# 5.12: Quantum Numbers

- Page ID
- 52971

If you attend a college or professional football game, you need a ticket to get in. It is very likely that your ticket may specify a gate number, a section number, a row, and a seat number. No other ticket can have the same four parts to it. It may have the same gate, section, and seat number, but it would have to be in a different row. Each seat is unique and allows only one occupant to fill it.

We use a series of specific numbers, called **quantum numbers**, to describe the location of an electron in an associated atom. Quantum numbers specify the properties of the atomic orbitals and the electrons in those orbitals. An electron in an atom or ion has four quantum numbers to describe its state. Think of them as important variables in an equation which describes the three-dimensional position of electrons in a given atom.

### Principal Quantum Number \(\left( n \right)\)

The **principal quantum number**, signified by \(n\), is the main energy level occupied by the electron. Energy levels are fixed distances from the nucleus of a given atom. They are described in whole number increments (e.g., 1, 2, 3, 4, 5, 6, ...). At location \(n=1\), an electron would be closest to the nucleus, while at \(n=2\) the electron would be farther, and at \(n=3\) farther yet. As we will see, the principal quantum number corresponds to the row number for an atom on the periodic table.

### Angular Momentum Quantum Number \(\left( l \right)\)

The **angular momentum quantum number**, signified by \(l\), describes the general shape or region an electron occupies - its orbital shape. The value of \(l\) depends on the value of the principal quantum number, \(n\). The angular momentum quantum number can have positive values of zero to \(\left( n-1 \right)\). If \(n=2\), \(l\) could be either \(0\) or \(1\).

### Magnetic Quantum Number \(\left( m_l \right)\)

The **magnetic quantum number**, signified as \(m_l\), describes the orbital orientation in space. Electrons can be situated in one of three planes in three dimensional space around a given nucleus (\(x\), \(y\), and \(z\)). For a given value of the angular momentum quantum number, \(l\), there can be \(\left( 2l+1 \right)\) values for \(m_l\). As an example:

\(n=2\)

\(l=0\) or \(1\)

for \(l=0\), \(m_l = 0\)

for \(l=1\), \(m_l = -1, 0, +1\)

Principal Energy Level |
Number of Possible Sublevels |
Possible Angular Momentum Quantum Numbers |
Orbital Designation by Principal Energy Level and Sublevel |
---|---|---|---|

\(n=1\) | 1 | \(l=0\) | \(1s\) |

\(n=2\) | 2 | \(l=0\) | \(2s\) |

\(l=1\) | \(2p\) | ||

\(n=3\) | 3 | \(l=0\) | \(3s\) |

\(l=1\) | \(3p\) | ||

\(l=2\) | \(3d\) | ||

\(n=4\) | 4 | \(l=0\) | \(4s\) |

\(l=1\) | \(4p\) | ||

\(l=2\) | \(4d\) | ||

\(l=3\) | \(4f\) |

The table above shows the possible angular momentum quantum number values \(\left( l \right)\) for the corresponding principal quantum numbers \(\left( n \right) of \(n = 1, n=2, n=3,\) and \(n=4\).

### Spin Quantum Number \(\left( m_s \right)\)

The **spin quantum number** describes the spin for a given electron. An electron can have one of two associated spins, \(\left( + \frac{1}{2} \right)\) spin, or \(\left( -\frac{1}{2} \right)\) spin. An electron cannot have zero spin. We also represent spin with arrows \(\uparrow\) or \(\downarrow\). A single orbital can hold a maximum of two electrons and each must have opposite spin.

### Summary

- Quantum numbers specify the arrangements of electrons in orbitals.
- There are four quantum numbers that provide information about various aspects of electron behavior.

### Contributors

CK-12 Foundation by Sharon Bewick, Richard Parsons, Therese Forsythe, Shonna Robinson, and Jean Dupon.