Hund’s rule

Definition

Hund's rule states that electrons will fill degenerate orbitals singly before pairing up. This minimizes electron-electron repulsions and results in the lowest energy configuration.

5 Must Know Facts For Your Next Test

1. Hund's rule is also known as the rule of maximum multiplicity.
2. It applies to orbitals within the same subshell, such as p, d, or f orbitals.
3. Electrons prefer to occupy empty orbitals first due to reduced electrostatic repulsion.
4. The application of Hund's rule explains why elements have specific magnetic properties.
5. This rule is essential for determining the ground state electron configurations of atoms.

Review Questions

• What is Hund's rule and why is it important for electron configurations?
• How does Hund's rule affect the way electrons fill p, d, and f orbitals?
• Explain why Hund's rule minimizes electron-electron repulsions.

Related terms

Pauli Exclusion Principle: States that no two electrons can have the same set of four quantum numbers within a single atom.

Aufbau Principle: Describes the process by which electrons are added to orbitals in order of increasing energy levels.

Degenerate Orbitals: Orbitals that have the same energy level within a given subshell.