An element $X$,which is a yellow solid at room temperature,shows catenation and allotropy. $X$ forms two oxides which are also formed during the thermal decomposition of ferrous sulphate crystals and are major air pollutants.
$(a)$ What would be the nature (acidic/basic) of the oxides formed?
$(b)$ Locate the position of the element in the Modern Periodic Table.

(A) The element $X$ is Sulphur $(S)$. When Sulphur burns in air,it forms Sulphur dioxide $(SO_2)$ and Sulphur trioxide $(SO_3)$. These oxides are non-metallic oxides,and non-metallic oxides are acidic in nature.
$(b)$ Sulphur has an atomic number of $16$. Its electronic configuration is $2, 8, 6$. Since it has $3$ shells,it belongs to the $3^{rd}$ period. Since it has $6$ valence electrons,it belongs to group $16$.