Which type of orbital is occupied by an electron with principal quantum number n = 3 and angular momentum quantum number l = 2?

• A. 3s orbital
• B. 2d orbital
• C. 3d orbital
• D. 3p orbital

Answer: (C)

Verified step by step guidance

1. Recall that the principal quantum number \(n\) indicates the main energy level or shell of the electron. Here, \(n = 3\) means the electron is in the third energy level.
2. The angular momentum quantum number \(l\) determines the shape of the orbital and corresponds to the subshell type. The values of \(l\) range from \$0\( to \)n-1$.
3. Each value of \(l\) corresponds to a specific type of orbital: \(l = 0\) is an \(s\) orbital, \(l = 1\) is a \(p\) orbital, \(l = 2\) is a \(d\) orbital, and \(l = 3\) is an \(f\) orbital.
4. Since \(l = 2\) in this problem, the electron occupies a \(d\) orbital.
5. Combine the principal quantum number \(n = 3\) with the orbital type \(d\) to identify the orbital as a \$3d$ orbital.