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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 ...
The electron's mass is approximately 1 / 1836 that of the proton. [15] Quantum mechanical properties of the electron include an intrinsic angular momentum of a half-integer value, expressed in units of the reduced Planck constant, ħ. Being fermions, no two electrons can occupy the same quantum state, per the Pauli exclusion principle. [14]
The CODATA recommended value is −e/m e = −1.758 820 008 38 (55) × 10 11 C⋅kg −1. [2] CODATA refers to this as the electron charge-to-mass quotient, but ratio is still commonly used. There are two other common ways of measuring the charge-to-mass ratio of an electron, apart from Thomson and Dunnington's methods.
From this information, one can deduce the mass (m) of a single atom; and since the molar mass (M) is known, the number of atoms in a mole can be calculated: N A = M/m. The value of F can be measured directly using Faraday's laws of electrolysis.
For example, an electron and a positron, each with a mass of 0.511 MeV/c 2, can annihilate to yield 1.022 MeV of energy. A proton has a mass of 0.938 GeV/c 2. In general, the masses of all hadrons are of the order of 1 GeV/c 2, which makes the GeV/c 2 a convenient unit of mass for particle physics: [4]
A closely related system is the International System of Electric and Magnetic Units, [18] which has a different unit of mass so that the formula for 𝜆′ is invalid. The unit of mass was chosen to remove powers of ten from contexts in which they were considered to be objectionable (e.g., P = VI and F = qE). Inevitably, the powers of ten ...
The relative isotopic mass (see section below) can be obtained by dividing the atomic mass m a of an isotope by the atomic mass constant m u yielding a dimensionless value. Thus, the atomic mass of a carbon-12 atom is 12 Da by definition, but the relative isotopic mass of a carbon-12 atom is simply 12.
In general, however, the value of effective mass depends on the purpose for which it is used, and can vary depending on a number of factors. For electrons or electron holes in a solid, the effective mass is usually stated as a factor multiplying the rest mass of an electron, m e (9.11 × 10 −31 kg).