Ms

Definition

The magnetic quantum number, denoted as $m_s$, describes the spin orientation of an electron within an orbital. It can take one of two possible values: $+\frac{1}{2}$ or $-\frac{1}{2}$.

5 Must Know Facts For Your Next Test

1. $m_s$ indicates the direction of the electron's intrinsic spin.
2. The possible values for $m_s$ are always $+\frac{1}{2}$ and $-\frac{1}{2}$.
3. An electron with $m_s = +\frac{1}{2}$ is said to have 'spin up,' while one with $m_s = -\frac{1}{2}$ has 'spin down.'
4. $m_s$ is crucial for determining the electron configuration and behavior in a magnetic field.
5. Pauli Exclusion Principle states that no two electrons in the same atom can have identical sets of quantum numbers, including $m_s$.

Review Questions

• What are the possible values for the magnetic quantum number $m_s$?
• How does the value of $m_s$ relate to an electron's spin orientation?
• Why is the magnetic quantum number $m_s$ important in determining electron configurations?

Related terms

$n$ (Principal Quantum Number): Defines the main energy level occupied by an electron in an atom and determines its relative distance from the nucleus.

$l$ (Azimuthal Quantum Number): Describes the shape of the orbital and subshell where an electron is located, ranging from 0 to $(n-1)$.

$m_l$ (Magnetic Quantum Number): Specifies the orientation of an orbital within a subshell, taking on integer values between $-l$ and $l$, inclusive.