![]() This increase in the atomic size is attributed to an increase in the number of shells. (iv) Atomic size: On moving down a group, the atomic size increases. As we move down a group, electronegativity decreases, owing to an increase in size. This is because of increasing atomic sizes. (iii) Ionization energy and electronegativity:įirst ionization decreases on moving down a group. This happens because of the inert pair effect. However, the stability of +5 oxidation state decreases down a group, whereas the stability of +3 oxidation state increases. In addition to the -3 state, N and P also show -1 and -2 oxidation states.Īll the elements present in this group show +3 and +5 oxidation states. The remaining elements of this group show a formal oxidation state of -3 in their covalent compounds. This can take place only with nitrogen as it is the smallest in size and the distance between the nucleus and the valence shell is relatively small. However, gaining electrons is very difficult as the nucleus will have to attract three more electrons. (ii) Oxidation states: All these elements have 5 valence electrons and require three more electrons to complete their octets. Their general electronic configuration is ns2 np3. (i) Electronic configuration: All the elements in group 15 have 5 valence electrons.
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