Question

Which of the following represents the noble gas configuration
A.\[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^{10}}4{s^2}4{p^6}4{d^{10}}5{s^2}5{p^6}\]
B. \[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^{10}}4{s^2}4{p^6}4{d^{10}}4{f^{14}}5{s^2}5{p^6}5{d^1}6{s^2}\]
C. \[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^{10}}4{s^2}4{p^6}4{d^{10}}5{d^1}6{s^2}\]
D. \[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^{10}}4{s^2}4{p^6}4{d^{10}}\]

Answer 1

Hint: The elements that are established in the last column of the periodic table are noble gases helium, neon, argon, krypton, xenon, and radon. A noble gas configuration of an atom comprises the elemental symbol of the noble gas which is present in the periodic table before that atom, then the configuration of the remaining electrons is represented.

Complete Step by Step Solution:
In this question, we have to find out the following represents the noble gas configuration.
A. \[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^{10}}4{s^2}4{p^6}4{d^{10}}5{s^2}5{p^6}\]
The total number of electrons in this configuration is 54 which is the atomic number of xenon.
Xenon is a noble gas element.
So, it is a noble gas configuration.
So, A is correct.

B. \[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^{10}}4{s^2}4{p^6}4{d^{10}}4{f^{14}}5{s^2}5{p^6}5{d^1}6{s^2}\]
The total number of electrons in this configuration is 71 which is the atomic number of lutetium.
It is not a noble gas element.
So, it is not a noble gas configuration.
So, B is incorrect.

C. \[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^{10}}4{s^2}4{p^6}4{d^{10}}5{d^1}6{s^2}\]
The total number of electrons in this configuration is 49 which is the atomic number of Indium.
It is not a noble gas element.
So, it is not a noble gas configuration.
So, C is incorrect.

D. \[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^{10}}4{s^2}4{p^6}4{d^{10}}\]
The total number of electrons in this configuration is 46 which is the atomic number of Palladium.
It is not a noble gas element.
So, it is not a noble gas configuration.
So, D is incorrect.
So, option A is correct.

Note: Sulphur has the atomic number 16 whose electron configuration is \[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}\]. The first ten electrons of the Sulphur atom are the inner-shell electrons and their configuration is identical to the configuration of the element Ne (Z=10). So, for Sulphur, we do the substitution of [Ne] for the \[1{s^2}2{s^2}2{p^6}\]part of the configuration. Sulphur's noble gas configuration is\[\left[ {Ne} \right]3{s^2}3{p^6}\].