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

Options

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

Answer

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 Orbitals**:
- Orbitals are regions in an atom where there is a high probability of finding electrons. The \( p \) orbitals are one type of orbital, which includes \( p_x \), \( p_y \), and \( p_z \).

2. **Identify the Quantum Numbers**:
- Each orbital is defined by a set of quantum numbers. The relevant quantum numbers for this question are:
- Principal quantum number (\( n \)): Indicates the energy level.
- Azimuthal quantum number (\( l \)): Indicates the shape of the orbital.

3. **Determine the Azimuthal Quantum Number for \( p \) Orbitals**:
- For \( p \) orbitals, the azimuthal quantum number \( l \) is equal to 1. This is a key point because it relates directly to the number of nodal planes.

4. **Relate Azimuthal Quantum Number to Nodal Planes**:
- The number of nodal planes in an orbital is given by the azimuthal quantum number \( l \). Specifically:
- For \( s \) orbitals (\( l = 0 \)): 0 nodal planes.
- For \( p \) orbitals (\( l = 1 \)): 1 nodal plane.
- For \( d \) orbitals (\( l = 2 \)): 2 nodal planes.

5. **Conclusion**:
- Since the \( p_x \) orbital is a \( p \) orbital, it has 1 nodal plane.

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

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