17. Acid and Base Equilibrium

Lewis Acid and Base

Acids and Bases, pH and pOH

Identify each of the compounds in the following chemical equation

16.1 Introduction to Acids and Bases | General Chemistry

If the central element has less than 8 valence electrons around it then it is more likely to accept an electron pair to follow the octet rule.&#160;

In the 1920s, Gilbert Lewis proposed a new set of definitions for acids and bases.&#160;

When hydrogen is connected to an electronegative element such as P, O, N, S or halogens then it gains a partially positive charge, which makes hydrogen act as a Lewis acid.&#160;

Compounds that have lone pair(s) on a central element can act as Lewis bases.&#160;

Classify each species as either a Lewis acid or a Lewis base.
b. OH

The fluoride ion reacts with water to produce HF. (c) Is fluoride acting as a Lewis acid or as a Lewis base when reacting with water?

Conjugate Acid Base Pairs, Arrhenius, Bronsted Lowry and Lewis Definition - Chemistry

Understanding Lewis Bases

Look at the electron-dot structures of the following molecules 
and ions: 
 
(b) Which can behave as a Lewis acid? Which can behave as 
a Lewis base?

Acid-base definitions | Chemical processes | MCAT | Khan Academy

Which would you expect to be the stronger Lewis acid in
each of the following pairs? Explain.
(a) BF3 or BH3

Classify each of the following as a Lewis acid or a Lewis
base.
(e) OH-

Identify the Lewis acid and Lewis base from among the reactants
in each equation.
b. AlBr3 + NH3H3NAlBr3

Understanding Lewis Acids

Compounds that possess a negative charge can act as Lewis Bases.&#160;

Classify each species as either a Lewis acid or a Lewis base.
a. BeCl2

Identify the Lewis acid and Lewis base among the reactants in each of the following reactions: 
(d) HIO1lq2 + NH2-1lq2 Δ NH31lq2 + IO-1lq2(lq denotes liquid ammonia as solvent)

Identify the Lewis acid and Lewis base from among the reactants
in each equation.
a. Ag+(aq) + 2 NH3(aq)Ag(NH3)2+(aq)

Classify each species as either a Lewis acid or a Lewis base.
c. B(OH)3

a) H+:acid, OH-:base; b) Cl-:acid, BCl3:base; c)SO3:acid, H2O:base

a) H+:base, OH-:acid; b) Cl-:acid, BCl3:base; c)SO3:base, H2O:acid

a) H+:acid, OH-:base; b) Cl-:base, BCl3:acid; c)SO3:acid, H2O:base

a) H+:acid, OH-:base; b) Cl-:base, BCl3:acid; c)SO3:base, H2O:acid

Identify the Lewis acids and bases in the following reactions.a) H+ + OH– ⇌ H2Ob) Cl– + BCl3 ⇋ BCl4–c) SO3 + H2O ⇌ H2SO4

Since these metal ions&#160;accept negative electron pairs then some Lewis Acids may be positively charged.&#160;

Consider the reaction: SO2 + OH- S HSO3
-. Which reaction scheme shows the correct use of the curved arrow notation representing the
donation of an electron pair and the correct labeling of the Lewis acid and Lewis base? (LO 16.14)
(a) 
(b) 
(c) 
(d)

Identify the Lewis acid and Lewis base in each of the following reactions: 
(b) FeBr31s2 + Br-1aq2 Δ FeBr4-1aq2

According to the Lewis definition an acid is an electron pair acceptor.&#160;

Identify each of the following compounds as either a Lewis acid, a Lewis base or neither.a) &nbsp;ZnCl2&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;b)&nbsp; CN&nbsp;–&nbsp;c)&nbsp; NH4+&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;d) Co3+

According to the Lewis definition a base is an electron pair donor.&#160;

Acid/Base Concepts

Identify the Lewis acid and Lewis base from among the reactants
in each equation.
a. Fe3 + (aq) + 6 H2O(l )Fe(H2O)63+(aq)

Classify each species as either a Lewis acid or a Lewis base.
d. CN-

 These species differ by more than just a proton. 

HNO2 / NO2&#8211;

 Correct combination - which differ only by one proton. 

H2CO3 / OH&#8211;

HC2H3O2 / H2O

 A conjugate acid&#8211;base pair will differ by only one proton. 

 Which of the following illustrates a conjugate acid&#8211;base pair? 

Which member of each pair produces the more acidic aqueous solution: (b) CuCl or Cu1NO322

Lewis Acids and Bases

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Ionic Salts

Polyprotic Acid

A&#160;polyprotic acid&#160;possesses more than 2 hydronium ions (H+).&#160;

Diprotic Acid

A diprotic acid&#160;is an acid that can donate two hydronium ions (H+).&#160;

Identifying Acids and Bases

Arrhenius Acid and Base

Bronsted Lowry Acid and Base

Amphoteric

pH and pOH

Ka and Kb

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