# Magnetic quantum number

The magnetic quantum number (symbol ml) is one of four quantum numbers in atomic physics. The set is: principal quantum number, azimuthal quantum number, magnetic quantum number, and spin quantum number. Together, they describe the unique quantum state of an electron; the magnetic quantum number distinguishes the orbitals available within a subshell, and is used to calculate the azimuthal component of the orientation of orbital in space. Electrons in a particular subshell (such as s, p, d, or f) are defined by values of (0, 1, 2, or 3); the value of ml can range from - to +, inclusive of zero. Thus the s, p, d, and f subshells contain 1, 3, 5, and 7 orbitals each, with values of m within the ranges 0, ±1, ±2, ±3 respectively; each of these orbitals can accommodate up to two electrons (with opposite spins), forming the basis of the periodic table.

## Derivation These orbitals have magnetic quantum numbers $m=-\ell ,\ldots ,\ell$ from left to right in ascending order. The $e^{mi\phi }$ dependence of the azimuthal component can be seen as a color gradient repeating m times around the vertical axis.

There is a set of quantum numbers associated with the energy states of the atom; the four quantum numbers $n$ , $\ell$ , $m_{l}$ , and $s$ [dubious ] specify the complete and unique quantum state of a single electron in an atom called its wavefunction or orbital. The Schrödinger equation for the wavefunction of an atom with one electron is a separable partial differential equation. (This is not the case for the helium atom or other atoms with mutually interacting electrons, which require more sophisticated methods for solution) This means that the wavefunction as expressed in spherical coordinates can be broken down into the product of three functions of the radius, colatitude (or polar) angle, and azimuth:

$\psi (r,\theta ,\phi )=R(r)P(\theta )F(\phi )$ The differential equation for $F$ can be solved in the form $F(\phi )=Ae^{\lambda \phi }$ . Because values of the azimuth angle $\phi$ differing by 2$\pi$ (360 degrees in radians) represent the same position in space, and the overall magnitude of $F$ does not grow with arbitrarily large $\phi$ as it would for a real exponent, the coefficient $\lambda$ must be quantized to integer multiples of $i$ , producing an imaginary exponent: $\lambda =im_{l}$ . These integers are the magnetic quantum numbers; the same constant appears in the colatitude equation, where larger values of $m_{l}$ 2 tend to decrease the magnitude of $P(\theta )$ , and values of $m_{l}$ greater than the azimuthal quantum number $\ell$ do not permit any solution for $P(\theta )$ .

Relationship between Quantum Numbers
Orbital Values Number of Values for $m$ Electrons per subshell
s $\ell =0,\quad m_{l}=0$ 1 2
p $\ell =1,\quad m_{l}=-1,0,+1$ 3 6
d $\ell =2,\quad m_{l}=-2,-1,0,+1,+2$ 5 10
f $\ell =3,\quad m_{l}=-3,-2,-1,0,+1,+2,+3$ 7 14
g $\ell =4,\quad m_{l}=-4,-3,-2,-1,0,+1,+2,+3,+4$ 9 18

## As a component of angular momentum Illustration of quantum mechanical orbital angular momentum. The cones and plane represent possible orientations of the angular momentum vector for $\ell =2$ and $m=-2,-1,0,1,2$ . Even for the extreme values of $m$ , the z component of this vector is less than its total magnitude.

The axis used for the polar coordinates in this analysis is chosen arbitrarily; the quantum number m refers to the projection of the angular momentum in this arbitrarily-chosen direction, conventionally called the z direction or quantization axis. Lz, the magnitude of the angular momentum in the z direction, is given by the formula:

$L_{z}=m_{l}\hbar .$ This is a component of the atomic electron's total orbital angular momentum, $\mathbf {L}$ , whose magnitude is related to the azimuthal quantum number of its subshell $\ell$ by the equation:

$L=\hbar {\sqrt {\ell (\ell +1)}}$ where $\hbar$ is the reduced Planck constant. Note this $L=0$ for $\ell =0$ and approximates $L=(\ell +0.5)\hbar$ for high $\ell$ . It is not possible to measure the angular momentum of the electron in all three axes simultaneously; these properties were first demonstrated in the Stern-Gerlach experiment, by Otto Stern and Walther Gerlach.

The energy of any wave is its frequency multiplied by Planck's constant; the wave displays particle-like packets of energy called quanta. The formula for the quantum number of each quantum state uses Planck's reduced constant, which only allows particular or discrete or quantized energy levels.

## Effect in magnetic fields

The quantum number $m$ refers, loosely, to the direction of the angular momentum vector. The magnetic quantum number $m$ only affects the electron's energy if it is in a magnetic field because in the absence of one, all spherical harmonics corresponding to the different arbitrary values of $m$ are equivalent. The magnetic quantum number determines the energy shift of an atomic orbital due to an external magnetic field (the Zeeman effect) — hence the name magnetic quantum number. However, the actual magnetic dipole moment of an electron in an atomic orbital arrives not only from the electron angular momentum, but also from the electron spin, expressed in the spin quantum number.

Since each electron has a magnetic moment in a magnetic field, it will be subject to a torque which tends to make the vector $\mathbf {L}$ parallel to the field, a phenomenon known as Larmor precession.