How many orbitals are present in a subshell when the angular momentum quantum number l = 2?

• A. 3
• B. 7
• C. 2
• D. 5

Answer: (D)

Verified step by step guidance

1. Recall that the angular momentum quantum number \( l \) defines the subshell type: \( l = 0 \) is s, \( l = 1 \) is p, \( l = 2 \) is d, and so on.
2. The number of orbitals in a subshell is given by the formula \( 2l + 1 \), where \( l \) is the angular momentum quantum number.
3. Substitute \( l = 2 \) into the formula: \( 2(2) + 1 \).
4. Calculate the expression to find the number of orbitals in the subshell.
5. Interpret the result as the total number of orbitals present when \( l = 2 \).