The electron present in `3d_(z^(2))` orbital can not be found :

Options

A. in `xy` plane
B. in `xz` plane
C. in `yz` plane
D. None of these

Explanation

To solve the question regarding the electron present in the `3d_(z^2)` orbital and where it cannot be found, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the `3d_(z^2)` Orbital**:
- The `3d_(z^2)` orbital is one of the five d-orbitals. It has a distinct shape characterized by a "doughnut" or torus around the z-axis and a lobe extending along the z-axis.

2. **Visualizing the Orbital**:
- The `3d_(z^2)` orbital can be visualized in three-dimensional space. It has lobes that extend along the z-axis and a toroidal shape around the xy-plane.

3. **Identifying Planes**:
- We need to consider the three principal planes: the xy-plane, the xz-plane, and the yz-plane.
- The probability density of finding an electron in these planes can be analyzed based on the shape of the orbital.

4. **Analyzing Electron Probability**:
- In the xz-plane, the `3d_(z^2)` orbital has no lobes. This means that the probability of finding an electron in this plane is zero.
- In the xy-plane, the toroidal part of the orbital is present, indicating a higher probability of finding an electron.
- In the yz-plane, similar to the xz-plane, the lobes do not extend into this plane, but the toroidal shape does contribute to some probability.

5. **Conclusion**:
- Since the `3d_(z^2)` orbital has zero probability of finding an electron in the xz-plane, we conclude that the electron cannot be found in this plane.

### Final Answer:
The electron present in the `3d_(z^2)` orbital cannot be found in the **xz-plane**.

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