So I\'ve been doing a fair amount of reading in my textbook and online. I\'m sli

Question

So I've been doing a fair amount of reading in my textbook and online. I'm slightly confused about the different molecular forces. Hydrogen bonding is simple and straightforward, so I get that. What I would like to do is be able to identify the type of intermolecular force present by not having to draw a lewis dot structure each and every time. The intermolecular forces featured in my text (exluding hydrogen bonding) include Ion-dipole, Dipole-dipole, Ion-induced dipole, dipole-induced dipole, and dispersion (london) forces. Could someone please rank these for me as most common to least common, and/or strongest to weakest? And fill me in on how to possibly easily identify which is which by looking at a compound? For example, would the ion-dipole simply be an ionic bond? And dipole-dipole be covalent? How do I know if the compound is "induced"? Are dipole-dipole, ion dipole sub categories of a general dispersion force? I know this is long winded, but I'm hoping someone will get where I am coming from. Thanks in advance.

Explanation / Answer

Intermolecular Forces are 1) Dipole-Dipole forces, 2) Ion-Dipole forces, 3) Dispersion forces, and 4) Hydrogen bonding

Dipole-Dipole forces are attractive forces between polar molecules, that is, between molecules that possess dipole moments.

Eg: HBr exsit dipole-dipole intraction

Ion-Dipole forces, which attract an ion and a polar molecule to each other. The strength of this interactions depends on the charge and size of the ions and on the magnitude of the dipole moment and size of the molecule.

Hydration is one of the example of ion-dipole intractions

The interaction between a polar molecule and the induced dipoles is called dipole-induced dipole interactions.

In nonpolar molecules only dispersion forces bettwen those molecules

The order of intermolecular force strength is as follows:

Hydrogen bonding > Dipole-Dipole interactions > Ion-Dipole forces > Dispersion forces.

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