Ionic vs Molecular Compounds

Introduction

• Objective: Understand the differences between ionic and molecular (covalent) compounds.
• Method: Learn classification based on elements and explore key differences between the two.

Classification of Compounds

• Ionic Compounds: Composed of metals and non-metals.
• Molecular (Covalent) Compounds: Composed of only non-metals.

Determining Type

• Periodic Table: Use the "staircase" line to differentiate metals (left) and non-metals (right).

Examples

• Sulfur Dioxide (SO2): Molecular (Sulfur & Oxygen are non-metals).
• Sodium Chloride (NaCl): Ionic (Sodium is a metal, Chlorine is a non-metal).
• Water (H2O): Molecular (Hydrogen, though on the metals side, is a non-metal along with Oxygen).
• Copper Fluoride: Ionic (Copper is a metal, Fluoride is a non-metal).
• Propanol: Molecular (Composed of Carbon, Hydrogen, and Oxygen - all non-metals).
• Lithium Nitrate: Ionic (Contains Lithium, a metal, and non-metals Nitrogen and Oxygen).
• Sodium Sulfate: Ionic (Contains Sodium, a metal, and non-metals Sulfur and Oxygen).

Polyatomic Ionic Compounds

• Definition: Ionic compounds with multiple non-metals.

Differences Between Ionic and Molecular Compounds

Bonding

• Molecular (Covalent): Atoms share electrons (example: H2O).
  • Atoms are like holding hands by sharing electrons.
• Ionic: One atom transfers electrons to another, leading to opposite charges that attract (example: NaCl).
  • Chlorine steals an electron from Sodium, creating Na⁺ and Cl⁻.

Structural Differences

• Molecular Compounds: Form molecules, which are clumps of atoms stuck together (example: sugar molecules).
• Ionic Compounds: Form lattice structures, organized, box-like shapes (example: salt lattice).

Dissolving in Water

• Molecular Compounds: Break into individual molecules.
• Ionic Compounds: Break into individual ions.

Additional Resources

• Videos available on physical properties and dissolution processes of ionic and molecular compounds.