Identify the group number of the element having its electronic configuration: $1 s^{2}$ $2 s^{2}$ $2 p^{6}$ $3 s^{2}$ $3 p^{6}$ $3 d^{5}$ $4 s^{2}$

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Solution

The correct option is B 7
The electronic configuration given is $1 s^{2}$ $2 s^{2}$ $2 p^{6}$ $3 s^{2}$ $3 p^{6}$ $3 d^{5}$ $4 s^{2}$
Here the last electron is in the $d$ - subshell and therefore the element is from the $d$ - block.

In $d$ - block:
Group number =
Number of electrons in the $n s$ subshell + Number of electrons in the $(n - 1) d$ subshell

$∴ G r o u p N u m b e r = 2 + 5 = 7$

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