Morse potential

The Morse potential, named after physicist Philip M. Morse, is a convenient model for the potential energy of a diatomic molecule. It is a better approximation for the vibrational structure of the molecule than the quantum harmonic oscillator because it explicitly includes the effects of bond breaking, such as the existence of unbound states. It also accounts for the anharmonicity of real bonds and the non-zero transition probability for overtone and combination bands. The Morse potential can also be used to model other interactions such as the interaction between an atom and a surface.

Potential Energy Function

The Morse potential (blue) and harmonic oscillator potential (green). Unlike the energy levels of the harmonic oscillator potential, which are evenly spaced by ħω, the Morse potential level spacing decreases as the energy approaches the dissociation energy. The dissociation energy D_e is larger than the true energy required for dissociation D₀ due to the zero point energy of the lowest (v = 0) vibrational level.

The Morse potential energy function is of the form

$V(r) = D_e ( 1-e^{-a(r-r_e)} )^2$

Here r is the distance between the atoms, r_e is the equilibrium bond distance, D_e is the well depth (defined relative to the dissociated atoms), and a controls the 'width' of the potential (the smaller a the larger the well). The dissociation energy of the bond can be calculated by subtracting the zero point energy E(0) from the depth of the well. The force constant of the bond can be found by Taylor expansion of V(r) around r = r_e to the second derivative of the potential energy function, from which it can be shown that the parameter, a, is

$a=\sqrt{k_e/2D_e}$,

where k_e is the force constant at the minimum of the well.

Since the zero of potential energy is arbitrary, the equation for the Morse potential can be rewritten any number of ways by adding or subtracting a constant value. When it is used to model the atom-surface interaction, the Morse potential is usually written in the form

$V(r) - D_e = D_e ( e^{-2a(r-r_e)}-2e^{-a(r-r_e)} )$

where r is now the coordinate perpendicular to the surface. This form approaches zero at infinite r and equals − D_e at its minimum. It clearly shows that the Morse potential is the combination of a short-range repulsion and a longer-range attractive tail.

Vibrational States and Energies

To write the stationary states on the Morse potential, i.e. solutions Ψ(v) and E(v) of the following Schrödinger equation:

$\left(-\frac{\hbar ^2 }{2 m }\frac{\partial ^2}{\partial r^2}+V(r)\right)\Psi(v)=E(v)\Psi(v),$

it is convenient to introduce the new variables:

$x=a r \text{; } x_e=a r_e \text{; } \lambda =\frac{\sqrt{2 m D_e}}{a \hbar } \text{; } \varepsilon _v=\frac{2 m }{a^2\hbar ^2}E(v).$

Then, the Schrödinger equation takes the simple form:

$\left(-\frac{\partial ^2}{\partial x^2}+V(x)\right)\Psi _n(x)=\varepsilon _n\Psi _n(x),$

$V(x)=\lambda ^2\left(e^{-2\left(x-x_e\right)}-2e^{-\left(x-x_e\right)}\right).$

Its eigenvalues and eigenstates can be written as:

$\varepsilon _n=-\left(\lambda -n-\frac{1}{2}\right)^2$

$\Psi _n(z)=N_nz^{\lambda -n-\frac{1}{2}}e^{-\frac{1}{2}z}L_n^{2\lambda -2n-1}(z),$

where $z=2\lambda e^{-\left(x-x_e\right)}$; $N_n=n![\frac{a\left(2\lambda-2n-1\right)}{\Gamma (n+1)\Gamma (2\lambda -n)}]^{\frac{1}{2}}$ and $L_n^{\alpha }(z)$ is Laguerre polynomial:

$L_n^{\alpha }(z) = \frac{z^{-\alpha }e^z}{n!} \frac{d^n}{d z^n}\left(z^{n + \alpha } e^{-z}\right)=\frac{\Gamma (\alpha + 2)/\Gamma (\alpha -n+2)}{\Gamma (n+1)} \, _1F_1(-n,\alpha +1,z),$

There also exists the following important analytical expression for matrix elements of the coordinate operator (here it is assumed that m > n and $N=\lambda -\frac{1}{2}$)

$\left\langle \Psi _m(x)|x|\Psi _n(x)\right\rangle =\frac{2(-1)^{m-n+1}}{(m-n)(2N-n-m)} \sqrt{\frac{(N-n)(N-m)\Gamma (2N-m+1)m!}{\Gamma (2N-n+1)n!}}.$

The eigenenergies in the initial variables have form:

$E(v) = h\nu_0 (v+1/2) - \frac{\left[h\nu_0(v+1/2)\right]^2}{4D_e}$

where v is the vibrational quantum number, and ν₀ has units of frequency, and is mathematically related to the particle mass, m, and the Morse constants via

$\nu_0 = \frac{a}{2\pi} \sqrt{2D_e/m}$.

Whereas the energy spacing between vibrational levels in the quantum harmonic oscillator is constant at hν₀, the energy between adjacent levels decreases with increasing v in the Morse oscillator. Mathematically, the spacing of Morse levels is

$E(v+1) - E(v) = h\nu_0 - (v+1) (h\nu_0)^2/2D_e\,$.

This trend matches the anharmonicity found in real molecules. However, this equation fails above some value of v_m where E(v_m + 1) − E(v_m) is calculated to be zero or negative. Specifically,

$v_m = \frac{2D_e-h\nu_0}{h\nu_0}$.

This failure is due to the finite number of bound levels in the Morse potential, and some maximum v_m that remains bound. For energies above v_m, all the possible energy levels are allowed and the equation for E(v) is no longer valid.

Below v_m, E(v) is a good approximation for the true vibrational structure in non-rotating diatomic molecules. In fact, the real molecular spectra are generally fit to the form¹

$E_v / hc = \omega_e (v+1/2) - \omega_e\chi_e (v+1/2)^2\,$

in which the constants ω_e and ω_eχ_e can be directly related to the parameters for the Morse potential.

Solving Schrödinger's equation for the Morse oscillator

Like the quantum harmonic oscillator, the energies and eigenstates of the Morse potential can be found using operator methods . One approach involves applying the factorization method to the Hamiltonian.

See also

• Lennard-Jones potential
• Molecular mechanics

References

• ¹ CRC Handbook of chemistry and physics, Ed David R. Lide, 87th ed, Section 9, SPECTROSCOPIC CONSTANTS OF DIATOMIC MOLECULES p. 9-82
• Morse, P. M. (1929,). "Diatomic molecules according to the wave mechanics. II. Vibrational levels". Phys. Rev. 34: pp. 57-64. Bibcode 1929PhRv...34...57M. doi:10.1103/PhysRev.34.57. 
• Girifalco, L. A.; Weizer, G. V. (1959). "Application of the Morse Potential Function to cubic metals". Phys. Rev. 114 (3): p. 687. Bibcode 1959PhRv..114..687G. doi:10.1103/PhysRev.114.687. 
• Shore, Bruce W. (1973). "Comparison of matrix methods applied to the radial Schrödinger eigenvalue equation: The Morse potential". J. Chem. Phys. 59 (12): p. 6450. doi:10.1063/1.1680025. 
• Keyes, Robert W. (1975). "Bonding and antibonding potentials in group-IV semiconductors". Phys. Rev. Lett. 34 (21): pp. 1334-1337. doi:10.1103/PhysRevLett.34.1334. 
• Lincoln, R. C.; Kilowad, K. M.; Ghate, P. B. (1967). "Morse-potential evaluation of second- and third-order elastic constants of some cubic metals". Phys. Rev. 157 (3): pp. 463-466. doi:10.1103/PhysRev.157.463. 
• Dong, Shi-Hai; Lemus, R.; Frank, A. (2001). "Ladder operators for the Morse potential". Int. J. Quant. Chem. 86 (5): pp. 433-439. doi:10.1002/qua.10038. 
• Zhou, Yaoqi; Karplus, Martin; Ball, Keith D.; Bery, R. Stephen (2002). "The distance fluctuation criterion for melting: Comparison of square-well and Morse Potential models for clusters and homopolymers". J. Chem. Phys 116 (5): pp. 2323-2329. doi:10.1063/1.1426419. 
• I.G. Kaplan, in Handbook of Molecular Physics and Quantum Chemistry, Wiley, 2003, p207.