Listed below are the electronic configuration of five elements. Arrange the elements in the increasing order of metallic character:

(a) $[A r] 3 d^{10} 4 s^{2}$
(b) $[A r] 4 s^{2}$
(c) $[A r] 3 d^{10} 4 s^{2} 4 p^{6} 5 s^{2}$
(d) $[A r] 3 d^{10} 4 s^{2} 4 p^{5}$
(e) $[A r] 3 d^{10} 4 s^{2} 4 p^{6} 5 s^{1}$

(d) < (a) < (b) < (c) < (e)

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(d) < (b) < (a) < (c) < (e)

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(d) < (a) < (b) < (e) < (c)

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None of these

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Solution

The correct option is C (d) < (a) < (b) < (c) < (e)
Metallic character depends on the ability of an element to lose its outer valence electrons.
An element belonging to group $I, I I$ and higher periods is most metallic which means element which has large size and one or two electrons in outermost shell is most metallic.
Elements with the outermost electron in p orbitals are non-metallic.

Hence, the order will be(d) < (a) < (b) < (c) < (e)

Hence, the correct option is $A$

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Listed below are the electronic configuration of five elements. Arrange the elements in the increasing order of metallic character:(a) [Ar]3d104s2 (b) [Ar]4s2(c) [Ar]3d104s24p65s2 (d) [Ar]3d104s24p5(e) [Ar]3d104s24p65s1