Question

The electronic configuration of four elements are
given below. Which element does not belong to
the same block as others -
(1)[Xe] 6s2 4f14 5d10 (2) [Ar] 4s2 3d
(3) [Rn] 7s2 5f76d! (4) [Kr] 4d6 552​

Answer 1

$\huge\mathcal{Answer:}$

1. [Xe] 6s² 4f$^{14}$5d $^{10}$ = Hg
2. [Ar]4s² 3d
3. [Rn] 7s² 5f$^{7}$6d
4. [Kr]4d$^{6}$ 5s² = Tc

Answer 2

Element $[Kr]4d^{6}5s^{2}$​ does not belong to  the same block as others.

Explanation:

The element with electronic configuration $[Xe]6s^{2}4f^{14}5d^{10}$ has atomic number 80. This element is mercury (Hg). It is a d-block element.

Element with electronic configuration $[Ar]4s^{2}3d$ is a d-block element.

Element with electronic configuration $[Rn]7s^{2}5f^{7}6d$ is also a d-block as the valence electrons are present in d-shell.

Element with electronic configuration $[Kr]4d^{6}5s^{2}$​ is not a d-block element.

Learn more about electronic configuration:

https://brainly.in/question/9963151

https://brainly.in/question/2571004

#Learnwithbrainly