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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
Valence Shell Electron Pair Repulsion Theory
Equatorial and Axial Positions
Electron Geometry
Molecular Geometry
Bond Angles
Molecular Orbital Theory
MO Theory: Homonuclear Diatomic Molecules
MO Theory: Heteronuclear Diatomic Molecules
MO Theory: Bond Order

Molecular Orbital Diagrams can be used to determine the bond order of a molecule.

Bond Order

Concept #1: Bond Order is a measurement of the number of electrons involved in bonds between two elements.

Example #1: Determine the bond order of the NO ion.

Concept #2: Bond Order & Type of Bond

Example #2: Using MO Theory and bond order, determine the number of bonds connecting the nitrogen atoms within the N22– ion.

Practice: Apply Molecular Orbital Theory to determine the bond order of HHe+ ion.

Practice: Apply molecular orbital theory to predict which species has the strongest bond. 

a) O                            b) O2–                           c) O2+                          d) All the bonds are equivalent 

Practice: Using Molecular Orbital Theory, answer the following questions dealing with carbon mononitride, CN.