(a) Complete the following chemical reaction equations :
(i) `P_(4)+SO_(2)Cl_(2) rightarrow`
(ii) `XeF_(4)+ H_(2)O rightarrow`
(b) Explain the following observations giving appropriate reasons :
(i) The stability of + 5 oxidation state decreases down the group in group 15 of the periodic table.
(ii) Solid phosphorus pentachloride behaves as an ionic compound.
(iii) Halogens are strong oxidizing agents.

Explanation

(a) (i) `P_(4)+10" " SO_(2)Cl_(2) rightarrow 4 PCl _(5) + 10" "SO_(2)`
(ii) `6" "XeF_(4)+12H_(2)Orightarrow2 " "eO_(3) + 4" "XeO_(3)+24HF +3O_(2)`
b (i)Because down the group, +3 oxidation state becomes more and more stable due to higher energy involved to unpair the electrons or due to inert pair effect.
(ii) Due to the formation of `[PCl_(4)]^(+)[PCI_(6)]^(-)`
(iii) Because halogens readily accept an electron