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

See all sections
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: Bond Energy: C=C is 602 kJ/mol; C-H is 413 kJ/mol; O-H is 463 kJ/mol, O=O is 498 kJ/mol; C=O is 799 kJ/mol. For the combustion reaction of ethylene (C2H4) C2H4 + 3 O2 → 2 CO2 + 2 H2O assume all reac

Problem

Bond Energy: C=C is 602 kJ/mol; C-H is 413 kJ/mol; O-H is 463 kJ/mol, O=O is 498 kJ/mol; C=O is 799 kJ/mol. For the combustion reaction of ethylene (C2H4)

C2H4 + 3 O2 → 2 CO2 + 2 H2O

assume all reactants and products are gases, and calculate the ∆H 0rxn using bond energies.

1. −251 kJ/mol

2. −680 kJ/mol

3. 1300 kJ/mol

4. 680 kJ/mol

5. 0 kJ/mol

6. −1300 kJ/mol 

7. 251 kJ/mol