Account for the following :
(i) `NH_(3)` is a stronger base than `PH_(3)`
(ii) Sulphur has a greater tendency for catenation than oxygen.
(iii) Bond dissociation energy of `F_(2)` is less than that of `Cl_(2)`.

Bond dissociation energy of F_(2) is less that of Cl_(2) give reason.

Draw the structures of the following : (i) H_(2)S_(2)O_(8) (ii) HClO_(4) (b) How would you account for the following : (i) NH_(3) is a stronger base than PH_(3) . (ii) Sulphur has a greater tendency for catenation than oxygen. (iii) F_(2) is stronger oxidising agent than Cl_(2) .

Explain the following situations : (ii) Sulfur exhibits greater tendency for catenation than selenium.

The bond dissociation energy of N_(2)^(+) is less than that of N_(2) . Show why this is the case.

(a) Draw the molecular structures of the following compounds : (i) N_(2)O_(5) " " (ii) XeOF_(4) (b) Explain the following observations : (i) Sulphur has a greater tendency for catenation than oxygen. (ii) ICI is more reactive than I_(2) . (iii) Despite lower value of its electron gain enthalpy with negative sign, fluorine (F_(2)) is a stronger oxidizing agent than Cl_(2) .

Account for the following BiCl_3 is less covalent than PCl_3 .

State reasons for each of the following : (i) All the P-Cl bonds in PCl_5 molecule are not equivalent. (ii) Sulphur has greater tendency for catenation than oxygen.

F_(2) is a stronger oxidising agent than Cl_(2)

C_6 H_5 N^(+)(CH_3)_3 OH -is a stronger base than NH_4 OH . Explain.

N_2 has greater bond energy than N_(2)^(+) but O_2 has lower bond dissociation energy than O_(2)^(+) . Explain.