Identify the following reaction as either oxidation or reduction:
$K - e^{-} \to K^{+}$

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Solution

Oxidation: Oxidation is said to take place when there is a loss of electrons.
Reduction: Reduction is said to take place when there is a gain of electrons.
In the given reaction, 1 electron (e^-) is removed from the reactant side (indicated by the minus sign). It shows that one electron is removed from Potassium (K) atom to form a Potassium ion (K⁺).
As there is a loss of 1 electron, therefore this reaction is an oxidation reaction.
Potassium atom has 19 electrons and after undergoing oxidation, it has a total of 18 electrons.
$K - e^{-} \overset{Oxidation}{\to} K^{+} (Potassium atom) (Potassium ion) (2, 8, 8, 1) (2, 8, 8)$
This reaction can also be written in the following manner:
$K \overset{Oxidation}{\to} K^{+} + e^{-} (Potassium atom) (Potassium ion) (2, 8, 8, 1) (2, 8, 8)$

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