Which set of quantum numbers correctly describes a 3p orbital?

• A. n = 3, l = 1, m_l = 0
• B. n = 3, l = 2, m_l = 1
• C. n = 3, l = 0, m_l = 0
• D. n = 2, l = 1, m_l = 0

Answer: (A)

Verified step by step guidance

1. Recall that the principal quantum number \(n\) indicates the energy level or shell of the electron. For a 3p orbital, \(n\) must be 3.
2. Understand that the azimuthal quantum number \(l\) defines the subshell or shape of the orbital: \(l = 0\) corresponds to an s orbital, \(l = 1\) to a p orbital, \(l = 2\) to a d orbital, and so on. Since we are dealing with a 3p orbital, \(l\) must be 1.
3. The magnetic quantum number \(m_l\) describes the orientation of the orbital in space and can take integer values from \(-l\) to \(+l\). For \(l = 1\), \(m_l\) can be \(-1\), \$0\(, or \)+1\(. Therefore, \)m_l = 0$ is a valid value for a 3p orbital.
4. Check each given set of quantum numbers against these rules: the correct set must have \(n = 3\), \(l = 1\), and \(m_l\) within the allowed range for \(l = 1\).
5. Conclude that the set \(n = 3\), \(l = 1\), \(m_l = 0\) correctly describes a 3p orbital because it satisfies all the quantum number conditions for that orbital.