If the electronic configuration of an element is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{2} 4 s^{2},$ the four electrons involved in chemical bond formation will be ---------

3 p^{6} 3 d^{2}

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3 p^{6} 4 s^{2}

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3 d^{2} 4 s^{2}

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3 p^{6}

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Solution

The correct option is C $3 d^{2} 4 s^{2}$
Valence shell electrons:

Outermost shell, having maximum $‘ n^{'}$ value, is called the valence shell and the electrons present in it are called valence shell electrons.

It is the electronic configuration of a $d -$ block element. In $d -$ block elements, the electrons present in d-orbital of penultimate shell also participate in chemical reactions. So, the electrons from the s-orbital of $4^{t h}$ shell (valence shell) and d-orbitals of $3^{r d}$ shell (penultimate shell) participate in bond formation.

Thus, the $4$ electrons involved in chemical bond formation will be $3 d^{2} 4 s^{2},$ i.e., correct answer is option $(D) .$

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The electronic configuration of Ti is 1 $s^{2}$ 2 $s^{2}$ 2 $p^{6}$ 3 $s^{2}$ 3 $p^{6}$ 3 $d^{2}$ 4 $s^{2}$ and it represents

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6} {4 s}^{2}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6} {3 d}^{6} {4 s}^{1}

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{1}

1 s^{2} 2 s^{2} 2 p^{6}

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3}

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}

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