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

Options

A. one
B. Two
C. Three
D. Zero

Answer

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

### Step 1: Understand the concept of nodal planes
A nodal plane is defined as a plane where the probability of finding an electron is zero. In other words, it is a region where the electron density is absent.

**Hint:** Remember that nodal planes indicate areas of zero electron density.

### Step 2: Identify the characteristics of \( p \) orbitals
The \( p \) subshell consists of three orbitals: \( p_x \), \( p_y \), and \( p_z \). Each of these orbitals is oriented along one of the three axes in three-dimensional space.

**Hint:** Recall that \( p \) orbitals are oriented along the x, y, and z axes.

### Step 3: Analyze the \( p_x \) orbital
The \( p_x \) orbital is specifically oriented along the x-axis. This means it has a certain shape that extends along the x-axis and has regions of high electron density on either side of the nucleus.

**Hint:** Visualize the \( p_x \) orbital as a dumbbell shape centered on the x-axis.

### Step 4: Determine the nodal planes for \( p_x \)
For the \( p_x \) orbital, we can analyze the planes:
- The \( xy \) plane contains the x-axis.
- The \( xz \) plane also contains the x-axis.
- The \( yz \) plane does not contain the x-axis.

Since the \( p_x \) orbital has no electron density in the \( yz \) plane, this plane acts as a nodal plane.

**Hint:** Consider how the orientation of the orbital affects the presence of nodal planes.

### Step 5: Conclusion
Therefore, the \( p_x \) orbital has **one nodal plane**, which is the \( yz \) plane.

**Final Answer:** The number of nodal planes in a \( p_x \) orbital is **1**.