The Quantum Atom: Orbitals and Quantum Numbers

Explain how solving the Schrödinger equation for hydrogen yields quantum numbers (n, l, ml) that define an electron's state.

Describe the physical meaning of each quantum number: principal (n) for energy level, azimuthal (l) for orbital shape, and magnetic (ml) for spatial orientation.

Describe the characteristic shapes and nodal structures of s, p, and d orbitals based on their quantum numbers.

Interpret the radial probability distribution for an orbital, explaining why an electron has a most probable, non-zero distance from the nucleus.

Explain the spin quantum number (ms) as an intrinsic, non-classical property of the electron, required by experimental observation.