Question

why is the electronic configuration of scandium - (2,8,9,2) and not not (2,8,8,3) although it belongs to group 3 and hence has a valency of 3? do all transition metals have this kind of electronic configuration......

Answer 1

Answer:

Every element adds one more electron to the outermost shell. Instead of having three electrons in the outer shell, scandium adds its electron to the second to last shell. The electron configuration is 2-8-9-2.

Explanation:

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Answer 2

Yes, all the transition metals have this kind of electronic configuration.

• In the transition metals, the electrons successively enter at the d orbital and two electrons reside at the next "s" orbital.
• Thus the electronic configuration of Sc is as follows-
• ${1s}^{2} {2s}^{2} {2p}^{6} {3s}^{2} {3p}^{6} {3d}^{1} {4s}^{2}$
• Hence it has one electron in the 3d orbital and 2 electrons in the 4s orbital and according to the Aufbau principle, after the 4s orbital 3d orbital is filled so, it does not show (2,8,8,3) type of electronic configuration.