How Many Radial Nodes and Angular Nodes are Present in 4p Orbital

Introduction

The region around the nucleus of an element where the probability of finding an electron is zero are called nodes. In a graph where the atomic wave function (radial and angular wave function) passes through zero is considered a node.

These points in this graph where the line touches the x-axis refer to nodes.

There are two types of nodes.

1. Angular node

2. Radial node

Angular Node

As we know there are 7 shells present in p orbitals and p orbitals are of dumbbells shared. Angular nodes are plane (or cones)surfaces where we cannot find an electron means the probability of findings an electron is zero. Angular nodes are situated at fixed angles.

The Formula of Angular Node

Angular nodes can be calculated by using this formula:

The value of the angular node depends only on the azimuthal quantum number.

The number of angular nodes = l

Where l is the azimuthal quantum number and it defines the orbital angular momentum of the shell and also defines its shape

Radial Node

Radial nodes are spherical regions where we cannot find any electrons which means no electrons are zero in these radial node areas. These are situated at a fixed radius from the nucleus. So we can determine it radially. Radial nodes are there when the principal quantum number increases.

The Formula of Radial Node

Radial nodes can be calculated by using this formula:

Number of radial nodes = n-l-1, where

n is a principal quantum number(principal quantum number describes the position and energy of the electron in an atom)

l is the azimuthal quantum number.

So the total number of nodes is as follows:

= No angular nodes + No radial nodes

= l+n-l-1 = n

Angular and Radial Nodes Present in 4p Orbital

Angular nodes are related to azimuthal quantum numbers. So in 4p orbitals, the azimuthal quantum number(l) is 1.

As angular nodes are directly related to the azimuthal quantum number.

The Azimuthal Quantum Number for Various Orbitals

We can say that the angular node in 4p is 1

As we know the radial nodes are given by n-l-1

where l we already know that is 1

And n is the principal quantum number which is given that is 4

After putting the values in the formula we get,

Step1: = n-l-1

Step2: = 4-1-1

Step3: = 2

So no of a radial node in 4p is 2

The total no of nodes (angular and radial ) in 4p orbital is 2+1=3

Conclusion

Nodes are the areas where the probability of finding an electron is zero. Angular and radial are types of nodes.

The angular node of any orbital is given by l where l is the azimuthal quantum number

The radial node of any orbital is given by n-l-1

The total nodes of any orbital are given by n-1

The total number of nodes in the 4p orbital is 3.

The angular node in the 4p orbital is 1

The radial node in the 4p orbital is 2