The electronic configurations of the elements are:-
Z(9) : 1s2 2s2 2p5
Z(12) : 1s2 2s2 2p6 3s2
Z(36) : 1s2 2s2 2p6 3s2 3p6 3d104s2 4p6
(a). The element with Z =9 (F), is highly electronegative because it requires only one electron to have the configuration of nearest noble gas element and has also very small size. It is infact, the most electronegative (4.0) in the period table.
(b). The element with Z= 36 (Kr) is an inert gas element as it has ns2 p6 electronic configuration.
(c). The element with Z =12 (Mg) is highly electropositive in nature since by using two valence electrons, it will have the configuration of the noble gas Neon.