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The Weiss magneton was experimentally derived in 1911 as a unit of magnetic moment equal to 1.53 × 10 −24 joules per tesla, which is about 20% of the Bohr magneton. In the summer of 1913, the values for the natural units of atomic angular momentum and magnetic moment were obtained by the Danish physicist Niels Bohr as a consequence of his ...
The value of the electron magnetic moment (symbol μ e) is −9.284 764 6917 (29) × 10 −24 J⋅T −1. [1] In units of the Bohr magneton ( μ B ), it is −1.001 159 652 180 59 (13) μ B , [ 2 ] a value that was measured with a relative accuracy of 1.3 × 10 −13 .
The magnetic moment of the electron is =, where μ B is the Bohr magneton, S is electron spin, and the g-factor g S is 2 according to Dirac's theory, but due to quantum electrodynamic effects it is slightly larger in reality: 2.002 319 304 36.
The above classical relation does not hold, giving the wrong result by the absolute value of the electron's g-factor, which is denoted g e: = | | =, where μ B is the Bohr magneton. The gyromagnetic ratio due to electron spin is twice that due to the orbiting of an electron.
The spin magnetic moment of a charged, spin-1/2 particle that does not possess any internal structure (a Dirac particle) is given by [1] =, where μ is the spin magnetic moment of the particle, g is the g-factor of the particle, e is the elementary charge, m is the mass of the particle, and S is the spin angular momentum of the particle (with magnitude ħ/2 for Dirac particles).
The best available measurement for the value of the magnetic moment of the neutron is μ n = −1.913 042 76 (45) μ N. [3] [4] Here, μ N is the nuclear magneton, a standard unit for the magnetic moments of nuclear components, and μ B is the Bohr magneton, both being physical constants.
This is known as the Curie law and the proportionality constant, C, is known as the Curie constant, whose value, for molar susceptibility, is calculated as [11] = (+) where N is the Avogadro constant, g is the Landé g-factor, and μ B is the Bohr magneton.
The orbital magnetic quantum number takes integer values in the range from to +, including zero. [3] Thus the s, p, d, and f subshells contain 1, 3, 5, and 7 orbitals each. Each of these orbitals can accommodate up to two electrons (with opposite spins), forming the basis of the periodic table.