8.4. Ans :-
In the diagram 4d-orbital have 6 electrons out of which only first orbital is completely filled i.e. 2 electrons, others orbitals are singly filled.
(a). The given element must belong to d-block because it has partially filled d-orbitals i.e. 4d6-electrons. Since, 2 electrons are removed therefore element must have two electrons less than the atomic number and this atom must have 5s-orbital outer most shell. Therefore, Group number of the element must be 6+2= 8th group and period number of the element must be 5th.
Hence, the element will be Ruthenium having symbol " Ru ".
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(b). The electronic configuration of the atom Ru (Z=4) is according to increasing order of energy of the orbitals is : 1s22s22p63s23p64s23d104p65s14d7.
and
Noble gas electronic configuration is = [Kr] 4d7 5s1
334 CH bond length ) Rank Lewiym 1.9 84 The orbital diagram that follows shows the valence elec trons for a 2+ ion...