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: Formation of the H2 molecule as atomic orbitals overlap. From the graph, what is the bond length in the H2 molecule?

Problem

A line graph has H-H distance on the X-axis (increasing), and energy (kilojoules per mole) on Y-axis (increasing).  At very short distances, the nucleus-nucleus repulsion is increasingly important.  As the distance increases, the energy rapidly drops; the potential energy decreases with increasing orbital overlap.  The energy decreases far below zero, reaching a minimum of negative 435 kilojoules per mole at an H-H distance of 0.74 angstroms. This point is the balance between attractive and repulsive forces. As the distance then increases further, the potential energy slowly increases, toward an asymptote with 0 kilojoules per mole.

Formation of the H2 molecule as atomic orbitals overlap.

From the graph, what is the bond length in the H2 molecule?