The correct order of increasing bond angle is

Cl₂O < \(ClO_{2}^{-}\) < ClO₂

* In \(ClO_{2}^{-}\) there are 2 lone pairs of electrons present on the central chlorine atom. Therefore the bond angle in \(ClO_{2}^{-}\) is less than 118° which is the bond angle in ClO₂ which has less number of electrons on central chlorine atom.

Since all the halogens have a strong tendency to accept electrons. Therefore halogens act as strong oxidising agents and their oxidising power decreases from fluorine to iodine.

MI > MBr > MCl > MF. As the size of the anion decreases covalent character also decreases.

(b, c) From the given options we find option (a) is correct.The oxidising power of halogens follow the order F₂> Cl₂> Br₂> I₂. Option(b)is incorrect because it in not the correct order of electron gain enthalpy of halogens.The correct order is Cl₂> F₂> Br₂ > I₂. The low value of F₂ than Cl₂ is due to its small size.Option(c) is incorrect. The correct order of bond dissociation energies of halogens is Cl₂> Br₂> F₂> I₂.Option(d) is correct. It is the correct order of electronegativity values of halogens. Thus option(b)and (c) are incorrect.

\(\underset{+1}{HOCl}< \underset{+3}{HOClO}< \underset{+5}{HOClO_{2}}< \underset{+7}{HOClO_{3}}\)

In case of oxyacids of similar element as the oxidation number of the central atom increases, strength of acid also increases.

PbO₂ does not contain peroxide ion. It is lead dioxide.

(i) The first ionization energy of xenon (1, 170 kJ mol^–1)is quite close to that of dioxygen (1,180 kJ mol^–1).(ii)The molecular diameters of xenon and dioxygen are almost identical.Based on the above similarities Barlett (who prepared \(O_{2}^{+}[ptF_{6}]^{-}\)compound) suggested that since oxygen combines with PtF₆, so xenon should also form similar compound with PtF₆.