# Quantum numbers: what are they for and what are they

We explain that what are quantum numbers: what are they for and what are they. The **nÂ ****UMBERS quantum** used to describe the quantum state of electrons in the atom and originate in the solution of the SchrÃ¶dinger equation for the simplest of all the hydrogen. what are quantum numbers

The SchrÃ¶dinger equation is a differential equation, the solutions of which areÂ *wave functions*Â and are denoted by the Greek letter Ïˆ.Â Infinite solutions can be proposed, and their square is equal to the probability of finding the electron in a small region of space, called theÂ *orbital*. what are quantum numbers

Each orbital has definite characteristics that distinguish it from the others, such as energy, angular momentum and spin, an entirely quantum property of the electron and which is responsible, among other things, for magnetic effects.

The way to identify each orbital is to distinguish it by a set of numbers that describe it, and these are precisely the quantum numbers: what are quantum numbers

-n: is the principal quantum number.

-â„“: the azimuthal quantum number.

-mÂ _{â„“}Â , is the magnetic number.

-mÂ _{s} , the number of spin.

**What are quantum numbers for?**

Quantum numbers are used to describe the state of the electrons inside the atom. That atomic model in which the electron goes around the nucleus is inaccurate, because it is not consistent with atomic stability or with a large number of observed physical phenomena. what are quantum numbers

That is why the Danish Niels Bohr (1885-1962) made an audacious proposal in 1913: the electron can only be found in certain stable orbits, the size of which depends on an integer called n.

Later, in 1925, the also Austrian physicist Erwin SchrÃ¶dinger (1887-1961) proposed a differential equation in partial derivatives, whose solutions describe the hydrogen atom.Â They are the wave functions Ïˆ mentioned at the beginning.

This differential equation includes the three spatial coordinates plus time, but when this is not included, the solution of the SchrÃ¶dinger equation is analogous to that of a standing wave (a wave that propagates between certain limits).

**Wave functions what are quantum numbers**

The time-independent SchrÃ¶dinger equation is solved in spherical coordinates and the solution is written as the product of three functions, one for each spatial variable.Â In this coordinate system, instead of using the coordinates of the Cartesian axesÂ *x*Â ,Â *y*Â andÂ *z*Â , the coordinatesÂ *r*Â ,Â *Î¸*Â andÂ *Ï† are used*Â .Â In this way:

Ïˆ (r, Î¸, Ï†) = R (r) â‹…f (Î¸) â‹…g (Ï†)

The wave function is intangible, however quantum mechanics tells us that the squared amplitude:

| Ïˆ (r, Î¸, Ï†) |Â ^{two}

That is, the module or absolute value of the wave function, squared, is a real number that represents the probability of finding the electron, in a certain region around the point whose coordinates areÂ *r*Â ,Â *Î¸*Â andÂ *Ï†.*

And this fact is something more concrete and tangible.

To find the wave function, you have to solve three ordinary differential equations, one for each variableÂ *r*Â ,Â *Î¸,*Â andÂ *Ï†*Â .

The solutions of each equation, which will be the functions R (r), f (Î¸) and g (Ï†), contain the first three quantum numbers mentioned. what are quantum numbers

**What are the quantum numbers?**

We briefly describe the nature of each quantum number below.Â The first three, as previously stated, arise from the solutions of the SchrÃ¶dinger equation.

The fourth issue was added by Paul Dirac (1902 – 1984) in 1928.

**Principal quantum number**

It is denoted byÂ *n*Â and indicates the size of the allowed orbital, as well as the energy of the electron.Â The higher its value, the further the electron is from the nucleus and its energy will also be higher, but in return it reduces its stability.

This number arises from the function R (r), which is the probability of finding the electron at a certain distanceÂ *r* from the nucleus, which is determined by: what are quantum numbers

-Planck constantÂ : h = 6.626 Ã— 10Â Â ^{-34}Â JsÂ -Mass of the electron mÂ _{e}Â = 9.1 Ã— 10Â ^{-31}Â kg

-Charge of the electron: e = 1.6 Ã— 10Â ^{-19}Â C.Â -Electrostatic constant

: k = 9 Ã— 10Â ^{9}Â NmÂ ^{2}Â / CÂ ^{2}

When n = 1 it corresponds to the Bohr radius which is approximately 5.3 Ã— 10Â ^{âˆ’11}Â m.

Except for the first layer, the others are subdivided into sub-layers or sublevels.Â Each shell has an energy in electron volt given by:

- K (n = 1)
- L (n = 2)
- M (n = 3)
- N (n = 4)
- O (n = 5)
- P (n = 6)
- Q (n = 7).

In theory there is no upper limit for n, but in practice it is observed that it only reaches n = 8. The lowest possible energy corresponds to n = 1 and is that ofÂ Â *the ground state*Â .

**Azimuthal or angular momentum quantum number what are quantum numbers**

Denoted by the italicized letter â„“, this number determines the shape of the orbitals, by quantifying the magnitude of the orbital angular momentum of the electron.

It can take positive integer values â€‹â€‹between 0 and n â€“ 1, for example:

-When n = 1, then â„“ = 0 and there is only one sublevel.

-If n = 2, then â„“ can be equal to 0 or 1, so there are two sublevels.

-And if n = 3, then â„“ assumes the values â€‹â€‹0, 1 and 2 and there are 3 sublevels.

It can be continued in this way indefinitely, although as said before, in practice n goes up to 8. The sublevels are denoted by the letters:Â *s*Â ,Â *p*Â ,Â *d*Â ,Â *f*Â andÂ *g*Â and they increase in energy.

**Magnetic quantum number mÂ **_{â„“}

_{â„“}

This number decides the orientation of the orbital in space and its value depends on that of â„“.

For a given â„“, there are (2â„“ + 1) integer values â€‹â€‹of mÂ _{â„“}Â , which correspond to the respective orbitals.Â These are:

-â„“, (- â„“ + 1),â€¦ 0,â€¦ (+ â„“ -1), + â„“.

**Example**

If n = 2, we know that â„“ = 0 and â„“ = 1, then mÂ _{â„“} takes the following values: what are quantum numbers

-For â„“ = 0: mÂ _{â„“}Â = 0.

-For â„“ = 1: mÂ _{â„“}Â = -1, mÂ _{â„“}Â = 0, mÂ _{â„“}Â = +1

The n = 2 orbital has two sublevels, the first with n = 2, â„“ = 0 and mÂ _{â„“}Â = 0. Then we have the second sublevel: n = 2, â„“ = 1, with 3 orbitals:

- n = 2, â„“ = 1, mÂ
_{â„“}Â = -1 - n = 2, â„“ = 1, mÂ
_{â„“}Â = 0 - n = 2, â„“ = 1, mÂ
_{â„“}Â = +1

All three orbitals have the same energy but different spatial orientation.

**Spin quantum number mÂ **_{s}

_{s}

When solving the SchrÃ¶dinger equation in three dimensions, the numbers already described emerge.Â However, in hydrogen there is an even finer structure that these numbers are not enough to explain.

Therefore, in 1921 another physical, Wolfgang Pauli, proposed the existence of a fourth number: the number of spin mÂ _{s}Â , taking values of + Â½ and -Â½.

This number describes a very important property of the electron, which is theÂ *spin*Â , a word that comes from the EnglishÂ Â *spin* (to rotate on itself).Â And the spin in turn is related to the magnetic properties of the atom. what are quantum numbers

One way to understand spin is by imagining that the electron behaves like a tiny magnetic dipole (a magnet with north and south poles), thanks to a rotation around its own axis.Â The rotation can be in the same direction as clockwise, or in the opposite direction.

Although Pauli suggested the existence of this number, the results of an experiment carried out by Otto Stern and Walter Gerlach in 1922 had already anticipated it. what are quantum numbers

These scientists managed to divide a bundle of silver atoms in two by applying a non-uniform magnetic field.

The value of mÂ _{s}Â does not depend on n, â„“ and mÂ _{â„“}Â .Â InÂ graphicÂ formÂ , it is represented by an arrow: an up arrow indicates a clockwise turn and a down arrow indicates a counterclockwise turn.

**Pauli Exclusion Principle**

The behavior of electrons in the atom is summarized in the Pauli exclusion principle, which states that two electrons in an atom cannot exist in the same quantum state.

Therefore, each electron must have a different set of quantum numbers n, â„“, mÂ _{â„“,}Â and mÂ _{s} . what are quantum numbers

The importance of quantum numbers and this principle lies in the understanding of the properties of the elements in the periodic table: electrons are organized in layers according to n, and then in sub-layers according to â„“ and the rest of the numbers.