Physics:Quantum Hydrogen atom

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The hydrogen atom is the simplest atomic system, consisting of a single electron bound to a proton by the Coulomb interaction. It is the only atom in quantum mechanics that admits a fully exact analytical solution of the Schrödinger equation, making it a fundamental model for understanding atomic structure, spectroscopy, and quantum theory.[1]

Energy levels and spectral series of the hydrogen atom showing Lyman (ultraviolet), Balmer (visible), and Paschen, Brackett, Pfund (infrared) transitions.

Schrödinger equation and Coulomb potential

The electron in a hydrogen atom is described by the time-independent Schrödinger equation in a central Coulomb potential:

[22m2e24πε0r]ψ(𝐫)=Eψ(𝐫)

Because the potential depends only on the radial coordinate r, the equation is separable in spherical coordinates.[2]

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Quantum numbers

The solutions are characterized by three quantum numbers:

  • Principal quantum number: n=1,2,3,
  • Orbital angular momentum: =0,1,,n1
  • Magnetic quantum number: m=,,

These arise from the separation of variables into radial and angular parts.[3]

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Energy levels

The allowed energy levels depend only on the principal quantum number:

En=13.6eVn2

This degeneracy is a consequence of the underlying symmetry of the Coulomb potential.[4]

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Wavefunctions and orbitals

The hydrogen wavefunctions are products of radial functions and spherical harmonics:

ψnm(r,θ,ϕ)=Rn(r)Ym(θ,ϕ)

These define the familiar atomic orbitals:

  • s-orbitals (=0) — spherical symmetry
  • p-orbitals (=1) — directional lobes
  • d-orbitals (=2) — more complex structures

[5]

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Angular momentum

The orbital angular momentum is quantized:

L2=2(+1),Lz=m

The hydrogen atom also includes electron spin, introducing total angular momentum when relativistic effects are considered.[6]

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Spectral lines

Transitions between energy levels produce photons with energy:

E=hν=EiEf

This gives rise to discrete spectral series:

  • Lyman series (n1) — ultraviolet
  • Balmer series (n2) — visible
  • Paschen, Brackett, Pfund — infrared

The wavelengths satisfy the Rydberg formula:

1λ=RH(1nf21ni2)

where RH is the Rydberg constant.[7][8]

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Fine and hyperfine structure

More accurate treatments include:

  • Fine structure — relativistic corrections and spin–orbit coupling
  • Hyperfine structure — interaction between electron and nuclear spin

These effects lift degeneracies and produce small spectral splittings.[9][10]

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Importance in quantum mechanics

The hydrogen atom plays a central role because:

  • It provides an exact solution of the Schrödinger equation
  • It explains atomic spectra quantitatively
  • It reveals hidden symmetries (e.g., Runge–Lenz vector)
  • It serves as the starting point for multi-electron approximations

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See also

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References


Author: Harold Foppele