consider the orbital diagram shown. which electron rule is broken in the diagram? 1s 2s 2p pauli exclusion…

Brief Explanations:

The Pauli exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers and is related to electron - spin and orbital occupancy in a single - orbital context. Hund's rule states that electrons will first singly occupy degenerate orbitals with parallel spins before pairing up. In the given 2p orbital diagram, electrons should first singly occupy each of the 2p orbitals before pairing up, but here they are paired in one 2p orbital while others are empty. So, Hund's rule is violated.

Answer:

Hund's rule