Properties of Ionic, Covalent, and Metallic Compounds

Flashcards covering the properties of ionic, covalent, and metallic compounds, including bonding, structure, volatility, solubility, melting/boiling points, electrical conductivity, and malleability.

Ionic Compounds

Bonding between a nonmetal and a metal.

Covalent Compounds

Bonding between a nonmetal and a nonmetal.

Metallic Compounds

Bonding between a metal and a metal.

Ionic Compound Bond Strength

Strongest bond strength among ionic, covalent, and metallic compounds.

Covalent Compound Bond Strength

Strong, but usually weaker than ionic and metallic compounds.

Metallic Compound Bond Strength

Strong, but usually weaker than ionic compounds.

Ionic Compounds at Room Temperature

Solid.

Covalent Compounds at Room Temperature

Usually liquid or gas.

Metallic Compounds at Room Temperature

Solid.

Ionic Bond Formation

Electrons are transferred from one atom to another.

Covalent Bond Formation

Electrons are shared between two atoms, usually in pairs.

Metallic Bond Formation

Outer electrons are given to create a delocalized sea of electrons.

Ionic Lattice Structure

A regular arrangement of alternating positive and negative ions.

Covalent Lattice Structure

Made up of individual molecules held together by weak intermolecular forces.

Metallic Lattice Structure

A structure of cations in a sea of delocalized electrons.

Volatility

How easily a substance evaporates into a gas.

Ionic Compound Volatility

Usually not volatile, do not evaporate easily due to strong electrostatic attraction.

Covalent Compound Volatility

Usually volatile, easily evaporate due to weak intermolecular (Van der Waals) forces.

Metallic Compound Volatility

Usually not volatile, do not evaporate easily due to electrostatic attraction.

Ionic Compound Solubility in Water

Usually soluble in water.

Covalent Compound Solubility in Water

Usually not soluble in water.

Metallic Compound Solubility in Water

Usually not soluble in water.

Ionic Compound Melting and Boiling Points

High due to strong electrostatic attraction.

Covalent Compound Melting and Boiling Points

Low due to weak intermolecular (Van der Waals) forces.

Metallic Compound Melting and Boiling Points

High due to strong electrostatic attraction.

Ionic Compound Electrical Conductivity

Conduct electricity when melted or dissolved, but not in the solid state.

Covalent Compound Electrical Conductivity

Do not conduct electricity because they don't involve charged particles (atoms share electrons and stay neutral).

Metallic Compound Electrical Conductivity

Can conduct electricity as solid or when melted due to delocalized electrons that are free to move.

Ionic Compound Malleability

Brittle due to rigid ionic lattice; force disrupts organization and causes breakage.

Covalent Compound Malleability

Soft since lattices are held together by weak intermolecular forces.

Metallic Compound Malleability

Malleable because layers of atoms can slide or slip over each other; delocalized electrons allow reformation of lattice.