591.Knowing the electron gain enthalpy values for O O– and O O2– as -141 and 702 kJ mol–1 respectively, how can you account for the formation of a large number of oxides having O2-species and not O–?
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592.Using VSEPR theory, predict the structures of SO3,2– IF7–, XeF2, ClO4–, ICl4– and IBr2–.
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593.
Assign a reason for each of the following statement: Ammonia is a stronger base than phosphine.
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594.Draw the structures of the following molecules (i) SF4, (ii) XeF4.
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595.Answer the following: Of Bi(V) and Sb(V) which may be a stronger oxidising agent and why?
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596.Assign a reason for the following statement? Phosphorus shows marked tendency for catenation but nitrogen shows little tendency for catenation.
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597.Assign a reason for the following statement? The electron gain enthalpy with negative sign for oxygen (–141'k] mol–1) is less that for sulphur (–200 kj mol– 1).
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598.Write chemical equation for the following process: Chlorine reacts with a hot concentrated solution of sodium hydroxide.
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599.Write chemical equation for the following : SO3 + H2SO4 →
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