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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
Sections
Valence Shell Electron Pair Repulsion Theory
Equatorial and Axial Positions
Electron Geometry
Molecular Geometry
Bond Angles
Hybridization
Molecular Orbital Theory
MO Theory: Homonuclear Diatomic Molecules
MO Theory: Heteronuclear Diatomic Molecules
MO Theory: Bond Order
Additional Guides
Molecular Geometry (IGNORE)
VSEPR Theory

Bond Angles result from surrounding elements and lone pairs around the central element positioning themselves at an optimal distance. 

 Bond Angles

Concept #1: Ideal Bond Angles

Ideal Bond Angle is the optimal angle elements take in order to minimize repulsion.

Example #1: If the H–C–H angle within the CH4 molecule is 109.5º, what is the H–N–H bond angle within NH3?

The more lone pairs on the central element, the more compressed the bond angle, and the greater the deviation from an ideal bond angle.

Concept #2: Bond Angles and Electron Groups.

Example #2: Determine the F–I–F bond angle for the following ion: IF4.

Practice: Determine the bond angle for the thiocyanate ion, SCN.

Practice:  In the PCl­3F2 molecule the chlorine atoms exist in the equatorial positions and the fluorine atoms exist in the axial positions. Based on this information, predict the Cl–P­–Cl bond angle.

Practice: Determine the O–N–O bond angle for N­2O4, which exists as O2N–N­O­2.