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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

Covalent compounds with 5 or 6 electron groups have equatorial and axial positions for surrounding elements

Equatorial and Axial Positions

Concept #1: Equatorial and Axial Positions

Example #1: Based on your knowledge of axial and equatorial positions, draw the most likely structure of PF2Cl3.

Concept #2: Lone Pair Positions

It's a lock as long as you remember the hands of the clock.

Example #2: Determine the molecular geometry for the following ion: SCl3.

Practice: Draw the most likely shape for the following compound: XeF4

Practice: Draw and determine the geometry for the following molecule: Br2CO

Practice: How many lone pairs reside in the equatorial position of the KrCl5ion.