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In quantum mechanics, the case of a particle in a one-dimensional ring is similar to the particle in a box. The system is composed of a single particle that has zero potential energy while on a circular ring, and infinite potential energy at all other points in space. This causes the particle to be bound to the ring, which leads to quantized energy levels. This model is one of the few quantum models which can be solved exactly. It is also a useful learning tool in demonstrating the concept of quantum angular momentum. The Schrödinger equation for a free particle which is restricted to a ring (whose configuration space is the circle $$S^1$$) is


 * $$ -\frac{\hbar^2}{2m}\nabla^2 \psi = E\psi $$
 * In which psi represents the wave function of the particle, and the operator on the left side of the equation represents the Hamiltonian for the system. As the potential energy is zero on the ring, the Hamiltonian is entirely comprised by a kinetic energy component.
 * The Schrödinger equation can also be represented in polar coordinates. Using this system (as opposed to a Cartesian coordinate system) will simplify further calculations.
 * $$-{\hbar^2\over 2I }{\partial^2\over\partial \theta_2}\psi(\theta)=E\psi(\theta)$$Solutions Schrodinger.jpg

Wave function
Using polar coordinates on the 1-dimensional ring of radius R, the wave function depends only on the angular coordinate, and so


 * $$ \nabla^2 = \frac{1}{R^2} \frac{\partial^2}{\partial \theta^2} $$J2 am.jpg

Requiring that the wave function be periodic in $$ \ \theta $$ with a period $$ 2 \pi$$ (from the demand that the wave functions be single-valued functions on the circle), and that they be normalized leads to the conditions


 * $$ \int_{0}^{2 \pi} \left| \psi ( \theta ) \right|^2 \, R d\theta = 1\ $$,

and


 * $$ \ \psi (\theta) = \ \psi ( \theta + 2\pi)$$

Under these conditions, the solution to the Schrödinger equation is given by


 * $$ \psi_{\pm}(\theta) = \frac{1}{\sqrt{2 \pi R}}\, e^{\pm i \frac{R}{\hbar} \sqrt{2 m E} \theta } $$

Energy eigenvalues
The energy eigenvalues $$ E $$ are quantized because of the periodic boundary conditions, and they are required to satisfy


 * $$ e^{\pm i \frac{R}{\hbar} \sqrt{2 m E} \theta } =  e^{\pm i \frac{R}{\hbar} \sqrt{2 m E} (\theta +2 \pi)}$$, or
 * $$ e^{\pm i 2 \pi \frac{R}{\hbar} \sqrt{2 m E} } = 1 = e^{i 2 \pi n}$$

The eigenfunctions and energy eigenvalues are
 * $$ \psi(\theta) = \frac{1}{\sqrt{2 \pi R}} \, e^{\pm i n \theta }$$
 * $$ E_n = \frac{n^2 \hbar^2}{2 m R^2} $$ where $$n = 0,\pm 1,\pm 2,\pm 3, \ldots$$

Therefore, there are two degenerate quantum states for every value of $$ n>0 $$ (corresponding to $$ \ e^{\pm i n \theta}$$). Therefore, there are 2n+1 states with energies up to an energy indexed by the number n.

The case of a particle in a one-dimensional ring is an instructive example when studying the quantization of angular momentum for an electron orbiting the nucleus. The azimuthal wave functions in that case are identical to the energy eigenfunctions of the particle on a ring.

The statement that any wavefunction for the particle on a ring can be written as a superposition of energy eigenfunctions is identical to the Fourier theorem about the development of any periodic function in a Fourier series.Circular_Standing_Wave.gif on a circular string, the circle is broken into exactly 8 wavelengths. A standing wave like this can have 0,1,2, or any integer number of wavelengths around the circle, but it cannot have a non-integer number of wavelengths like 8.3. In quantum mechanics, angular momentum is quantized for a similar reason.

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Angular Momentum of a Particle in a Ring
­By constraining the motion of the particle to the x, y-plane, the angular momentum vector will be in the z direction. However, according to quantum mechanics, it is not possible to know the direction of the angular momentum vector. Our knowledge of the angular momentum does allow for the determination of the length of the angular momentum vector and any one component. If the vector is found in the z-axis, then the x and y components are zero and all three components are known.

Application
In organic chemistry, aromatic compounds contain ring structures, such as benzene, consisting of five or six, usually carbon, atoms. So does the surface of "buckyballs" (buckminsterfullerene). This ring behaves like a circular waveguide, with the valence electrons orbiting in both directions. To fill all energy levels up to n requires $$2\times(2n+1)=4n+2$$ electrons, as electrons have additionally two possible orientations of their spins. This is known as Hückel's rule. Continuous overlap of unhybridized p-orbitals around the ring gives exceptional stability (aromaticity). Because of this stability, the electrons of the pi system are bound to the ring structure; as such, the energies of the pi electrons can be well approximated by the particle on a ring system.