Enter your Principal Quantum Number (n) into the Quantum Number Calculator, choose What to Calculate, and optionally specify an Angular Momentum Quantum Number (l) to get your Possible l Values, along with Possible ml and ms Values, Maximum Electrons in Shell, and all Orbital Types Available for that energy level.
Possible l Values
--
Possible ml Values
--
Possible ms Values
--
Maximum Electrons in Shell
--
Orbital Types Available
--
The four quantum numbers are: Principal (n) - determines energy level and size; Angular momentum (l) - determines shape of orbital; Magnetic (ml) - determines orientation in space; and Spin (ms) - determines electron spin direction (+1/2 or -1/2).
The magnetic quantum number (ml) ranges from -l to +l, including zero. For example, if l = 2 (d orbital), then ml can be -2, -1, 0, +1, or +2, giving 5 possible orientations.
The principal quantum number (n) determines the electron's energy level and the average distance from the nucleus. Higher n values mean higher energy and greater distance from the nucleus.
The angular momentum quantum number (l) describes the shape of the orbital. l = 0 gives s orbitals (spherical), l = 1 gives p orbitals (dumbbell-shaped), l = 2 gives d orbitals (complex shapes), and l = 3 gives f orbitals.
The maximum number of electrons in a shell is given by 2n², where n is the principal quantum number. For example, the first shell (n=1) holds 2 electrons, the second shell (n=2) holds 8 electrons.
Pauli's exclusion principle states that no two electrons in an atom can have identical sets of quantum numbers. This means each electron has a unique 'address' defined by its four quantum numbers.
The spin quantum number (ms) can only have two values: +1/2 (spin up) or -1/2 (spin down). This represents the two possible orientations of electron spin in a magnetic field.