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
Electron Geometry
Bond Angles
Molecular Orbital Theory
MO Theory: Heteronuclear Diatomic Molecules
Additional Practice
Delocalized Electrons
Additional Guides
Molecular Geometry (ignored)
VSEPR Theory
Molecular Orbital Diagrams

molecular orbital diagram explains chemical bonds within molecules based on the union of atomic orbials. 

Concept #1: A heteronuclear diatomic molecule is composed of two different elements covalently bonded together.

Concept #2: There are some key similarities and differences when comparing heteronuclear and homonuclear diatomic molecules. 

Example #1: Using your knowledge of molecular orbital diagrams, determine the bond order of the NO- ion.