A subshell with n=6 , l= 2 can accommodate a maximum of

Options

A. 12 electron
B. 36 electron
C. 10 electron
D. 72 electron

Answer

To determine the maximum number of electrons that a subshell can accommodate, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Principal Quantum Number (n)**:
The principal quantum number (n) indicates the energy level of the electron. In this case, n = 6.

2. **Identify the Azimuthal Quantum Number (l)**:
The azimuthal quantum number (l) defines the shape of the orbital. Here, l = 2 corresponds to the d subshell.

3. **Determine the Number of Orbitals in the Subshell**:
The number of orbitals in a subshell can be calculated using the formula (2l + 1). For l = 2:
\[ \text{Number of orbitals} = 2(2) + 1 = 5 \]

4. **Calculate the Maximum Number of Electrons**:
Each orbital can hold a maximum of 2 electrons. Therefore, the maximum number of electrons that can be accommodated in the d subshell is:
\[ \text{Maximum electrons} = \text{Number of orbitals} \times 2 = 5 \times 2 = 10 \]

5. **Conclusion**:
A subshell with n = 6 and l = 2 can accommodate a maximum of 10 electrons.

### Final Answer:
The maximum number of electrons that a subshell with n = 6 and l = 2 can accommodate is **10**.