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Chapter 15: Problem 2

In order for a species to act as a Brønsted base, an atom in the species must possess a lone pair of electrons. Explain why this is so.

Short Answer

Expert verified
An atom in a species needs a lone pair of electrons to act as a Brønsted base because the lone pair can form a coordinate covalent bond with a proton (H+), effectively taking up the proton from another species, which is the characteristic action of a base according to Brønsted-Lowry Acid-Base theory.

Step by step solution

01

Definition of a Brønsted base

A Brønsted base, according to the Brønsted-Lowry Acid-Base theory, is a chemical species that can accept (or combine with) a proton. A proton is a hydrogen ion (H+). This means that a base must have a means to attract and hold such a proton.
02

Understanding the Role of Lone pairs

In a molecule or ion, a lone pair refers to a pair of valence electrons that are not shared with another atom. Lone pairs in a species are critical in that they can readily form a bond with H+ - which is just a single proton with no electrons. This bond results in the formation of a coordinate covalent bond between the species, acting as a base, and the incoming proton.
03

Illustration of Brønsted base action

For example, ammonia (NH3) can act as a Brønsted base. It has a nitrogen atom with a lone pair of electrons, which can form a coordinate covalent bond with a H+ ion. The resulting species NH4+ is formed when NH3 accepts a proton from another species, thus acting as a base.

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Most popular questions from this chapter

Classify each of the following species as a Lewis acid or a Lewis base: (a) \(\mathrm{CO}_{2},\) (b) \(\mathrm{H}_{2} \mathrm{O},\) (c) \(\mathrm{I}^{-}\), (f) \(\mathrm{OH}^{-},(\mathrm{g}) \mathrm{H}^{+},\) (d) \(\mathrm{SO}_{2}\), (e) \(\mathrm{NH}_{3}\), (h) \(\mathrm{BCl}_{3}\).

Classify the following oxides as acidic, basic, amphoteric, or neutral: (a) \(\mathrm{CO}_{2},\) (b) \(\mathrm{K}_{2} \mathrm{O},\) (c) \(\mathrm{CaO}\), (d) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (e) CO, (f) \(\mathrm{NO}\) (g) \(\mathrm{SnO}_{2}\), (h) \(\mathrm{SO}_{3}\), (i) \(\mathrm{Al}_{2} \mathrm{O}_{3},(\mathrm{j}) \mathrm{BaO}\)

\(\mathrm{Al}(\mathrm{OH})_{3}\) is an insoluble compound. It dissolves in excess \(\mathrm{NaOH}\) in solution. Write a balanced ionic equation for this reaction. What type of reaction is this?

Classify each of the following species as a weak or strong acid: (a) \(\mathrm{HNO}_{3},\) (b) HF, (c) \(\mathrm{H}_{2} \mathrm{SO}_{4},\) (d) \(\mathrm{HSO}_{4}^{-}\), (e) \(\mathrm{H}_{2} \mathrm{CO}_{3},\) (f) \(\mathrm{HCO}_{3}^{-},(\mathrm{g}) \mathrm{HCl}\) (h) \(\mathrm{HCN}\), (i) \(\mathrm{HNO}_{2}\).

When the concentration of a strong acid is not substantially higher than \(1.0 \times 10^{-7} M,\) the ionization of water must be taken into account in the calculation of the solution's pH. (a) Derive an expression for the \(\mathrm{pH}\) of a strong acid solution, including the contribution to \(\left[\mathrm{H}^{+}\right]\) from \(\mathrm{H}_{2} \mathrm{O}\). (b) Calculate the \(\mathrm{pH}\) of a \(1.0 \times 10^{-7} M \mathrm{HCl}\) solution.
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