Term symbol

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In quantum mechanics, the term symbol is an abbreviated description of the (total) angular momentum quantum numbers in a multi-electron atom (however, even a single electron can be described by a term symbol). Each energy level of an atom with a given electron configuration is described by not only the electron configuration but also its own term symbol, as the energy level also depends on the total angular momentum including spin. The usual atomic term symbols assume LS coupling (also known as Russell-Saunders coupling or Spin-Orbit coupling). The ground state term symbol is predicted by Hund's rules. Tables of atomic energy levels identified by their term symbols have been compiled by the National Institute of Standards and Technology. In this database, neutral atoms are identified as I, singly ionized atoms as II, etc.

The use of the word term for an energy level is based on the Rydberg-Ritz combination principle, an empirical observation that the wavenumbers of spectral lines can be expressed as the difference of two terms. This was later explained by the Bohr quantum theory, which identified the terms (multiplied by hc, where h is the Planck constant and c the speed of light) with quantized energy levels and the spectral wavenumbers (again multiplied by hc) with photon energies.

Video Term symbol

LS coupling and symbol

For light atoms, the spin-orbit interaction (or coupling) is small so that the total orbital angular momentum L and total spin S are good quantum numbers. The interaction between L and S is known as LS coupling, Russell-Saunders coupling or Spin-Orbit coupling. Atomic states are then well described by term symbols of the form

^2S+1L_J

where

S is the total spin quantum number. 2S + 1 is the spin multiplicity, which represents the number of possible states of J for a given L and S, provided that L >= S. (If L < S, the maximum number of possible J is 2L + 1). This is easily proved by using J_max = L + S and J_min = |L - S|, so that the number of possible J with given L and S is simply J_max - J_min + 1 as J varies in unit steps.

J is the total angular momentum quantum number.

L is the total orbital quantum number in spectroscopic notation. The first 17 symbols of L are:

The nomenclature (S, P, D, F) is derived from the characteristics of the spectroscopic lines corresponding to (s, p, d, f) orbitals: sharp, principal, diffuse, and fundamental; the rest being named in alphabetical order, except that J is omitted. When used to describe electron states in an atom, the term symbol usually follows the electron configuration. For example, one low-lying energy level of the carbon atom state is written as 1s²2s²2p^2 3P₂. The superscript 3 indicates that the spin state is a triplet, and therefore S = 1 (2S + 1 = 3), the P is spectroscopic notation for L = 1, and the subscript 2 is the value of J. Using the same notation, the ground state of carbon is 1s²2s²2p^2 3P₀.

Maps Term symbol

Terms, levels, and states

The term symbol is also used to describe compound systems such as mesons or atomic nuclei, or molecules (see molecular term symbol). For molecules, Greek letters are used to designate the component of orbital angular momenta along the molecular axis.

For a given electron configuration

• The combination of an S value and an L value is called a term, and has a statistical weight (i.e., number of possible microstates) equal to (2S+1)(2L+1);
• A combination of S, L and J is called a level. A given level has a statistical weight of (2J+1), which is the number of possible microstates associated with this level in the corresponding term;
• A combination of S, L, J and M_J determines a single state.

The product (2S+1)(2L+1) as a number of possible microstates ${\displaystyle |S,m_{S},L,m_{L}\rangle }$ with given S and L is also a number of basis states in the uncoupled representation, where S, m_S, L, m_L (m_S and m_L are z-axis components of total spin and total orbital angular momentum respectively) are good quantum numbers whose corresponding operators mutually commute. With given S and L, the eigenstates ${\displaystyle |S,m_{S},L,m_{L}\rangle }$ in this representation span function space of dimension (2S+1)(2L+1), as ${\displaystyle m_{S}=S,S-1,...,-S+1,-S}$ and ${\displaystyle m_{L}=L,L-1,...,-L+1,-L}$. In the coupled representation where total angular momentum (spin + orbital) is treated, the associated microstates (or eigenstates) are ${\displaystyle |J,M_{J},S,L\rangle }$ and these states span the function space with dimension of ${\displaystyle \sum _{J=J_{min}=|L-S|}^{J_{max}=L+S}(2J+1)}$ as ${\displaystyle m_{J}=J,J-1,...-J+1,-J}$. Obviously the dimension of function space in both representation must be the same.

As an example, for S = 1, L = 2, there are (2×1+1)(2×2+1) = 15 different microstates (= eigenstates in the uncoupled representation) corresponding to the ³D term, of which (2×3+1) = 7 belong to the ³D₃ (J = 3) level. The sum of (2J+1) for all levels in the same term equals (2S+1)(2L+1) as the dimensions of both representations must be equal as described above. In this case, J can be 1, 2, or 3, so 3 + 5 + 7 = 15.

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Term symbol parity

The parity of a term symbol is calculated as

${\displaystyle P=(-1)^{\sum _{i}l_{i}}\ ,\!}$

where l_i is the orbital quantum number for each electron. ${\displaystyle P=1}$ means even parity while ${\displaystyle P=-1}$ is for odd parity. In fact, only electrons in odd orbitals (with l odd) contribute to the total parity: an odd number of electrons in odd orbitals (those with an odd l such as in p, f,...) correspond to an odd term symbol, while an even number of electrons in odd orbitals correspond to an even term symbol. The number of electrons in even orbitals is irrelevant as any sum of even numbers is even. For any closed subshell, the number of electron is 2(2l+1) which is even, so the summation of l_i in closed subshell is always an even number. The summation of quantum numbers ${\displaystyle \sum _{i}l_{i}}$ over open (unfilled) subshells of odd orbitals (l odd) determines the parity of the term symbol. If the number of electrons in this reduced summation is odd (even) then the parity is also odd (even).

When it is odd, the parity of the term symbol is indicated by a superscript letter "o", otherwise it is omitted:

²Po
½ has odd parity, but ³P₀ has even parity.

Alternatively, parity may be indicated with a subscript letter "g" or "u", standing for gerade (German for "even") or ungerade ("odd"):

²P_½,u for odd parity, and ³P_0,g for even.

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Ground state term symbol

It is relatively easy to calculate the term symbol for the ground state of an atom using Hund's rules. It corresponds with a state with maximum S and L.

1. Start with the most stable electron configuration. Full shells and subshells do not contribute to the overall angular momentum, so they are discarded.
   • If all shells and subshells are full then the term symbol is ¹S₀.
2. Distribute the electrons in the available orbitals, following the Pauli exclusion principle. First, fill the orbitals with highest m_l value with one electron each, and assign a maximal m_s to them (i.e. +½). Once all orbitals in a subshell have one electron, add a second one (following the same order), assigning m_s = -½ to them.
3. The overall S is calculated by adding the m_s values for each electron. According to Hund's first rule, the ground state has all unpaired electron spins parallel with the same value of m_s, conventionally chosen as +½. The overall S is then ½ times the number of unpaired electrons. The overall L is calculated by adding the m_l values for each electron (so if there are two electrons in the same orbital, add twice that orbital's m_l).
4. Calculate J as
   • if less than half of the subshell is occupied, take the minimum value J = |L - S|;
   • if more than half-filled, take the maximum value J = L + S;
   • if the subshell is half-filled, then L will be 0, so J = S.

As an example, in the case of fluorine, the electronic configuration is 1s²2s²2p⁵.

1. Discard the full subshells and keep the 2p⁵ part. So there are five electrons to place in subshell p (l = 1).

2. There are three orbitals (m_l = 1, 0, -1) that can hold up to 2(2l + 1) = 6 electrons. The first three electrons can take m_s = ½ (?) but the Pauli exclusion principle forces the next two to have m_s = -½ (?) because they go to already occupied orbitals.

3. S = ½ + ½ + ½ - ½ - ½ = ½; and L = 1 + 0 - 1 + 1 + 0 = 1, which is "P" in spectroscopic notation.

4. As fluorine 2p subshell is more than half filled, J = L + S = ³/₂. Its ground state term symbol is then ^2S+1L_J = ²P_³/2.

Periodic table common column term symbols

In the periodic table, because elements in a column usually have the same outer electron structure, and always have the same electron structure in the "s-block" and "p-block" elements (see block (periodic table)), all elements may share the same ground state term symbol for the column. Thus, hydrogen and the alkali metals are all ²S_¹/2, the alkali earth metals are ¹S₀, the boron column elements are ²P_¹/2, the carbon column elements are ³P₀, the pnictogens are ⁴S_³/2, the chalcogens are ³P₂, the halogens are ²P_³/2, and the inert gases are ¹S₀, per the rule for full shells and subshells stated above.

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Term symbols for an electron configuration

The process to calculate all possible term symbols for a given electron configuration is a bit longer.

• First, calculate the total number of possible microstates N for a given electron configuration. As before, we discard the filled (sub)shells, and keep only the partially filled ones. For a given orbital quantum number l, t is the maximum allowed number of electrons, t = 2(2l+1). If there are e electrons in a given subshell, the number of possible microstates is

${\displaystyle N={t \choose e}={t! \over {e!\,(t-e)!}}.}$

As an example, let's take the carbon electron structure: 1s²2s²2p². After removing full subshells, there are 2 electrons in a p-level (l = 1), so we have

${\displaystyle N={6! \over {2!\,4!}}=15}$

different microstates.

• Second, draw all possible microstates. Calculate M_L and M_S for each microstate, with ${\displaystyle M=\sum _{i=1}^{e}m_{i}}$ where m_i is either m_l or m_s for the i-th electron, and M represents the resulting M_L or M_S respectively:

• Third, count the number of microstates for each M_L--M_S possible combination

• Fourth, extract smaller tables representing each possible term. Each table will have the size (2L+1) by (2S+1), and will contain only "1"s as entries. The first table extracted corresponds to M_L ranging from -2 to +2 (so L = 2), with a single value for M_S (implying S = 0). This corresponds to a ¹D term. The remaining terms fit inside the middle 3×3 portion of the table above. Then we extract a second table, removing the entries for M_L and M_S both ranging from -1 to +1 (and so S = L = 1, a ³P term). The remaining table is a 1×1 table, with L = S = 0, i.e., a ¹S term.

• Fifth, applying Hund's rules, deduce which is the ground state (or the lowest state for the configuration of interest.) Hund's rules should not be used to predict the order of states other than the lowest for a given configuration. (See examples at Hund's rules#Excited states.)
• If only two equivalent electrons are involved, there is an "Even Rule" which states

For two equivalent electrons the only states that are allowed are those for which the sum (L + S) is even.

Case of three equivalent electrons

• For three equivalent electrons (with the same orbital quantum number l), there is also a general formula (denoted by X(L,S,l) below) to count the number of any allowed terms with total orbital quantum number "L" and total spin quantum number "S".

${\displaystyle X(L,S,l)={\begin{cases}L-\lfloor {\frac {L}{3}}\rfloor ,&{\text{if }}S=1/2{\text{ and }}0\leq L<l\\l-\lfloor {\frac {L}{3}}\rfloor ,&{\text{if }}S=1/2{\text{ and }}l\leq L\leq 3l-1\\\lfloor {\frac {L}{3}}\rfloor -\lfloor {\frac {L-l}{2}}\rfloor +\lfloor {\frac {L-l+1}{2}}\rfloor ,&{\text{if }}S=3/2{\text{ and }}0\leq L<l\\\lfloor {\frac {L}{3}}\rfloor -\lfloor {\frac {L-l}{2}}\rfloor ,&{\text{if }}S=3/2{\text{ and }}l\leq L\leq 3l-3\\0,&{\text{ other cases}}\end{cases}}}$

where the floor function ${\displaystyle \lfloor x\rfloor }$ denotes the greatest integer not exceeding x.

The detailed proof could be found in Renjun Xu's original paper.

• For a general electronic configuration of l^k, namely k equivalent electrons occupying one subshell, the general treatment and computer code could also be found in this paper.

Alternative method using group theory

For configurations with at most two electrons (or holes) per subshell, an alternative and much quicker method of arriving at the same result can be obtained from group theory. The configuration 2p² has the symmetry of the following direct product in the full rotation group:

?⁽¹⁾ × ?⁽¹⁾ = ?⁽⁰⁾ + [?⁽¹⁾] + ?⁽²⁾,

which, using the familiar labels ?⁽⁰⁾ = S, ?⁽¹⁾ = P and ?⁽²⁾ = D, can be written as

P × P = S + [P] + D.

The square brackets enclose the anti-symmetric square. Hence the 2p² configuration has components with the following symmetries:

S + D (from the symmetric square and hence having symmetric spatial wavefunctions);

P (from the anti-symmetric square and hence having an anti-symmetric spatial wavefunction).

The Pauli principle and the requirement for electrons to be described by anti-symmetric wavefunctions imply that only the following combinations of spatial and spin symmetry are allowed:

¹S + ¹D (spatially symmetric, spin anti-symmetric)

³P (spatially anti-symmetric, spin symmetric).

Then one can move to step five in the procedure above, applying Hund's rules.

The group theory method can be carried out for other such configurations, like 3d², using the general formula

?^(j) × ?^(j) = ?^(2j) + ?^(2j-2) + ... + ?⁽⁰⁾ + [?^(2j-1) + ... + ?⁽¹⁾].

The symmetric square will give rise to singlets (such as ¹S, ¹D, & ¹G), while the anti-symmetric square gives rise to triplets (such as ³P & ³F).

More generally, one can use

?^(j) × ?^(k) = ?^(j+k) + ?^(j+k-1) + ... + ?^(|j-k|)

where, since the product is not a square, it is not split into symmetric and anti-symmetric parts. Where two electrons come from inequivalent orbitals, both a singlet and a triplet are allowed in each case.

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Summary of various coupling schemes and corresponding term symbols

Basic concepts for all coupling schemes:

• ${\displaystyle {\overrightarrow {l}}}$: individual orbital angular momentum vector for an electron, ${\displaystyle {\overrightarrow {s}}}$: individual spin vector for an electron, ${\displaystyle {\overrightarrow {j}}}$: individual total angular momentum vector for an electron, ${\displaystyle {\overrightarrow {j}}={\overrightarrow {l}}+{\overrightarrow {s}}}$.
• ${\displaystyle {\overrightarrow {L}}}$: Total orbital angular momentum vector for all electrons in an atom (${\displaystyle {\overrightarrow {L}}=\sum _{i}{\overrightarrow {l_{i}}}}$).
• ${\displaystyle {\overrightarrow {S}}}$: total spin vector for all electrons (${\displaystyle {\overrightarrow {S}}=\sum _{i}{\overrightarrow {s_{i}}}}$).
• ${\displaystyle {\overrightarrow {J}}}$: total angular momentum vector for all electrons. The way the angular momenta are combined to form ${\displaystyle {\overrightarrow {J}}}$ depends on the coupling scheme: ${\displaystyle {\overrightarrow {J}}={\overrightarrow {L}}+{\overrightarrow {S}}}$ for LS coupling, ${\displaystyle {\overrightarrow {J}}=\sum _{i}{\overrightarrow {j_{i}}}}$ for jj coupling, etc.
• A quantum number corresponding to the magnitude of a vector is a letter without an arrow (ex: l is the orbital angular momentum quantum number for ${\displaystyle {\overrightarrow {l}}}$ and ${\displaystyle {{\hat {l}}^{2}}\left|l,m,\ldots \right\rangle ={{\hbar }^{2}}l\left(l+1\right)\left|l,m,\ldots \right\rangle }$)
• The parameter called multiplicity represents the number of possible values of the total angular momentum quantum number J for certain conditions.
• For a single electron, the term symbol is not written as S is always 1/2 and L is obvious from the orbital type.
• For two electron groups A and B with their own terms, each term may represent S, L and J which are quantum numbers corresponding to the ${\displaystyle {\overrightarrow {S}}}$,${\displaystyle {\overrightarrow {L}}}$ and ${\displaystyle {\overrightarrow {J}}}$ vectors for each group. "Coupling" of terms A and B to form a new term C means finding quantum numbers for new vectors ${\displaystyle {\overrightarrow {S}}={\overrightarrow {S_{A}}}+{\overrightarrow {S_{B}}}}$, ${\displaystyle {\overrightarrow {L}}={\overrightarrow {L_{A}}}+{\overrightarrow {L_{B}}}}$ and ${\displaystyle {\overrightarrow {J}}={\overrightarrow {L}}+{\overrightarrow {S}}}$. This example is for LS coupling and which vectors are summed in a coupling is depending on which scheme of coupling is taken. Of course, the angular momentum addition rule is that ${\displaystyle X=X_{A}+X_{B},X_{A}+X_{B}-1,...,|X_{A}-X_{B}|}$where X can be s, l, j, S, L, J or any other angular momentum-magnitude-related quantum number.

LS coupling (Russell-Saunders coupling)

• Coupling scheme: ${\displaystyle {\overrightarrow {L}}}$ and ${\displaystyle {\overrightarrow {S}}}$ are calculated first then ${\displaystyle {\overrightarrow {J}}={\overrightarrow {L}}+{\overrightarrow {S}}}$ is obtained. In practical point of view, it means L, S and J are obtained by using addition rule of angular momentums with given electronics groups that are to be coupled.
• Electronic configuration + Term symbol: ${\displaystyle n{{l}^{N}}{{(}^{(2S+1)}}{{L}_{J}})}$. ${\displaystyle {{(}^{(2S+1)}}{{L}_{J}})}$ is a Term which is from coupling of electrons in ${\displaystyle n{{l}^{N}}}$group. n,l are principle quantum number, orbital quantum number and ${\displaystyle n{{l}^{N}}}$means there are N (equivalent) electrons in nl subshell. For ${\displaystyle L>S}$, (2S+1) is equal to multiplicity, a number of possible values in J (final total angular momentum quantum number) from given S and L. For ${\displaystyle S>L}$, multiplicity is (2L+1) but (2S+1) is still written in the Term symbol. Strickly speaking, ${\displaystyle {{(}^{(2S+1)}}{{L}_{J}})}$ is called Level and ${\displaystyle {^{\left(2S+1\right)}{L}}}$ is called Term. Sometimes superscript o is attached to the Term, means the parity ${\displaystyle P={{\left(-1\right)}^{{\underset {i}{\mathop {\sum }}}\,{{l}_{i}}}}}$of group is odd (P = -1).
• Example:
  1. ${\displaystyle 3{{d}^{7}}{{{\text{ }}\!\!~\!\!{\text{ }}}\ ^{4}}{{F}_{7/2}}}$: ${\displaystyle ^{4}{{F}_{7/2}}}$ is Level of 3d⁷ group in which are equivalent 7 electrons are in 3d subshell.
  2. ${\displaystyle 3{{d}^{7}}{{(}^{4}}F)4s4p{{(}^{3}}{{p}^{0}}){{\text{ }}\ ^{6}}F_{9/2}^{0}}$: Terms are assigned for each group (with different principal quantum number n) and rightmost Level ${\displaystyle {^{6}{{\text{F}}_{9/2}^{o}}}}$ is from coupling of Terms of these groups so ${\displaystyle {^{6}{{\text{F}}_{9/2}^{o}}}}$ represents final total spin quantum number S, total orbital angular momentum quantum number L and total angular momentum quantum number J in this atomic energy level.
  3. ${\displaystyle 4{{f}^{7}}\left(^{8}{{S}^{0}}\right)5d\ \ \left(^{7}{{D}^{o}}\right)6p\ \ ^{8}F_{13/2}^{0}}$: There is a space between 5d and ${\displaystyle \left(^{7}{{D}^{o}}\right)}$. In means ${\displaystyle \left(^{8}{{S}^{0}}\right)}$ and 5d are coupled to get ${\displaystyle \left(^{7}{{D}^{o}}\right)}$. Final level ${\displaystyle {^{8}{F_{13/2}^{o}}}}$ is from coupling of ${\displaystyle \left(^{7}{{D}^{o}}\right)}$ and 6p.
  4. ${\displaystyle 4f\left(^{2}{{F}^{0}}\right)\ \ 5{{d}^{2}}\left(^{1}G\right)6s\ \ {{\left(^{2}G\right)}\ \ ^{1}}P_{1}^{0}}$: There is only one Term ${\displaystyle \left({^{2}{{F}^{o}}}\right)}$ which is isolated in the left of the leftmost space. It means ${\displaystyle \left({^{2}{{F}^{o}}}\right)}$ is coupled lastly; ${\displaystyle \left({^{1}{G}}\right)}$ and 6s are coupled to get ${\displaystyle \left({^{2}{G}}\right)}$ then ${\displaystyle \left({^{2}{G}}\right)}$ and ${\displaystyle \left({^{2}{{F}^{o}}}\right)}$ are coupled to get final Term ${\displaystyle {^{1}{P_{1}^{o}}}}$.

jj Coupling

• Coupling scheme: ${\displaystyle {\overrightarrow {J}}=\sum _{i}{\overrightarrow {j_{i}}}}$.
• Electronic configuration + Term symbol: ${\displaystyle {{\left({{n}_{1}}{{l}_{1}}_{{j}_{1}}^{{N}_{1}}{{n}_{2}}{{l}_{2}}_{{j}_{2}}^{{N}_{2}}\ldots \right)}_{J}}}$
• Example:
  1. ${\displaystyle {{\left(6p_{\frac {1}{2}}^{2}6p_{\frac {3}{2}}^{}\right)}^{o}}_{3/2}}$: There are two groups. One is ${\displaystyle 6p_{1/2}^{2}}$ and the other is ${\displaystyle 6p_{\frac {3}{2}}^{}}$. In ${\displaystyle 6p_{1/2}^{2}}$, there are 2 electrons having ${\displaystyle j=1/2}$ in 6p subshell while there is an electron having ${\displaystyle j=3/2}$ in the same subshell in ${\displaystyle 6p_{\frac {3}{2}}^{}}$.Coupling of these two groups results in J = 3/2 (coupling of j of three electrons).
  2. ${\displaystyle 4d_{5/2}^{3}4d_{3/2}^{2}~\ {{\left({\frac {9}{2}},2\right)}_{11/2}}}$: 9/2 in () is ${\displaystyle {{J}_{1}}}$ for 1st group ${\displaystyle 4d_{5/2}^{3}}$ and 2 in () is J₂ for 2nd group ${\displaystyle 4d_{3/2}^{2}}$. Subscript 11/2 of Term symbol is final J of ${\displaystyle {\overrightarrow {J}}={\overrightarrow {J_{1}}}+{\overrightarrow {J_{2}}}}$.

J₁L₂ coupling

• Coupling scheme: ${\displaystyle {\overrightarrow {K}}={\overrightarrow {J_{1}}}+{\overrightarrow {L_{2}}}}$ and ${\displaystyle {\overrightarrow {J}}={\overrightarrow {K}}+{\overrightarrow {S_{2}}}}$.
• Electronic configuration + Term symbol: ${\displaystyle {{n}_{1}}{{l}_{1}}^{{N}_{1}}\left(Ter{{m}_{1}}\right){{n}_{2}}{{l}_{2}}^{{N}_{2}}\left(Ter{{m}_{2}}\right)~\ {^{\left(2{{S}_{2}}+1\right)}{{\left[K\right]}_{J}}}}$. For K > S₂, (2S₂+1) is equal to multiplicity, a number of possible values in J (final total angular momentum quantum number) from given S₂ and K. For S₂ > K, multiplicity is (2K + 1) but (2S₂ + 1) is still written in the Term symbol.
• Example:
  1. ${\displaystyle 3{{p}^{5}}\left({^{2}{P_{\frac {1}{2}}^{o}}}\right)5g~\ {^{2}{\left[9/2\right]_{5}^{o}}}}$: ${\displaystyle {{J}_{1}}={\frac {1}{2}},{{l}_{2}}=4,~{{s}_{2}}=1/2}$. 9/2 is K, which comes from coupling of J₁ and l₂. Subscript 5 in Term symbol is J which is from coupling of K and s₂.
  2. ${\displaystyle 4{{f}^{13}}\left({^{2}{F_{\frac {7}{2}}^{o}}}\right)5{{d}^{2}}\left({^{1}{D}}\right)\ ~{^{1}{\left[7/2\right]_{7/2}^{o}}}}$: ${\displaystyle {{J}_{1}}={\frac {7}{2}},{{L}_{2}}=2,~{{S}_{2}}=0}$. 7/2 is K, which comes from coupling of J₁ and L₂. Subscript 7/2 in Term symbol is J which is from coupling of K and S₂.

LS₁ coupling

• Coupling scheme:${\displaystyle {\overrightarrow {K}}={\overrightarrow {L}}+{\overrightarrow {S_{1}}}}$, ${\displaystyle {\overrightarrow {J}}={\overrightarrow {K}}+{\overrightarrow {S_{2}}}}$.
• Electronic configuration + Term symbol: ${\displaystyle {{n}_{1}}{{l}_{1}}^{{N}_{1}}\left(Ter{{m}_{1}}\right){{n}_{2}}{{l}_{2}}^{{N}_{2}}\left(Ter{{m}_{2}}\right)\ ~L~\ {^{\left(2{{S}_{2}}+1\right)}{{\left[K\right]}_{J}}}}$. For K > S₂, (2S₂ + 1) is equal to multiplicity, a number of possible values in J (final total angular momentum quantum number) from given S₂ and K. For S₂ > K, multiplicity is (2K+1) but (2S₂ + 1) is still written in the Term symbol.
• Example:
  1. ${\displaystyle 3{{\text{d}}^{7}}\left({^{4}{P}}\right)4s4p\left({^{3}{{P}^{o}}}\right)\ ~{{D}^{o}}~\ {^{3}{\left[5/2\right]_{7/2}^{o}}}}$: ${\displaystyle {{L}_{1}}=1,~{{L}_{2}}=1,~{{S}_{1}}={\frac {3}{2}},~{{S}_{2}}=1}$. ${\displaystyle L=2,K=5/2,J=7/2}$.

Most famous coupling schemes are introduced here but these schemes can be mixed together to express energy state of atom. This summary is based on [1].

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Racah notation and Paschen notation

These are notations for describing states of singly excited atoms, especially noble gas atoms. Racah notation is basically a combination of LS or Russell-Saunder coupling and J₁L₂ coupling. LS coupling is for a parent ion and J₁L₂ coupling is for an coupling of the parent ion and the excited electron. The parent ion is an unexcited part of the atom. For example, in Ar atom excited from a ground state ...3p⁶ to an excited state ...3p⁵4p in electronic configuration, 3p⁵ is for the parent ion while 4p is for the excited electron.

In Racah notation, states of excited atoms are denoted as ${\displaystyle \left(^{\left(2{{S}_{1}}+1\right)}{{L}_{1}}_{{J}_{1}}\right)nl\left[K\right]_{J}^{o}}$. Quantities with a subscript 1 are for the parent ion, n and l are principal and orbital quantum numbers for the excited electron, K and J are quantum numbers for ${\displaystyle {\overrightarrow {K}}={\overrightarrow {{J}_{1}}}+{\vec {l}}}$ and ${\displaystyle {\overrightarrow {J}}={\overrightarrow {K}}+{\vec {s}}}$ where ${\displaystyle {\vec {l}}}$ and ${\displaystyle {\vec {s}}}$ are orbital angular momentum and spin for the excited electron respectively. "o" represents a parity of excited atom. For an inert (noble) gas atom, usual excited states are Np⁵nl where N = 2, 3, 4, 5, 6 for Ne, Ar, Kr, Xe, Rn, respectively in order. Since the parent ion can only be ²P_1/2 or ²P_3/2, the notation can be shortened to ${\displaystyle nl\left[K\right]_{J}^{o}}$ or ${\displaystyle nl'\left[K\right]_{J}^{o}}$, where nl means the parent ion is in ²P_3/2 while nl? is for the parent ion in ²P_1/2 state.

Paschen notation is a somewhat odd notation; it is an old notation made to attempt to fit an emission spectrum of neon to a hydrogen-like theory. It has a rather simple structure to indicate energy levels of an excited atom. The energy levels are denoted as n'l#. l is just an orbital quantum number of the excited electron. n'l is written in a way that 1s for (n = N + 1, l = 0), 2p for (n = N + 1, l = 1), 2s for (n = N + 2, l = 0), 3p for (n = N + 2, l = 1), 3s for (n = N + 3, l = 0), and etc. Rules of writing n'l from the lowest electronic configuration of the excited electron are: (1) l is written first, (2) n' is consecutively written from 1 and the relation of l = n' - 1, n' - 2, ... , 0 (like a relation between n and l) is kept. n'l is an attempt to describe electronic configuration of the excited electron in a way of describing electronic configuration of hydrogen atom. # is an additional number denoted to each energy level of given n'l (there can be multiple energy levels of given electronic configuration, denoted by the term symbol). # denotes each level in order, for example, # = 10 is for a lower energy level than # = 9 level and # = 1 is for the highest level in a given n'l. An example of Paschen notation is below.

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See also

• Angular quantum numbers
• Angular momentum coupling
• Molecular term symbol
• Hole formalism

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Notes

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References

Source of article : Wikipedia