Chapter 15: Problem 25
Define Lewis acid and Lewis base.
Short Answer
Step by step solution
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Chapter 15: Problem 25
Define Lewis acid and Lewis base.
These are the key concepts you need to understand to accurately answer the question.
All the tools & learning materials you need for study success - in one app.
Get started for freeAluminum chloride, \(\mathrm{AlCl}_{3}\), forms molecules with itself with the formula \(\mathrm{Al}_{2} \mathrm{Cl}_{6}\). Its structure is Use Lewis structures to show how the reaction \(2 \mathrm{AlCl}_{3} \longrightarrow\) \(\mathrm{Al}_{2} \mathrm{Cl}_{6}\) is a Lewis acid-base reaction.
The ion \(\mathrm{Hg}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{2+}\) acts as an acid. Write an equation showing its behavior as a Brønsted-Lowry acid in water.
\(\mathrm{HClO}_{4}\) is a stronger proton donor than \(\mathrm{HNO}_{3}\), but in water both acids appear to be of equal strength; they are both \(100 \%\) ionized. Why is this so? What solvent property would be necessary in order to distinguish between the acidities of these two Brønsted-Lowry acids?
Sodium hydroxide, \(\quad \mathrm{NaOH},\) is basic. Aluminum hydroxide, \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3}(\mathrm{OH})_{3},\) is amphoteric. The compound \(\mathrm{O}_{3} \mathrm{ClOH}\) (usually written \(\mathrm{HClO}_{4}\) ) is acidic. Considering that each compound contains one or more OH groups, why are their acid-base properties so different?
Explain why the addition of a proton to a water molecule to give \(\mathrm{H}_{3} \mathrm{O}^{+}\) can be considered a Lewis acid-base reaction.
What do you think about this solution?
We value your feedback to improve our textbook solutions.