(a) (i)H3PO3:Oxidation number of O=+ 3
H3PO4 : Oxidation number of P = +5
The H3PO3 contains one P-H bond in addition to P=O and P-OH bonds. These types of oxoacids tend to undergo disproportionation to give orthophosphoric acid. Whereas in H3PO4 is at +5 oxidation state hence no disproportionation takes places.
(ii) When we react Cl2 with an excess of F2, ClF3 is formed and not FCl3 because fluorine can exist only in – 1 oxidation state whereas chlorine can show positive oxidation states when combined with the more electronegative atom.
In ClF3 oxidation number of Cl is + 3 which is possible due to the availability of d-orbitals.
(iii) In oxygen molecule, there is p-p overlap between two oxygen atoms forming a double bond. The intermolecular forces in oxygen are weak Vander Waal’s forces, and therefore oxygen exists as a gas, on the other hand, the S are linked by single bonds and form polyatomic complex molecules. Hence sulphur in a solid.
(i) The structure of XeF4 is square planar in structure.
(ii) HCLO3 or chloric acid is
(i) The brown gas A is NO2 or nitrogen dioxide. On cooling, it dimerises to N2O4 and solidifies as a colourless solid.
(ii) The structures of A and B.
(iii) Compound A that is NO2 contains an odd number of molecules. On dimerization, it is converted to stable N2O4 molecule with even numbers of electrons and have better intermolecular forces to get solidified. Thus it changes to solid on cooling.
(b) Decreasing order of reducing character-
(c) Xef4 + SbF5→[XeF3]+ +[SbF6]-
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