In particle physics, the electron mass (symbol: m_e) is the mass of a stationary electron, also known as the invariant mass of the electron. It is one of the fundamental constants of physics. It has a value of about 9.109×10⁻³¹ kilograms or about 5.486×10⁻⁴ daltons, which has an energy-equivalent of about 8.187×10⁻¹⁴ joules or about 0.511 MeV.^[3]

Terminology

The term "rest mass" is sometimes used because in special relativity the mass of an object can be said to increase in a frame of reference that is moving relative to that object (or if the object is moving in a given frame of reference). Most practical measurements are carried out on moving electrons. If the electron is moving at a relativistic velocity, any measurement must use the correct expression for mass. Such correction becomes substantial for electrons accelerated by voltages of over 100 kV.

For example, the relativistic expression for the total energy, E, of an electron moving at speed v is

$${\displaystyle E=\gamma m_{\mathrm {e} }c^{2},}$$

where

• c is the speed of light;
• γ is the Lorentz factor, ${\displaystyle \gamma =1/{\sqrt {1-{\tfrac {v^{2}}{c^{2}}}}}}$
• m_e is the "rest mass", or more simply just the "mass" of the electron.

This quantity m_e is frame invariant and velocity independent. However, some texts group the Lorentz factor with the mass factor to define a new quantity called the relativistic mass, m_relativistic = γm_e.

Determination

Since the electron mass determines a number of observed effects in atomic physics, there are potentially many ways to determine its mass from an experiment, if the values of other physical constants are already considered known.

Historically, the mass of the electron was determined directly from combining two measurements. The mass-to-charge ratio of the electron was first estimated by Arthur Schuster in 1890 by measuring the deflection of "cathode rays" due to a known magnetic field in a cathode ray tube. Seven years later J. J. Thomson showed that cathode rays consist of streams of particles, to be called electrons, and made more precise measurements of their mass-to-charge ratio again using a cathode ray tube.

The second measurement was of the charge of the electron. This was determined with a precision of better than 1% by Robert A. Millikan in his oil drop experiment in 1909. Together with the mass-to-charge ratio, the electron mass was determined with reasonable precision. The value of mass that was found for the electron was initially met with surprise by physicists, since it was so small (less than 0.1%) compared to the known mass of a hydrogen atom.

The electron rest mass can be calculated from the Rydberg constant R_∞ and the fine-structure constant α obtained through spectroscopic measurements. Using the definition of the Rydberg constant:

${\displaystyle R_{\infty }={\frac {m_{\rm {e}}c\alpha ^{2}}{2h}},}$

thus

${\displaystyle m_{\rm {e}}={\frac {2R_{\infty }h}{c\alpha ^{2}}},}$

where c is the speed of light and h is the Planck constant.^[4] The relative uncertainty, 5×10⁻⁸ in the 2006 CODATA recommended value,^[5] is due entirely to the uncertainty in the value of the Planck constant. With the re-definition of kilogram in 2019, there is no uncertainty by definition left in Planck constant anymore.

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 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, as detailed above.^[4][5]

Relationship to other physical constants

The electron mass is used to calculate the Avogadro constant N_A:

${\displaystyle N_{\rm {A}}={\frac {M_{\rm {u}}A_{\rm {r}}({\rm {e}})}{m_{\rm {e}}}}={\frac {M_{\rm {u}}A_{\rm {r}}({\rm {e}})c\alpha ^{2}}{2R_{\infty }h}}.}$

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

${\displaystyle m_{\rm {u}}={\frac {M_{\rm {u}}}{N_{\rm {A}}}}={\frac {m_{\rm {e}}}{A_{\rm {r}}({\rm {e}})}}={\frac {2R_{\infty }h}{A_{\rm {r}}({\rm {e}})c\alpha ^{2}}},}$

where

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

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,^[4]

${\displaystyle A_{\rm {r}}({\rm {X}})=A_{\rm {r}}({\rm {X}}^{Z+})+ZA_{\rm {r}}({\rm {e}})-{\frac {E_{\rm {b}}}{m_{\rm {u}}c^{2}}}}$

As relative atomic masses are measured as ratios of masses, the corrections must be applied to both ions: 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).^[6] 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):

${\displaystyle {\frac {\nu _{c}({}^{12}{\rm {C}}^{6+})}{\nu _{c}({\rm {e}})}}={\frac {6A_{\rm {r}}({\rm {e}})}{A_{\rm {r}}({}^{12}{\rm {C}}^{6+})}}=0.000\,274\,365\,185\,89(58)}$

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), 5.4863037178×10⁻⁴. This approximate value is then used to calculate a first approximation to A_r(¹²C⁶⁺), knowing that ${\displaystyle {\tfrac {E_{b}(^{12}\mathrm {C} )}{m_{\rm {u}}c^{2}}}}$ (from the sum of the six ionization energies of carbon) is 1.1058674×10⁻⁶: A_r(¹²C⁶⁺) ≈ 11.9967087236367. 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) = 5.485799111(12)×10⁻⁴ for these data.

References