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Chapter 14: Problem 24

In terms of orbitals and electron arrangements, what must be present for a molecule or an ion to act as a Lewis acid? What must be present for a molecule or an ion to act as a Lewis base?

Short Answer

Expert verified
In order for a molecule or ion to act as a Lewis acid, it must have an empty orbital available to accept a pair of electrons, typically having a central atom with an incomplete octet. On the other hand, to act as a Lewis base, a molecule or ion must have a lone pair of electrons (nonbonding electron pair) that can be donated to the empty orbital of a Lewis acid. The electrons are usually located in the valence shell of a more electronegative atom.

Step by step solution

01

Definition of Lewis Acids and Bases

Lewis acids and bases are defined by the way they interact with electron pairs. A Lewis acid is a molecule or ion that can accept a pair of electrons, while a Lewis base is a molecule or ion that can donate a pair of electrons.
02

Lewis Acid Electron Arrangements

For a molecule or ion to act as a Lewis acid, it must have an empty orbital available to accept a pair of electrons. This empty orbital can be a vacant atomic orbital (such as the p or d orbitals) or a molecular orbital formed by the overlap of atomic orbitals. Most commonly, Lewis acids have a central atom with an incomplete octet (less than 8 electrons in its valence shell) that can accommodate an additional pair of electrons to stabilize its structure. Some examples of Lewis acids include BF3, AlCl3, and Fe3+.
03

Lewis Base Electron Arrangements

For a molecule or ion to act as a Lewis base, it must have a lone pair of electrons (nonbonding electron pair) that it can donate to an empty orbital of a Lewis acid. The electrons are usually located in the valence shell of a more electronegative atom, such as nitrogen, oxygen, or halogens. Some examples of Lewis bases include NH3, OH-, and F-. In summary, a molecule or ion must have an empty orbital to accept a pair of electrons to act as a Lewis acid, and it must have a lone pair of electrons to donate to act as a Lewis base.

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Most popular questions from this chapter

A solution is prepared by adding \(50.0 \mathrm{~mL}\) concentrated hydrochloric acid and \(20.0 \mathrm{~mL}\) concentrated nitric acid to \(300 \mathrm{~mL}\) water. More water is added until the final volume is \(1.00 \mathrm{~L}\). Calculate \(\left[\mathrm{H}^{+}\right],\left[\mathrm{OH}^{-}\right]\), and the \(\mathrm{pH}\) for this solution. [Hint: Concentrated HCl is \(38 \%\) HCl (by mass) and has a density of \(1.19\) \(\mathrm{g} / \mathrm{mL} ;\) concentrated \(\mathrm{HNO}_{3}\) is \(70 . \% \mathrm{HNO}_{3}\) (by mass) and has a density of \(1.42 \mathrm{~g} / \mathrm{mL} .\) ]

Will \(0.10 M\) solutions of the following salts be acidic, basic, or neutral? See Appendix 5 for \(K_{\mathrm{a}}\) values. a. ammonium bicarbonate b. sodium dihydrogen phosphate c. sodium hydrogen phosphate d. ammonium dihydrogen phosphate e. ammonium formate

What are the major species present in \(0.250 \mathrm{M}\) solutions of each of the following acids? Calculate the \(\mathrm{pH}\) of each of these solutions. a. \(\mathrm{HNO}_{2}\) b. \(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)\)

Hemoglobin (abbreviated \(\mathrm{Hb}\) ) is a protein that is responsible for the transport of oxygen in the blood of mammals. Each hemoglobin molecule contains four iron atoms that are the binding sites for \(\mathrm{O}_{2}\) molecules. The oxygen binding is pH-dependent. The relevant equilibrium reaction is $$\mathrm{HbH}_{4}^{4+}(a q)+4 \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{Hb}\left(\mathrm{O}_{2}\right)_{4}(a q)+4 \mathrm{H}^{+}(a q)$$ Use Le Châtelier's principle to answer the following. a. What form of hemoglobin, \(\mathrm{HbH}_{4}{ }^{4+}\) or \(\mathrm{Hb}\left(\mathrm{O}_{2}\right)_{4}\), is favored in the lungs? What form is favored in the cells? b. When a person hyperventilates, the concentration of \(\mathrm{CO}_{2}\) in the blood is decreased. How does this affect the oxygenbinding equilibrium? How does breathing into a paper bag help to counteract this effect? (See Exercise 148.) c. When a person has suffered a cardiac arrest, injection of a sodium bicarbonate solution is given. Why is this necessary?

A solution is prepared by adding \(50.0 \mathrm{~mL}\) of \(0.050 M \mathrm{HBr}\) to \(150.0 \mathrm{~mL}\) of \(0.10 \mathrm{M}\) HI. Calculate the concentrations of all species in this solution. HBr and HI are both considered strong acids.
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