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Unit 2: Section 4 (part 2) - Reactions of ions in aqueous solution

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Total cards: 6•Content version: v4•Public deck•Updated: 8/1/2026

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#1
Front (Question)

Are 2+ ions or 3+ ions more acidic in solution? Why?

Back (Answer)

• 3+ ions are much more acidic • 3+ ions are smaller and more highly charged, so have a higher charge density • They attract the electrons from the oxygen of the ligands more strongly • This weakens the O-H bonds, so the complex readily releases a H+ ion into the solution, making it acidic

#2
Front (Question)

Write an equation for the hydrolysis of a 3+ ion to release a proton

Back (Answer)

[Fe(H2O)6]^3+(aq) ⇌ [Fe(H2O)5(OH)]^2+(aq) + H+(aq)

#3
Front (Question)

What kind of acid is the complex ion acting as? Why? [Fe(H2O)6]^3+(aq) ⇌ [Fe(H2O)5(OH)]^2+(aq) + H+(aq)

Back (Answer)

Bronsted-Lowry - donates a proton

#4
Front (Question)

Define a Lewis acid

Back (Answer)

Electron pair acceptor

#5
Front (Question)

Define a Lewis base

Back (Answer)

Electron pair donor

#6
Front (Question)

What is acting as the Lewis acid and what is acting as the Lewis base during the formation of complex ions?

Back (Answer)

The metal ion is acting at the Lewis acid and the ligands as Lewis bases