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: Use the molar bond enthalpy data in the table to estimate the value of change in Hrxn for the equation: CCl4 (g) + 2 F2 (g) yields CF4 (g) + 2 Cl2 (g). Average Molar bond enthalpies: (C-Cl) = 331 kJ/m

Solution: Use the molar bond enthalpy data in the table to estimate the value of change in Hrxn for the equation: CCl4 (g) + 2 F2 (g) yields CF4 (g) + 2 Cl2 (g). Average Molar bond enthalpies: (C-Cl) = 331 kJ/m

Problem

Use the molar bond enthalpy data in the table to estimate the value of change in Hrxn for the equation: CCl(g) + 2 F(g) yields CF(g) + 2 Cl(g). Average Molar bond enthalpies: (C-Cl) = 331 kJ/mol; (F-F) = 155 kJ/mol; (C-F) = 439 kJ/mol; (Cl-Cl) = 243 kJ/mol. 

Solution

To find the enthalpy of formation in terms of bond energies, use the equation:

$\Delta H_{rxn} = Bond \; energy\; of\; reactants - Bond \; energy \; of \; products $

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The first reactant has 4 C-Cl bonds. Each C-Cl bond has a bond enthalpy of $331 kJ/mol.$

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