The maximum number of electrons that can be accomoddated in `d_(x^(2)-y^(2))` orbital is

Options

A. 10
B. 5
C. 2
D. 1

Answer

To solve the question regarding the maximum number of electrons that can be accommodated in the \(d_{x^2 - y^2}\) orbital, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Orbitals**:
- The \(d\) subshell consists of five different orbitals: \(d_{xy}\), \(d_{xz}\), \(d_{yz}\), \(d_{x^2 - y^2}\), and \(d_{z^2}\).

**Hint**: Remember that each type of subshell has a specific number of orbitals: \(s\) has 1, \(p\) has 3, \(d\) has 5, and \(f\) has 7.

2. **Capacity of an Orbital**:
- Each orbital can hold a maximum of 2 electrons. This is due to the Pauli Exclusion Principle, which states that no two electrons in an atom can have the same set of quantum numbers. Therefore, two electrons in the same orbital must have opposite spins.

**Hint**: Recall the Pauli Exclusion Principle when considering how many electrons can fit in a single orbital.

3. **Identifying the Specific Orbital**:
- The question specifically asks about the \(d_{x^2 - y^2}\) orbital. Since it is one of the five \(d\) orbitals, it follows the same rule regarding electron capacity.

**Hint**: Focus on the fact that the question is asking about one specific orbital, not the entire subshell.

4. **Calculating the Maximum Number of Electrons**:
- Since the \(d_{x^2 - y^2}\) is one orbital, it can hold a maximum of 2 electrons.

**Hint**: Think about how many electrons can fit in one orbital based on the rules of quantum mechanics.

5. **Conclusion**:
- Therefore, the maximum number of electrons that can be accommodated in the \(d_{x^2 - y^2}\) orbital is **2**.

### Final Answer:
The maximum number of electrons that can be accommodated in the \(d_{x^2 - y^2}\) orbital is **2**.