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Explain redox reactions on the basis of electron transfer. Give suitable examples.

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When a redox reaction takes place, the species which loses the electrons is regarded as undergoing the oxidation reaction. It therefore acts as an oxidizing agent or oxidant. For the species that accepts electrons is regarded as undergoing reduction and therefore it behaves as a reductant.

The above mentioned transfer is largely based on the relative electronegativity of difference between two interacting species. The higher electronegative element attracts more electrons while on the other hand the electropositive element loses electrons.

Splitting of the reaction into two halves here proves that sodium is oxidised, and hydrogen is reduced. Here, the sodium atom is oxidised, and the hydrogen atom is reduced; therefore, it is a redox reaction.


2Na(s) + H_{2}(g) \rightarrow 2NaH(s) is a redox change.

2Na(s) \rightarrow 2Na+(g) + 2e^{-} and the other half-reaction is:

H_{2}(g) + 2e^{-} \rightarrow 2H^{-}(g)

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