http://www.brightstorm.com/science/chemistry/chemical-bonds/tips-for-identifying-intermolecular-forces/

http://www.amazon.com/Intermolecular-Surface-Forces-Third-Edition/dp/0123919274

new & simple 

contents: http://www.sciencedirect.com/science/book/9780123751829

Dear Prs. SAKTHIDHARAN C.P. & Joseph Dubrovkin

Thank you very much for this first help, it's very fruitful for me and for my collegues.

http://www.brightstorm.com/science/chemistry/chemical-bonds/tips-for-identifying-intermolecular-forces/

https://au.answers.yahoo.com/question/index?qid=20071128174008AAkJX2m

https://www.khanacademy.org/test-prep/mcat/chemical-processes/covalent-bonds/v/intermolecular-forces-and-molecular-bonds

http://chemistry.bd.psu.edu/jircitano/IMforces.html

https://www.youtube.com/watch?v=PwveQxLLqD0

A better mathematical treatment of long range forces ( electrostatic, inductive & dispersion) as well as short range forces due to electron exchange is given in the The theory of Intermolecular forces, by Anthony Stone.  http://www.amazon.com/The-Theory-Intermolecular-Forces-Edition/dp/0199672393

Dear all,

Me, and all my colleagues thank you a lot for this first step of anwers.

There are many helpful and interesting things.

If I guess correctly your question, you are not so much interested in the theoretical classification of different kind of forces but you may be more interested in understanding the reasons to describe a specific liquid system with one or another of the possible different kind of interactions .

Am I right ? In this case, the answer is that in most of the cases it may be difficult, on a purely experimental basis,  to assign the real interactions to one or more of the many existing theoretical models.

You have to think that every classical interaction between atoms is actually coming from the electrostatic interaction between nuclei and (quantum) electrons. However, under reasonable hypothesis one can average over (trace out) the electronic degrees of freedom  and remaining with an effective inter-ionic interaction. As matter of fact, in general such interaction is a many-body interaction,but in many cases it may be well approximated by pair-wise ion-ion interactions.

So, having clear in mind that any of the interaction in your list is just an approximation, the practical problem is how to judge which approximation is the best for a specific system.

Here again, the answer is not simple. In may cases, you may well reproduce a given set of experimental results with more than a single interaction model. However, larger is the set of properties you may want to reproduce and larger the set of thermodynamic states you  include in your database, better you can discriminate between different models. But take into account that in some cases my be very difficult to discriminate between different interaction models, even if they may be very different.

A much better procedure is to  combine the analysis of experimental results via some model of interaction with some additional knowledge about the system of interest coming from investigation of completely different phases.

For example, even if a purely ionic model and  an alternative model where some screening is introduced in the inter-ionic interaction of a simple molten salt like NaCl may  provide equivalent   good agreement with the experimental  pair distribution function, the direct evidence provided by the experimental determination of the electronic redistribution provides a stronger support for an ionic model. An independent knowledge about the ionic dipolar polarizability may motivate to introduce an induced dipole interaction model etc.

This answer is from Saad Hashim Khalilb:

Saad Hashim Khalilb (to you 8 days ago).

Hello, try this link http://www.mikeblaber.org/oldwine/chm1045/notes/Forces/Intermol/Forces02.htm. This is from Michael Blaber, 1996, Professor of Biomedical Sciences at Florida State University. E-mail: [email protected].

I hope this can help, thank you

The dipole - dipole interactions could be recognized by measuring surface tension and viscosity together. The water and DMSO could be chosen as dipolar systems  for such measurements. The data for them individually and their mixtures could be determined. The difference in surface tension and viscosity data of their mixtures as compared to their individual gives quantitative recognition of dipole-dipole interactions. However, further, the product of frictional forces basis of viscosity and cohesive forces the basis of surface tension depicted as friccohesity could demarcate and recognize sharply, the dipolar interactions.  

Here are some documents (# 1) in French,

I hope they will be useful.

Here are some other documents (# 2) in French,

I hope they will be useful.

Here are some other documents (# 3) in French,

I hope they will be useful.

Here are some other documents (# 4) in French,

I hope they will be useful.

Here are some other documents (# 5) in French,

I hope they will be useful.

Here are some other documents (# 6),

I hope they will be useful.

Here are some other documents (# 7),

I hope they will be useful.

Here are some other documents (# 8), application

I hope they will be useful.

Thanks to Pr. Man Singh who has send us these documents:

Pl have a look at few relevant papers, hope your may get some insight about interactions taking place in liquid mixtures.

Simultaneous study of interfacial tension, surface tension, and viscosity of few surfactant solutions with survismeter

Man Singh∗

Effect of potassiumhalide salts on mutual solubility of water+ aromatic hydrocarbons liquid–liquid interface studied with surface and interfacial tensions

Man Singh

Dispersion and optical activities of newly synthesized magnetic nanoparticles with organic acids and dendrimers in DMSO studied with UV/vis spectrophotometry

Shivani R. Pandya a, Man Singh

Influence of Urea on Shifting Hydrophilic to Hydrophobic Interactions of Pr(NO3)3, Sm(NO3)3, and Gd(NO3)3 with BSA in Aqueous Citric Acid: A Volumetric, Viscometric, and Surface Tension Study

Dinesh Kumar,† Abhishek Chandra,† and Man Singh

Physicochemical and friccohesity study of glycine, L-alanine and L-phenylalanine with aqueous methyltrioctylammonium and cetylpyridinium chloride from T = (293.15 to 308.15) K

Abhishek Chandra a, Vivek Patidar a, Man Singh a,⇑, R.K. Kale

Intermolecular forces and intermolecular attraction. 

The molecules of the liquid that will escape easily from the surface imply that the intermolecular forces are “relatively weak” and therefore do not require “much heat” to break the bonds (or interactions) to boil the liquid.

http://www.ukessays.co.uk/essays/chemistry/vapour-pressure.php