For an electron in an orbital with an angular momentum quantum number l = 2, which of the following lists all possible values of the magnetic quantum number m_l?

• A. -2, -1, 0, +1, +2
• B. -1, 0, +1, +2
• C. -2, -1, 0, +1
• D. 0, +1, +2

Answer: (A)

Verified step by step guidance

1. Recall that the magnetic quantum number \(m_l\) depends on the angular momentum quantum number \(l\) and can take integer values ranging from \(-l\) to \(+l\), including zero.
2. Given \(l = 2\), list all integers starting from \(-2\) up to \(+2\): \(-2, -1, 0, +1, +2\).
3. Understand that these values represent the possible orientations of the orbital angular momentum in space relative to an external magnetic field.
4. Verify that no values outside this range are allowed for \(m_l\) when \(l = 2\).
5. Conclude that the complete set of possible \(m_l\) values for \(l = 2\) is \(-2, -1, 0, +1, +2\).