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
Sections
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: Does a chlorate ion have resonance structures?

Problem

Does a chlorate ion have resonance structures?

Solution

We are asked to determine if chlorate ion has a resonance structure


• Chlorate ion is a polyatomic anion with a formula ClO3-

Recall:

          • the suffix ‘ide’ is used to refer to monoatomic anions

          • the suffix ‘ite’ is used to refer to oxyanion with the lower oxidation state

          • the suffix ‘ate’ is used to refer to the oxyanion in the higher oxidation state


First, we must draw the  Lewis structure for ClO3-

• We need to determine the total number of valence electrons present:

ClO3-

           Group            Valence Electrons

Cl       7A                   1 × 7 e = 7 e

O        6A                   3 × 6 e = 18 e

                                + 1 e-

Total:  26 valence e


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