Question

how many orbitals in the n = 3 energy level? 25 16 9 4 1

Explanation:

Step1: Determine possible subshells for n=3

For principal quantum number \( n = 3 \), the azimuthal quantum number \( l \) can be 0, 1, 2 (since \( l = 0 \) to \( n-1 \)).

Step2: Calculate orbitals per subshell

• \( l=0 \) (s-subshell): number of orbitals = \( 2l+1 = 1 \)
• \( l=1 \) (p-subshell): number of orbitals = \( 2l+1 = 3 \)
• \( l=2 \) (d-subshell): number of orbitals = \( 2l+1 = 5 \)

Step3: Sum total orbitals

Total orbitals = \( 1 + 3 + 5 = 9 \)

Answer:

9