For an `4p_y` orbital, there are nodal plane……… and azimuthal quantum number l……

Options

A. (a) 1,0
B. (b) 0,1
C. (c) 1,1
D. (d) 2,1

Answer

To solve the question regarding the `4p_y` orbital, we will break it down into two parts: identifying the nodal plane and determining the azimuthal quantum number \( l \).

### Step-by-Step Solution:

1. **Identify the Orbital Type**:
- The given orbital is `4p_y`. The notation indicates that it is a p-orbital with a principal quantum number \( n = 4 \).

2. **Determine the Nodal Plane**:
- A nodal plane is defined as a region in space where the probability of finding an electron is zero. For p-orbitals, there is one nodal plane.
- In the case of the `p_y` orbital, the electron density is concentrated in the y-direction, and the nodal plane will be perpendicular to this direction.
- Therefore, for the `4p_y` orbital, the nodal plane is the XZ plane. This means there is no electron density in this plane.

3. **Determine the Azimuthal Quantum Number \( l \)**:
- The azimuthal quantum number \( l \) determines the shape of the orbital. The values of \( l \) can range from \( 0 \) to \( n-1 \).
- For \( n = 4 \), the possible values for \( l \) are \( 0, 1, 2, 3 \).
- The values correspond to the following subshells:
- \( l = 0 \) for s-orbitals
- \( l = 1 \) for p-orbitals
- \( l = 2 \) for d-orbitals
- \( l = 3 \) for f-orbitals
- Since we are dealing with a p-orbital, the azimuthal quantum number \( l \) is \( 1 \).

### Final Answer:
- The nodal plane for the `4p_y` orbital is the XZ plane (1 nodal plane).
- The azimuthal quantum number \( l \) for the `4p_y` orbital is \( 1 \).

### Summary:
- Nodal Plane: 1 (XZ plane)
- Azimuthal Quantum Number \( l \): 1

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