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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 $ℓ$ is a quantum number for an atomic orbital that determines its orbital angular momentum and describes aspects of the angular 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 $m ℓ$ , and the spin quantum number $m s$ ).

For a given value of the principal quantum number $n$ (electron shell), the possible values of $ℓ$ are the integers from 0 to $n - 1$ . For instance, the $n = 1$ shell has only orbitals with $\ell =0$ , and the $n = 2$ shell has only orbitals with $\ell =0$ , and $\ell =1$ .

For a given value of the azimuthal quantum number $ℓ$ , the possible values of the magnetic quantum number $m ℓ$ are the integers from $m ℓ =-ℓ$ to $m ℓ =+ℓ$ , including 0. In addition, the spin quantum number $m s$ can take two distinct values. The set of orbitals associated with a particular value of $ℓ$ are sometimes collectively called a subshell.

While originally used just for isolated atoms, atomic-like orbitals play a key role in the configuration of electrons in compounds including gases, liquids and solids. The quantum number $ℓ$ plays an important role here via the connection to the angular dependence of the spherical harmonics for the different orbitals around each atom.

Nomenclature

The term "azimuthal quantum number" was introduced by Arnold Sommerfeld in 1915^[1]^: II:132 as part of an ad hoc description of the energy structure of atomic spectra. Only later with the quantum model of the atom was it understood that this number, $ℓ$ , arises from quantization of orbital angular momentum. Some textbooks^[2]^: 199 and the ISO standard 80000-10:2019^[3] call $ℓ$ the orbital angular momentum quantum number.

The energy levels of an atom in an external magnetic field depend upon the $m ℓ$ value so it is sometimes called the magnetic quantum number.^[4]^: 240

The lowercase letter $ℓ$ , is used to denote the orbital angular momentum of a single particle. For a system with multiple particles, the capital letter $L$ is used.^[3]

Relation to atomic orbitals

There are four quantum numbers—n, ℓ, m_ℓ, m_s— connected with the energy states of an isolated 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.

An electron's angular momentum, $L$ , is related to its quantum number $ℓ$ by the following equation: $\mathbf {L} ^{2}\Psi =\hbar ^{2}\ell (\ell +1)\Psi ,$ where $ħ$ is the reduced Planck constant, $L$ is the orbital angular momentum operator and $\Psi$ 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^[5]^: II:133	Maximum electrons	Shape
0	s	sharp	2	Spherical (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		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 m_ℓ (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, m_ℓ orbital can be occupied by two electrons with opposing spins (given by the quantum number m_s = ±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 and the corresponding spherical harmonic govern 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. $L$ has the value ${\sqrt {2}}\hbar$ .

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:

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

Addition of quantized angular momenta

Given a quantized total angular momentum $\mathbf {j}$ that is the sum of two individual quantized angular momenta ${\boldsymbol {\ell }}_{1}$ and ${\boldsymbol {\ell }}_{2}$ , $\mathbf {j} ={\boldsymbol {\ell }}_{1}+{\boldsymbol {\ell }}_{2}$ the quantum number $j$ associated with its magnitude can range from $|\ell _{1}-\ell _{2}|$ to $\ell _{1}+\ell _{2}$ in integer steps where $\ell _{1}$ and $\ell _{2}$ are quantum numbers corresponding to the magnitudes of the individual angular momenta.

Total angular momentum of an electron in the atom

Due to the spin–orbit interaction in an 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 as $\mathbf {J} =\mathbf {L} +\mathbf {S}$ $L$ being the orbital angular momentum and $S$ the spin. The total angular momentum satisfies the same commutation relations as orbital angular momentum, namely $[J_{i},J_{j}]=i\hbar \varepsilon _{ijk}J_{k}$ from which it follows that $\left[J_{i},J^{2}\right]=0$ where $J i$ stand for $J x$ , $J y$ , and $J z$ .

The quantum numbers describing the system, which are constant over time, are now $j$ and $m j$ , defined through the action of $J$ on the wavefunction $\Psi$ ${\begin{aligned}\mathbf {J} ^{2}\Psi &=\hbar ^{2}j(j+1)\Psi \\[1ex]\mathbf {J} _{z}\Psi &=\hbar m_{j}\Psi \end{aligned}}$

So that $j$ is related to the norm of the total angular momentum and $m j$ to its projection along a specified axis. The j number has a particular importance for relativistic quantum chemistry, often featuring in subscript in for deeper states near to the core for which spin-orbit coupling is important.

As with any angular momentum in quantum mechanics, the projection of $J$ along other axes cannot be co-defined with $J z$ , because they do not commute. The eigenvectors of $j$ , $s$ , $m j$ and parity, which are also eigenvectors of the Hamiltonian, are linear combinations of the eigenvectors of $ℓ$ , $s$ , $m ℓ$ and $m s$ .

Beyond isolated atoms

The angular momentum quantum numbers strictly refer to isolated atoms. However, they have wider uses for atoms in solids, liquids or gases. The $ℓ m$ quantum number corresponds to specific spherical harmonics and are commonly used to describe features observed in spectroscopic methods such as X-ray photoelectron spectroscopy^[6] and electron energy loss spectroscopy.^[7] (The notation is slightly different, with X-ray notation where K, L, M are used for excitations out of electron states with $n=0,1,2$ .)

The angular momentum quantum numbers are also used when the electron states are described in methods such as Kohn–Sham density functional theory^[8] or with gaussian orbitals.^[9] For instance, in silicon the electronic properties used in semiconductor device are due to the p-like states with $l=1$ centered at each atom, while many properties of transition metals depend upon the d-like states with $l=2$ .^[10]

History

The azimuthal quantum number was carried over from the Bohr model of the atom, and was posited by Arnold Sommerfeld.^[11] The Bohr model was derived from spectroscopic analysis of atoms 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.^[12] 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.

References

^ Whittaker, Edmund Taylor (1989). A history of the theories of aether and electricity. Dover classics of science and mathematics. New York: Dover. ISBN 978-0-486-26126-3.
^ Schiff, Leonard (1949). Quantum mechanics. McGraw-Hill.
^ ^a ^b "ISO Online Browsing Platform". 10-13.3. Retrieved 2024-02-20.
^ Eisberg, Robert M.; Resnick, Robert (2009). Quantum physics of atoms, molecules, solids, nuclei, and particles (2. ed., 37. [Nachdr.] ed.). New York: Wiley. ISBN 978-0-471-87373-0.
^ Whittaker, E. T. (1989). A history of the theories of aether & electricity. New York: Dover Publications. ISBN 978-0-486-26126-3.
^ Hüfner, Stefan (2003). Photoelectron Spectroscopy. Advanced Texts in Physics. Berlin, Heidelberg: Springer Berlin Heidelberg. doi:10.1007/978-3-662-09280-4. ISBN 978-3-642-07520-9.
^ Egerton, R.F. (2011). Electron Energy-Loss Spectroscopy in the Electron Microscope. Boston, MA: Springer US. doi:10.1007/978-1-4419-9583-4. ISBN 978-1-4419-9582-7.
^ Kohn, W.; Sham, L. J. (1965). "Self-Consistent Equations Including Exchange and Correlation Effects". Physical Review. 140 (4A): A1133–A1138. doi:10.1103/PhysRev.140.A1133. ISSN 0031-899X.
^ Gill, Peter M.W. (1994), "Molecular integrals Over Gaussian Basis Functions", Advances in Quantum Chemistry, vol. 25, Elsevier, pp. 141–205, doi:10.1016/s0065-3276(08)60019-2, ISBN 978-0-12-034825-1, retrieved 2024-02-20
^ Pettifor, D. G. (1996). Bonding and structure of molecules and solids. Oxford science publications (Reprint with corr ed.). Oxford: Clarendon Press. ISBN 978-0-19-851786-3.
^ 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.
^ R.B. Lindsay (1927). "Note on "pendulum" orbits in atomic models". Proc. Natl. Acad. Sci. 13 (6): 413–419. Bibcode:1927PNAS...13..413L. doi:10.1073/pnas.13.6.413. PMC 1085028. PMID 16587189.

External links

[1] Whittaker, Edmund Taylor (1989). A history of the theories of aether and electricity. Dover classics of science and mathematics. New York: Dover. ISBN 978-0-486-26126-3.

[Schiff-2] Schiff, Leonard (1949). Quantum mechanics. McGraw-Hill.

[iso-3] "ISO Online Browsing Platform". 10-13.3. Retrieved 2024-02-20.

[4] Eisberg, Robert M.; Resnick, Robert (2009). Quantum physics of atoms, molecules, solids, nuclei, and particles (2. ed., 37. [Nachdr.] ed.). New York: Wiley. ISBN 978-0-471-87373-0.

[5] Whittaker, E. T. (1989). A history of the theories of aether & electricity. New York: Dover Publications. ISBN 978-0-486-26126-3.

[6] Hüfner, Stefan (2003). Photoelectron Spectroscopy. Advanced Texts in Physics. Berlin, Heidelberg: Springer Berlin Heidelberg. doi:10.1007/978-3-662-09280-4. ISBN 978-3-642-07520-9.

[7] Egerton, R.F. (2011). Electron Energy-Loss Spectroscopy in the Electron Microscope. Boston, MA: Springer US. doi:10.1007/978-1-4419-9583-4. ISBN 978-1-4419-9582-7.

[8] Kohn, W.; Sham, L. J. (1965). "Self-Consistent Equations Including Exchange and Correlation Effects". Physical Review. 140 (4A): A1133–A1138. doi:10.1103/PhysRev.140.A1133. ISSN 0031-899X.

[9] Gill, Peter M.W. (1994), "Molecular integrals Over Gaussian Basis Functions", Advances in Quantum Chemistry, vol. 25, Elsevier, pp. 141–205, doi:10.1016/s0065-3276(08)60019-2, ISBN 978-0-12-034825-1, retrieved 2024-02-20

[10] Pettifor, D. G. (1996). Bonding and structure of molecules and solids. Oxford science publications (Reprint with corr ed.). Oxford: Clarendon Press. ISBN 978-0-19-851786-3.

[11] 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.

[12] R.B. Lindsay (1927). "Note on "pendulum" orbits in atomic models". Proc. Natl. Acad. Sci. 13 (6): 413–419. Bibcode:1927PNAS...13..413L. doi:10.1073/pnas.13.6.413. PMC 1085028. PMID 16587189.

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@@ Line 4: / Line 4: @@
 In [[quantum mechanics]], the '''azimuthal quantum number''' {{mvar|ℓ}} is a [[quantum number]] for an [[atomic orbital]] that determines its [[angular momentum operator|orbital angular momentum]] and describes aspects of the angular shape of the orbital. The [[azimuth]]al 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]] {{mvar|n}}, the [[magnetic quantum number]] {{mvar|''m''{{sub|ℓ}}}}, and the [[spin quantum number]] {{mvar|''m''{{sub|s}}}}).
-For a given value of the principal quantum number {{mvar|n}} (''[[electron shell]]''), the possible values of {{mvar|ℓ}} are the integers from 0 to {{math|1=''n''-1}}. For instance, the {{math|1=''n'' = 1}}&nbsp;shell has only orbitals with <math>\ell=0</math>, and the {{math|1=''n'' = 2}}&nbsp;shell has only orbitals with <math>\ell=0</math>, and <math>\ell=1</math>.
+For a given value of the principal quantum number {{mvar|n}} (''[[electron shell]]''), the possible values of {{mvar|ℓ}} are the integers from 0 to {{math|1=''n'' − 1}}. For instance, the {{math|1=''n'' = 1}}&nbsp;shell has only orbitals with <math>\ell=0</math>, and the {{math|1=''n'' = 2}}&nbsp;shell has only orbitals with <math>\ell=0</math>, and <math>\ell=1</math>.
 For a given value of the azimuthal quantum number {{mvar|ℓ}}, the possible values of the magnetic quantum number {{mvar|''m''{{sub|ℓ}}}} are the integers from {{math|1=''m''{{sub|ℓ}}=-ℓ}} to {{math|1=''m''{{sub|ℓ}}=+ℓ}}, including 0. In addition, the spin quantum number {{mvar|''m''{{sub|s}}}} can take two distinct values. The set of orbitals associated with a particular value of&nbsp;{{mvar|ℓ}} are sometimes collectively called a ''subshell''.
@@ Line 11: / Line 11: @@
 == Nomenclature ==
-The term "azimuthal quantum number" was introduced by [[Arnold Sommerfeld]] in 1915<ref>{{Cite book |last=Whittaker |first=Edmund Taylor |title=A history of the theories of aether and electricity |date=1989 |publisher=Dover |isbn=978-0-486-26126-3 |series=Dover classics of science and mathematics |location=New York}}</ref>{{rp|II:132}} as part of an ad hoc description of the energy structure of atomic spectra. Only later with the quantum model of the atom was it understood that this number, {{mvar|ℓ}}, arises from quantization of orbital angular momentum. Some textbooks<ref name=Schiff>{{Cite book |last=Schiff |first= Leonard  |title=Quantum mechanics |publisher= McGraw-Hill |year= 1949}}</ref>{{rp|199}} and the ISO standard 80000-10:2019<ref>{{Cite web |title=ISO Online Browsing Platform |url=https://www.iso.org/obp/ui/en/#iso:std:iso:80000:-10:ed-2:v1:en |access-date=2024-02-20 |at=10-13.3}}</ref> call {{mvar|ℓ}} the '''orbital angular momentum quantum number'''.
+The term "azimuthal quantum number" was introduced by [[Arnold Sommerfeld]] in 1915<ref>{{Cite book |last=Whittaker |first=Edmund Taylor |title=A history of the theories of aether and electricity |date=1989 |publisher=Dover |isbn=978-0-486-26126-3 |series=Dover classics of science and mathematics |location=New York}}</ref>{{rp|II:132}} as part of an ad hoc description of the energy structure of atomic spectra. Only later with the quantum model of the atom was it understood that this number, {{mvar|ℓ}}, arises from quantization of orbital angular momentum. Some textbooks<ref name=Schiff>{{Cite book |last=Schiff |first= Leonard  |title=Quantum mechanics |publisher= McGraw-Hill |year= 1949}}</ref>{{rp|199}} and the ISO standard 80000-10:2019<ref name="iso">{{Cite web |title=ISO Online Browsing Platform |url=https://www.iso.org/obp/ui/en/#iso:std:iso:80000:-10:ed-2:v1:en |access-date=2024-02-20 |at=10-13.3}}</ref> call {{mvar|ℓ}} the '''orbital angular momentum quantum number'''.
 The energy levels of an atom in an external magnetic field depend upon the {{mvar|''m''{{sub|ℓ}}}} value so it is sometimes called the  magnetic quantum number.<ref>{{Cite book |last=Eisberg |first=Robert M. |title=Quantum physics of atoms, molecules, solids, nuclei, and particles |last2=Resnick |first2=Robert |date=2009 |publisher=Wiley |isbn=978-0-471-87373-0 |edition=2. ed., 37. [Nachdr.] |location=New York}}</ref>{{rp|240}}
+The lowercase letter {{mvar|ℓ}}, is used to denote the orbital angular momentum of a single particle. For a system with multiple particles, the capital letter {{mvar|L}} is used.<ref name="iso"/>
 == Relation to atomic orbitals ==
 There are four quantum numbers{{mdash}}''n'', ''ℓ'', ''m''<sub>''ℓ''</sub>, ''m''<sub>''s''</sub>{{mdash}} connected with the energy states of an isolated 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 ''[[atomic orbital#Electron properties|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{{mdash}}relying on the [[spherical coordinate system]], which generally works best with models having sufficient aspects of [[spherical symmetry]].
-[[File:Vector model of orbital angular momentum.svg|left|thumb|Azimuthal quantum number: Illustrating (five) alternative ''orbital angular momentum'' shapes  as "cones"{{mdash}}here portraying (five) alternative values for the reduced Planck's constant, {{math|''ħ''}}.]]
+[[File:Vector model of orbital angular momentum.svg|left|thumb|Azimuthal quantum number: Illustrating (five) alternative ''orbital angular momentum'' shapes  as "cones"{{mdash}}here portraying (five) alternative values for the reduced Planck constant, {{math|''ħ''}}.]]
 An electron's angular momentum, {{math|''L''}}, is related to its quantum number {{math|''ℓ''}} by the following equation:
 <math display="block">\mathbf{L}^2\Psi = \hbar^2 \ell(\ell + 1) \Psi,</math>
-where {{math|''ħ''}} is the [[reduced Planck's constant]], {{math|'''L'''}} is the orbital ''[[angular momentum operator]]'' and <math>\Psi</math> is the wavefunction of the electron. The quantum number {{math|''ℓ''}} is always a non-negative integer: 0, 1, 2, 3, etc. (Notably, {{math|'''L'''}} has no real meaning except in its use as the angular momentum operator; thus, it is standard practice to use the quantum number {{math|''ℓ''}} when referring to angular momentum).
+where {{math|''ħ''}} is the [[reduced Planck constant]], {{math|'''L'''}} is the orbital ''angular momentum operator'' and <math>\Psi</math> is the wavefunction of the electron. The quantum number {{math|''ℓ''}} is always a non-negative integer: 0, 1, 2, 3, etc. (Notably, {{math|'''L'''}} has no real meaning except in its use as the angular momentum operator; thus, it is standard practice to use the quantum number {{math|''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 [[Spectroscopic notation#Atomic and molecular orbitals|spectroscopy]]) denote the shape of the [[atomic orbital]]. The wavefunctions of these orbitals take the form of [[spherical harmonic]]s, and so are described by [[associated Legendre polynomials|Legendre polynomials]]. The several orbitals relating to the different (integer) values of ''ℓ'' are sometimes called '''sub-shells'''{{mdash}}referred to by lowercase [[Latin letters]] chosen for historical reasons{{mdash}}as shown in the table "Quantum subshells for the azimuthal quantum number".
+Atomic orbitals have distinctive shapes, (see top graphic) in which letters, '''s''', '''p''', '''d''', '''f''', etc., (employing a convention originating in [[Spectroscopic notation#Atomic and molecular orbitals|spectroscopy]]) denote the shape of the atomic orbital. The wavefunctions of these orbitals take the form of [[spherical harmonic]]s, and so are described by [[associated Legendre polynomials|Legendre polynomials]]. The several orbitals relating to the different (integer) values of ''ℓ'' are sometimes called '''sub-shells'''{{mdash}}referred to by lowercase [[Latin letters]] chosen for historical reasons{{mdash}}as shown in the table "Quantum subshells for the azimuthal quantum number".
 {{Clear}}
 {| class="wikitable"
@@ Line 34: / Line 35: @@
 ! style="text-align: center; vertical-align: bottom;"| Azimuthal<br/>quantum<br/>number&nbsp;(''ℓ'')
 ! style="text-align: center; vertical-align: bottom;"| Historical<br/>letter
-! style="text-align: center; vertical-align: bottom;"| Historical<br/>name
+! style="text-align: center; vertical-align: bottom;"| Historical<br/>name<ref>{{Cite book |last=Whittaker |first=E. T. |title=A history of the theories of aether & electricity |date=1989 |publisher=Dover Publications |isbn=978-0-486-26126-3 |location=New York}}</ref>{{rp|II:133}}
 ! style="text-align: center; vertical-align: bottom;"| Maximum<br/>electrons
 ! style="text-align: left; vertical-align: bottom;"| Shape
@@ Line 64: / Line 65: @@
 | style="text-align: center;"| 4
 | style="text-align: center;"| '''g'''
-| style="text-align: left;"| '''g'''allant
+| style="text-align: left;"|
 | style="text-align: center;"| 18
 |-
@@ Line 79: / Line 80: @@
 | colspan=5 style="text-align: left; text-align: center;" | The letters after the '''g''' sub-shell follow in alphabetical order{{mdash}}excepting letter&nbsp;''j'' and those already used.
 |}
 Each of the different angular momentum states can take 2(2''ℓ''&nbsp;+&nbsp;1) electrons. This is because the third quantum number ''m''<sub>ℓ</sub> (which can be thought of loosely as the [[angular momentum quantization|quantized]] projection of the angular momentum vector on the z-axis) runs from &minus;''ℓ'' to ''ℓ'' in integer units, and so there are 2''ℓ''&nbsp;+&nbsp;1 possible states. Each distinct ''n'', ''ℓ'', ''m''<sub>ℓ</sub> orbital can be occupied by two electrons with opposing spins (given by the quantum number ''m''<sub>s</sub>&nbsp;=&nbsp;±{{1/2}}), giving 2(2''ℓ''&nbsp;+&nbsp;1) electrons overall. Orbitals with higher ''ℓ'' than given in the table are perfectly permissible, but these values cover all atoms so far discovered.
@@ Line 100: / Line 100: @@
 == Addition of quantized angular momenta ==
 {{further|Angular momentum coupling}}
-Given a quantized total angular momentum <math>\mathbf{j}</math> which is the sum of two individual quantized angular momenta <math>\boldsymbol{\ell}_1</math> and <math>\boldsymbol{\ell}_2</math>,
+Given a quantized total angular momentum <math>\mathbf{j}</math> that is the sum of two individual quantized angular momenta <math>\boldsymbol{\ell}_1</math> and <math>\boldsymbol{\ell}_2</math>,
 <math display="block">\mathbf{j} = \boldsymbol{\ell}_1 + \boldsymbol{\ell}_2</math>
 the [[quantum number]] <math>j</math> associated with its magnitude can range from <math>|\ell_1 - \ell_2|</math> to <math>\ell_1 + \ell_2</math> in integer steps
@@ Line 124: / Line 124: @@
 So that {{math|''j''}} is related to the norm of the total angular momentum and {{math|''m''<sub>''j''</sub>}} to its projection along a specified axis. The ''j'' number has a particular importance for [[relativistic quantum chemistry]], often featuring in subscript in for deeper states near to the core for which spin-orbit coupling is important.
-As with any [[Angular momentum operator|angular momentum in quantum mechanics]], the projection of {{math|'''J'''}} along other axes cannot be co-defined with {{math|''J''<sub>z</sub>}}, because they do not commute.
+As with any angular momentum in quantum mechanics, the projection of {{math|'''J'''}} along other axes cannot be co-defined with {{math|''J''<sub>z</sub>}}, because they do not commute.
 The [[eigenvector]]s of {{math|''j''}}, {{math|''s''}}, {{math|''m''<sub>''j''</sub>}} and parity, which are also eigenvectors of the Hamiltonian, are linear combinations of the eigenvectors of {{math|''ℓ''}}, {{math|''s''}}, {{math|''m''<sub>''ℓ''</sub>}} and {{math|''m''<sub>''s''</sub>}}.
@@ Line 130: / Line 130: @@
 {{See also|Density functional theory|History of spectroscopy}}
 [[File:Electron_energy_loss_spectroscopy_coreloss_lsmo.svg|thumb|Example of inner shell ionization edge (core loss) EELS data from La<sub>0.7</sub>Sr<sub>0.3</sub>MnO<sub>3</sub>, acquired in a [[Scanning transmission electron microscopy|scanning transmission electron microscope]].]]
 The angular momentum quantum numbers strictly refer to isolated atoms. However, they have wider uses for atoms in solids, liquids or gases. The {{math|''ℓ m''}} quantum number corresponds to specific [[spherical harmonics]] and are commonly used to describe features observed in spectroscopic methods such as [[X-ray photoelectron spectroscopy]]<ref>{{Cite book |last=Hüfner |first=Stefan |url=http://link.springer.com/10.1007/978-3-662-09280-4 |title=Photoelectron Spectroscopy |date=2003 |publisher=Springer Berlin Heidelberg |isbn=978-3-642-07520-9 |series=Advanced Texts in Physics |location=Berlin, Heidelberg |doi=10.1007/978-3-662-09280-4}}</ref> and [[electron energy loss spectroscopy]].<ref>{{Cite book |last=Egerton |first=R.F. |url=https://link.springer.com/10.1007/978-1-4419-9583-4 |title=Electron Energy-Loss Spectroscopy in the Electron Microscope |date=2011 |publisher=Springer US |isbn=978-1-4419-9582-7 |location=Boston, MA |language=en |doi=10.1007/978-1-4419-9583-4}}</ref> (The notation is slightly different, with [[X-ray notation]] where K, L, M are used for excitations out of electron states with <math>n=0, 1, 2</math>.)
-The angular momentum quantum numbers are also used when the electron states are described in methods such as [[Kohn–Sham equations|Kohn–Sham density functional theory]]<ref>{{Cite journal |last=Kohn |first=W. |last2=Sham |first2=L. J. |date=1965 |title=Self-Consistent Equations Including Exchange and Correlation Effects |url=https://link.aps.org/doi/10.1103/PhysRev.140.A1133 |journal=Physical Review |language=en |volume=140 |issue=4A |pages=A1133–A1138 |doi=10.1103/PhysRev.140.A1133 |issn=0031-899X}}</ref> or with [[Gaussian orbital|gaussian orbitals]].<ref>{{Citation |last=Gill |first=Peter M.W. |title=Molecular integrals Over Gaussian Basis Functions |date=1994 |work=Advances in Quantum Chemistry |volume=25 |pages=141–205 |url=https://linkinghub.elsevier.com/retrieve/pii/S0065327608600192 |access-date=2024-02-20 |publisher=Elsevier |language=en |doi=10.1016/s0065-3276(08)60019-2 |isbn=978-0-12-034825-1}}</ref> For instance, in [[silicon]] the electronic properties used in [[semiconductor device]] are due to the p-like states with <math>l=1</math> centered at each atom, while many properties of [[transition metal|transition metals]] depend upon the d-like states with <math>l=2</math>.<ref>{{Cite book |last=Pettifor |first=D. G. |title=Bonding and structure of molecules and solids |date=1996 |publisher=Clarendon Press |isbn=978-0-19-851786-3 |edition=Reprint with corr |series=Oxford science publications |location=Oxford}}</ref>
+The angular momentum quantum numbers are also used when the electron states are described in methods such as [[Kohn–Sham equations|Kohn–Sham density functional theory]]<ref>{{Cite journal |last=Kohn |first=W. |last2=Sham |first2=L. J. |date=1965 |title=Self-Consistent Equations Including Exchange and Correlation Effects |url=https://link.aps.org/doi/10.1103/PhysRev.140.A1133 |journal=Physical Review |language=en |volume=140 |issue=4A |pages=A1133–A1138 |doi=10.1103/PhysRev.140.A1133 |issn=0031-899X}}</ref> or with [[gaussian orbital]]s.<ref>{{Citation |last=Gill |first=Peter M.W. |title=Molecular integrals Over Gaussian Basis Functions |date=1994 |work=Advances in Quantum Chemistry |volume=25 |pages=141–205 |url=https://linkinghub.elsevier.com/retrieve/pii/S0065327608600192 |access-date=2024-02-20 |publisher=Elsevier |language=en |doi=10.1016/s0065-3276(08)60019-2 |isbn=978-0-12-034825-1}}</ref> For instance, in [[silicon]] the electronic properties used in [[semiconductor device]] are due to the p-like states with <math>l=1</math> centered at each atom, while many properties of [[transition metal]]s depend upon the d-like states with <math>l=2</math>.<ref>{{Cite book |last=Pettifor |first=D. G. |title=Bonding and structure of molecules and solids |date=1996 |publisher=Clarendon Press |isbn=978-0-19-851786-3 |edition=Reprint with corr |series=Oxford science publications |location=Oxford}}</ref>
 == History ==
@@ Line 145: / Line 145: @@
 == References ==
+{{reflist}}
-<references/>
-==External links==
+== External links ==
 * [http://galileo.phys.virginia.edu/classes/252/Bohr_Atom/Bohr_Atom.html Development of the Bohr atom]
 * [http://hyperphysics.phy-astr.gsu.edu/hbase/quantum/hydazi.html#c1 The azimuthal equation explained]

v t e Electron configuration
Electron shell Atomic orbital Quantum mechanics Introduction to quantum mechanics
Quantum numbers	Principal quantum number ( $n$ ) Azimuthal quantum number ( $ℓ$ ) Magnetic quantum number ( $m$ ) Spin quantum number ( $s$ )
Ground-state configurations	Periodic table (electron configurations) Electron configurations of the elements (data page)
Electron filling	Pauli exclusion principle Hund's rule Aufbau principle
Electron pairing	Electron pair Unpaired electron
Bonding participation	Valence electron Core electron
Electron counting rules	Octet rule 18-electron rule