupric oxide to copper (Cu).

$CuO+H_{2}rightarrow Cu+H_{2}O$

Cupric oxide + Hydrogen $rightarrow$ copper + water

(ii) Stannous chloride is a reducing agent. It reduces ferric chloride to ferrous chloride.

$SnCl_{2}+2FeCl_{2}rightarrow SnCl_{2}+2FeCl_{2}$

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