Which of the following configuration represent alkaline earth metal:

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

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

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

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1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{6} 4 d^{10} 5 s^{2} 5 p^{6} 6 s^{2}

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Solution

The correct option is D $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{6} 4 d^{10} 5 s^{2} 5 p^{6} 6 s^{2}$
Alkaline earth metals have two electrons in their valence shell and the last electron enters in s-subshell.
In the configuration, $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{6} 4 d^{10} 5 s^{2} 5 p^{6} 6 s^{2}$ , the last electron enters the s-subshell and has 2 electrons as valence electrons.Therefore it represents an alkaline earth metal.

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Similar questions

(a) How do alkaline earth metals occur in nature ?

(b) Write the electronic configuration of the first two alkaline earth metals.

The correct electronic configuration of an alkaline earth metals can be:

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