How To Draw Lewis Dot Structures (Easiest Method) - Chad's Prep®

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Chapter 1 – Matter and Measurement
- 1.1 Matter
- 1.2 Significant Figures
- 1.3 Units and Conversions
Chapter 2 – Atoms, Molecules, and Ions
- 2.1 Atomic Structure and Introduction to the Periodic Table
- 2.2 Naming Ionic Compounds
- 2.3 Naming Molecular Compounds
- 2.4 Naming Acids
Chapter 3 – Stoichiometry
- 3.1 Chemical Reactions & Chemical Equations
- 3.2 Calculations With Moles
- 3.3 Mass Percent and Empirical and Molecular Formulas
- 3.4 Limiting Reagent Calculations
Chapter 4 – Aqueous Reactions and Solution Stoichiometry
- 4.1 Solutions and Electrolytes
- 4.2 Double Displacement Reactions
- 4.3 Oxidation-Reduction Reactions
- 4.4 Molarity and Dilutions
- 4.5 Solution Stoichiometry
Chapter 5 – Thermochemistry
- 5.1 First Law of Thermodynamics and Enthalpy
- 5.2 Calorimetry
- 5.3 Hess’s Law and Enthalpies of Formation
Chapter 6 – Electronic Structure
- 6.1 Nature of Light and the Photoelectric Effect
- 6.2 Electronic Transitions (Absorption and Emission)
- 6.3 The de Broglie Relation and the Heisenberg Uncertainty Principle
- 6.4 Quantum Numbers and Atomic Orbitals
- 6.5 Electronic Configuration
Chapter 7 – Periodic Trends
- 7.1 Atomic Radius
- 7.2 Ionization Energy
- 7.3 Electron Affinity & Electronegativity
- 7.4 Properties of Elements & Compounds
Chapter 8 – Bonding and Lewis Structures
- 8.1 Ionic Bonding
- 8.2 Lewis Dot Structures
- 8.3 Bond Enthalpy
Chapter 9 – Molecular Geometry
- 9.1 VSEPR Theory and Molecular Geometry
- 9.2 Polarity
- 9.3 Hybridization
- 9.4 Sigma and Pi Bonds
- 9.5 Molecular Orbital Theory
Chapter 10 – Gases
- 10.1 Properties of Gases
- 10.2 Gas Laws Including the Ideal Gas Law
- 10.3 Additional Gas Laws
- 10.4 Real Gases & the Van der Waals Equation
Chapter 11 – Intermolecular Forces, Liquids, and Solids
- 11.1 Intermolecular Forces
- 11.2 Phase Diagrams
- 11.3 Structures of Solids
Chapter 13 – Solutions
- 13.1 Solution Formation and Solubility
- 13.2 Units of Concentration
- 13.3 Colligative Properties
Chapter 14 – Kinetics
- 14.1 Rate Expressions and the Rate of Reaction
- 14.2 Rate Laws
- 14.3 Reaction Mechanisms, Catalysts, and Reaction Coordinate Diagrams
- 14.4 Collision Theory and the Arrhenius Equation
- 14.5 Integrated Rate Laws
Chapter 15 – Equilibrium
- 15.1 Equilibrium and Equilibrium Constants
- 15.2 Le Chatelier’s Principle
- 15.3 Equilibrium Calculations (ICE Tables)
Chapter 16 – Acids and Bases
- 16.1 Introduction to Acids and Bases
- 16.2 Binary Acids, Oxoacids, and Polyprotic Acids
- 16.3 Introduction to the pH Scale and pH Calculations
- 16.4 pH Calculations for Strong Acids and Bases
- 16.5 pH Calculations for Weak Acids and Bases
- 16.6 Acidity and Basicity of Salts
Chapter 17 – Buffers, Titrations, and Solubility
- 17.1 Buffers
- 17.2 Titrations and Titration Curves
- 17.3 pH Calculations Involving Titrations
- 17.4 Solubility and Ksp
- 17.5 Common Ion Effect and Precipitation
- 17.6 pH Effects on Solubility
Chapter 18 – Thermodynamics
- 18.1 The Laws of Thermodynamics
- 18.2 Entropy
- 18.3 Gibbs Free Energy and the Relationship between ΔG, ΔH, & ΔS
- 18.4 ΔG, ΔH, ΔS, and Formation Reactions
- 18.5 Gibbs Free Energy and the Equilibrium Constant
Chapter 19 – Electrochemistry
- 19.1 How to Assign Oxidation Numbers
- 19.2 How to Balance Oxidation Reduction Reactions
- 19.3 Galvanic Cells
- 19.4 How to Calculate Standard Cell Potential
- 19.5 How to Calculate Nonstandard Cell Potential [Nernst Equation]
- 19.6 Cell Potential, Delta G, and the Equilibrium Constant
- 19.7 Electrolytic Cells
- 19.8 Electrolysis Calculations
Chapter 20 – Nuclear Chemistry
- 20.1 Introduction to Nuclear Chemistry
- 20.2 Balancing Nuclear Reactions
- 20.3 Spontaneous Routes of Nuclear Decay, Fission, & Fusion
- 20.4 Kinetics of Nuclear Decay
- 20.5 Energy of Nuclear Reactions and Nuclear Binding Energy
Chapter 21 – Coordination Chemistry
- 21.1 Introduction to Coordination Chemistry
- 21.2 Naming Complex Ions and Coordination Compounds
- 21.3 Isomers in Coordination Chemistry
- 21.4 Crystal Field Theory
- 21.5 Color & Paramagnetism of Coordination Compounds

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8.1 Ionic Bonding

8.3 Bond Enthalpy

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Octet Rule

The octet rule states that most atoms will transfer electrons (ionic bonding) or share electrons (covalent bonding) to obtain a total of 8 electrons in its valence shell.

OCTET RULE EXCEPTIONS
1. A few atoms routinely go under the octet rule H only 2 Be only 4 B and Al only 6
2. Third row and lower can exceed the octet rule
3. Molecules with odd numbers of electrons (ex. NO)

How to Draw Lewis Structures

Rules for Drawing Lewis Structures
1. Set up skeleton with single bonds (central atom is the atom which can make the most bonds).
2. Fill the octets of the outside atoms with lone pairs of electrons.
3. Any remaining valence electrons go on central atom.
4. Once all electrons are used, form multiple bonds to the central atom if not “full.”