Question

Which of the following options does not represent ground state electronic configuration of an atom?

• A. $1s^2\,2s^2\,2p^6\,3s^2\,3p^6\,3d^{8}\,4s^2$
• B. $1s^2\,2s^2\,2p^6\,3s^2\,3p^6\,3d^{9}\,4s^1$
• C. $1s^2\,2s^2\,2p^6\,3s^2\,3p^6\,3d^{10}\,4s^1$
• D. $1s^2\,2s^2\,2p^6\,3s^2\,3p^6\,3d^{5}\,4s^1$

Answer 1

Answer: (C)

The Aufbau principle dictates the manner in which electrons are filled in the atomic orbitals of an atom in its ground state. It states that electrons are filled into atomic orbitals in the increasing order of orbital energy level. According to the Aufbau principle, the available atomic orbitals with the lowest energy levels are occupied before those with higher energy levels.
Correct configuration of (b) should be $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{1}$ for the copper which has atomic number $29\left({ }_{29} Cu\right.$.) Due to extra stability of full filled orbital of $d$ - subshell, the last electron enter into d-orbital insted of s-orbital.