The tendency to form + 2 ionic state increase on moving down the group due to inert pair effect.
Most characteristic oxidation state for lead and tin are + 2, + 4 respectively.

Shape of $$SnC{l_2}$$  is angular due to $$s{p^2}$$  hybridisation and having the following structure

The species $$C{l_2}{O_7},S{O_2}$$   and $${P_4}{O_{10}}$$  are the anhydrides of $$HCl{O_4},{H_2}S{O_3}$$    and $${H_3}P{O_4}$$  respectively. The acid strength of these acids follows the order $$HCl{O_4} > {H_2}S{O_3} > {H_3}P{O_4}.$$      The corresponding anhydrides also followthe same order.

$$PC{l_5}$$  is yellowish white powder.

\[\underset{\left( \text{from air} \right)}{\mathop{4N{{H}_{3\left( g \right)}}+5{{O}_{2\left( g \right)}}}}\,\xrightarrow[500\text{ }K,\,9\text{ }bar]{Pt/Rh\text{ gauge catalyst}}\]       \[4N{{O}_{\left( g \right)}}+6{{H}_{2}}{{O}_{\left( g \right)}}\]
Thus, 2 moles of $$NO$$  will be produced by the oxidation of 2 moles of $$N{H_3}.$$

\[\begin{align} & 2Ca{{F}_{2}}+Si{{O}_{2}}+{{H}_{2}}S{{O}_{4}}\to \\ & Si{{F}_{4}}+{{H}_{2}}O+CaS{{O}_{4}}\xrightarrow{\text{hydrolysis}}CaSi{{F}_{4}} \\ \end{align}\]

The fluorine has low dissociation energy of $$F{\text{ - }}F$$  bond and reaction of atomic fluorine is exothermic in nature

(i) The first ionization energy of xenon ( 1, 170 $$kJ\,\,mo{l^ - }$$   ) is quite close to that of dioxygen $$\left( {1,180\,\,kJ\,\,mo{l^{ - 1}}} \right).$$
(ii) The molecular diameters of xenon and dioxygen are almost identical.
Based on the above similarities Barlett ( who prepared $$O_2^ + {\left[ {Pt{F_6}} \right]^ - }$$   compound ) suggested that since oxygen combines with $$Pt{F_6},$$  so xenon should also form similar compound with $$Pt{F_6}.$$

Silicon chloride is easily hydrolysed to give white fumes, so it is used as a smoke screen in warfare.
$$SiC{l_4} + 4{H_2}O \to Si{\left( {OH} \right)_4} + 4HCl$$

All hexafluorides of group 16 elements are gaseous in nature.