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Chapter 16: Problem 78

In terms of orbitals and electron arrangements, what must be present for a molecule or an ion to act as a Lewis acid (use \(\mathrm{H}^{+}\) and \(\mathrm{BF}_{3}\) as examples)? What must be present for a molecule or ion to act as a Lewis base (use \(\mathrm{OH}^{-}\) and \(\mathrm{NH}_{3}\) as examples)?

Short Answer

Expert verified
A Lewis acid must have an empty orbital that can accept a pair of electrons, like \(\mathrm{H}^{+}\) and \(\mathrm{BF}_{3}\). A Lewis base must have a spare pair of electrons in its outer energy level that it can donate, like \(\mathrm{OH}^{-}\) and \(\mathrm{NH}_{3}\).

Step by step solution

01

Define Lewis Acids and Lewis Bases

A Lewis acid is a substance that can accept a pair of electrons to form a covalent bond. A Lewis base, on the other hand, is a substance that can donate a pair of electrons to form a covalent bond.
02

Identify Characteristics of a Lewis Acid

In terms of orbitals and electron arrangements, a Lewis acid must have an empty orbital or orbitals that can accept a pair of electrons. The \(\mathrm{H}^{+}\) ion is a Lewis acid because it has no electrons and can easily accept a pair of electrons. The \(\mathrm{BF}_{3}\) molecule is also a Lewis acid because the boron atom has an empty orbital that can accept a pair of electrons.
03

Identify Characteristics of a Lewis Base

A Lewis base must have an unshared pair of electrons in its outer energy level that it can donate. The \(\mathrm{OH}^{-}\) ion is a Lewis base because it has a spare pair of electrons that it can donate. Similarly, the \(\mathrm{NH}_{3}\) molecule is a Lewis base because the nitrogen atom has an unshared pair of electrons that it can donate.

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Most popular questions from this chapter

In a certain experiment a student finds that the \(\mathrm{pHs}\) of \(0.10 M\) solutions of three potassium salts \(K X, K Y\) and \(\mathrm{KZ}\) are 7.0,9.0 , and 11.0 , respectively. Arrange the acids HX, HY, and HZ in order of increasing acid strength.

Write an equation relating \(\left[\mathrm{H}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) in solution at \(25^{\circ} \mathrm{C}\).

Which of the following solutions has the highest \(\mathrm{pH} ?\) (a) \(0.40 \mathrm{M} \mathrm{HCOOH},\) (b) \(0.40 \mathrm{M} \mathrm{HClO}_{4}\) (c) \(0.40 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}\).

Oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) has the following structure: An oxalic acid solution contains these species in varying concentrations: \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}, \mathrm{HC}_{2} \mathrm{O}_{4}^{-}, \mathrm{C}_{2} \mathrm{O}_{4}^{2-}\), and \(\mathrm{H}^{+}\). (a) Draw Lewis structures of \(\mathrm{HC}_{2} \mathrm{O}_{4}^{-}\) and \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\). (b) Which of the four species listed here can act only as acids, which can act only as bases, and which can act as both acids and bases?

Teeth enamel is largely hydroxyapatite \(\left[\mathrm{Ca}_{5}\left(\mathrm{PO}_{4}\right)_{3} \mathrm{OH}\right]\). When it dissolves in water (a process called demineralization), it dissociates as follows: $$\mathrm{Ca}_{5}\left(\mathrm{PO}_{4}\right)_{3} \mathrm{OH} \longrightarrow 5 \mathrm{Ca}^{2+}+3 \mathrm{PO}_{4}^{3-}+\mathrm{OH}^{-}$$ The reverse process, called remineralization, is the body's natural defense against tooth decay. Acids produced from food remove the \(\mathrm{OH}^{-}\) ions and thereby weaken the enamel layer. Most toothpastes contain a flouride compound such as \(\mathrm{NaF}\) or \(\mathrm{SnF}_{2}\). What is the function of these compounds in preventing tooth decay?
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