Questions

Elements a, b, c, d, and e have the following electronic configurations.
(a) $1 s^{2}, 2 s^{2} 2 p^{1}$
(b) $1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{1}$
(c) $1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{2}$
(d) $1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{5}$
(e) $1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6}$
Which among these will belong to the same group in the periodic table?

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detailed solution

Correct option is B

In the periodic table, the same group of elements possessed the same outermost shell in electronic configuration. Thus, a and b have the same number of valence electrons in its outer shell.

Hence, The correct option is B

(A) $1 s^{2} 2 s^{2} 2 p^{1}$

(B) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1}$

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Elements a, b, c, d, and e have the following electronic configurations.(a)1s2,2s22p1(b)1s2,2s22p6,3s23p1 (c)1s2,2s22p6,3s23p2(d)1s2,2s22p6,3s23p5(e) 1s2,2s22p6,3s23p6Which among these will belong to the same group in the periodic table?