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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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: Which of the molecules or ions below will have the shortest nitrogen-oxygen bond?a. NO+b.NO2- c. NO3-


Which of the molecules or ions below will have the shortest nitrogen-oxygen bond?

a. NO+


c. NO3-


We are asked to determine the shortest nitrogen-oxygen bond among NO+NO2- and NO3-

We can use Bond Order to determine the length of a bond. Remember that the higher the bond order, the stronger the bond and therefore, the shorter the bond.

Let us draw the Lewis structures of each and its resonance structures and calculate for the average bond order of an N-O bond in all three molecules or ions. We must take note that the bond order of a molecule is the number of bonds between a pair of atoms. The formula we are going to use is:

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