Which two of the four quantum numbers determine the energy level of an orbital in a multielectron atom?

Key Concepts

Quantum Numbers

Quantum numbers are sets of numerical values that describe the unique quantum state of an electron in an atom. There are four quantum numbers: principal (n), azimuthal (l), magnetic (m_l), and spin (m_s). Each quantum number provides specific information about the electron's energy, shape, orientation, and spin.

Principal Quantum Number (n)

The principal quantum number (n) indicates the main energy level or shell of an electron in an atom. It can take positive integer values (1, 2, 3, ...), with higher values corresponding to higher energy levels and greater distances from the nucleus. In multielectron atoms, n significantly influences the energy of the orbitals.

Azimuthal Quantum Number (l)

The azimuthal quantum number (l) defines the shape of the orbital and is associated with the angular momentum of the electron. It can take integer values from 0 to (n-1) for each principal quantum number. The value of l determines the type of orbital (s, p, d, f) and contributes to the energy of the electron in a multielectron atom.