Question

explain quantum numbers give the importance of quantum numbers in paulus Paul's exclusion principal​

Answer 1

$\huge{\mathcal{\purple{A}\green{N}\pink{S}\blue{W}\purple{E}\green{R}\pink{!}}}$

The Pauli exclusion principle states that an electron in a atom cam be described by a unique set of quantum numbers. This means that in an atom with more than one electron, no two electrons can have the same set of 4 quantum numbers.

Answer 2

Answer:

There are four quantum numbers they are;

• Principal quantum number (n)

It provides the size of the orbit.

It gives energy of electron in an orbit.

It gives average distance between electron & nucleus.

It gives the cell in which the electron is placed.

• Azimuthal or Subsidiary quantum number (l)

It give the shape of the orbit.

It gives the subshell in which the electron is located.

It gives the orbital angular momentum of the electron.

• Magnetic quantum number (m or ml)

It give the orientation of orbitals in space.

• Spin quantum number (s or ms)

It gives the spin orientation of the electron.

It may be either clockwise or anticlockwise

Explanation:

Pauli's exclusion principle states that, no two electrons in an atom can have the same set of four quantum numbers.