Explain the following observations :
(i) Fluorine does not exhibit any positive oxidation state.
(ii) The majority of known noble gas compounds are those of Xenon.
(iii) Phosphorus is much more reactive than nitrogen.

Explanation

(i) Since fluorine is the most electronegative element , it shows only a negative oxidation state of -1, and does not show any positive oxidation state.
(ii) Since Xenon (Xe) has least ionization energy among noble gases and hence it is readily form chemical compounds particularly with `O_(2)` and `F_(2)` .
(iii) Since nitrogen forms triple bond between the two N-atoms and the phosphorus forms single between two P-atoms and bonds dissociation energy of nitrogen (941.4 kJ `mol^(-1)` is larger than the bond dissociation energy of phosphorus (213 kJ `mol^(-1)` ) . Hence phosphorus is much more reactive than nitrogen.