For an electron in a 4p orbital, what are the possible values of the principal quantum number n and the magnetic quantum number ml?

• A. n = 4; ml = -2, -1, 0, +1, or +2
• B. n = 4; ml = -1, 0, or +1
• C. n = 4; ml = 0 only
• D. n = 3; ml = -1, 0, or +1

Answer: (B)

Verified step by step guidance

1. Identify the principal quantum number \(n\) for the electron. Since the electron is in a 4p orbital, the principal quantum number \(n\) is 4.
2. Determine the azimuthal (angular momentum) quantum number \(l\) for a p orbital. Recall that \(l\) corresponds to the type of orbital: \(l = 0\) for s, \(l = 1\) for p, \(l = 2\) for d, and \(l = 3\) for f. For a p orbital, \(l = 1\).
3. Find the possible values of the magnetic quantum number \(m_l\). The magnetic quantum number \(m_l\) can take integer values from \(-l\) to \(+l\), including zero. Since \(l = 1\), \(m_l\) can be \(-1\), \$0\(, or \)+1$.
4. Summarize the quantum numbers for the electron in the 4p orbital: \(n = 4\) and \(m_l = -1, 0, +1\).
5. Note that other options with incorrect \(n\) values or incorrect ranges for \(m_l\) do not match the quantum number rules for a 4p electron.