The number of nodal planes in a `p_(x)` orbital is :

Options

A. one
B. two
C. three
D. four

Explanation

To determine the number of nodal planes in a \( p_x \) orbital, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Concept of Nodal Planes**:
Nodal planes are regions in an atomic orbital where the probability of finding an electron is zero. For p-orbitals, which have a specific shape, these planes are significant.

**Hint**: Remember that nodal planes are areas where the electron density is zero.

2. **Identify the Shape of p-Orbitals**:
The p-orbitals (including \( p_x \), \( p_y \), and \( p_z \)) have a dumbbell shape. Each p-orbital consists of two lobes on either side of the nucleus, with a nodal plane between them.

**Hint**: Visualize the shape of p-orbitals to understand where the nodal planes are located.

3. **Determine the Number of Nodal Planes**:
Each p-orbital has one nodal plane. For the \( p_x \) orbital specifically, the nodal plane is the plane that passes through the nucleus and is perpendicular to the direction of the lobes (which in this case is along the x-axis).

**Hint**: Recall that for each type of p-orbital (i.e., \( p_x \), \( p_y \), \( p_z \)), there is one distinct nodal plane.

4. **Conclusion**:
Since the \( p_x \) orbital has one nodal plane, the answer to the question is:

**Answer**: 1

### Summary of the Solution:
The number of nodal planes in a \( p_x \) orbital is 1, as it has one plane where the probability of finding an electron is zero.