701.

How would you account for the following:
Interhalogen compounds are strong oxidising agents.

702.

How would you account for the following:
Sulphur hexafluoride is less reactive than sulphur tetrafluoride.

703.

How would you account for the following:
In the noble gases only xenon forms known chemical compounds.

704. Compare the structural shapes of the following species: SF₆ and SF₄.

705.

Write balanced chemical equations for the following reactions:
(a)     ${\mathrm{Ca}}_3{\mathrm{P}}_2+{\mathrm{H}}_2\mathrm{O} \to$
(b)     ${\mathrm{XeF}}_6+3{\mathrm{H}}_2\mathrm{O} \to$

706. Explain the following:
(i) Most of the known noble gas compounds are those of Xenon.
(ii) ClF₃exists but FCl₃ does not.
(iii) Among the hydrides of elements of Group 16, water shows unusual physical
properties.
(iv) Unlike phosphorus, nitrogen shows little tendency for catenation.
(v) Despite lower electron affinity, fluorine is a stronger oxidising agent than chlorine.

707. Discuss the properties of oxygen, sulphur, selenium, tellurium and polonium (group 16 elements) with reference of following: (i) metallic (non-metallic character), (ii) catenation, (iii) thermal stability of hydrides, (iv) oxidation states (v) allotropy.

708.

Describe the molecular shapes of the following: (i) SF₄, (ii) BrF₅, (iii) IF₃, (iv) PF₅, (v) XeF₂.

709. Give reasons for:
(i) Ozone is more reactive than oxygen.
(ii) An acidified K₂Cr₂O₇ paper on being exposed to SO₂ turns green.
(iii) Sulphuric acid never acts as a reducing agent.
(iv) Noble gases are mostly chemically inert.
(v) Nitrogen is fairly inert.

710. Describe the following about halogen family (group 17 elements):
(i)    Relative oxidising power.
(ii)    Relative acidic strength of their hydrides.
(iii)    Oxyacids and their relative oxidising ability.