Quantum Numbers and Atomic Orbitals

This set of flashcards covers the fundamental concepts related to quantum numbers and atomic orbitals, providing definitions for key terms and principles in chemistry.

Principal Quantum Number (n)

Defines the main energy level or principal shell, and can only be a positive integer (n = 1, 2, 3, …).

Orbital Angular Momentum Quantum Number (ℓ)

Can have positive integer values from 0 to (n - 1) and determines the shape of the orbital.

Magnetic Quantum Number (ml)

Values range from -l to +l, including zero, and relate to the orientation in space of the angular momentum associated with the orbital.

Subshells

Designated by quantum number ℓ; includes s (ℓ=0), p (ℓ=1), d (ℓ=2), and f (ℓ=3) orbitals.

Pauli Exclusion Principle

States that no two electrons in the same atom can have the same set of four quantum numbers.

Degenerate Orbitals

Orbitals that have the same energy.

Shapes of s Orbitals

Spherical, with 2s being larger than 1s.

Shapes of p Orbitals

Dumbbell-shaped regions of space with three orientations: px, py, pz.

Electron Spin Quantum Number (ms)

Has values of +½ and -½, representing the spin direction of the electron.

Energy Levels

In quantum mechanics, energy levels depend on the principal quantum number (n) and increase with larger n.