Electron rest mass

The electron rest mass (symbol: m_e) is the mass of a stationary electron. It is one of the fundamental constants of physics and is also very important in chemistry because of its relation to the Avogadro constant. It has a value of about 6969911000000000000♠9.11×10⁻³¹ kilograms or about 6996548600000000000♠5.486×10⁻⁴ atomic mass units, equivalent to an energy of about 6986818999999999999♠8.19×10⁻¹⁴ joules or about 0.511 megaelectronvolts.^[1]

Terminology

The term "rest mass" + kinetic energy comes from the need to take account of the effects of special relativity on the apparent (or "observed") mass of an electron. It is impossible to "weigh" a stationary electron, and so all practical measurements must be carried out on moving electrons. The same is true with any other sub-atomic particle. For particles like photons or gluons the situation is even more problematic since the very concept of a stationary or "at rest" massless particle lacks meaning.

Determination

The electron rest mass in kilograms is calculated from the definition of the Rydberg constant R_∞:

where α is the fine structure constant and h is the Planck constant.^[1] The relative uncertainty, 5×10⁻⁸ in the 2006 CODATA recommended value,^[2] is due entirely to the uncertainty in the value of the Planck constant.

The electron relative atomic mass can be measured directly in a Penning trap. It can also be inferred from the spectra of antiprotonic helium atoms (helium atoms where one of the electrons has been replaced by an antiproton) or from measurements of the electron g-factor in the hydrogenic ions ¹²C⁵⁺ or ¹⁶O⁷⁺. The 2006 CODATA recommended value has a relative uncertainty of 4.2×10⁻¹⁰.^[1]

The electron relative atomic mass is an adjusted parameter in the CODATA set of fundamental physical constants, while the electron rest mass in kilograms is calculated from the values of the Planck constant, the fine structure constant and the Rydberg constant.^[1] The correlation between the two values is negligible (r = 0.0003).^[2]

Relationship to other physical constants

As mentioned above, the electron mass is used to calculate the Avogadro constant N_A:

Hence it is also related to the atomic mass constant m_u:

where M_u is molar mass constant (defined in SI) and A_r(e) is a directly measured quantity, the relative mass of electron.

Note that m_u is defined in terms of A_r(e), and not the other way round, and so the name "electron mass in atomic mass units" for A_r(e) involves a circular definition (at least in terms of practical measurements).

The electron relative atomic mass also enters into the calculation of all other relative atomic masses. By convention, relative atomic masses are quoted for neutral atoms, but the actual measurements are made on positive ions, either in a mass spectrometer or a Penning trap. Hence the mass of the electrons must be added back on to the measured values before tabulation. A correction must also be made for the mass equivalent of the binding energy E_b. Taking the simplest case of complete ionization of all electrons, for a nuclide X of atomic number Z,^[1]

As relative atomic masses are measured as ratios of masses, the corrections must be applied to both ions: fortunately, the uncertainties in the corrections are negligible, as illustrated below for hydrogen 1 and oxygen 16.

The principle can be shown by the determination of the electron relative atomic mass by Farnham et al. at the University of Washington (1995).^[3] It involves the measurement of the frequencies of the cyclotron radiation emitted by electrons and by ¹²C⁶⁺ ions in a Penning trap. The ratio of the two frequencies is equal to six times the inverse ratio of the masses of the two particles (the heavier the particle, the lower the frequency of the cyclotron radiation; the higher the charge on the particle, the higher the frequency):

As the relative atomic mass of ¹²C⁶⁺ ions is very nearly 12, the ratio of frequencies can be used to calculate a first approximation to A_r(e), 5.486 303 7178×10⁻⁴. This approximate value is then used to calculate a first approximation to A_r(¹²C⁶⁺), knowing that E_b(¹²C)/m_uc² (from the sum of the six ionization energies of carbon) is 1.105 8674×10⁻⁶: A_r(¹²C⁶⁺) ≈ 11.996 708 723 6367. This value is then used to calculate a new approximation to A_r(e), and the process repeated until the values no longer vary (given the relative uncertainty of the measurement, 2.1×10⁻⁹): this happens by the fourth cycle of iterations for these results, giving A_r(e) = 5.485 799 111(12)×10⁻⁴ for these data.

References