Quantum Numbers

n

Indicates the size and energy of the orbital (shell).

l

Represents the shape of atomic orbitals (subshell).

ml

Indicates the orientation of the orbital in space.

What does Heisenberg's uncertainty principle state?

We do not have the ability to know an electron's position and velocity at the same time.

What does Schrödinger’s equation incorporate?

It describes the wave-like and particle-like behaviors of electrons

Principal Quantum Number (n)

Positive integers (n = 1, 2, 3, …) indicating the energy level

Azimuthal or Angular Momentum Quantum Number (l)

Integers (l = 0, 1, 2, …, n-1) that specify the shape of atomic orbitals (subshells): l=0 (s), l=1 (p), l=2 (d), l=3 (f).

Magnetic Quantum Number (ml)

Values ranging from -l to +l (ml = -l, …, 0, …, l) describing an orbital's orientation in space

Spin Quantum Number (ms)

Quantized values of +1/2 or -1/2 representing the spin of an electron

higher n values

correlate with greater energy and larger orbits.

why is ms important

essential for determining an electron’s magnetic behavior