Given below are two statements :

Statement I : Elements ' $X$ ' and ' $Y$ ' are the most and least electronegative elements, respectively among $\mathrm{N}, \mathrm{As}, \mathrm{Sb}$ and P . The nature of the oxides $\mathrm{X}_2 \mathrm{O}_3$ and $\mathrm{Y}_2 \mathrm{O}_3$ is acidic and amphoteric, respectively.

Statement II : $\mathrm{BCl}_3$ is covalent in nature and gets hydrolysed in water. It produces $\left[\mathrm{B}(\mathrm{OH})_4\right]^{-}$ and $\left[\mathrm{B}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{3+}$ in aqueous medium.

In the light of the above statements, choose the correct answer from the options given below :

Given below are two statements :

Statement I : The halogen that makes longest bond with hydrogen in HX, has the smallest covalent radius in its group.

Statement II : A group 15 element's hydride $\mathrm{EH}_3$ has the lowest boiling point among corresponding hydrides of other group 15 elements. The maximum covalency of that element E is 4 .

In the light of the above statements, choose the correct answer from the options given below

A 'p'-block element $(\mathrm{E})$ and hydrogen form a binary cation $\left(\mathrm{EH}_{\mathrm{x}}\right)^{+}$, while $\mathrm{EH}_3$ on treatment with $\mathrm{K}_2 \mathrm{HgI}_4$ in alkaline medium gives a precipitate of basic mercury(II)amido-iodine. Given below are first ionisation enthalpy values $\left(\mathrm{kJ} \mathrm{mol}^{-1}\right)$ for first element each from group 13, 14, 15 and 16. Identify the correct first ionisation enthalpy value for element E.

Consider the following reactions.

$\underset{\text { (Hot solution) }}{\mathrm{PbCl}_2}+\mathrm{K}_2 \mathrm{CrO}_4 \rightarrow A+2 \mathrm{KCl}$

$$ \begin{aligned} & \mathrm{A}+\mathrm{NaOH} \rightleftharpoons \mathrm{~B}+\mathrm{Na}_2 \mathrm{CrO}_4 \\ & \mathrm{PbSO}_4+4 \mathrm{CH}_3 \mathrm{COONH}_4 \rightarrow\left(\mathrm{NH}_4\right)_2 \mathrm{SO}_4+\mathrm{X} \end{aligned} $$

In the above reactions, $\mathrm{A}, \mathrm{B}$ and X are respectively.