If the electronic configuration of an element is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{1}$ then the number electrons involved in bonding will be:

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Solution

The electrons involved in chemical bond formation will be $3 d^{5} 4 s^{1}$
According to the given electronic configuration we can say that the element is a transition metal.
For transition elements, the $n s$ and $(n - 1) d$ orbitals' electrons take part in the chemical bond formation. All other inner electrons are part of a fully filled shells so they are non reactive.
In the above electronic configuration the outermost subshells are $3 d$ and $4 s$ .
They have 5 and 1 electrons respectively in their subshell which will contribute to bond formation.
So, total electrons will be 6.

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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

(a) $3 p^{6}$

(b) $3 p^{6}, 4 s^{2}$

(d) $3 d^{2}, 4 s^{2}$

Q. The electronic configuration of an element is

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

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How can the valency of an element be determined if its electronic configuration is known? What will be the valency of an element of atomic number 9 (nine)?

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If the electronic configuration of an element is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{1}$ then the number electrons involved in bonding will be: