# How to use Lewis theory to differentiate between an acid and a base?

According to Lewis theory a material is an acid if it accepts an electron pair, and a material is base if it donates an electron pair. But if we compare the structures of $$\ce{HNO3}$$ and $$\ce{NaOH}$$, i.e.

$$\ce{H-\underset{.\!.}{\overset{.\!.}{O}}-\underset{\underset{\huge :O:}{||}}{\overset{+}{N}}-\underset{.\!.}{\overset{.\!.}{O}^}\!:^-} \quad \text{and} \quad \ce{[Na]+ [:\!\underset{.\!.}{\overset{.\!.}{O}}H]-}$$

there are so many lone pair of electrons which can be shared, and in both structures there is a positive atom, so they can accept a lone pair. How can I say that one of them is acid and the other one is a base?

First of all, within the Lewis framework, you may have substances that can act as both acid and base (though most of the time as one or the other, not both at the same time).$$^{1}$$ The adjective for such substances is "amphoteric".

It comes down to a bit of chemical intuition to decide which is which. It is true that almost anything that has a lone pair can act as a base - though it may take a strong acid to form an actual Lewis pair. For acids, one should look for an obvious gap in the electron cloud ($$\ce{AlCl3}$$) or candidates for complex formation ($$\ce{FeCl3}$$).$$^2$$

For nitric acid, the situation is pretty clear: the hindrance provided by three oxygen atoms around the central nitrogen prevents access, so it will hardly act as a Lewis acid. It can act as a base, however, weak Brønsted bases are usually also weak Lewis bases because they are content on their own.

For sodium hydroxide, one must realize that in an aqueous medium, the two ions will fully dissociate. The hydroxide anion will act as a Lewis base, but the sodium cation with its full outer electron shell will hardly act as an acid.$$^3$$

$$^1$$ Adducts of e.g. $$\ce{CO2}$$ in frustrated Lewis pairs, wherein the $$\ce{CO2}$$ acts as a sort-of bridge between the two Lewis sites, are an example of when "both at the same time" can occur.

$$^2$$ I am aware that these compounds will form dimers or more complex structures in reality. If you are able to spot this behavior and understand why, you are already able to spot Lewis acids.

$$^3$$ Note that the sodium cation in water will be solvated, i.e. some water molecules will orient their lone pairs towards the ion. The border between solvation and Lewis adduct formation can be blurry.

• @adeshmishra In the question, you wrote "and in both structures there is a positive atom", which I take to mean that you are wondering about the nitrogen as an electron acceptor. $\ce{H^+}$ is, of course, a Lewis acid. – TAR86 Apr 5 '19 at 18:59
• Yes you are right. Your answer has really helped me a lot. One question I wanna ask can hydrogen ion accept electron pair without getting disassociated? – Knight wants Loong back Apr 5 '19 at 20:11
• @adeshmishra Both happen simultaneously in proton exchange. In hydrogen bonds hydrogen is coordinated to two or more atoms. – Mithoron Apr 6 '19 at 21:05
• @TAR86 There are orthonitrates though. I don't think sterics is main factor why they're less stable then "normal" ones. – Mithoron Apr 6 '19 at 21:11