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Chapter 16: Problem 58

Why is \(\mathrm{BF}_{3}\) a Lewis acid but not a Brensted-Lowry acid?

Short Answer

Expert verified
Explain. Answer: \(\mathrm{BF}_{3}\) is a Lewis acid because it can accept an electron pair due to its empty 2p orbital on the boron atom. However, it is not a Br酶nsted-Lowry acid because it does not contain any hydrogen atoms and therefore cannot donate a proton (H鈦�) to a base.

Step by step solution

01

Define a Lewis Acid and a Br酶nsted-Lowry Acid

A Lewis acid is a substance that can accept a pair of electrons from another atom, while a Br酶nsted-Lowry acid is a substance that donates a proton (H鈦�) to a base.
02

Determine the molecular structure of \(\mathrm{BF}_{3}\)

\(\mathrm{BF}_{3}\) has a central boron atom which is bound to three fluorine atoms, forming a trigonal planar molecule. The boron atom has 3 valence electrons and forms 3 single bonds with the fluorine atoms, also using their valence electrons. Note that Boron has an empty 2p orbital that can accommodate a pair of electrons.
03

Assess if \(\mathrm{BF}_{3}\) is a Lewis Acid

A Lewis acid accepts an electron pair. The boron atom in \(\mathrm{BF}_{3}\) has an empty 2p orbital, allowing it to accept an electron pair from another atom, making \(\mathrm{BF}_{3}\) act as a Lewis acid.
04

Assess if \(\mathrm{BF}_{3}\) is a Br酶nsted-Lowry Acid

A Br酶nsted-Lowry acid must donate a proton (H鈦�) to a base. \(\mathrm{BF}_{3}\) has no hydrogen atoms in its molecular structure, which means it is incapable of donating a proton. Thus, \(\mathrm{BF}_{3}\) is not a Br酶nsted-Lowry acid.
05

Conclusion

\(\mathrm{BF}_{3}\) is a Lewis acid because it can accept an electron pair due to its empty 2p orbital on the boron atom. However, it is not a Br酶nsted-Lowry acid because it does not contain any hydrogen atoms and therefore cannot donate a proton (H鈦�) to a base.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Br酶nsted-Lowry acid
The Br酶nsted-Lowry theory is a fundamental concept in chemistry used to distinguish between acids and bases. According to this theory, an acid is any substance that can donate a proton, which is a positively charged hydrogen ion ( H^+ ).

This means that for a substance to be considered a Br酶nsted-Lowry acid, it must contain hydrogen atoms that can be released as protons.
If there are no hydrogen atoms in the molecule, as is the case with BF_3 , it cannot act as a Br酶nsted-Lowry acid.

While this concept can sometimes be confusing, it is essential to remember that the defining feature of a Br酶nsted-Lowry acid is its ability to donate a proton.
BF3 molecular structure
The molecular structure of BF_3 plays a key role in its reactivity as an acid. BF_3 , or boron trifluoride, consists of a central boron atom surrounded by three fluorine atoms. This creates a trigonal planar shape, where the bond angles are approximately 120 degrees.

Boron, in this structure, has three valence electrons and forms three covalent bonds with fluorine atoms. Each bond involves the sharing of an electron from both boron and fluorine.
  • This leaves boron with an incomplete octet, having only six electrons instead of the usual eight.
  • Additionally, there is an empty 2p orbital on boron that can accept more electrons.
Understanding this structure helps explain the behavior of BF_3 as an acid under the Lewis definition.
electron pair acceptance
Electron pair acceptance is the cornerstone of the Lewis acid concept. A Lewis acid is defined as a compound that can accept an electron pair.

The empty 2p orbital in boron within BF_3 is perfectly suited for this. When BF_3 encounters a molecule or ion with a lone pair of electrons, it can act as an electron pair acceptor.
  • The presence of this empty orbital allows BF_3 to form a coordinate covalent bond with a suitable electron donor.
  • This interaction is the primary reason why BF_3 behaves as a Lewis acid.
Understanding electron pair acceptance clarifies the unique role BF_3 plays in various chemical reactions, despite not having the capability to act as a Br酶nsted-Lowry acid.

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Most popular questions from this chapter

For each titration, predict whether the equivalence point is less than, equal to, or greater than \(\mathrm{pH}=7\) a. HCN titrated with \(\mathrm{Ca}(\mathrm{OH})_{2}\) b. LiOH titrated with HI c. \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}\) titrated with \(\mathrm{KOH}\)

Solution \(A\) is \(0.0200 M\) in \(A g^{+}\) ions and \(P b^{2+}\) ions. You have access to two other solutions: (B) \(0.250 M\) NaCl and (C) \(0.250 M\) NaBr. a. Which solution, B or \(\mathrm{C}\), would be the better one to add to Solution \(A\) to separate \(A g^{+}\) ions from \(P b^{2+}\) by selective precipitation? b. Using the solution you selected in part (a), is the separation of the two ions complete?

If the solubility of a compound increases with increasing temperature, does \(K_{\mathrm{sp}}\) increase or decrease?

Draw Lewis structures that show how electron pairs move and bonds form and break in this reaction, and identify the Lewis acid and Lewis base. $$ \mathrm{SeO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{H}_{2} \mathrm{SeO}_{4}(a q) $$

What is the pH of \(1.00 M \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2} ?\)
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