An element is placed in $2^{nd}$ Group and $3^{rd}$ Period of the Periodic Table,burns in the presence of oxygen to form a basic oxide.
$(a)$ Identify the element.
$(b)$ Write the electronic configuration.
$(c)$ Write the balanced chemical equation when it burns in the presence of air.

(A) The element is Magnesium $(Mg)$,as it belongs to Group $2$ and Period $3$.
$(b)$ The electronic configuration of Magnesium $(Z=12)$ is $2, 8, 2$ in the $K, L, M$ shells respectively.
$(c)$ The balanced chemical equation for the combustion of Magnesium in air is: $2Mg(s) + O_2(g) \rightarrow 2MgO(s)$.