2.3 Naming Ionic Compounds

Chad's General Chemistry Videos

Chapter 1 – Matter and Measure
- 1.1 Matter
- 1.2 Units, Conversions, and Significant Figures
Chapter 2 – Atoms, Molecules, Ions
- 2.1 Atomic Structure and Introduction to the Periodic Table
- 2.2 Classifying Compounds
- 2.3 Nomenclature of Ionic Compounds
- 2.4 Nomenclature of Molecular Compounds
- 2.5 Naming Acids
Chapter 3 – Stoichiometry
- 3.1 Reactions and Calculations With Moles
- 3.2 Mass Percents and Empirical and Molecular Formulas
- 3.3 Limiting Reagent Calculations
Chapter 4 – Aqueous Reactions
- 4.1 Solutions and Electrolytes
- 4.2 Double Displacement Reactions
- 4.3 Molarity, Solution Stoichiometry, and Dilutions
- 4.4 Oxidation Reduction Reactions
Chapter 5 – Thermochemistry
- 5.1 The First Law of Thermodynamics, Enthalpy, and Phase Changes
- 5.2 Calorimetry
- 5.3 Hess’s Law and Enthalpies of Formation
Chapter 6 – Electronic Structure
- 6.1 Electromagnetic Radiation and the Photoelectric Effect
- 6.2 Electronic Transitions Absorption and Emission
- 6.3 The de Broglie Relation, the Heisenberg Uncertainty Principle, and Orbitals
- 6.4 Quantum Numbers
- 6.5 Electronic Configurations
Chapter 7 – Periodic Trends
- 7.1 Overview of Trends and Atomic Radius
- 7.2 Ionization Energy
- 7.3 Electron Affinity, Electronegativity, and Descriptive Chemistry
Chapter 8 – Bonding and Lewis Structures
- 8.1 Bonding and Lattice Energy
- 8.2 Lewis Dot Structures
- 8.3 Bond Enthalpies
Chapter 9 – Molecular Geometry
- 9.1 VSEPR Theory and Molecular Geometry
- 9.2 Hybridization
- 9.3 Polarity
- 9.4 Sigma and Pi Bonds
- 9.5 Molecular Orbital Theory
Chapter 10 – Gases
- 10.1 Properties of Gases and the Ideal Gas Law
- 10.2 Gas Laws
- 10.3 Partial Pressures, Density, and the Volume of Ideal Gases at STP
- 10.4 Graham’s Law of Effusion and Real Gases
Chapter 11 – Liquids and Solids
- 11.1 Intermolecular Forces
- 11.2 Phase Diagrams
Chapter 13 – Solutions
- 13.1 Introduction to Colligative Properties, the van’t Hoff factor, and Molality
- 13.2 Calculations Involving Freezing Point Depression and Boiling Point Elevation
- 13.3 Vapor Pressure Depression and Raoult’s Law
- 13.4 Osmotic Pressure
Chapter 14 – Kinetics
- 14.1 Rates and Rate Expressions
- 14.2 Rate Laws
- 14.3 Mechanisms, Catalysts, and Reaction Coordinate Diagrams
- 14.4 Collision Theory and the Arrhenius Equation
- 14.5 Integrated Rate Laws and Half Lives
Chapter 15 – Equilibrium
- 15.1 Equilibrium and Equilibrium Constants
- 15.2 Le Chatelier’s Principle
- 15.3 Equilibrium Calculations
Chapter 16 – Acids and Bases
- 16.1 Introduction to Acids and Bases
- 16.2 Introduction to the pH Scale and pH Calculations
- 16.3 pH Calculations for Strong Acids and Bases
- 16.4 pH Calculations for Weak Acids and Bases
- 16.5 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 The 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 | Delta G = Delta H – T Delta S
- 18.4 Delta G, Delta H, Delta S and Formation Reactions
- 18.5 Gibbs Free Energy and the Equilibrium Constant
Chapter 19 – Electrochemistry
- 19.1 Oxidation Reduction Reactions and Oxidation States
- 19.2 Balancing Oxidation Reduction Reactions
- 19.3 Galvanic Cells
- 19.4 Standard Cell Potentials aka emf or Voltage
- 19.5 Nonstandard Cell Potentials the Nernst Equation
- 19.6 Reduction Potentials and the Relationship between 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 and Trends in Radioactivity
- 20.2 Balancing Nuclear Reactions
- 20.3 Routes of Nuclear Decay, Fission, and 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 Nomenclature of Complex Ions and Coordination Compounds
- 21.3 Isomers
- 21.4 Review of Electronic Configurations
- 21.5 Crystal Field Theory
- 21.6 Color
- 21.7 Magnetism

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Naming Ionic Compounds

1. Name the cation (metal or polyatomic cation).

2. State the metal’s oxidation state as a roman numeral in parenthesis.

(except Group I/II metals, Al³⁺, Zn²⁺, Cd²⁺, Ag⁺)

3. Name the non-metal with an -ide ending (or name the polyatomic anion).

Polyatomic Ions

SO₄^2- sulfate
SO₃^2- sulfite
NO₃^- nitrate
NO₂^- nitrite
PO₄^3- phosphate
CO₃^2- carbonate
HCO₃^- bicarbonate
OH^- hydroxide
MnO₄^- permanganate
CrO₄^2- chromate
Cr₂O₇^2- dichromate
NH₄⁺ ammonium
CN^- cyanide

ClO^- hypochlorite
ClO₂^- chlorite
ClO₃^- chlorate
ClO₄^- perchlorate

(for Br and I also)