Question

for n=2, total number of orbitals are a 3 b 2 c 1 d 4

Explanation:

Step1: Recall orbital rules

For a principal quantum number \( n \), the number of subshells is \( l = 0 \) to \( l = n - 1 \). For \( n = 2 \), \( l = 0 \) (s - subshell) and \( l = 1 \) (p - subshell).

Step2: Calculate orbitals per subshell

• For \( l = 0 \) (s - subshell), number of orbitals \( = 2l + 1 = 2(0)+1 = 1 \).
• For \( l = 1 \) (p - subshell), number of orbitals \( = 2(1)+1 = 3 \).

Step3: Total orbitals for \( n = 2 \)

Sum the orbitals of each subshell: \( 1 + 3 = 4 \).

Answer:

D. 4