(a) Account for the following :

(i) Tendency to show -3 oxidation state decreases from N to Bi in group 15.

(ii) Acidic character increases from H_2O to H_2Te.

(iii) F_2 is more reactive than CIF_3, whereas CIF_3, is more reactive than Cl_2.

(b) Draw the structure of (i) XeF_2,(ii)H_4P_2O_7.

 

 

 

 

 

 
 
 
 
 

Answers (1)

(a)

(i) The tendency to exhibit-3 oxidation state decreases down the group due to increase in size and metallic character.

(ii) Acidic character increases from H_2O to H_2Te because down the group, bond enthalpy for dissociation decreases.

(iii) F-F bond is weaker than Cl-F bond due to small size and high electron density, more repulsion between fluorine atoms therefore F_2 is more reactive than ClF_3. Whereas in Cl_2,\: Cl-Cl bond is stronger than ClF_3. Therefore, ClF_3 is more reactive than Cl_2

(b)

(i) XeF_2   

    

(ii) H_4P_2O_7

 

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