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Question

(a) Complete the following chemical equation :

(i) Cu+HNO3(dil.)
(ii) XeF4+O2F2
(b) Explain the following observations :

(i) Phosphorus has a grater tendency for catenation than nitrogen.
(ii) Oxygen is a gas but sulphur a solid.
(iii) The halogens are coloured. Why?

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Solution

(a) (i) 3Cu+8HNO3(dilute)3Cu(NO3)2+2NO+4H2O
(ii) XeF4+O2F2XeF6+O2

(b)
(i) Catenation is much more common in phosphorous compounds than in nitrogen compounds. This is because of the relative weakness of the N-N single bond as compared to the P-P single bond. Since nitrogen atom is smaller, there is greater repulsion of electron density of two nitrogen atoms, thereby weakening the N-N single bond.

(ii) Oxygen is smaller in size as compared to sulphur. Due to its smaller size, it can effectively form pπpπ bonds and form O2(O=O) molecule. Also, the intermolecular forces in oxygen are weak van der Waal forces, which causes it to exist as a gas. On the other hand, sulphur does not form S2 molecule but exists as a puckered structure held together by strong covalent bonds.
Hence, it is solid.

(iii) Almost all halogens are coloured. This is because of halogens absorb radiations in the visible region. This results in the excitation of valence electrons to a higher energy region. Since the amount of energy required for excitation differs for each halogen, each halogen displays a different colour.

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