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(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) $H_4P_2O_7$

Posted by

Sumit Saini

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