For an orbital with angular momentum quantum number l = 2, which of the following lists correctly represents all possible values of the magnetic quantum number ml?

• A. -2, -1, 0, +1, +2
• B. 0, +1, +2
• C. -2, -1, 0, +1
• D. -1, 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 integer values starting from \(-2\) up to \(+2\): \(-2, -1, 0, +1, +2\).
3. Verify that the total number of \(m_l\) values is \$2l + 1\(, which for \)l=2\( equals \)5$ values, matching the list above.
4. Check each provided option to see which one contains all these values without omission or addition.
5. Conclude that the correct list of \(m_l\) values for \(l=2\) is \(-2, -1, 0, +1, +2\).