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: Which member of the following pairs would you expect to be more energetically stable? Justify each choice.a. NaBr or NaBr 2

Solution: Which member of the following pairs would you expect to be more energetically stable? Justify each choice.a. NaBr or NaBr 2

Problem

Which member of the following pairs would you expect to be more energetically stable? Justify each choice.

a. NaBr or NaBr 2

Solution

The more energetically stable compound is, the lower energy it has. We will look at how the compounds are formed to determine which is more stable. 

Comparing the two compounds, both NaBr and NaBr2 have ionic bonds. Ionic bond is formed from the transfer of valence electrons from a metal to a non-metal. In this case, Na is our metal and Br is our non-metal.

Let us determine the valence electrons of our metal and non-metal:

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