A set of the four quantum numbers describes the unique properties of one specific electron in an atom. Since each set is unique, they serve as a way of uniquely naming individual electrons (i.e. a kind of coordinate system). The first three, \(n,\) \(\ell,\) and \(m_\ell,\) come from the solution to the spherical Schrödinger equation and describe the orbital of the electron, which is the shape of its wave function. The fourth number, \(m_s,\) accounts for the fermion status of the electron by describing its spin.
\[ \]
| Symbol | Name | Associated property | Describes |
| \(n\) | Principal quantum number | Energy level | Orbital size |
| \(\ell\) | Angular quantum number | Magnitude of the angular momentum | Orbital shape |
| \(m_\ell\) | Magnetic quantum number | Z component of the angular momentum | Orientation in space |
| \(m_s\) | Spin quantum number | Z component of spin | Whether electron is spin up or spin down |
\[ \]
This is a representation of a hydrogen atom in the state \(n = 12, \ell = 6, m_{\ell}=6.\)[1]
Contents
- Principal Quantum Number
- Angular Quantum Number
- Magnetic Quantum Number
- Spin Quantum Number
- References
Principal Quantum Number
It was given by Niels Bohr. The principle quantum number, \(n,\) represents the energy level of an electron. As \(n\) increases, more electrons are permitted in the shell, the electron is farther from the nucleus, and the electron is bound more loosely to the atom. In order to represent the quantization of the energy levels, the principle quantum number may only take on positive integer values.
The energy of an electron in the \(nth\) shell of any hydrogen-like atom is \[E_n = \frac{-13.6 \text{ eV}}{n^2}.\]
Angular Quantum Number
It was given by Sommerfeld who suggested the presence of elliptical orbits. 
Each of these concentric rings of latitude represents a different azimuthal position measured from the geographic North pole.[2]
The angular quantum number describes the azimuthal component of the angular momentum of the electron. As an orbiting particle's energy increases, the amount of angular momentum it may have increases accordingly. But since the energy of an electron is restricted to specific values, the angular momentum is also restricted. The relationship between the quantization of the energy and the angular momentum is expressed in terms of the quantum numbers associated with each:
\[\ell = 0, 1, 2, ..., n-1.\]
What are the permitted values of \(\ell\) for the \(n=4\) orbital?
As \(\ell\) can take any positive integer value less than \(n\), the possible values are \[0, 1, 2, \text{ and } 3.\]
\[n=3, \ell=1\] \[n=2, \ell=2\] \[n=5, \ell=3\] \[n=4, \ell=0\]
Which of these pairs of quantum numbers is not permitted?
It turns out the magnitude of the angular momentum of an electron orbiting an atom is described by the angular quantum number \(\ell\) according to \[L = \sqrt{\ell(\ell+1)}\hbar.\]
What are the possible angular momenta of an electron in the \(n=3\) orbital?
First, write down the permitted angular quantum numbers: \[\ell = 0, 1, 2.\]
Next, calculate the angular momentum associated with each value of \(\ell.\)
\(\ell\text{ }\) \(L\) 0 0 1 \(\sqrt{2}\hbar\) 2 \(\sqrt{6}\hbar\)
The angular momentum of an electron located in the \(\ell = 4\) subshell of an atom can be expressed \(\sqrt{a}\hbar.\) What is the value of \(a?\)
Magnetic Quantum Number
It was given by Lande. The magnetic quantum number, \(m_{\ell},\) describes the number of preferred orientations of the electrons present in a subshell. It is restricted by \(\ell.\)
The permitted values of \(m_{\ell}\) are \[m_{\ell} = -\ell, -(\ell-1), -(\ell-2), \text{ ...} ,(\ell-2), (\ell-1), \ell.\]
What are the possible orbitals of the \(n=3\) shell?
First, \(\ell\) is permitted to have the values \[\ell = 0, 1, 2, 3.\]
Next, the values of \(m_{\ell}\) must satisfy the relation \(|m_{\ell}| \leq \ell.\)
\(\ell\text{ }\) \(m_{\ell}\) 0 0 1 -1, 0, 1 2 -2, -1, 0, 1, 2 3 -3, -2, -1, 0, 1, 2, 3
\[n = 4, \ell = 3, m_{\ell}=-2\] \[n = 3, \ell = 1, m_{\ell}=-1\] \[n = 2, \ell = 1, m_{\ell}=-2\] \[n = 1, \ell = 0, m_{\ell}=0\] \[n = 4, \ell = 2, m_{\ell}=-2\]
Which of the following sets of quantum numbers is not allowed?
Spin Quantum Number
It was given by Ulhenbeck and Goud Smit. The spin quantum number, \(m_s,\) represents the spin of an electron. Since electrons are fermions, they may only have half-integer spin, sometimes called "spin up" and "spin down." Also, as a consequence of their fermion status, electrons obey the Pauli's exclusion principle, which is why each set of quantum numbers within an atom is unique to the electron it describes.
The permitted spin quantum numbers of an electron are \[m_s = \pm \frac12.\]
References
- Berndthaller, . Hydrogen atom with magnetic quantum number m=1.jpg. Retrieved April 27, 2016, from https://commons.wikimedia.org/wiki/File:Hydrogen_atom_with_magnetic_quantum_number_m%3D1.jpg
- Liao, C. Northern-Hemisphere-Azimuthal-projections. Retrieved April 26, 2016, from https://upload.wikimedia.org/wikipedia/commons/thumb/5/59/Northern_Hemisphere_Azimuthal_projections.svg/1200px-Northern_Hemisphere_Azimuthal_projections.svg.png
