Chemical Bonding and Solid Types
Overview of covalent, ionic, and metallic bonding and solid properties.
Chemical Bonding and Solid Types
Covalent Bonds: formed between two non-metals; electrons are shared; ΔEN is relatively low (e.g., Sugar, Water).
Ionic Bonds: formed between a metal and a non-metal; electrons are transferred; ΔEN is large (e.g., NaCl, CaCl2).
Metallic Bonds: formed between two metals; electrons are delocalized; ΔEN is low (e.g., Steel, Brass).
Metallic Solids: held by metallic bonds; varying strength; high boiling point, malleable, ductile, conducts electricity (e.g., Bronze, Gold).
Molecular Solids: held by IMFs; very weak strength; low boiling point, non-conductive, brittle (e.g., Ice, Sucrose).
Ionic Solids: held by ionic bonds; strength determined by lattice energy; high boiling point, brittle, non-conductive as solid, conductive when liquid or aqueous (e.g., NaCl, MgO).
Network Covalent Solids: held by covalent bonds; very strong; extremely high boiling point, rigid, non-conductive (e.g., Diamond, Graphite, Quartz).
