Types of attractions

[8039]

Just wondering for some rule of thumb about the main attractions.

Last year there was a question that expected you to know ion-dipole attractions and how they are more water soluable.

What are all the types that exist (or we need to know about) and what do I need to know about them?

[kyzoo]

All Unit 1/2 stuff

~ H-bonding
~ Dipole-dipole bonding
~ Ionic bonding/interaction/attraction
~ Dispersion force bonding
~ Ion-dipole bonding/attraction
~ Covalent bonds

There's also metal bonding but I've never seen anything relating to that in Unit 3

[8039]

What's the difference between dipole-dipole bonding and ion-dipole bonding?

[kyzoo]

A dipole is a molecule which has a partial positive charge on one side, and a partial negative side on the other, due to differences in electronegativity of the atoms in the molecules. Basically if you have a molecule A-B, and molecule A is more electronegative, the electrons will be more attracted to A.

The result is the molecule A-B having a partial negative charge on the A side, and partial positive charge (due to lack of electrons) on the B side.

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An ion on the other hand is an atom or molecule that has actually lost or gained an electron, and hence has a full negative or positive charge.

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The difference is that dipoles haven't lost/gained electrons and only have a partial charge at each end. Ions have lost/gained electrons and have a full charge (1+, 2+, 1-, 2-, etc). Also, the whole ion is positively/negatively charged, as opposed to one side being positive and the other being negative

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Ion-dipole = ion + dipole
dipole-dipole = dipole + dipole


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Sorry probably not clear enough lol

[chansthename]

Sorry probably not clear enough lol

I think mighty fine effort, it is simple and gets to the point (yet still informative)

[Greggler]

Is H bonding a form of dipole dipole bonding?

And are instantaneous dipoles basically just dispersion forces?

[chansthename]

Is H bonding a form of dipole dipole bonding?

And are instantaneous dipoles basically just dispersion forces?

Yes however H bonding happens between H and N O or F which are very electronegative making it a much stronger bond (relatively)

[8039]

Hey thanks that makes sense. So I'm wondering, when COO- reacts with Na+ why is it an ion/dipole bond and not ion/ion bond? this was last years exam and confusing me :/

And also, dispersion forces are weakest, dipole-dipole<ion-dipole<hydrogen<covalent<ion or something like that?

[Toothpaste]

And also, dispersion forces are weakest, dipole-dipole<ion-dipole<hydrogen<covalent<ion or something like that?

Covalent is stronger than ionic

[kyzoo]

Actually, I have no idea if ionic bonding is stronger than covalent or not, I think it depends on the particular compound.

And H-bonding should be weaker than ion-dipole since H-bonding = dipole-dipole = 2 partial charges. Whilst ion-dipole = full charge + partial charge.

[Toothpaste]

Actually, I have no idea if ionic bonding is stronger than covalent or not, I think it depends on the particular compound.

This. There are other factors which could influence the strength, but speaking generally, covalent is accepted as stronger. (Sharing of electrons over electrostatic)

[chansthename]

from weakest to strongest

Intermolecular
dispersion forces
dipole-dipole
hydrogen
ion-dipole

intramolecular
ion-ion
Covalent
metallic

[8039]

Thanks guys! I guess I only need to really know how each one would make an element react with water?

Btw, what is it when a covalent bond has one more electronegatively charged side? is there a special name for that? I thought that was what dipole bonds but apparently that's only intermolecular :/

[Toothpaste]

Covalent polar bond I think, if I'm thinking of what you're thinking.

[olly_s15]

Thanks guys! I guess I only need to really know how each one would make an element react with water?

Btw, what is it when a covalent bond has one more electronegatively charged side? is there a special name for that? I thought that was what dipole bonds but apparently that's only intermolecular :/

polar?