Written by the Fiveable Content Team • Last updated September 2025
Written by the Fiveable Content Team • Last updated September 2025
Definition
The magnetic quantum number ($m_l$) specifies the orientation of an orbital around the nucleus. It can take on integer values between $-l$ and $+l$, where $l$ is the azimuthal quantum number.
5 Must Know Facts For Your Next Test
$m_l$ determines the number of orbitals and their orientation within a subshell.
For a given subshell with azimuthal quantum number $l$, $m_l$ can have $(2l + 1)$ possible values.
$m_l$ values range from $-l$ to $+l$, including zero.
$m_l$ is crucial for understanding the splitting of spectral lines in a magnetic field, known as the Zeeman effect.
The total number of orbitals in an energy level is given by $n^2$, where $n$ is the principal quantum number.
Denoted by $n$, it indicates the main energy level occupied by an electron and determines its average distance from the nucleus.
Azimuthal Quantum Number: Denoted by $l$, it defines the shape of an orbital and can have integer values from $0$ to $(n-1)$.
Zeeman Effect: A phenomenon where spectral lines are split into multiple components in the presence of a magnetic field due to interactions involving different orientations of orbitals.