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: From the bond energies given below, estimate the ΔH° for the reaction:H2(g) + I2(g) → 2HI(g)Bond energies (kJ/mol):H–H = 436H–I = 297I–I = 151


From the bond energies given below, estimate the ΔH° for the reaction:

H2(g) + I2(g) → 2HI(g)

Bond energies (kJ/mol):
H–H = 436
H–I = 297
I–I = 151


To calculate the ΔH°rxn using bond energies, we’re going to use the following equation:

Horxn = Hbond reactants - Hbond products

Let’s first figure out what kind of bonds and how many moles are present in each reactant and products because the given bond energies are per mole.

Balanced Reaction:  H2(g) + I2(g) → 2 HI(g)

*always make sure that the given reaction is balanced

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