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: You may want to reference (Pages 316 - 319) Section 8.5 while completing this problem.The following three Lewis structures can be drawn for N2O:The N–N bond length in N2O is 1.12 Å, slightly longer th

Problem

You may want to reference (Pages 316 - 319) Section 8.5 while completing this problem.

The following three Lewis structures can be drawn for N2O:
A nitrogen atom with one lone pair of electrons is bound by a triple bond to a second nitrogen atom with no lone pairs. This nitrogen atom is bound by a single bond to an oxygen atom with three lone pairs. This structure is in resonance with a structure that has a nitrogen atom with three lone pair of electrons bound by a single bond to a second nitrogen atom with no lone pairs. This nitrogen atom is bound by a single bond to an oxygen atom with one lone pairs. There is a third resonance contributor that has a nitrogen atom with three lone pair of electrons bound by a single bond to a second nitrogen atom with no lone pairs. This nitrogen atom is bound by a single bond to an oxygen atom with one lone pairs.
The N–N bond length in N2O is 1.12 Å, slightly longer than a typical N≡N bond; and the N–O bond length is 1.19 Å, slightly shorter than a typical N=O bond (see table below). Based on these data, which resonance structure best represents N2O?