(a) (i) Write the disproportionation reaction of H3PO3.(ii) Draw the structure of XeF4.(b) Account for the following:(i) Although Fluorine has less negative electron gain enthalpy yet F2 is strong oxidizing agent.(ii) Acidic character decreases from N2O3 to Bi2O3 in group 15.(c) Write a chemical reaction to test sulphur dioxide gas. Write chemical equation involved.

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(a) (i) Write the disproportionation reaction of H₃PO₃.
(ii) Draw the structure of XeF₄.
(b) Account for the following:
(i) Although Fluorine has less negative electron gain enthalpy yet F₂ is strong oxidizing agent.
(ii) Acidic character decreases from N₂O₃ to Bi₂O₃in group 15.
(c) Write a chemical reaction to test sulphur dioxide gas. Write chemical equation involved.

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Detailed Solution

(a) (i) $H_{3} {PO}_{3} \to 3 H_{3} {PO}_{4} + {PH}_{3}$
(ii) Question Image
(b) (i) Fluorine has small size low bond dissociation enthalpy which makes it a strong oxidizing agent.
(ii) On going down the group the size of elements increases. It decreases the electronegativity. Due to which acidic character decreases.
(c) $5 {SO}_{2} + 2 {MnO}_{4}^{-} + 2 H_{2} O \to 5 {SO}_{4}^{2 -} + 4 H^{+} + 2 {Mn}^{2 +}$

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