Dihydrogen cation

Bonding in H⁺
₂ can be described as a covalent one-electron bond, which has a formal bond order of one half.^[3]

The ground state energy of the ion is -0.597 Hartree.^[4]

The bond length in the ground state is 2.00 Bohr radius.

The dihydrogen cation has six isotopologues. Each of the two nuclei can be one of the following: proton (p, the most common one), deuteron (d), or triton (t).^[5][6]

• H+2 = ¹H+2 (dihydrogen cation, the common one)^[5][6]
• [HD]⁺ = [¹H²H]⁺ (hydrogen deuterium cation)^[5]
• D+2 = ²H+2 (dideuterium cation)^[5][6]
• [HT]⁺ = [¹H³H]⁺ (hydrogen tritium cation)
• [DT]⁺ = [²H³H]⁺ (deuterium tritium cation)
• T+2 = ³H+2 (ditritium cation)^[6]

An approximate description of the dihydrogen cation starts with the neglect of the motion of the nuclei - the so-called clamped-nuclei approximation. This is a good approximation because the nuclei (proton, deuteron or triton) are more than a factor 1000 heavier than the electron. Therefore, the motion of the electron is treated first, for a given (arbitrary) nucleus-nucleus distance R. The electronic energy of the molecule E is computed and the computation is repeated for different values of R. The nucleus-nucleus repulsive energy e²/(4πε₀R) has to be added to the electronic energy, resulting in the total molecular energy E_tot(R).

The energy E is the eigenvalue of the Schrödinger equation for the single electron. The equation can be solved in a relatively straightforward way due to the lack of electron–electron repulsion (electron correlation). The wave equation (a partial differential equation) separates into two coupled ordinary differential equations when using prolate spheroidal coordinates instead of cartesian coordinates. The analytical solution of the equation, the wave function, is therefore proportional to a product of two infinite power series.^[7] The numerical evaluation of the series can be readily performed on a computer. The analytical solutions for the electronic energy eigenvalues are also a generalization of the Lambert W function^[8] which can be obtained using a computer algebra system within an experimental mathematics approach.

Quantum chemistry and Physics textbooks usually treat the binding of the molecule in the electronic ground state by the simplest possible ansatz for the wave function: the (normalized) sum of two 1s hydrogen wave functions centered on each nucleus. This ansatz correctly reproduces the binding but is numerically unsatisfactory.

Early attempts to treat H⁺
₂ using the old quantum theory were published in 1922 by Karel Niessen^[9] and Wolfgang Pauli,^[10] and in 1925 by Harold Urey.^[11]

The first successful quantum mechanical treatment of H⁺
₂ was published by the Danish physicist Øyvind Burrau in 1927,^[1] just one year after the publication of wave mechanics by Erwin Schrödinger.

In 1928, Linus Pauling published a review putting together the work of Burrau with the work of Walter Heitler and Fritz London on the hydrogen molecule.^[12] The complete mathematical solution of the electronic energy problem for H⁺
₂ in the clamped-nuclei approximation was provided by Wilson (1928) and Jaffé (1934). Johnson (1940) gives a succinct summary of their solution,.^[7]

 

The electronic Schrödinger wave equation for the hydrogen molecular ion H⁺
₂ with two fixed nuclear centers, labeled A and B, and one electron can be written as

${\displaystyle \left(-{\frac {\hbar ^{2}}{2m}}\nabla ^{2}+V\right)\psi =E\psi ~,}$ 

where V is the electron-nuclear Coulomb potential energy function:

${\displaystyle V=-{\frac {e^{2}}{4\pi \varepsilon _{0}}}\left({\frac {1}{r_{a}}}+{\frac {1}{r_{b}}}\right)}$ 

and E is the (electronic) energy of a given quantum mechanical state (eigenstate), with the electronic state function ψ = ψ(r) depending on the spatial coordinates of the electron. An additive term ⁠1/R⁠, which is constant for fixed internuclear distance R, has been omitted from the potential V, since it merely shifts the eigenvalue. The distances between the electron and the nuclei are denoted r_a and r_b. In atomic units (ħ = m = e = 4πε₀ = 1) the wave equation is

${\displaystyle \left(-{\tfrac {1}{2}}\nabla ^{2}+V\right)\psi =E\psi \qquad {\mbox{with}}\qquad V=-{\frac {1}{r_{a}}}-{\frac {1}{r_{b}}}\;.}$ 

We choose the midpoint between the nuclei as the origin of coordinates. It follows from general symmetry principles that the wave functions can be characterized by their symmetry behavior with respect to the point group inversion operation i (r ↦ −r). There are wave functions ψ_g(r), which are symmetric with respect to i, and there are wave functions ψ_u(r), which are antisymmetric under this symmetry operation:

${\displaystyle \psi _{g/u}(-{\mathbf {r} })={}\pm \psi _{g/u}({\mathbf {r} })\;.}$ 

The suffixes g and u are from the German gerade and ungerade) occurring here denote the symmetry behavior under the point group inversion operation i. Their use is standard practice for the designation of electronic states of diatomic molecules, whereas for atomic states the terms even and odd are used. The ground state (the lowest state) of H⁺
₂ is denoted X²Σ⁺
_g^[13] or 1sσ_g and it is gerade. There is also the first excited state A²Σ⁺
_u (2pσ_u), which is ungerade.

 

Asymptotically, the (total) eigenenergies E_g/u for these two lowest lying states have the same asymptotic expansion in inverse powers of the internuclear distance R:^[14][15]

${\displaystyle E_{g/u}=-{\frac {1}{2}}-{\frac {9}{4R^{4}}}+O\left(R^{-6}\right)+\cdots }$ 

This and the energy curves include the internuclear 1/R term. The actual difference between these two energies is called the exchange energy splitting and is given by:^[16]

${\displaystyle \Delta E=E_{u}-E_{g}={\frac {4}{e}}\,R\,e^{-R}\left[\,1+{\frac {1}{2R}}+O\left(R^{-2}\right)\,\right]}$ 

which exponentially vanishes as the internuclear distance R gets greater. The lead term ⁠4/e⁠Re^−R was first obtained by the Holstein–Herring method. Similarly, asymptotic expansions in powers of ⁠1/R⁠ have been obtained to high order by Cizek et al. for the lowest ten discrete states of the hydrogen molecular ion (clamped nuclei case). For general diatomic and polyatomic molecular systems, the exchange energy is thus very elusive to calculate at large internuclear distances but is nonetheless needed for long-range interactions including studies related to magnetism and charge exchange effects. These are of particular importance in stellar and atmospheric physics.

The energies for the lowest discrete states are shown in the graph above. These can be obtained to within arbitrary accuracy using computer algebra from the generalized Lambert W function (see eq. (3) in that site and reference^[8]). They were obtained initially by numerical means to within double precision by the most precise program available, namely ODKIL.^[17] The red solid lines are ²Σ⁺
_g states. The green dashed lines are ²Σ⁺
_u states. The blue dashed line is a ²Π_u state and the pink dotted line is a ²Π_g state. Note that although the generalized Lambert W function eigenvalue solutions supersede these asymptotic expansions, in practice, they are most useful near the bond length.

The complete Hamiltonian of H⁺
₂ (as for all centrosymmetric molecules) does not commute with the point group inversion operation i because of the effect of the nuclear hyperfine Hamiltonian. The nuclear hyperfine Hamiltonian can mix the rotational levels of g and u electronic states (called ortho-para mixing) and give rise to ortho-para transitions.^[18][19]

Once the energy function E_tot(R) has been obtained, one can compute the quantum states of rotational and vibrational motion of the nuclei, and thus of the molecule as a whole. The corresponding `'nuclear'´ Schrödinger equation is a one-dimensional ordinary differential equation, where the nucleus-nucleus distance R is the independent coordinate. The equation describes the motion of a fictitious particle of mass equal to the reduced mass of the two nuclei, in the potential E_tot(R)+V_L(R), where the second term is the centrifugal potential due to rotation with angular momentum described by the quantum number L. The eigenenergies of this Schrödinger equation are the total energies of the whole molecule, electronic plus nuclear.

The Born-Oppenheimer approximation is unsuited for describing the dihydrogen cation accurately enough to explain the results of precision spectroscopy.

The full Schrödinger equation for this cation, without the approximation of clamped nuclei, is much more complex, but nevertheless can be solved numerically essentially exactly using a variational approach.^[20] Thereby, the simultaneous motion of the electron and of the nuclei is treated exactly. When the solutions are restricted to the lowest-energy orbital, one obtains the rotational and ro-vibrational states' energies and wavefunctions. The numerical uncertainty of the energies and the wave functions found in this way is negligible compared to the systematic error stemming from using the Schrödinger equation, rather than fundamentally more accurate equations. Indeed, the Schrödinger equation does not incorporate all relevant physics, as is known from the hydrogen atom problem. More accurate treatments need to consider the physics that is described by the Dirac equation or, even more accurately, by quantum electrodynamics. The most accurate solutions of the ro-vibrational states are found by applying non-relativistic quantum electrodynamics (NRQED) theory.^[21]

For comparison with experiment, one requires differences of state energies, i.e. transition frequencies. For transitions between ro-vibrational levels having small rotational and moderate vibrational quantum numbers the frequencies have been calculated with theoretical fractional uncertainty of approximately 8×10⁻¹².^[21] Additional contributions to the uncertainty of the predicted frequencies arise from the uncertainties of fundamental constants, which are input to the theoretical calculation, especially from the ratio of the proton mass and the electron mass.

Using a sophisticated ab initio formalism, also the hyperfine energies can be computed accurately, see below.

Because of its relative simplicity, the dihydrogen cation is the molecule that is most precisely understood, in the sense that theoretical calculations of its energy levels match the experimental results with the highest level of agreement.

Specifically, spectroscopically determined pure rotational and ro-vibrational transition frequencies of the particular isotopologue HD⁺ agree with theoretically computed transition frequencies. Four high-precision experiments yielded comparisons with total uncertainties between 2×10⁻¹¹ and 5×10⁻¹¹, fractionally.^[22] The level of agreement is actually limited neither by theory not by experiment but rather by the uncertainty of the current values of the masses of the particles, that are used as input parameters to the calculation.

In order to measure the transition frequencies with high accuracy, the spectroscopy of the dihydrogen cation had to be performed under special conditions. Therefore, ensembles of HD⁺ ions were trapped in a quadrupole ion trap under ultra-high vacuum, sympathetically cooled by laser-cooled beryllium ions, and interrogated using particular spectroscopic techniques.

The hyperfine structure of the homonuclear isotopologue H₂⁺ has been measured extensively and precisely by Jefferts in 1969. Finally, in 2021, ab initio theory computations were able to provide the quantitative details of the structure with uncertainty smaller than that of the experimental data, 1 kHz. Some contributions to the measured hyperfine structure have been theoretically confirmed at the level of approximately 50 Hz.^[23]

The implication of these agreements is that one can deduce a spectroscopic value of the ratio of electron mass to reduced proton-deuteron mass, m_e/m_p+m_e/m_d, that is an input to the ab initio theory. The ratio is fitted such that theoretical prediction and experimental results agree. The uncertainty of the obtained ratio is comparable to the one obtained from direct mass measurements of proton, deuteron, electron, and HD⁺ via cyclotron resonance in Penning traps.

The dihydrogen ion is formed in nature by the interaction of cosmic rays and the hydrogen molecule. An electron is knocked off leaving the cation behind.^[24]

H₂ + cosmic ray → H⁺
₂ + e⁻ + cosmic ray.

Cosmic ray particles have enough energy to ionize many molecules before coming to a stop.

The ionization energy of the hydrogen molecule is 15.603 eV. High speed electrons also cause ionization of hydrogen molecules with a peak cross section around 50 eV. The peak cross section for ionization for high speed protons is 70000 eV with a cross section of 2.5×10⁻¹⁶ cm². A cosmic ray proton at lower energy can also strip an electron off a neutral hydrogen molecule to form a neutral hydrogen atom and the dihydrogen cation, (p⁺ + H₂ → H + H⁺
₂) with a peak cross section at around 8000 eV of 8×10⁻¹⁶ cm².^[25]

In nature the ion is destroyed by reacting with other hydrogen molecules:

H⁺
₂ + H₂ → H⁺
₃ + H.

In the laboratory, the ion is easily produced by electron bombardment from an electron gun.

An artificial plasma discharge cell can also produce the ion.^{[citation needed]}

• Symmetry of diatomic molecules
• Dirac Delta function model (one-dimensional version of H⁺
  ₂)
• Di-positronium
• Euler's three-body problem (classical counterpart)
• Few-body systems
• Helium atom
• Helium hydride ion
• Trihydrogen cation
• Triatomic hydrogen
• Lambert W function
• Molecular astrophysics
• Holstein–Herring method
• Three-body problem
• List of quantum-mechanical systems with analytical solutions