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

Bond Energy

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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: Predict whether the N-O bonds in NO3- are stronger or weaker than the N-O bond in NO+.

Solution: Predict whether the N-O bonds in NO3- are stronger or weaker than the N-O bond in NO+.

Problem

Predict whether the N-O bonds in NO3- are stronger or weaker than the N-O bond in NO+.

Solution

We have to predict if the N–O bonds in NO3- are stronger or weaker than the N–O bonds in NO+.


To solve this problem, we need the Lewis structure and resonance forms for the NO3- and NO+ ions.

resonance structure shows the delocalization of electrons in a molecule.

Resonance structures differ only in the placement of electrons over the atoms in the molecule.


We will be following these steps:

Step 1: Determine the central atom in the molecule.

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

Step 3: Draw the Lewis structure for the molecule.

Step 4: Draw the resonance structures.

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