Given 4p so n is 4 and l is 1 radial nodes = n-l-1 =4-1-1= 2
angular nodes = l = 1.
total 3 nodes

Introduction:
In chemistry, orbitals are the regions around the nucleus where electrons are most likely to be found. The 4p orbital is one of several orbitals in the fourth energy level of an atom. It is characterized by four sub-orbitals, each of which has a specific shape and orientation in space.

Explanation:
The total number of nodes present in 4p orbital can be determined by understanding the shape and orientation of the sub-orbitals. Each sub-orbital has a specific number of nodes, which are regions where the probability of finding an electron is zero. The number of nodes in each sub-orbital can be determined using the following formula:

Number of Nodes = n - l - 1

Where n is the principal quantum number (4 in this case) and l is the azimuthal quantum number (1 for p orbitals).

Sub-Orbitals in 4p Orbital:
The 4p orbital consists of four sub-orbitals, each of which has a different orientation in space. These sub-orbitals are designated as:

- 4px
- 4py
- 4pz
- 4pd

Number of Nodes in 4px, 4py, and 4pz Sub-Orbitals:
The 4px, 4py, and 4pz sub-orbitals are dumbbell-shaped and have one nodal plane that runs through the nucleus. Therefore, the number of nodes in each of these sub-orbitals is:

Number of Nodes = 4 - 1 - 1 = 2

Number of Nodes in 4pd Sub-Orbital:
The 4pd sub-orbital is more complex in shape, and has two nodal planes that run through the nucleus. Therefore, the number of nodes in this sub-orbital is:

Number of Nodes = 4 - 2 - 1 = 1

Total Number of Nodes in 4p Orbital:
To determine the total number of nodes in the 4p orbital, we simply add up the number of nodes in each sub-orbital:

Total Number of Nodes = (2 x 3) + 1 = 7

Therefore, the total number of nodes present in the 4p orbital is 7.