HCl is an acid or H+?

HCl fully dissociates in aqueous solution, meaning H+ and Cl- ions exist in the solution.

A Lewis Acid is one that accepts electrons right? So in this case NH3 + H+ -> NH4+ where the H+ is accepting electrons and a bond is formed.

Well I have to but in here......

H+ doesn't actually exist. The acidic molecule found in aqueous solutions of acids is the hydronium ion H3O+

This is different for all solvents but you'll only ever cover aqueous.

Now to say that HCl isn't a lewis acid is just wrong. Of course it can accept electrons, what do you think happens when you form the hydronium?

Bear in mind that the lewis definition is a far better and broader definition, you just cover it later so you assume it's somehow less important. Actually to the contrary. Bronsted acids are a seb-set of acids according to the lewis definition.

I thought I had understood it but this actually helped further... Thanks!

Well.... Just realise that A-level is just scratching the surface (and often just downright incorrect!)

As is the H₃O⁺

Well.... Just realise that A-level is just scratching the surface (and often just downright incorrect!)

..... I hope you're just joking

Oh, I'm doing IB by the way... downright incorrect? Like half truths or something?

Well what you said was not entirely correct as well, since you are neglecting the fact that the excess proton in water often forms symmetric molecule H5O2+ in addition to the H3O+ form (i.e. Zundel complex).

I have far less experience of IB but higher IB is a lot more in depth than A-level so far as i have seen.

I hadn't ever heard of those. They're not surprising though being the intermediate form between proton exchange between water and hydronium. No reason why hydronium shouldn't be hydrated like any other ion

..... I hope you're just joking

Seems to be a common misconception that IB HL is more 'in-depth'

I've worked wth several A' level boards and currently with the IB and it's not the case.

There are areas where each out-performs the other. A' level is much better for organic and spectroscopy. IB is better for redox and acids.

Seems to be a common misconception that IB HL is more 'in-depth'

I've worked wth several A' level boards and currently with the IB and it's not the case.

There are areas where each out-performs the other. A' level is much better for organic and spectroscopy. IB is better for redox and acids.

No - Doctor_Einstein already mentioned what I was aiming at.

Hydrated protons have the general formula (H₂O)_nH⁺. n depends on the concentration, unfortunately to some extent it also depends on the method used to determine its value. Table in Electrochemistry by Koryta, Dvorak and Bohackova that I happen to have here lists 5 as determined using entropy of hydration and 1 or 2 as determined using compressibility.