Question

The laws violated in the given electronic configuration of oxygen atoms are
Aufbau rule
Pauli exclusion principle
Hund’s rule

A.a and b
B.b and c
C.a and c
D.a, b and c

Answer 1

The electronic configuration of Oxygen is $1{s^2}2{s^2}2{p^4}$ In Aufbau rule, lower energy orbitals fill before the higher one. In Pauli exclusion principle, no two electrons can be identified by the same sets of quantum numbers and in Hund’s rule, one electron goes first in all orbitals before pairing up.

Complete step by step answer:
While writing the electronic configuration for oxygen, the first two electrons will go in 1s orbital, next two in 2s and remaining four in 2p orbital.
According to the Aufbau principle, it states that electrons are filled into atomic orbitals in the increasing order of orbital energy level. The electrons first occupy those orbitals whose energy is the lowest. For example, the orbitals in $n = 1$ will before orbital in $n = 2$ . But in a given electronic configuration, we see that there is only one electron in 2s orbital but two in 2p.
The Pauli exclusion principle explains that, it is important to note that each orbital can hold a maximum of two electrons and no two electrons have the same four electronic quantum numbers.
According to Hund’s rule, every orbital in a given subshell must be singly occupied before it is doubly occupied in an orbital. The electrons first fill all the orbitals with the same energy.
As per the Hund’s rule, the electronic configuration of oxygen atom should be:

Hence, the given electronic configuration violates the Aufbau rule, Pauli exclusion principle as well as the Hund’s rule.

Therefore, the correct answer is option (D).

Note: The order in which the orbitals are filled with electrons is: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, and so on.