Which of the following orbitals has `//` have zero `-` probability of finding the electron in xy plane ?

Options

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

Explanation

To determine which orbital has zero probability of finding the electron in the xy-plane, we need to analyze the characteristics of different orbitals. Let's go through the steps:

### Step 1: Understand the Orbital Types
- Orbitals are regions in space where there is a high probability of finding an electron. The common types of orbitals are s, p, d, and f.
- The s orbital is spherical and has a non-zero probability in all planes, including the xy-plane.
- The p orbitals (px, py, pz) have specific orientations in space.

### Step 2: Analyze the p Orbitals
- The p orbitals can be visualized as having two lobes on either side of the nucleus along a specific axis:
- **px**: oriented along the x-axis (has non-zero probability in the xy-plane).
- **py**: oriented along the y-axis (has non-zero probability in the xy-plane).
- **pz**: oriented along the z-axis (does not extend into the xy-plane).

### Step 3: Identify the Orbital with Zero Probability in the xy-plane
- Since the pz orbital is aligned with the z-axis, it does not have any electron density in the xy-plane. Therefore, the probability of finding an electron in the xy-plane for the pz orbital is zero.

### Conclusion:
The orbital that has zero probability of finding the electron in the xy-plane is the **pz orbital**.

### Summary:
- The answer is **pz orbital** because it is oriented along the z-axis and does not extend into the xy-plane.

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