Question

Calculate the total number of angular nodes and radial nodes present in $3p$ orbital.

Answer 1

To calculate the number of angular nodes and the radial nodes present in $3p$ orbital, first we should know that the azimuthal quantum number is the angular nodes of any orbital, with the help of angular nodes, we can find the radial nodes.

Complete step by step answer:
For $3p$ orbital:
here, $n = 3$
Number of angular node (azimuthal quantum number) $l = 1$
So, number of radial nodes $= n - l - 1 = 3 - 1 - 1 = 3 - 2 = 1$
Therefore, total number of nodes $= n - 1 = 3 - 1 = 2$
A nuclear orbital or electronic orbital is the district of a particle where an electron can be found with the most noteworthy likelihood. A molecule contains protons and neutrons at the focal point of the iota, which is known as the core. There are no electrons in the core. Electrons are scattered around the core. Be that as it may, these electrons are in development around the core in explicit ways known as electron orbitals or electron shells. These electron shells are made out of subshells. Contingent upon the precise energy quantum number, a subshell contains at least one orbitals: s orbital, p orbital, d orbital, and f orbital. These orbitals can be in various planes. Each orbital in a specific plane is known as a flap. Electrons are found inside these flaps. In any case, there are planes where no electrons can be found. These are called hubs. There are two kinds of hubs as outspread hubs and rakish hubs. The principle distinction between spiral hubs and rakish hubs is that outspread hubs are round though precise hubs are normally level planes.

Note: The 3d orbital has two angular nodes, and therefore no radial nodes! 2. The difference between radial and angular nodes Radial nodes are nodes inside the orbital lobes as far as I can understand.