# (a) Draw the structure of the following :(i) $\inline HClO_{3}$(ii) $\inline H_{2}S_{2}O_{8}$(b) Give reasons for the following :(i) Above $\inline 1000\; K$ sulphur shows paramagnetism.(ii) Although electron gain enthalpy of fluorine is less negative than that of chlorine, yet flourine is a better oxidising agent than chlorine.(iii) In solid state $\inline PCl_{5}$ exists as an ionic compound.

(a) (1) $\inline HClO_{3}$

(2) $\inline H_{2}S_{2}O_{8}$

(b) (i) Above$1000\; K$, sulphur exhibits paramagnetism, $\delta$ is in vapour state, it partly exists as $S_{2}$ molecule which has two unpaired electrons in the antibonding $(\pi )$ orbitals.

(ii) Although electron gain enthalpy of flumine is less negative than that of chlorine, yet fluorine is a better oxidising agent than chlorine because bond dissociation enthalpy of f-f much lower than $\inline Cl-Cl$ and hydration enthalpy of $\inline F^{-}$ is much higher than $\inline Cl^{-}$. These two factors more than comperrate the negative electron gain enthalpy of $\inline F^{-}$.

(iii) In solid state, $\inline PCl_{5}$ exists in ionic compound as it exists as $\inline \left [ PCl_{4} \right ]^{+}$$\inline \left [ PCl_{6} \right ]^{-}$ containing tetra and hexa coordinated species.

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