Multiple Choice
What is the only possible value of the magnetic quantum number, m_l, for an electron in an s orbital?
9. Quantum Mechanics
Quantum Numbers: Magnetic Quantum Number
Multiple Choice
How many possible values of the magnetic quantum number, m_l, are allowed for an electron in a 2s subshell?
A
2
B
3
C
0
D
1
Verified step by step guidance1
Recall that the magnetic quantum number \(m_l\) depends on the azimuthal quantum number \(l\), which defines the subshell type (s, p, d, f, etc.).
Identify the value of \(l\) for the 2s subshell. Since it is an s subshell, \(l = 0\).
Use the rule that \(m_l\) can take integer values from \(-l\) to \(+l\), including zero. So, \(m_l = -l, -(l-1), ..., 0, ..., (l-1), l\).
For \(l = 0\), the only possible value of \(m_l\) is 0, meaning there is exactly one allowed value.
Therefore, the number of possible \(m_l\) values for an electron in the 2s subshell is 1.
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