In the third energy level (n = 3), how many electrons can occupy the 3d subshell?

• A. 2
• B. 14
• C. 6
• D. 10

Answer: (D)

Verified step by step guidance

1. Recall that the principal quantum number \(n\) indicates the energy level, and the azimuthal quantum number \(l\) defines the subshell type: \(l = 0\) for s, \(l = 1\) for p, \(l = 2\) for d, and \(l = 3\) for f subshells.
2. Identify the subshell in question: the 3d subshell corresponds to \(n = 3\) and \(l = 2\).
3. Determine the number of orbitals in the 3d subshell using the formula: number of orbitals = \$2l + 1\(. For \)l = 2\(, this gives \)2 \times 2 + 1 = 5$ orbitals.
4. Recall that each orbital can hold a maximum of 2 electrons with opposite spins according to the Pauli exclusion principle.
5. Calculate the total number of electrons in the 3d subshell by multiplying the number of orbitals by 2: \$5 \times 2 = 10$ electrons.