Term symbol
In atomic physics, a term symbol is a concise notation that describes the quantum mechanical state of an electron configuration in a multi-electron atom, specifying the total orbital angular momentum, total spin angular momentum, and their coupling to the total angular momentum.[1] It is primarily used within the Russell-Saunders (LS) coupling scheme, which is applicable for lighter atoms where spin-orbit interactions are relatively weak compared to electrostatic interactions among electrons.[2] The standard form of the term symbol is ^{2S+1}L_J, where: The values of L and S arise from vector coupling of the individual electrons' orbital (l_i) and spin (s_i = 1/2) angular momenta, respectively, while adhering to the Pauli exclusion principle to determine allowed terms for a given electron configuration.[2] For example, the ground state of the helium atom in its $1s^2 configuration is denoted ^1S_0, indicating a singlet state (S=0), zero orbital angular momentum (L=0), and total angular momentum J=0.[3] In contrast, the carbon atom's ground configuration $1s^2 2s^2 2p^2 yields multiple terms, including the lowest-energy ^3P term (with J=0,1,2 sublevels), determined by Hund's rules, which prioritize maximum S and then maximum L for the ground state energy ordering.[2] Term symbols are essential for interpreting atomic spectra, as they label energy levels and predict allowed transitions between them, governed by selection rules such as \Delta L = 0, \pm 1 (except no $0 \leftrightarrow 0), \Delta S = 0, and \Delta J = 0, \pm 1 (with J=0 \not\to J=0 forbidden).[1] Parity, indicated by a superscript "o" for odd (e.g., ^3P^\circ) or omitted for even, further refines the symbol to account for the wavefunction's behavior under spatial inversion, crucial for dipole-allowed transitions in spectroscopy.[2] This notation facilitates the analysis of fine structure, hyperfine structure, and the overall electronic structure in fields ranging from astrophysics to quantum chemistry, enabling precise identification of atomic lines in emission or absorption spectra.[3]Basic Notation and Terminology
Components of Term Symbols
The term symbol in atomic spectroscopy is a compact notation that describes the angular momentum quantum numbers of an electronic state in multi-electron atoms. It is conventionally written in the form ^{2S+1}L_J, where L denotes the total orbital angular momentum quantum number using spectroscopic notation (S for L = 0, P for L = 1, D for L = 2, F for L = 3, and so on for higher values), $2S+1 represents the spin multiplicity (with S being the total spin quantum number), and the subscript J indicates the total angular momentum quantum number.[1] Physically, L arises from the vector sum of the individual orbital angular momenta of the electrons, characterizing the overall orbital motion. The total spin quantum number S results from the coupling of the individual electron spins, each contributing s = 1/2. The value of J is obtained by vectorially coupling \mathbf{L} and \mathbf{S}, yielding possible magnitudes from |L - S| to L + S in steps of 1; J is an integer if both L and S are integers or half-integers, or a half-integer otherwise.[1] This notation originated in the context of Russell-Saunders coupling, proposed by Henry Norris Russell and Frederick Albert Saunders in their 1925 analysis of alkaline-earth spectra, where they identified patterns in spectral lines attributable to the coupling of orbital and spin angular momenta; however, the term symbol convention has since been applied more broadly across various coupling schemes in atomic physics.[1] In the vector model underlying this notation, the total orbital angular momentum vector \mathbf{L} and total spin vector \mathbf{S} precess around their resultant total angular momentum vector \mathbf{J}, with the magnitudes of L, S, and J determining the possible orientations and energy splittings due to spin-orbit interactions, particularly valid for lighter atoms where spin-orbit coupling is weak compared to electrostatic interactions.[1] Representative examples illustrate these components: the ground state of the hydrogen atom, with a single 1s electron (l = 0, s = 1/2), is denoted ^2\mathrm{S}_{1/2} (L = 0, S = 1/2, J = 1/2); the ground state of neutral helium, with a closed 1s shell (L = 0, S = 0), is ^1\mathrm{S}_0 (J = 0).[1]Terms, Levels, and States
In atomic spectroscopy, a term refers to a set of atomic states characterized by specific values of the total orbital angular momentum quantum number L and the total spin angular momentum quantum number S, denoted by the symbol ^{2S+1}L, where $2S+1 is the spin multiplicity and L is represented by a letter (S for L=0, P for L=1, D for L=2, etc.).[3][4] This notation describes the uncoupled representation without specifying the total angular momentum J. A level, in contrast, incorporates the coupling of L and S to form the total angular momentum J, denoted as ^{2S+1}L_J, where J ranges from |L - S| to L + S in integer steps; each such level represents a distinct energy substructure due to spin-orbit interactions.[3][4] Finally, a state corresponds to one of the $2J + 1 degenerate substates within a level, specified by the magnetic quantum number m_J (the projection of J along a quantization axis).[4] The degeneracy of a term arises from the possible orientations of L and S, given by (2L + 1)(2S + 1), reflecting the number of microstates sharing the same L and S but differing in their projections.[4] For a level, this degeneracy is reduced to $2J + 1, accounting for the distinct m_J values within that J.[3][4] These degeneracies are lifted in the presence of external fields; in the Zeeman effect, an applied magnetic field splits the states of a level according to their m_J projections, producing observable spectral line components that reveal the underlying atomic structure.[3] While Hund's rules provide a means to predict the relative ordering of term energies based on maximum multiplicity and orbital angular momentum, the concepts of terms, levels, and states focus on the structural hierarchy independent of such energy assignments.[4] For illustration, consider the p^2 electron configuration, which yields terms such as ^1D (singlet, S=0, L=2) and ^3P (triplet, S=1, L=1); the ^3P term further divides into levels ^3P_0, ^3P_1, and ^3P_2, each with degeneracies of 1, 3, and 5, respectively.[4]LS Coupling
Principles and Applicability
The Russell-Saunders coupling scheme, also known as LS coupling, describes the angular momentum coupling in multi-electron atoms through a vector model where the individual orbital angular momenta \mathbf{l}_i of the electrons first couple to form the total orbital angular momentum \mathbf{L} = \sum_i \mathbf{l}_i, and the individual spin angular momenta \mathbf{s}_i couple to form the total spin angular momentum \mathbf{S} = \sum_i \mathbf{s}_i. Subsequently, \mathbf{L} and \mathbf{S} couple to yield the total angular momentum \mathbf{J} = \mathbf{L} + \mathbf{S}.[1][5] This hierarchical coupling arises because the electrostatic interactions between electrons dominate, allowing the orbital and spin degrees of freedom to be treated somewhat independently before their mutual interaction.[6] The scheme rests on key assumptions about the atomic Hamiltonian, which can be approximated asH = H_0 + H_{ee} + \lambda \mathbf{L} \cdot \mathbf{S},
where H_0 represents the central field potential for individual electrons, H_{ee} accounts for electron-electron repulsion (the residual Coulomb interaction), and the spin-orbit term \lambda \mathbf{L} \cdot \mathbf{S} is a small perturbation with coupling constant \lambda.[5][2] This approximation holds when the spin-orbit interaction is negligible compared to the electrostatic terms, i.e., H_{ee} \gg \lambda \mathbf{L} \cdot \mathbf{S}, which is valid for atoms with low atomic number Z where relativistic effects are weak.[1][6] LS coupling is applicable primarily to light atoms (typically Z < 57), such as those in the first and second rows of the periodic table, and is particularly effective for partially filled p and d shells in transition metals where electron-electron interactions govern the term structure.[1][5] It fails for heavy atoms (high Z), where strong spin-orbit coupling disrupts the separation of L and S, necessitating alternative schemes like jj coupling.[6] This approach was developed in the 1920s by Henry Norris Russell and Frederick Albert Saunders to explain regularities in the spectra of alkaline earth atoms.
Constructing Term Symbols for Configurations
The construction of term symbols for a given electron configuration in LS coupling relies on the microstate method, which systematically enumerates all possible states of the electrons while adhering to the Pauli exclusion principle. A microstate is defined by assigning specific values of the orbital magnetic quantum number m_l and spin magnetic quantum number m_s (\pm 1/2) to each electron in the configuration. For non-equivalent electrons, such as those in different principal or azimuthal quantum number subshells (e.g., 2p and 3d), all combinations of these assignments are permitted because the electrons occupy distinct orbitals, with no restrictions beyond single occupancy per orbital-spin state. The total number of microstates for such a configuration is given by the product over the subshells of the binomial coefficients accounting for the available states: specifically, for single electrons in subshells with angular momenta l_i, it is \prod_i \binom{2(2l_i + 1)}{n_i}, where n_i = 1 yields $2(2l_i + 1) per electron, simplifying to the product of the orbital-spin degeneracies of each subshell.[7] To derive the term symbols, calculate the total orbital projection M_L = \sum m_{l_i} and total spin projection M_S = \sum m_{s_i} for every microstate. Construct a table tabulating the number of microstates for each possible pair (M_L, M_S), where M_L ranges from the maximum possible sum of |m_l| down to its negative, and M_S from the maximum sum of |m_s| (typically n/2 for n unpaired electrons) down to zero in steps of 1 (considering only M_S \geq 0 due to symmetry). The possible terms are then identified by starting with the highest M_S and its corresponding highest M_L; this defines the maximum spin S = \max M_S and orbital angular momentum L = \max M_L for the leading term ^{2S+1}L. Subtract the degeneracy of this term, (2L+1)(2S+1), from the table by removing that many microstates from the relevant (M_L, M_S) entries (following the pattern of a full L, S multiplet). Repeat the process with the remaining highest M_L and M_S until all microstates are accounted for. This procedure ensures all possible terms are found without duplication.[7] For non-equivalent electrons like the (2p)^1 (3d)^1 configuration (relevant in LS coupling for light atoms where spin-orbit effects are small), the process yields the following terms: ^3F, ^3D, ^3P, ^1F, ^1D, and ^1P. The total of 60 microstates is fully partitioned: ^3F (21 microstates), ^3D (15), ^3P (9), ^1F (7), ^1D (5), and ^1P (3). The microstate table would span M_L from 3 to -3 and M_S from 1 to 0, with the highest entry at M_L = 3, M_S = 1 (from m_l = 1 in p and m_l = 2 in d, both m_s = +1/2) assigning the ^3F term first, followed by systematic subtraction for the others. This example illustrates how all combinations are allowed, contrasting with equivalent electron cases.[8] Once the terms are obtained, Hund's rules can be applied to order their energies: the term with maximum S (highest multiplicity $2S+1) lies lowest, and for degenerate multiplicities, the one with maximum L is lowest; further details on J ordering appear in ground state determination.[7]Equivalent Electrons and Exclusion Rules
When electrons occupy the same subshell, they are termed equivalent electrons, sharing the same principal quantum number n and orbital angular momentum quantum number l. The Pauli exclusion principle dictates that no two electrons in an atom can have the same set of four quantum numbers (n, l, m_l, m_s), ensuring the total wavefunction remains antisymmetric under particle exchange for fermions like electrons.[9] This principle significantly restricts the possible term symbols for equivalent electrons compared to non-equivalent cases, as certain combinations of total orbital angular momentum L and total spin S lead to wavefunctions that violate antisymmetry, resulting in zero-probability states or vanishing integrals in the Slater determinant construction.[10] For the p^2 configuration (two equivalent p electrons, with six possible spin-orbitals), the Pauli principle excludes terms like ^3D and ^1P, leaving only ^1S, ^1D, and ^3P as allowed, as these correspond to properly antisymmetrized wavefunctions. The exclusion arises because symmetric spatial parts must pair with antisymmetric spin parts (triplet states) and vice versa (singlet states) to maintain overall antisymmetry, eliminating incompatible pairings.[10] The allowed terms for various equivalent electron configurations in s, p, and d subshells are summarized in the following table, derived from systematic enumeration of antisymmetric microstates under LS coupling.[1]| Configuration | Allowed Terms |
|---|---|
| s^1 | ^2S |
| s^2 | ^1S |
| p^1 | ^2P |
| p^2 | ^1S, ^1D, ^3P |
| p^3 | ^2D, ^2P, ^4S |
| p^4 | ^1D, ^1S, ^3P |
| p^5 | ^2P |
| p^6 | ^1S |
| d^1 | ^2D |
| d^2 | ^1G, ^1D, ^1S, ^3F, ^3P |
| d^3 | ^4P, ^4F, ^2H, ^2G, ^2F, ^2D, ^2P |
| d^4 | ^5D, ^3H, ^3F, ^3P, ^1G, ^1D, ^1S |
Other Coupling Schemes
jj Coupling
In jj coupling, the orbital angular momentum \mathbf{l}_i and spin angular momentum \mathbf{s}_i of each individual electron are first coupled to form the total angular momentum \mathbf{j}_i = \mathbf{l}_i + \mathbf{s}_i for that electron, with j_i = l_i \pm 1/2. These individual j_i are then vectorially coupled to yield the total angular momentum \mathbf{J} = \sum \mathbf{j}_i, where the possible values of J range from the maximum \sum j_i down to the minimum consistent with angular momentum addition rules, in steps of 1. This scheme assumes the spin-orbit interaction within each electron is much stronger than the inter-electron electrostatic repulsion, making total L and S poor quantum numbers.[11] The notation for jj coupling specifies the j subshells explicitly, often grouping equivalent electrons as (nl_j^N)_J, with the total J as a subscript and parity as a superscript (even or odd). For non-equivalent electrons, it is written as (j_1 j_2 \dots )_J, enclosed in parentheses or brackets to indicate the coupling. For instance, a configuration involving one p_{1/2} electron and one p_{3/2} electron is denoted (p_{1/2} p_{3/2})_J, where J can be 1 or 2. Term symbols in this scheme omit the total orbital L and spin multiplicity $2S+1, focusing instead on the configuration, J, and parity, as L and S are not conserved.[11] jj coupling is applicable to heavy atoms with high atomic numbers (Z \gtrsim 50), where the spin-orbit coupling parameter scales as Z^4 and dominates the weaker electrostatic interactions scaling as Z. This is evident in elements like mercury (Z = 80), whose spectra, such as the ground configuration $6s^2 and excited states like $6s 6p, are better described by jj than by LS coupling. In contrast to LS coupling, which prioritizes total L and S for lighter atoms, jj coupling provides a more accurate vector model for such systems. The relation to LS coupling is handled through intermediate coupling schemes, which mix the two limits based on the relative strengths of interactions.[11][12] A representative example is the iodine atom (Z = 53) in the $5p^5 6s configuration, where the $5p^5 core splits into ^2P_{3/2} and ^2P_{1/2} due to strong spin-orbit coupling. The resulting jj terms include $5p^5(^2P_{3/2})6s [3/2]^\circ_2 and [3/2]^\circ_1, as well as $5p^5(^2P_{1/2})6s [1/2]^\circ_1, capturing the energy levels more precisely than pure LS notation.[13]Intermediate Couplings (J1L2 and LS1)
Intermediate coupling schemes bridge the gap between pure LS (Russell-Saunders) and jj coupling approximations, arising in atoms where spin-orbit interactions are comparable in strength to inter-electron electrostatic repulsions, typically for elements with atomic numbers Z ≈ 30–80. These hybrid schemes are particularly relevant for configurations involving a stable core and one or more valence electrons, where relativistic effects begin to influence the angular momentum coupling without fully dominating as in jj coupling. They allow for more accurate description of spectral fine structure by considering partial uncoupling of orbital and spin angular momenta.[1] J1L2 coupling applies to systems where the total angular momentum J<sub>1</sub> of the core (often from a subshell with significant spin-orbit splitting) couples first with the total orbital angular momentum L<sub>2</sub> of the valence shell to form an intermediate K = J<sub>1</sub> + L<sub>2</sub>, which then couples with the valence spin S<sub>2</sub> to yield the total J. The notation is commonly written as (core term) [K]<sub>J</sub>, with multiplicity 2S<sub>2</sub> + 1 prefixed if greater than 1, and parity indicated by superscript o for odd. This scheme is suitable for excited states in lighter atoms like alkali metals, where the core's spin-orbit coupling is stronger than the valence electron's but weaker than electrostatic interactions. For example, in configurations such as 3p^5 (^2P^o_{1/2}) 5g^2 [9/2]^o_5 in appropriate atomic ions, J1L2 captures deviations from pure LS coupling due to core-valence interactions.[1][14] LS1 coupling is employed when the core's orbital angular momentum L<sub>1</sub> couples with the valence electron's orbital angular momentum <i>l</i> to form a total L, which then couples with the core spin S<sub>1</sub> to an intermediate K, finally coupling with the valence spin <i>s</i> = 1/2 to the total J. The notation follows ^{2S+1}L [K]<sub>J</sub>, where L is the resultant from L<sub>1</sub> + <i>l</i>, often with the core term in parentheses. This approach is applicable to intermediate-Z atoms, including transition metals and rare earths, where relativistic effects partially decouple spins and orbits in open-shell cores. A representative example is the configuration 3s<sup>2</sup>3p(<sup>2</sup>P<sup>o</sup>)4f in silicon-like ions, denoted as G<sub>2</sub> [7/2]<sub>3</sub>, which illustrates the coupling for excited states in rare earth spectra. In rare earth elements like europium, LS1 coupling aids in interpreting the intricate 4f<sup>n</sup> configurations perturbed by valence electrons.[1][14] In both schemes, the true eigenstates result from perturbation mixing between LS and jj basis functions, where the Hamiltonian includes electrostatic (H<sub>el</sub>) and spin-orbit (H<sub>SO</sub>) terms treated via matrix diagonalization: H = H_\text{el} + H_\text{SO}, yielding wave functions as superpositions, e.g., |\psi\rangle = c_1 |^{2S+1}L_J\rangle + c_2 | (j_1 j_2) J \rangle + \cdots, with coefficients |c_i| determined by the relative strengths of interactions; for Z ≈ 40–70, mixing coefficients often show <50% purity in either basis. This perturbative approach, essential for accurate energy level predictions, contrasts with pure jj coupling used for heavier atoms (Z > 80) by focusing on configuration-specific partial couplings.[1]Parity and Ground States
Parity Designation
The parity of an atomic state in the context of term symbols refers to the eigenvalue of the spatial inversion operator applied to the electronic wave function, which determines whether the function is symmetric (even parity) or antisymmetric (odd parity) under reflection through the origin.[1] This quantum number is calculated as (-1)^{\sum_i l_i}, where the sum is over the orbital angular momentum quantum numbers l_i of all electrons in the atom; the parity is even if the sum is even and odd if the sum is odd.[1] Closed-shell configurations always contribute even parity because the total sum of l_i for a filled subshell is even, so only open shells affect the overall parity.[1] In term symbol notation, even parity is typically omitted, while odd parity is indicated by a superscript "o" (or sometimes "°") attached to the right of the symbol, such as ^{2}P_{1/2}^o for the odd-parity level of a p-electron configuration.[1] This convention, established in early atomic spectroscopy, ensures compact representation while distinguishing states relevant to spectral analysis. Parity plays a critical role in selection rules for atomic transitions, particularly for electric dipole (E1) radiation, where a change in parity (from even to odd or vice versa) is required for the transition to be allowed; transitions conserving parity are forbidden in this approximation.[15] For example, an s electron (l=0) has even parity, while a single p electron (l=1) has odd parity, so a transition from an ns to np configuration changes parity and is E1-allowed.[1] In multi-electron configurations like 1s^2 2p (sum of l_i = 1), the parity is odd regardless of principal quantum numbers, as parity depends solely on the l_i values.[1] The rule applies identically to equivalent electrons, where the total parity is the product of individual orbital parities, yielding the same even/odd determination as for non-equivalent cases.[1]Determining Ground State Terms
To determine the ground state term symbol among the possible terms arising from an atomic electron configuration, Hund's rules provide a systematic procedure based on the principles of LS coupling. These rules, formulated by Friedrich Hund in the 1920s, prioritize the term with the highest total spin angular momentum quantum number S, followed by the highest total orbital angular momentum quantum number L for that S, and then specify the total angular momentum quantum number J based on the shell filling.[16][1] Hund's first rule states that the ground state term has the maximum possible value of S, corresponding to the highest spin multiplicity $2S + 1. This arises because parallel electron spins minimize the Coulomb repulsion through the exchange interaction, where the exchange integral K_{ij} = \langle \psi_i(1)\psi_j(2) | 1/r_{12} | \psi_j(1)\psi_i(2) \rangle contributes a negative term to the energy for each pair of electrons with parallel spins, lowering the overall energy as the number of such pairs increases. For example, in the carbon atom configuration $1s^2 2s^2 2p^2, the possible terms are ^3P, ^1D, and ^1S; the triplet ^3P (with S = 1) is the ground state due to its three unpaired spins allowing more favorable exchange contributions.[16][17] Hund's second rule specifies that, among terms with the same S, the ground state has the maximum L. This preference stems from configurations with higher L having electrons in orbitals that are more spatially separated on average, reducing the direct Coulomb repulsion integral J_{ij} = \langle \psi_i(1)\psi_j(2) | 1/r_{12} | \psi_i(1)\psi_j(2) \rangle. Continuing the carbon example, the ^3P term (with L = 1) lies below any hypothetical triplet with lower L. For the oxygen atom ($1s^2 2s^2 2p^4), the ground state is also ^3P ( S = 1, L = 1 ), selected over ^1S and ^1D by these first two rules.[16][1] Hund's third rule addresses the ordering within a multiplet (terms with the same L and S but different J): for subshells less than half-filled, the lowest J = |L - S| has the lowest energy; for subshells more than half-filled, the highest J = L + S is lowest; and for exactly half-filled, J = S. This follows from the spin-orbit interaction, where the energy shift is proportional to \mathbf{L} \cdot \mathbf{S}, given by E \propto [J(J+1) - L(L+1) - S(S+1)]/2. For carbon's ^3P ground term (p², less than half-filled p shell), the ordering is ^3P_0 < ^3P_1 < ^3P_2. These rules hold generally for light atoms under LS coupling but have exceptions in cases like closed subshells (e.g., d¹⁰ or f¹⁴ configurations yield a ^1S_0 ground state with S = L = 0, trivially satisfying the rules) or heavier elements where jj coupling dominates.[16][1] Parity plays a supplementary role in identifying the ground state, as it is determined by the configuration's total \sum l_i (even for even parity, odd for odd). For neutral atoms, the ground state term is typically of even parity, reflecting common configurations like np² or np⁴ where the sum of odd l values from p electrons is even. In the carbon and oxygen examples, the ^3P terms have even parity, consistent with observed spectra.[1]Term Symbols of Chemical Elements
The ground state term symbols for neutral atoms provide a spectroscopic designation of their lowest-energy electronic states, encapsulating the total orbital angular momentum quantum number L, total spin quantum number S, and total angular momentum J in LS coupling. These are derived from the electron configurations using Hund's rules, as detailed in prior sections. Data for neutral atoms up to oganesson (Z=118) are compiled in the NIST Atomic Spectra Database, though for superheavy elements (Z ≥ 113), values are often based on theoretical predictions due to experimental challenges in producing and observing these short-lived species.[18] In the s-block, alkali metals (group 1) exhibit ^2S_{1/2} ground states due to a single valence s-electron, while alkaline earth metals (group 2) have closed-shell ^1S_0 configurations. p-block elements show increasing spin multiplicity with unpaired p-electrons: for example, group 13 has ^2P^o_{1/2}, group 15 ^4S^o_{3/2}, and group 17 ^2P^o_{3/2}, reflecting half-filled or nearly filled subshells. d-block transition metals display more varied terms, such as ^7S_3 for Cr and Mn (exceptions with high-spin s^1 d^{n-1} configurations), while f-block lanthanides and actinides often involve complex 4f or 5f terms influenced by intermediate coupling. These trends illustrate the periodic variation in electronic structure, with parity (even or odd, denoted by superscript o for odd) determined by the number of unpaired electrons in odd-l orbitals.[19] The table below summarizes representative ground state term symbols for neutral atoms, organized by periodic table block, focusing on key elements to highlight patterns. Full listings, including J values and uncertainties, are available in the NIST database; note that excited states exist for all elements but are not ground configurations. For superheavies like nihonium (Nh, Z=113) and moscovium (Mc, Z=115), predicted terms include ^2P^o_{1/2} and ^4S^o_{3/2}, respectively, based on relativistic Dirac-Fock calculations, though experimental confirmation remains limited as of 2025.[18]| Block | Z | Element | Configuration (valence) | Ground Term Symbol |
|---|---|---|---|---|
| s | 1 | H | 1s | ^2S_{1/2} |
| s | 3 | Li | 2s | ^2S_{1/2} |
| s | 11 | Na | 3s | ^2S_{1/2} |
| s | 2 | He | 1s^2 | ^1S_0 |
| s | 4 | Be | 2s^2 | ^1S_0 |
| s | 20 | Ca | 4s^2 | ^1S_0 |
| p | 5 | B | 2s^2 2p | ^2P^o_{1/2} |
| p | 13 | Al | 3s^2 3p | ^2P^o_{1/2} |
| p | 6 | C | 2s^2 2p^2 | ^3P_0 |
| p | 14 | Si | 3s^2 3p^2 | ^3P_0 |
| p | 7 | N | 2s^2 2p^3 | ^4S^o_{3/2} |
| p | 15 | P | 3s^2 3p^3 | ^4S^o_{3/2} |
| p | 8 | O | 2s^2 2p^4 | ^3P_2 |
| p | 16 | S | 3s^2 3p^4 | ^3P_2 |
| p | 9 | F | 2s^2 2p^5 | ^2P^o_{3/2} |
| p | 17 | Cl | 3s^2 3p^5 | ^2P^o_{3/2} |
| p | 10 | Ne | 2s^2 2p^6 | ^1S_0 |
| p | 18 | Ar | 3s^2 3p^6 | ^1S_0 |
| d | 21 | Sc | 3d 4s^2 | ^2D_{3/2} |
| d | 24 | Cr | 3d^5 4s | ^7S_3 |
| d | 25 | Mn | 3d^5 4s^2 | ^6S_{5/2} |
| d | 26 | Fe | 3d^6 4s^2 | ^5D_4 |
| d | 29 | Cu | 3d^{10} 4s | ^2S_{1/2} |
| d | 30 | Zn | 3d^{10} 4s^2 | ^1S_0 |
| f | 58 | Ce | 4f 5d 6s^2 | ^1G_4 |
| f | 59 | Pr | 4f^3 6s^2 | ^4I_{9/2} |
| f | 64 | Gd | 4f^7 5d 6s^2 | ^9D_2 |
| Superheavy | 113 | Nh | 7p^1 (predicted) | ^2P^o_{1/2} |
| Superheavy | 115 | Mc | 7s^2 7p^3 (predicted) | ^4S^o_{3/2} |
| Superheavy | 117 | Ts | 7s^2 7p^5 (predicted) | ^2P^o_{3/2} |
| Superheavy | 118 | Og | 7s^2 7p^6 (predicted) | ^1S_0 |