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I'm in AP Chemistry and we are learning about the Brønsted-Lowry model and my teacher mentioned that "for the most part" acids have hydrogen, could there be such a thing as an acid that has no hydrogen in it?

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    $\begingroup$ By definition, Bronsted-Lowry acids (proton donors) must have a proton, so they must have hydrogen. Lewis acids are a different matter altogether though, and chances are you'll come across it soon enough. PS @JonCuster question was changed, OP meant "without hydrogen" not "anhydrous". $\endgroup$ – orthocresol Apr 3 '17 at 14:44
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    $\begingroup$ @R.M. - certainly one could say that the reactions/equations that determine the hydrogen ion concentration are different between anhydrous HF and aqueous HF. $\endgroup$ – Jon Custer Apr 3 '17 at 18:10
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    $\begingroup$ Not totally related, but most students don't realize that a hydrogen ion is simply a proton. You'll benefit from that knowledge in college level chem. $\endgroup$ – gogators Apr 3 '17 at 21:10
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    $\begingroup$ @gogators my teacher actually taught that to us at the beginning of the chapter, and it makes some of the actions of acid base reactions a lot more intuitive $\endgroup$ – mcchucklezz Apr 3 '17 at 21:11
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    $\begingroup$ $\ce{AlCl3}$ and $\ce{BF3}$ are acids without hydrogen. :) $\endgroup$ – Pritt says Reinstate Monica Apr 27 '17 at 2:48
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It depends on which definition of acids and bases you are using.

According to the Arrhenius theory, acids are defined as a compound or element that releases hydrogen (H+) ions into the solution. Therefore, there are no Arrhenius acids without a hydrogen atom.

According to the Brønsted–Lowry acid–base theory, an acid is any substance that can donate a proton and a base as any substance that can accept a proton. Hence, there are no acids without a hydrogen atom according to this theory.

But according to the Lewis theory of acids and bases, an acid is any substance that can accept a pair of nonbonding electrons. In other words, a Lewis acid accepts a lone pair of electrons. According to this theory, acids without a hydrogen atom can exist. (A coordinate bond is formed between the Lewis acid and base. The compound formed by the Lewis acid and base is called a Lewis adduct)

A great example of this would be $\ce{BF3}$. It is neither an Arrhenius acid nor a Brønsted–Lowry acid but it is a Lewis acid. The boron atom accepts a pair of nonbonding electrons from another atom or ion to complete its octet. Here $\ce{BF3}$ is a Lewis acid as it accepts a pair of nonbonding electrons.

Fluorine ion plus Boron trifluoride

The fluorine ion here is a Lewis base as it donates a pair of electrons.

If you want to get more rigorous about the definition of Lewis acids: "a Lewis acid is a type of chemical that reacts with a Lewis base to form a Lewis adduct".

More about Lewis acids and bases here.

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  • $\begingroup$ Just out of curiosity, would such thing form acid-like solution in high pressure liquid form of oxygen difluoride? (assuming it didn't have access to anything else to react with, I know I'm probably showing just how little I know by asking this question) $\endgroup$ – barteks2x Apr 4 '17 at 17:26
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There are quite a number of theories regarding acidity and basicity, but in this case, will explain the Lewis acid.

The Lewis Theory of acids and bases

This theory extends well beyond the things you normally think of as acids and bases.

The theory

  • An acid is an electron pair acceptor.

  • A base is an electron pair donor

The Lewis acid-base theory explains why $\ce{BF3}$ reacts with ammonia. $\ce{BF3}$ is a trigonal planar molecule because electrons can be found in only three places in the valence shell of the boron atom.

As a result, the boron atom is sp2 hybridized, which leaves an empty 2pz orbital on the boron atom. $\ce{BF3}$ can, therefore, act as an electron-pair acceptor or Lewis acid. It can use the empty 2pz orbital to pick up a pair of nonbonding electrons from a Lewis base to form a covalent bond.

$\ce{BF3}$, therefore, reacts with Lewis bases such as $\ce{NH3}$ to form acid-base complexes in which all of the atoms have a filled shell of valence electrons, as shown in the figure below:

a

Consider another scenario:

b

Water is an example of a lewis base. Carbocations are examples of lewis acids. When water reacts with a carbocation, as shown above, one of the electrons pairs from oxygen is used to form a new sigma bond to the central carbon in the carbocation.

References

  1. The Lewis Theory of acids and bases

  2. The Lewis Definitions of Acids and Bases

  3. Lewis acids Chemistry

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As noted by others, there is the concept of Lewis acids, and other answers to this question explain that concept well. To reiterate: A Lewis acid is a chemical that will accept electron pair donation from another chemical (which is called a Lewis base in this context). It is also true that Brønsted-Lowry defined acids as $\ce{H+}$-donors and bases as $\ce{H+}$-acceptors. As such, a BL acid without hydrogen is strictly not existent.

I note two important exceptions that sort of defy the strict definition. Boric acid $\ce{B(OH)3}$ does not detach one of its original protons but accepts an electron pair from $\ce{OH-}$. This raises the concentration of $\ce{H+}$ through protolysis of water. $\ce{FeCl3}$ reacts likewise. Of course, these reactions require water, thus, in the strict sense, a complex of water and the substances noted constitutes the BL acid, not the substances themselves.

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I just wish to clarify the other answers. The definition of a "Lewis Acid" is a chemical species which reacts with the electron lone pair of a "Lewis Base" (and a Lewis Base is a species which has a reactive lone pair of electrons). This is a generalization and abstraction of the more common Brønsted-Lowry theory.

Consider that Science is full of 'levels' of abstraction. We have positive integers (the natural numbers), but then we add zero, then negative integers, then rationals, finally we might think we're done when we get to real numbers, but then along come complex numbers, and quaternions, octonions, vectors, fields, and on and on.

While historically a fact, so you need to be familiar with the concept of Lewis Acid/Lewis Base/Lewis Adduct, you should also be aware that all chemistry has to do with the (partial or total) donation and accepting of electronic charge, so while lone pair chemistry is a large enough area to justify its own terminology, it's just the same old, same old "chemistry is about the electrostatic interactions of atoms" story.

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Plenty of answers here focused on the definitions of Brønsted-Lowry and Lewis acids, which is great. But there is an important point I saw mentioned only in passing (in TAR86's answer), and I think it comes closer to answering your question that reciting the somewhat arbitrary acid-base definitions of our forefathers (useful as they are).

Could there be such a thing as a Brønsted-Lowry acid that has no hydrogen in it?

Yes! At least in a pragmatic sense. As elaborated here, highly-charged metal cations such as $\ce{Al^{3+}}$ and $\ce{Fe^{3+}}$ can liberate protons in aqueous media. When such cations are placed in water, water molecules coordinate/associate with the metal ion:

$$\ce{Al^{3+} + 6H2O -> [Al(H2O)6]^{3+}}$$

Here is a structural cartoon of the hexavalent aluminum hydrated complex:

enter image description here

This complex easily releases three protons:

$$\ce{[Al(H2O)6]^{3+} -> Al(H2O)3(OH)3 + 3H+}$$

So, not only is $\ce{Al^{3+}}$ a Lewis acid, but practically speaking it is also a Brønsted-Lowry acid (and triprotic, nonetheless!) Such highly-charged metal cations are as close as you're going to come to a Brønsted-Lowry acid without hydrogen. While they are not acids in a literal (single-step) sense, if we are considering aqueous solutions, then functionally speaking they are indeed Brønsted-Lowry acids because they effect the release of protons and thus lower the solution's pH.

I'm not sure if your teacher had this in mind, or was just trying to cover their arsenic in case there were exceptions they had forgotten about, but there is your answer.

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