Relative to electrons and electron states, what does each of the four quantum numbers specify?

The four quantum numbers related to electrons and electron states are: 1. Principal Quantum Number (n): Specifies the energy level of an electron in an atom and the size of the orbital. It is a positive integer with values like n = 1, 2, 3, etc. Higher 'n' values indicate higher energy and electron distance from the nucleus. 2. Azimuthal Quantum Number (l): Defines the shape of the electron's orbital and depends on the value of the principal quantum number (n). It ranges from 0 to (n-1), with each value representing a unique orbital shape (e.g., l = 0 for s orbitals, l = 1 for p orbitals). 3. Magnetic Quantum Number (m_l): Gives information about the orientation of the orbital in space and depends on the value of the azimuthal quantum number (l). It ranges from -l to +l, including 0, with different values corresponding to unique orbital orientations. 4. Spin Quantum Number (m_s): Describes the intrinsic angular momentum or "spin" of the electron. There are two possible values: +1/2 (spin up) and -1/2 (spin down). The Pauli Exclusion Principle states that no two electrons in an atom can have the same set of quantum numbers, ensuring electrons have unique spin states.