Ch.9 - Bonding & Molecular StructureWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Chemical Bonds
Lattice Energy
Lattice Energy Application
Born Haber Cycle
Dipole Moment
Lewis Dot Structure
Octet Rule
Formal Charge
Resonance Structures
Additional Practice
Bond Energy

Solution: Show resonance structures for acetate ion (CH 3CO2-)

Solution: Show resonance structures for acetate ion (CH 3CO2-)


Show resonance structures for acetate ion (CH 3CO2-)


We are being asked to identify the resonance structures of acetate ion (CH3CO2-). We will have to draw the Lewis Structure of CH3CO2- first.

Step 1: Determine the central atom in this molecule.

C and H are less electronegative than O but H can only make one bond
C is the central atom and is bonded to the other C atom

Step 2: Calculate the total number of valence electrons present.          


          Group              Valence Electrons

C         4A                    4 valence e x 2
H         1A                    1 valence e x 3
O         6A                    6 valence e- x 2
                                 = 23 valence e

-1 charge                     +1 e­-

 Total = 24 valence e- 

Step 3: Draw the Lewis Structure for the molecule

O and C → prefers to have complete octet (8 e- around them)

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