Ch.10 - Molecular Shapes & Valence Bond TheoryWorksheetSee 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

Solution: Use molecular orbital theory to predict whether or not each of the following molecules or ions should exist in a relatively stable form.Ne2

Solution: Use molecular orbital theory to predict whether or not each of the following molecules or ions should exist in a relatively stable form.Ne2

Problem

Use molecular orbital theory to predict whether or not each of the following molecules or ions should exist in a relatively stable form.

Ne2

Solution

Recall: The bond order determines the stability of a molecule based on it's molecular orbital diagram.

A positive bond order means there are more electrons in the bonding molecular orbitals than in antibonding molecular orbitals, which means the molecule can exist in a relatively stable form. The greater the bond order, the stronger the bond.

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