Question

Separate this redox reaction into its balanced component half-reactions. What is the oxidation and reduction half reactions
Cl2 + 2Cs yields 2CsCl

Answer 1

Answer:

The reduction reaction is: Cl₂ + 2 e⁻ ⇄ 2 Cl⁻

The oxidation reaction is: Cs ⇄ Cs⁺ + 1 e⁻

Explanation:

In a redox reaction, two half-reactions happen simultaneously. The oxidation refers to a species losing electrons. The reduction refers to a species gaining electrons.

Let's consider the following reaction.

Cl₂ + 2 Cs ⇄ 2CsCl

We can write the ionic equation.

Cl₂ + 2 Cs ⇄ 2 Cs⁺ + 2 Cl⁻

The reduction reaction is: Cl₂ + 2 e⁻ ⇄ 2 Cl⁻

We added 2 electrons to the left (electrons gained) to balance the half-reaction electrically.

The oxidation reaction is: Cs ⇄ Cs⁺ + 1 e⁻

We added 1 electron to the right (electrons lost) to balance the half-reaction electrically.

Answer 2

The redox reaction involves the electron transfer between the species. In reduction, the electrons are gained, while in oxidation the electrons are lost.

What is reduction-oxidation?

In reduction reactions, the chemical species gains electrons, whereas, in oxidation reactions, the electrons are donated or lost by the chemical species.

The overall balanced reaction is given as,

$\rm Cl_{2} + 2 Cs \leftrightarrow 2CsCl$

The ionic reaction for the above reaction is given as,

$\rm Cl_{2} + 2 Cs \leftrightarrow 2 Cs^{+} + 2 Cl^{-}$

The reduction half of the reaction is given by adding electrons on the left side of the reaction as:

$\rm Cl_{2} + 2 e^{-} \leftrightarrow 2 Cl^{-}$

The oxidation half of the reaction is given by adding electrons on the right side of the reaction as:

$\rm Cs \leftrightarrow Cs^{+} + 1 e^{-}$

Therefore, electrons are lost in the oxidation reaction and are gained in the reduction reaction.

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