[Ari Ben Canaan]

I know of Instantaneous Induced Dipole-Dipole bonding, Permanent Dipole Bonding and Hydrogen bonding.

I understand them fully but what I dont get is which type of bonding applies to what type of molecules :S

That is when does a molecule have Instantaneous Induced Dipole-Dipole bonding, Permanent Dipole Bonding or Hydrogen bonding ?

Are there certain pre-requisites that molecule X must have to have a certain type of bonding?

[rabolisk]

I understand them fully but what I dont get is which type of bonding applies to what type of molecules :S

Are you confused about specific examples? Because I don't see how you understand them but don't know when they occur/apply.

[Ari Ben Canaan]

Are you confused about specific examples? Because I don't see how you understand them but don't know when they occur/apply.

I actually knew you would say something like that

No, its a bit complicated.

For example ,do simple covalent molecules always have instantaneous induced dipole bonds ?

To reiterate, do you have a list of pre-requisites that molecule X must have to have a certain type of bonding ?

[rabolisk]

Yes, any covalent molecule or atom is considered to have dispersion forces, no matter how weak they may be.

[rabolisk]

To clarify a bit more, substances that exist as discrete molecules have intermolecular bonding. Most chemical compounds, like gases, organic compounds, and things that exist in solutions fall into this category. Ionic compounds, in the solid state, are in a lattice and have ionic bonds between the ions, and do not have intermolecular forces, because there are no discrete molecules. Metals are similar; they exhibit metallic bonding. Diamond is covalently bonded sp3 hybridized carbon atoms arranged in a lattice, and do not have intermolecular bonding. The recurring theme is that you have to have discrete molecules in order to have intermolecular bonding.

[rabolisk]

AND FINALLY, to clarify one last bit...

Molecular solids, such as ice or iodine, do have intermolecular forces because they are composed of discrete molecules that are arranged in a crystal lattice. The IMFs bond the molecules together.

It's clear, then, that IMFs of solids > liquids> gases. One of the defining characteristics of perfect gases (ideal gases) is that there is no IMF between the molecules, because they are too far away from each other to feel any attraction. All gases approach this state as temperature approaches infinity. In another sense, stronger IMFs tend to attract molecules to each other and condense them. Thus strength of IMFs are correlated with boiling point.

Any other questions??

[Ari Ben Canaan]

No, I think you've pretty much nailed it all.

Though I have one small query :

London Dispersion Forces and Van der Waals forces are one and the same, right ?

In addition, Hydrogen Bonding, Instantaneous-Induced Dipole bonds and Permanent dipole bonds are all Van Der Waals forces, right ?

[rabolisk]

London Dispersion Forces mean induced-dipole interactions. Van der Waals forces is more tricky, because I have seen different definitions.

http://en.wikipedia.org/wiki/Van_der_Waals_force