Dipole-Dipole Interactions

[LaughingMan]

I seem to have come across some conflicting information a while back that I cannot ID the source.

I am wanting to confirm, that a molecule such as CCl4, would NOT have Dipole-Dipole interactions with another molecule of CCl4, due to the fact that the molecule has no net dipole-movement/polarity.

True yes?

---

Members don't see this ad.

 

[gwjib04]

That would be intuitive but it turns out that non-polar compounds form induced dipoles. Induced dipoles are transient since its a non-polar molecule.

This is how non-polar substances can be attracted to each other.

So polar molecules are attracted by hydrogen-bonding which is a type of dipole-dipole interaction and non-polar molecules are attracted by induced-dipoles, a type of dipole-dipole interaction.

The same but different I guess

According to ExamKrackers Audio Osmosis (highly recommended)

 

[BerkReviewTeach]

When induced dipoles interact, it's called London dispersion forces. When two dipoles interact, it's called polar attraction. When there is a directionality associated with it (O--H^d+ - - - ^d-O) that obeys orbital overlap, then it's called hydrogen bonding.

 

[LaughingMan]

When induced dipoles interact, it's called London dispersion forces. When two dipoles interact, it's called polar attraction. When there is a directionality associated with it (O--H^d+ - - - ^d-O) that obeys orbital overlap, then it's called hydrogen bonding.

So CCl4 would have induced dipoles--and only have London Dispersion Forces?

 

[mehc012]

So CCl4 would have induced dipoles--and only have London Dispersion Forces?

👍

 

[gettheleadout]

So CCl4 would have induced dipoles--and only have London Dispersion Forces?

Seconding mehc here, this is correct. CCl4 is nonpolar, so no permanent dipoles to interact.