Which of the following correctly represents the subshell with principal quantum number n = 2 and angular momentum quantum number l = 1?

• A. 2p
• B. 2d
• C. 1p
• D. 1d

Answer: (A)

Verified step by step guidance

1. Recall that the principal quantum number \(n\) indicates the energy level or shell of an electron in an atom. Here, \(n = 2\) means we are looking at the second energy level.
2. Understand that the angular momentum quantum number \(l\) defines the subshell or shape of the orbital. The values of \(l\) range from \$0\( to \)n-1\(. For \)l = 0\(, the subshell is labeled as 's'; for \)l = 1\(, it is 'p'; for \)l = 2\(, it is 'd'; and for \)l = 3$, it is 'f'.
3. Since \(l = 1\), the subshell corresponds to the 'p' type orbitals.
4. Combine the principal quantum number \(n = 2\) with the subshell letter 'p' to write the correct notation for the subshell, which is \$2p$.
5. Verify that the other options are invalid because: \$2d\( is not possible since \)l\( cannot be 2 when \)n=2\( (because \)l\( must be less than \)n\(), and \)1p\( or \)1d\( are invalid because \)l=1\( or \)2\( cannot exist when \)n=1\( (since \)l\( must be less than \)n$).