A shining metal 'M', on burning gives a dazzling white flame and changes to a white powder 'N'.

(a) Identify 'M' and 'N'.

(b) Represent the above reaction in the form of a balanced chemical equation.

(c) Does 'M' undergo oxidation or reduction in this reaction? Justify.

(a) Metal 'M' is Magnesium ($Mg$) and the white powder 'N' is Magnesium oxide ($MgO$).

(b) The balanced chemical equation for the reaction is:

$$2\text{Mg}(\text{s}) + \text{O}_2(\text{g}) \rightarrow 2\text{MgO}(\text{s})$$

(c) Metal 'M' (Magnesium) undergoes oxidation in this reaction.

Justification: Oxidation is defined as the gain of oxygen by a substance. Here, magnesium ($Mg$) reacts with oxygen ($O_2$) to gain oxygen atoms and form magnesium oxide ($MgO$). Therefore, magnesium is oxidized.