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

Options

A. `p_(x)`
B. `p_(y)`
C. `p_(z)`
D. `d_(yz)`

Explanation

To determine which orbital has zero probability of finding an electron in the yz plane, we need to analyze the characteristics of different orbitals.

### Step-by-Step Solution:

1. **Understanding the yz Plane**:
- The yz plane consists of the y-axis and z-axis. Therefore, any orbital that has a component along the x-axis will not have any probability of finding an electron in the yz plane.

2. **Identifying Orbitals**:
- Common orbitals include:
- **s orbital**: spherically symmetric, has probability in all directions including the yz plane.
- **p orbitals**: There are three p orbitals: px, py, and pz.
- **px orbital**: Has a lobe along the x-axis and thus has zero probability in the yz plane.
- **py orbital**: Has a lobe along the y-axis, so it has a probability in the yz plane.
- **pz orbital**: Has a lobe along the z-axis, so it also has a probability in the yz plane.
- **d orbitals**: There are five d orbitals, but for this question, we focus on the p orbitals.

3. **Conclusion**:
- The only orbital that has zero probability of finding an electron in the yz plane is the **px orbital**. This is because it is oriented along the x-axis and does not extend into the yz plane.

### Final Answer:
The orbital that will have zero probability of finding the electron in the yz plane is the **px orbital**.