# Kinetic diameter

Kinetic diameter is a measure applied to atoms and molecules that expresses the likelihood that a molecule in a gas will collide with another molecule. It is an indication of the size of the molecule as a target. The kinetic diameter is not the same as atomic diameter defined in terms of the size of the atom's electron shell, which is generally a lot smaller, depending on the exact definition used. Rather, it is the size of the sphere of influence that can lead to a scattering event.
Kinetic diameter is related to the mean free path of molecules in a gas. Mean free path is the average distance that a particle will travel without collision. For a fast moving particle (that is, one moving much faster than the particles it is moving through) the kinetic diameter is given by,
    $d^{2}={1 \over \pi ln}$
    where,
    d is the kinetic diameter,
    r is the kinetic radius, r = d/2,
    l is the mean free path, and
    n is the number density of particles
However, a more usual situation is that the colliding particle being considered is indistinguishable from the population of particles in general. Here, the Maxwell–Boltzmann distribution of energies must be considered, which leads to the modified expression,
    $d^{2}={1 \over {\sqrt {2}}\pi ln}$

## List of diameters

The following table lists the kinetic diameters of some common molecules;
| Molecule | Molecule | Molecular mass | Kinetic diameter (pm) | ref |
| Name | Formula | Molecular mass | Kinetic diameter (pm) | ref |
| Hydrogen | H$_2$ | 2 | 289 | |
| Helium | He | 4 | 260 | |
| Methane | CH$_4$ | 16 | 380 | |
| Ammonia | NH$_3$ | 17 | 260 | |
| Water | H$_2$O | 18 | 265 | |
| Neon | Ne | 20 | 275 | |
| Acetylene | C$_2$H$_2$ | 26 | 330 | |
| Nitrogen | N$_2$ | 28 | 364 | |
| Carbon monoxide | CO | 28 | 376 | |
| Ethylene | C$_2$H$_4$ | 28 | 390 | |
| Nitric oxide | NO | 30 | 317 | |
| Oxygen | O$_2$ | 32 | 346 | |
| Hydrogen sulfide | H$_2$S | 34 | 360 | |
| Hydrogen chloride | HCl | 36 | 320 | |
| Argon | Ar | 40 | 340 | |
| Propylene | C$_3$H$_6$ | 42 | 450 | |
| Carbon dioxide | CO$_2$ | 44 | 330 | |
| Nitrous oxide | N$_2$O | 44 | 330 | |
| Propane | C$_3$H$_8$ | 44 | 430 | |
| Sulfur dioxide | SO$_2$ | 64 | 360 | |
| Chlorine | Cl$_2$ | 70 | 320 | |
| Benzene | C$_6$H$_6$ | 78 | 585 | |
| Hydrogen bromide | HBr | 81 | 350 | |
| Krypton | Kr | 84 | 360 | |
| Xenon | Xe | 131 | 396 | |
| Sulfur hexafluoride | SF$_6$ | 146 | 550 | |
| Carbon tetrachloride | CCl$_4$ | 154 | 590 | |
| Bromine | Br$_2$ | 160 | 350 | |

## Dissimilar particles

Collisions between two dissimilar particles occur when a beam of fast particles is fired into a gas consisting of another type of particle, or two dissimilar molecules randomly collide in a gas mixture. For such cases, the above formula for scattering cross section has to be modified.
The scattering cross section, σ, in a collision between two dissimilar particles or molecules is defined by the sum of the kinetic diameters of the two particles,
    $\sigma =\pi (r_{1}+r_{2})^{2}$
    where.
    r$_1$, r$_2$ are, half the kinetic diameter (ie, the kinetic radii) of the two particles, respectively.
We define an intensive quantity, the scattering coefficient α, as the product of the gas number density and the scattering cross section,
    $\alpha \equiv n\sigma$
The mean free path is the inverse of the scattering coefficient,
    $l={1 \over \alpha }={1 \over \sigma n}$
For similar particles, r$_1$ = r$_2$ and,
    $l={1 \over \sigma n}={1 \over 4\pi r^{2}n}={1 \over \pi d^{2}n}$
as before.