8.22. Consider the elements: 

Cs, Ne, I, F 
(a) Identify the element that exhibits negative oxidation state.
(b) Identify the element that exhibits positive oxidation state.
(c) Identify the element that exhibits both positive and negative oxidation states.
(d) Identify the element which neither exhibits negative nor does the positive oxidation state.

<p><strong> (a)</strong> F. Fluorine being the most electronegative element shows only a -ve oxidation state of -1.</p><p><strong> (b)</strong> Cs. Alkali metals because of the presence of a single electron in the valence shell, exhibit an oxidation state of +1.</p><p><strong> (c)</strong> I. Because of the presence of seven electrons in the valence shell, I shows an oxidation state of -1 (in compounds of I with more electropositive elements such as H, Na, K, Ca, etc.) or an oxidation state of +1 compounds of I with more electronegative elements, i.e., O, F, etc.) and because of the presence of d-orbitals it also exhibits +ve oxidation states of +3, +5 and +7.</p><p><strong> (d)</strong> Ne. It is an inert gas (with high ionization enthalpy and high positive electron gain enthalpy) and hence it neither exhibits -ve nor +ve oxidation states.</p>

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