Azimuthal quantum number

Short description: Quantum number denoting orbital angular momentum

The atomic orbital wavefunctions of a hydrogen atom: The azimuthal quantum number (ℓ) is denoted by letter at the top of each column. The principal quantum number (n) is shown at the right of each row.

In quantum mechanics, the azimuthal quantum number is a quantum number for an atomic orbital that determines its orbital angular momentum and describes the shape of the orbital. The azimuthal quantum number is the second of a set of quantum numbers that describe the unique quantum state of an electron (the others being the principal quantum number n, the magnetic quantum number mℓ, and the spin quantum number ms). It is also known as the orbital angular momentum quantum number, orbital quantum number, subsidiary quantum number, or second quantum number, and is symbolized as ℓ (pronounced ell).

## Contents

* 1 Derivation
* 2 Addition of quantized angular momenta
* 2.1 Total angular momentum of an electron in the atom
* 2.1.1 Relation between new and old quantum numbers
* 3 List of angular momentum quantum numbers
* 4 History
* 5 See also
* 6 References
* 7 External links

## Derivation

There are four quantum numbers—n, ℓ, mℓ, ms— connected with the energy states of an atom's electrons. These four numbers specify the unique and complete quantum state of any single electron in the atom, and they combine to compose the electron's wavefunction, or orbital.

When solving to obtain the wave function, the Schrödinger equation resolves into three equations that lead to the first three quantum numbers, meaning that the three equations are interrelated. The azimuthal quantum number arises in solving the polar part of the wave equation—relying on the spherical coordinate system, which generally works best with models having sufficient aspects of spherical symmetry.

Azimuthal quantum number: Illustrating (five) alternative orbital angular momentum shapes as "cones"—here portraying (five) alternaive values for the reduced Planck's constant, ħ.

An electron's angular momentum, L, is related to its quantum number ℓ by the following equation: [math]\displaystyle{ \mathbf{L}^2\Psi = \hbar^2 \ell(\ell + 1) \Psi, }[/math] where ħ is the reduced Planck's constant, L is the orbital angular momentum operator and [math]\displaystyle{ \Psi }[/math] is the wavefunction of the electron. The quantum number ℓ is always a non-negative integer: 0, 1, 2, 3, etc. (Notably, L has no real meaning except in its use as the angular momentum operator; thus, it is standard practice to use the quantum number ℓ when referring to angular momentum).

Atomic orbitals have distinctive shapes, (see top graphic) in which letters, s, p, d, f, etc, (employing a convention originating in spectroscopy) denote the shape of the atomic orbital. The wavefunctions of these orbitals take the form of spherical harmonics, and so are described by Legendre polynomials. The several orbitals relating to the different (integer) values of ℓ are sometimes called sub-shells—referred to by lowercase Latin letters chosen for historical reasons—as shown in the table "Quantum subshells for the azimuthal quantum number".

Quantum subshells for the azimuthal quantum number  Azimuthal
quantum
number (ℓ)  | Historical
letter  | Historical
name  | Maximum
electrons  | Shape

|
|
|
|

0  | s | sharp  | 2  | Spherical atomic orbital; (see: this picture of spherical harmonics, top row).
1  | p | principal  | 6  | Three dumbbell-shaped polar-aligned orbitals; one lobe on each pole of the x, y, and z axes (on both + and − axes).
2  | d | diffuse  | 10  | Nine dumbbells and one doughnut, or "Unique shape #1"; (see: this picture of spherical harmonics, third row center).
3  | f | fundamental  | 14  | "Unique shape #2"; (see: this picture of spherical harmonics, bottom row center).
4  | g | gallant  | 18
5  | h |  | 22
6  | i |  | 26
The letters after the g sub-shell follow in alphabetical order—excepting letter j and those already used.

Each of the different angular momentum states can take 2(2ℓ + 1) electrons. This is because the third quantum number mℓ (which can be thought of loosely as the quantized projection of the angular momentum vector on the z-axis) runs from −ℓ to ℓ in integer units, and so there are 2ℓ + 1 possible states. Each distinct n, ℓ, mℓ orbital can be occupied by two electrons with opposing spins (given by the quantum number ms = ±​1⁄2), giving 2(2ℓ + 1) electrons overall. Orbitals with higher ℓ than given in the table are perfectly permissible, but these values cover all atoms so far discovered.

For a given value of the principal quantum number n, the possible values of ℓ range from 0 to n − 1; therefore, the n = 1 shell only possesses an s subshell and can only take 2 electrons, the n = 2 shell possesses an s and a p subshell and can take 8 electrons overall, the n = 3 shell possesses s, p, and d subshells and has a maximum of 18 electrons, and so on.

A simplistic one-electron model results in energy levels depending on the principal number alone. In more complex atoms these energy levels split for all n > 1, placing states of higher ℓ above states of lower ℓ. For example, the energy of 2p is higher than of 2s, 3d occurs higher than 3p, which in turn is above 3s, etc. This effect eventually forms the block structure of the periodic table. No known atom possesses an electron having ℓ higher than three (f) in its ground state.

The angular momentum quantum number, ℓ, governs the number of planar nodes going through the nucleus. A planar node can be described in an electromagnetic wave as the midpoint between crest and trough, which has zero magnitudes. In an s orbital, no nodes go through the nucleus, therefore the corresponding azimuthal quantum number ℓ takes the value of 0. In a p orbital, one node traverses the nucleus and therefore ℓ has the value of 1. [math]\displaystyle{ L }[/math] has the value [math]\displaystyle{ \sqrt{2}\hbar }[/math].

Depending on the value of n, there is an angular momentum quantum number ℓ and the following series. The wavelengths listed are for a hydrogen atom:

* [math]\displaystyle{ n = 1, L = 0 }[/math], Lyman series (ultraviolet)
* [math]\displaystyle{ n = 2, L = \sqrt{2}\hbar }[/math], Balmer series (visible)
* [math]\displaystyle{ n = 3, L = \sqrt{6}\hbar }[/math], Ritz–Paschen series (near infrared)
* [math]\displaystyle{ n = 4, L = 2\sqrt{3}\hbar }[/math], Brackett series (short-wavelength infrared)
* [math]\displaystyle{ n = 5, L = 2\sqrt{5}\hbar }[/math], Pfund series (mid-wavelength infrared).

## Addition of quantized angular momenta

Further information: Physics:Angular momentum coupling

Given a quantized total angular momentum [math]\displaystyle{ \mathbf{j} }[/math] which is the sum of two individual quantized angular momenta [math]\displaystyle{ \boldsymbol{\ell}_1 }[/math] and [math]\displaystyle{ \boldsymbol{\ell}_2 }[/math], [math]\displaystyle{ \mathbf{j} = \boldsymbol{\ell}_1 + \boldsymbol{\ell}_2 }[/math] the quantum number [math]\displaystyle{ j }[/math] associated with its magnitude can range from [math]\displaystyle{ |\ell_1 - \ell_2| }[/math] to [math]\displaystyle{ \ell_1 + \ell_2 }[/math] in integer steps where [math]\displaystyle{ \ell_1 }[/math] and [math]\displaystyle{ \ell_2 }[/math] are quantum numbers corresponding to the magnitudes of the individual angular momenta.

### Total angular momentum of an electron in the atom

"Vector cones" of total angular momentum J (purple), orbital L (blue), and spin S (green). The cones arise due to quantum uncertainty between measuring angular momentum components (see vector model of the atom).

Due to the spin–orbit interaction in the atom, the orbital angular momentum no longer commutes with the Hamiltonian, nor does the spin. These therefore change over time. However the total angular momentum J does commute with the one-electron Hamiltonian and so is constant. J is defined through [math]\displaystyle{ \mathbf{J} = \mathbf{L} + \mathbf{S} }[/math] L being the orbital angular momentum and S the spin. The total angular momentum satisfies the same commutation relations as orbital angular momentum, namely [math]\displaystyle{ [J_i, J_j ] = i \hbar \varepsilon_{ijk} J_k }[/math] from which follows [math]\displaystyle{ \left[J_i, J^2 \right] = 0 }[/math] where Ji stand for Jx, Jy, and Jz.

The quantum numbers describing the system, which are constant over time, are now j and mj, defined through the action of J on the wavefunction [math]\displaystyle{ \Psi }[/math] [math]\displaystyle{ \begin{align} \mathbf{J}^2\Psi &= \hbar^2 j(j+1) \Psi \\\\[1ex] \mathbf{J}_z\Psi &= \hbar m_j\Psi \end{align} }[/math]

So that j is related to the norm of the total angular momentum and mj to its projection along a specified axis. The j number has a particular importance for relativistic quantum chemistry, often featuring in subscript in electron configuration of superheavy elements.

As with any angular momentum in quantum mechanics, the projection of J along other axes cannot be co-defined with Jz, because they do not commute.

#### Relation between new and old quantum numbers

j and mj, together with the parity of the quantum state, replace the three quantum numbers ℓ, mℓ and ms (the projection of the spin along the specified axis). The former quantum numbers can be related to the latter.

Furthermore, the eigenvectors of j, s, mj and parity, which are also eigenvectors of the Hamiltonian, are linear combinations of the eigenvectors of ℓ, s, mℓ and ms.

## List of angular momentum quantum numbers

* Intrinsic (or spin) angular momentum quantum number, or simply spin quantum number
* orbital angular momentum quantum number (the subject of this article)
* magnetic quantum number, related to the orbital momentum quantum number
* total angular momentum quantum number

## History

The azimuthal quantum number was carried over from the Bohr model of the atom, and was posited by Arnold Sommerfeld.[1] The Bohr model was derived from spectroscopic analysis of the atom in combination with the Rutherford atomic model. The lowest quantum level was found to have an angular momentum of zero. Orbits with zero angular momentum were considered as oscillating charges in one dimension and so described as "pendulum" orbits, but were not found in nature.[2] In three-dimensions the orbits become spherical without any nodes crossing the nucleus, similar (in the lowest-energy state) to a skipping rope that oscillates in one large circle.

## See also

* Angular momentum operator
* Introduction to quantum mechanics
* Particle in a spherically symmetric potential
* Angular momentum coupling
* Clebsch–Gordan coefficients

## References

1. ↑ Eisberg, Robert (1974). Quantum Physics of Atoms, Molecules, Solids, Nuclei and Particles. New York: John Wiley & Sons Inc. pp. 114–117. ISBN 978-0-471-23464-7.
2. ↑ R.B. Lindsay (1927). "Note on "pendulum" orbits in atomic models". Proc. Natl. Acad. Sci. 13 (6): 413–419. doi:10.1073/pnas.13.6.413. PMID 16587189. Bibcode: 1927PNAS...13..413L.

## External links

* Development of the Bohr atom
* Detailed explanation of the Orbital Quantum Number l
* The azimuthal equation explained

* v
* t
* e

Electron configuration

* Electron shell
* Introduction to quantum mechanics
* Quantum mechanics

Quantum numbers|

* Principal quantum number (n)
* Azimuthal quantum number (ℓ)
* Magnetic quantum number (m)
* Spin quantum number (s)

Periodic table|

* Periodic table (electron configurations)

Principles|

* Pauli exclusion principle
* Hund's rule
* Aufbau principle

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