 # Quantum Numbers Class 11 Chemistry Notes

Do you Know !!

## What isQuantum Number ?

These are certain numbers which are used to locate electron in an atom or in other words these are address of electron. They are of four types out of which three are obtained by mathematical solution of Schrödinger wave equation.

# 4 Quantum Numbers

(i)   Principal Quantum Number (n):

It is obtained by mathematical solution of r-part of Schrödinger wave equation.

Its values are:

n = 1, 2, 3, ………..,∞

• It represents the shells or orbits or energy levels

When n = 1    It means 1st shell or K-shell

n = 2    It means 2nd shell or L-shell

n = 3    It means 3rd shell or M-shell

• It also indicates energy. Higher is the value of “n” more is the energy.
• It also indicates distance of electron from the nucleus. Higher is the value of “n” away is the electron from the nucleus.
• Numbers of electrons in a shell are calculated by it as 2n2.

(ii)  Azimuthal Quantum Number (ℓ):

It is obtained by mathematical solution of θ-part of Schrödinger wave equation. It is also called secondary quantum number. Its values are:

ℓ = 0, 1, 2, 3, ……….., n-1

• It represents the sub shells or  energy sub-levels

When ℓ = 0    It means s-sub shell (spherical shaped)

s    stands for sharp

ℓ = 1    It means p-sub shell

(dumbbell shaped)

p  stands for principal

ℓ = 2    It means d-sub shell

(sausage shaped)

d     stands for diffused

ℓ = 3    It means f-sub shell

f   stands for fundamental

• It also indicates energy up to some extent. Higher is the value of “ℓ” more is the energy.
• It also represents shapes of orbitals.
• Number of orbitals in a sub-shell can be calculated by it.

Number of orbitals in a sub-shell = 2 ℓ + 1

• Number of electrons in a sub-shell can be calculated by it.

Number of electrons in a sub-shell = 2(2 ℓ + 1)

(iii)      Magnetic Quantum Number (m ):

It is obtained by mathematical solution of Ø-part of Schrödinger wave equation. Its values are:

Values of     m = – ℓ , …,0 ,……..,+ ℓ

## The number of values of      mℓ   = 2 ℓ + 1

• It represents orbitals and their orientations

e.g ( i)   if     ℓ = 1    It means p-sub shell and for p-sub shell,

Values of m  = 2ℓ + 1 = 2 x 1 +1 = 3

These values of m  = -1,0,+1

It means that p-sub shell has three orbitals with three different orientations.

orbitals            px         py         pz

m                    +1        -1         0

e.g(ii)  if          ℓ  = 2   It means d-sub shell

and for d-sub shell, number of values of m   = 2ℓ + 1 = 2 x 2 +1 = 5

these values of m are = -2, -1, 0, +1, +2

It means that d-sub shell has five orbitals with five different orientations.

orbitals          dxy       dyz       dz2        dxz       dx2-y2

m                 -2         -1         0          +1        +2

Spin Quantum Number (ms):

It describes the spin of electrons. Its values are

ms = + ½ , – ½

When  ms = – ½          electron shows clock wise spin (↑)

ms = + ½         electron shows anti-clock wise spin (↓)

## Recommended video :

Also Watch !!!

Difference between Shell ,Subshell and Orbital

Rating: 1 out of 5.

### 4 thoughts on “Quantum Numbers Class 11 Chemistry Notes”

1. Excellent site. Plenty of helpful information here.
I am sending it to several pals ans additionally sharing in delicious.
And certainly, thanks to your effort!

2. I was just searching for this information for
a while. After six hours of continuous Googleing, finally I got
it in your web site. I wonder what’s the lack of Google strategy that do not rank this kind
of informative web sites in top of the list. Generally the top websites are full of garbage.

Also visit my web site SynoGut Side Effects

3. This is a very good tip particularly to those new to the blogosphere.
Brief but very accurate information… Thanks for sharing this one.
4. 