This is my published method in IJOAR journal in the field of chemistry in oct 2015 edition,By using this method one can magnetic moment of any diatomic molecule or ion having total electron 1-20 within a few second without concept of MOT.

1. International Journal of Advance Research, IJOAR .org
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IJOAR© 2015
http://www.ijoar.org
International Journal of Advance Research, IJOAR .org
Volume 3, Issue 10, October 2015, Online: ISSN 2320-9178
New Rapid And Innovative Method For Prediction of
Magnetic Moment of Mono And Diatomic Molecules And
Ions Without M.O.T.
PRITAM DEBNATH
Department of Civil Engineering, U.G. Student (2nd year), NIT Agartala, Tripura(W), India
Phone no:+91 9436584888
Email:pritam.oam@gmail.com
KeyWords
Even electron number, Molecules, Magnetic properties, M.O.T., Odd electron number, Total electron number, Value of ‘l’.
ABSTRACT
Determination of magnetic moment and magnetic properties of different molecules and ions, plays a very important rule in inorganic chem-
istry. But, finding of magnetic moment by using M.O.T. is time consuming. So, in this manuscript, I tried to show a rapid and innovative
method for finding the Magnetic Moment of different mono and diatomic molecules or ions having total electron (01-20). One can easily
find the Magnetic Moment of different mono and diatomic molecules and ions using this rapid method, even if he is unknown to M.O.T..
This method is only applicable for mono and diatomic molecules and ions having total electron (01-20), but not applicable for polyatomic
molecules, such as SF4, SO2, BCl3, CCl4 etc.

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MAIN PAPER STARTS HERE…
Introduction
The method of prediction of magnetic moment is very important in inorganic chemistry. But the conventional method of determina-
tion of magnetic moment is time consuming. In various competitive examination, magnetic moment related question plays a very
important part. So, by using a rapid method of prediction of magnetic moment
[9],[10]
, one can save their valuable time in exam hall.
So, keeping all this things in mind, this new innovative method is introduced, which will be time saving for students in various com-
petitive examination.
This method contains four(4) new formulae, with four(4) set of electron no.; by placing only the value of ‘l’(described as below)
in the respective formula, one can easily calculate the magnetic moment of different molecules. So, we can use this rapid method in
place of the conventional formula of finding magnetic moment, μ = �𝑛(𝑛 + 2) B.M., where B.M. = Bohr Magneton = Unit of Mag-
netic Moment, n = number of unpaired electron.
I believe, this rapid method will be very much helpful for all students, who are facing various competitive examination and by
using these formulae, students can save their valuable time in exam hall.
So, on the basis of all these things, I can strongly recommend that this method will be most rapid method for the prediction of
magnetic moment of mono and diatomic molecules and ions having total electron no (01-20) without using M.O.T.
[1]-[8]
.
Result and Discussions
First of all, we take certain range of total electron of different mono and diatomic molecules or ions, which are shown in four sets
as follows.
Set-1:- Molecules or ions having (1-10 and 16)e
-
s, (consider only even electron no. in this range)
Set-2:- Molecules or ions having (11-20, ≠16)e
-
s, (consider only even electron no. in this range)
Set-3:- Molecules or ions having (1-8)e
-
s, (consider only odd electron no. in this range)
Set-4:- Molecules or ions having (9-20)e
-
s, (consider only odd electron no. in this range)
The above four sets, with their corresponding formulae are shown in table 1.
Table:-1
Range of Total Electron No. Formula
1-10 and 16 (consider only even ‘e-’ no. in this
range)
√𝟖𝟖
11-20 (≠16) (consider only even ‘e-’ no. in this range
without 16)
√𝟖𝟖 − 𝟖
1-8 (consider only odd ‘e-’ no. In this range) √𝟑𝟖 + 𝟑
9-20 (consider only odd ‘e-’ no. in this range) √𝟑𝟖

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Introduction to ‘l’
‘l’ is a variable, which can take only two value 0 or 1 depending on the total electron number of a molecule or ion.
If, the total electron no. for a molecule or ion lies between ‘1-8’, then value of l = 0.
If, the total electron no. for a molecule or ion lies between ‘9-20’, then value of l = 1.
Source of conception behind the value of l
Actually this concept is taken from azimuthal quantum no.
[11],[12]
in quantum chemistry ,where we have found, for s orbital, quantum
no l is taken as 0 (l is azimuthal quantum no.), for p orbital l is taken as 1. The same concept I have used here. If an atom contains
only s orbital, the value of l is taken as 0, and if an atom contains s and p orbital both, then the value of l is taken as 1. The value of l
depends on the two atom by which a diatomic molecule is composed. But in case of such diatomic molecule, where one atom has
only s orbital and another atom has both s and p orbital, then I have observed if I take the atom consisting both s and p orbital in my
consideration, then my experiment goes in a suitable way and give me a suitable result. But, if I take the atom, which has only s or-
bital, then my experiment does not give any suitable result. That’s why, I have taken that atom in my consideration, which contains
both s and p orbital in case of the ionic molecule or heteronuclear diatomic molecule to find the value of l.
After all, I have found, for the molecules which contains (1-8) total electron, the value of l for those molecules is 0, and for the
molecules which contains (9-20) total electron, the value of l for those molecules is 1.
E.g.:
1. N + N = N2
Electronic configuration of N : 1S
2
2S
2
2P
3
We can observe that N2 contain two N (nitrogen atom), and both N atom contain both s and p orbital. So, the value of l for N2 mole-
cule is taken as 1.
2. H + F = HF
Electronic configuration of H : 1S
1
Electronic configuration of F : 1S
2
2S
2
2P
5
We can observe that HF contains one H (hydrogen) atom and one F (fluorine) atom. And, H atom has only s orbital, whereas F atom
has both s and p orbital. So, according to the considering rule, value of l is taken as 1.
Discussion for set 1:
Total electron range : 1- 10 and 16 (consider only even electron no.)
In this case, Formula for magnetic moment = √𝟖𝟖 B.M.
where, B.M. = Bohr Magneton = unit of magnetic moment
E.g.: O2, which has total electron no. 16, therefore value of l = 1.
Hence, magnetic moment for O2 = √8.1 = √8 = 2.82 B.M.= Para magnetic
Discussion for set 2:
Total electron range : 11- 20 , ≠16 (consider only even electron no.)
In this case, Formula for magnetic moment = √𝟖𝟖 − 𝟖 B.M.
where, B.M. = Bohr Magneton = unit of magnetic moment
E.g.: N2, which has total electron no. 14, therefore value of l = 1.
Hence, magnetic moment for N2 = √8.1 − 8 = √0 = 0 B.M. = Diamagnetic
Discussion for set 3:
Total electron range : 1- 8 (consider only odd electron no.)
In this case, Formula for magnetic moment = √𝟑𝟑 + 𝟑 B.M.
where, B.M. = Bohr Magneton = unit of magnetic moment
E.g.: Be2
+, which has total electron no. 7, therefore value of l = 0.
Hence, magnetic moment for Be2
+ = √3.0 + 3 = √3 = 1.73 B.M. = Paramagnetic
Discussion for set 4:
Total electron range : 9- 20 (consider only odd electron no.)
In this case, Formula for magnetic moment = √𝟑𝟑 B.M.
where, B.M. = Bohr Magneton = unit of magnetic moment
E.g.: NO, which has total electron no. 15, therefore value of l = 1.
Hence, magnetic moment for NO= √3.1 = √3 = 1.73 B.M. = Para magnetic

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The magnetic moments of different molecules and ions with their magnetic properties are shown in table 2.
Table :- 2
Different
Molecules
Total
Electron
No.
Unpaired
Electron
No.
(n)
Value of
‘l’
Magnetic Moment using
Conventional formula
�𝒏(𝒏 + 𝟐)
(in B.M)
Magnetic Moment using
New formula(in B.M)
Magnetic
Properties
H2 2 0 0 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟎=0 Diamagnetic
He2 4 0 0 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟎=0 Diamagnetic
Li2 6 0 0 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟎=0 Diamagnetic
Be2 8 0 0 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟎=0 Diamagnetic
B2 10 2 1 �𝟐(𝟐 + 𝟐)=√𝟖 √𝟖. 𝟏=√𝟖 Para magnetic
C2 12 0 1 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟎=0 Diamagnetic
N2 14 0 1 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟎=0 Diamagnetic
O2 16 2 1 �𝟐(𝟐 + 𝟐)=√𝟖 √𝟖. 𝟏=√𝟖 Para magnetic
F2 18 0 1 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟎=0 Diamagnetic
Ne2 20 0 1 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟎=0 Diamagnetic
H2
+ 1 1 0 �𝟏(𝟏 + 𝟐)=√𝟑 √ 𝟑. 𝟎 + 𝟑=√𝟑 Para magnetic
H2
- 3 1 0 �𝟏(𝟏 + 𝟐)=√𝟑 √ 𝟑. 𝟎 + 𝟑=√𝟑 Para magnetic
He2
+ 3 1 0 �𝟏(𝟏 + 𝟐)=√𝟑 √ 𝟑. 𝟎 + 𝟑=√𝟑 Para magnetic
Li2
+ 5 1 0 �𝟏(𝟏 + 𝟐)=√𝟑 √ 𝟑. 𝟎 + 𝟑=√𝟑 Para magnetic
Be2
+ 7 1 0 �𝟏(𝟏 + 𝟐)=√𝟑 √ 𝟑. 𝟎 + 𝟑=√𝟑 Para magnetic
HF 10 2 1 �𝟐(𝟐 + 𝟐)=√𝟖 √𝟖. 𝟏=√𝟖 Para magnetic
C2
+ 11 1 1 �𝟏(𝟏 + 𝟐)=√𝟑 √𝟑. 𝟏=√𝟑 Para magnetic
C2
- 13 1 1 �𝟏(𝟏 + 𝟐)=√𝟑 √𝟑. 𝟏=√𝟑 Para magnetic
N2
+ 13 1 1 �𝟏(𝟏 + 𝟐)=√𝟑 √𝟑. 𝟏=√𝟑 Para magnetic
N2
- 15 1 1 �𝟏(𝟏 + 𝟐)=√𝟑 √𝟑. 𝟏=√𝟑 Para magnetic
O2
+2 14 0 1 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟏 − 𝟖=0 Diamagnetic

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O2
-2 18 0 1 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟏 − 𝟖=0 Diamagnetic
O2
- 17 1 1 �𝟏(𝟏 + 𝟐)=√𝟑 √𝟑. 𝟏=√𝟑 Para magnetic
O2
+ 15 1 1 �𝟏(𝟏 + 𝟐)=√𝟑 √𝟑. 𝟏=√𝟑 Para magnetic
NO+ 14 0 1 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟏 − 𝟖=0 Diamagnetic
NO- 16 2 1 �𝟐(𝟐 + 𝟐)=√𝟖 √𝟖. 𝟏=√𝟖 Para magnetic
CN 13 1 1 �𝟏(𝟏 + 𝟐)=√𝟑 √𝟑. 𝟏=√𝟑 Para magnetic
CN+ 12 0 1 �𝟎(𝟎 + 𝟐)=0 √𝟖. 𝟏 − 𝟖=0 Diamagnetic
Conclusion
After all, I approach a new innovative and rapid method for prediction of magnetic moment and their corresponding magnetic
properties. This method will be very much helpful for all students of chemistry. And by using this rapid method, one can easily pre-
dict the magnetic moment of different molecules and ions and also, students will be able to answer very rapidly in competitive exam-
ination of magnetic moment related questions.
Acknowledgment
The corresponding author Sri.Pritam Debnath, would be grateful to Dr.Subhojit Das, Department of chemistry, NIT Agartala,
Tripura(W) for giving his valuable time in this regard and also grateful to the Dr.Arijit Das, Department of chemistry, Ramthakur col-
lege, Agartala, Tripura(W) for his great inspiration for prediction of new methods.
References
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