(a) Draw the structure of the following :

(i) HClO_{3}

(ii) H_{2}S_{2}O_{8}

(b) Give reasons for the following :

(i) Above 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 PCl_{5} exists as an ionic compound.

 

 

 

 
 
 
 
 

Answers (1)
S Sumit

(a) (1) HClO_{3}

       

(2) H_{2}S_{2}O_{8}

     

(b) (i) Above1000\; 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 Cl-Cl and hydration enthalpy of F^{-} is much higher than Cl^{-}. These two factors more than comperrate the negative electron gain enthalpy of F^{-}.

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

 

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