Two-electron atom

In atomic physics, a two-electron atom or helium-like ion is a quantum mechanical system consisting of one nucleus with a charge of Ze and just two electrons. This is the first case of many-electron systems where the Pauli exclusion principle plays a central role.

It is an example of a three-body problem.

The first few two-electron atoms are:

Z=1:	H⁻	hydrogen anion
Z=2:	He	helium atom
Z=3:	Li⁺	lithium ion
Z=4:	Be²⁺	beryllium ion
Z=5:	B³⁺	boron ion

Schrödinger equation

The Schrödinger equation for any two-electron system, such as the neutral Helium atom (He, Z = 2), the negative Hydrogen ion (H⁻, Z = 1), or the positive Lithium ion (Li⁺, Z = 3) is:^[1] For a more rigorous mathematical derivation of Schrödinger's equation, see also.^[1] $E\psi =-\hbar ^{2}\left[{\frac {1}{2\mu }}\left(\nabla _{1}^{2}+\nabla _{2}^{2}\right)+{\frac {1}{M}}\nabla _{1}\cdot \nabla _{2}\right]\psi +{\frac {e^{2}}{4\pi \varepsilon _{0}}}\left[{\frac {1}{r_{12}}}-Z\left({\frac {1}{r_{1}}}+{\frac {1}{r_{2}}}\right)\right]\psi$ where r₁ is the position of one electron (r₁ = |r₁| is its magnitude), r₂ is the position of the other electron (r₂ = |r₂| is the magnitude), r₁₂ = |r₁₂| is the magnitude of the separation between them given by $|\mathbf {r} _{12}|=|\mathbf {r} _{2}-\mathbf {r} _{1}|$ μ is the two-body reduced mass of an electron with respect to the nucleus of mass M $\mu ={\frac {m_{e}M}{m_{e}+M}}$ and Z is the atomic number for the element (not a quantum number).

The cross-term of two Laplacians ${\frac {1}{M}}\nabla _{1}\cdot \nabla _{2}$ is known as the mass polarization term, which arises due to the motion of atomic nuclei. The wavefunction is a function of the two electron's positions: $\psi =\psi (\mathbf {r} _{1},\mathbf {r} _{2})$

There is no closed form solution for this equation.

Spectrum

The optical spectrum of the two electron atom has two systems of lines. A para system of single lines, and an ortho system of triplets (closely spaced group of three lines). The energy levels in the atom for the single lines are indicated by ¹S₀ ¹P₁ ¹D₂ ¹F₃ etc., and for the triplets, some energy levels are split: ³S₁ ³P₂ ³P₁ ³P₀ ³D₃ ³D₂ ³D₁ ³F₄ ³F₃ ³F₂.^[2] Alkaline earths and mercury also have spectra with similar features, due to the two outer valence electrons.^[2]

References

^ ^a ^b Physics of Atoms and Molecules, B.H. Bransden, C.J.Joachain, Longman, 1983, ISBN 0-582-44401-2
^ ^a ^b Herzberg, Gerhard; J W T Spinks (1944). Atomic Spectra and Atomic Structure (2nd ed.). New York: Dover Publications. p. 75.

[Bransden-1] Physics of Atoms and Molecules, B.H. Bransden, C.J.Joachain, Longman, 1983, ISBN 0-582-44401-2

[Herzberg-2] Herzberg, Gerhard; J W T Spinks (1944). Atomic Spectra and Atomic Structure (2nd ed.). New York: Dover Publications. p. 75.

[1]

[2]

Schrödinger equation

Spectrum

See also

References