Types of Solids

Metallic Solids

• Bond: Bonded together by metallic bonds.

  • Electrostatic attractions between delocalized electrons and metal ions. 

• Molecular Structure: Lattice of metal cations surrounded by a "sea" of delocalized electrons.

• Melting Point: Variable depending on the element or alloy, but it is generally high. 

• Conductivity: Effective conductors of electricity and heat. 

• Solubility: Insoluble in most solvents. 

• Physical Properties: Malleable, ductile, has luster. 

Examples: Iron ingots (Fe), aluminum foil (Al), copper rods (Cu). 

Ionic Solids

• Bond: Bonded together by ionic bonds.

  • Electrostatic attractions between ions of opposite charges. 

• Molecular Structure: Crystal lattice. 

• Melting Point: High

• Conductivity: Not conductive. 

  • Effective conductors of electricity in aqueous or liquid phases. 

• Solubility: Generally soluble in most polar solvents. 

• Physical Properties: Brittle. 

Examples: Table salt (NaCl), rust (Fe₂O₃), calcium carbonate (Ca₂CO₃). 

Covalent Network Solids

• Bond: Bonded together by covalent bonds.

  • The sharing of valence electrons between atoms. 

• Molecular Structure: Crystal lattice. 

• Melting Point: High

• Conductivity: Not conductive. 

  • An exception is graphite, which is conductive due to the presence of delocalized electrons. 

• Solubility: Insoluble in most solvents. 

• Physical Properties: Hard and brittle. 

Examples: Graphite (C), sand (SiO₂), diamond (C). 

Molecular Solids

• Bond: Bonded together by covalent bonds.

  • The sharing of valence electrons between atoms. 

• Molecular Structure: Amorphous or crystalline. 

• Melting Point: Low

• Conductivity: Not conductive. 

• Solubility: Depends on the polarity of the solid and the solvent. 

• Physical Properties: Generally softer than other types of solids. 

Examples: Ice (H₂O), dry ice (CO₂), glucose (C₆H₁₂O₆).