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Term symbols usually specify the total for all electrons in an atom, but are sometimes used to describe electrons in a given subshell or set of subshells, for example to describe each open subshell in an atom having more than one. The ground state term symbol for neutral atoms is described, in most cases, by Hund's rules.
This notation is used to specify electron configurations and to create the term symbol for the electron states in a multi-electron atom. When writing a term symbol, the above scheme for a single electron's orbital quantum number is applied to the total orbital angular momentum associated to an electron state. [4]
For one like atom in a 1 S g state and one in a 1 P u state, the possible diatomic states are 1 Σ g +, 1 Σ u +, 1 Π g and 1 Π u. [5] The parity of an atomic term is g if the sum of the individual angular momentum is even, and u if the sum is odd.
The lightest atom that requires the second rule to determine the ground state term is titanium (Ti, Z = 22) with electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 3d 2 4s 2. In this case the open shell is 3d 2 and the allowed terms include three singlets ( 1 S, 1 D, and 1 G) and two triplets ( 3 P and 3 F).
When S > L there are only 2L+1 orientations of total angular momentum possible, ranging from S+L to S-L. [2] [3] The ground state of the nitrogen atom is a 4 S state, for which 2S + 1 = 4 in a quartet state, S = 3/2 due to three unpaired electrons. For an S state, L = 0 so that J can only be 3/2 and there is only one level even though the ...
This page shows the electron configurations of the neutral gaseous atoms in their ground states. For each atom the subshells are given first in concise form, then with all subshells written out, followed by the number of electrons per shell. For phosphorus (element 15) as an example, the concise form is [Ne] 3s 2 3p 3.
The N atom and the O + ion are isoelectronic because each has five valence electrons, or more accurately an electronic configuration of [He] 2s 2 2p 3. Similarly, the cations K +, Ca 2+, and Sc 3+ and the anions Cl −, S 2−, and P 3− are all isoelectronic with the Ar atom. CO, CN −, N 2, and NO +
For example, the ground state of the nitrogen atom has the electron configuration 1s 2 2s 2 2p 3, and is identified by the term symbol 4 S o, where the superscript o denotes odd parity. However the third excited term at about 83,300 cm −1 above the ground state has electron configuration 1s 2 2s 2 2p 2 3s has even parity since there are only ...