Question

in which orbital diagram is paulis exclusion and hunds rule violated? * 1 point a b c d

Explanation:

• Pauli's exclusion principle: No two electrons in an atom can have the same set of four quantum numbers. In an orbital, electrons must have opposite spins (represented as \(↑↓\)).
• Hund's rule: Electrons will occupy degenerate orbitals (orbitals of the same energy) singly before pairing up.

Let's analyze each option:

• Option A:
• Violation of Pauli's principle: In the second set of orbitals, two electrons in the same orbital have the same spin (\(↓↓\)), violating Pauli's principle.
• Violation of Hund's rule: Electrons are paired in the second orbital before filling all orbitals singly.
• Option B:
• Pauli's principle: No violation (electrons in each orbital have opposite spins \(↑↓\)).
• Hund's rule: No violation (orbitals are filled correctly).
• Option C:
• Pauli's principle: No violation (electrons in each orbital have opposite spins \(↑↓\)).
• Hund's rule: No violation (orbitals are filled correctly as per Hund's rule).
• Option D:
• Pauli's principle: No violation (electrons in each orbital have opposite spins \(↑↓\)).
• Hund's rule: No violation (orbitals are filled correctly).

Answer:

A.