Which of the following orbitals will have zero probability of finding the electron in the yz plane

Options

A. px
B. py
C. pz
D. dyz

Answer

To determine which orbital has zero probability of finding the electron in the yz plane, we need to analyze the characteristics of the different p orbitals: \( p_x \), \( p_y \), and \( p_z \).

### Step-by-Step Solution:

1. **Understanding Orbital Orientation**:
- The p orbitals are oriented along specific axes in three-dimensional space.
- The \( p_x \) orbital has lobes oriented along the x-axis, meaning that the electron density is concentrated along this axis.

2. **Analyzing the \( p_x \) Orbital**:
- For the \( p_x \) orbital, the lobes are located on the x-axis, and there is a node (zero probability) in the yz plane.
- Therefore, there is zero probability of finding an electron in the yz plane for the \( p_x \) orbital.

3. **Analyzing the \( p_y \) Orbital**:
- The \( p_y \) orbital has lobes oriented along the y-axis. This means that the electron density is present in the yz plane.
- Thus, there is a non-zero probability of finding an electron in the yz plane for the \( p_y \) orbital.

4. **Analyzing the \( p_z \) Orbital**:
- The \( p_z \) orbital has lobes oriented along the z-axis. This means that the electron density is also present in the yz plane.
- Therefore, there is a non-zero probability of finding an electron in the yz plane for the \( p_z \) orbital.

5. **Conclusion**:
- The only orbital that has zero probability of finding an electron in the yz plane is the \( p_x \) orbital.

### Final Answer:
The orbital with zero probability of finding the electron in the yz plane is the **\( p_x \) orbital**.

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