Question

which orbital diagram shows a violation of hunds rule? a) 1s 2s 2p b) 1s 2s 2p c) 1s 2s 2p d) 1s 2s 2p a b c d

Explanation:

Hund's Rule states that electrons must occupy degenerate orbitals (same - energy orbitals) singly before pairing up. In option D, for the \(2p\) orbitals, electrons start to pair up (there is an orbital with two electrons) without all the \(2p\) orbitals first having one electron each. In option A, the \(2s\) orbital has two electrons with parallel spins which violates the Pauli Exclusion Principle (not Hund's Rule). In option B, the \(2p\) orbitals follow Hund's Rule (electrons occupy orbitals singly with parallel spins). In option C, the \(2s\) orbital has only one electron (which is not a violation of Hund's Rule as Hund's Rule is about degenerate orbitals when there are multiple electrons to fill them).

Answer:

D.