Ch.9 - Bonding & Molecular StructureWorksheetSee 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
Lewis Dot Symbols
Chemical Bonds
Dipole Moment
Octet Rule
Formal Charge
Lewis Dot Structures: Neutral Compounds
Lewis Dot Structures: Sigma & Pi Bonds
Lewis Dot Structures: Ions
Lewis Dot Structures: Exceptions
Lewis Dot Structures: Acids
Resonance Structures
Average Bond Order
Bond Energy
Coulomb's Law
Lattice Energy
Born Haber Cycle
Additional Practice
Lewis Dot Structure: Formal Charge

Dipole arrows are used anytime a molecule possesses a dipole moment, which happens when a molecule is polar. 

Dipole Moments & Arrows

Concept #1: Periodic Trend

Example #1: Calculate the difference in electronegativity values between carbon and fluorine.

Practice: Arrange the following molecules in order of decreasing dipole moment.

H–I           H–F         H–Br         H–Cl

Concept #3: Further Chemical Bond Classifications

Example #2: For those listed below, which has the most polar bond?

Practice: Which of the following correctly identifies the chemical bond between a carbon and oxygen atom?

a) Polar Covalent

b) Pure Covalent

c) Nonpolar 

d) Ionic