Structure & Bonding

    Cards (29)

    • Ionic bonding - metals + non metals
      Electrostatic attraction between oppositely charged ions
    • What are cations?
      Positively charged ions
    • What are anions?
      Negatively charged ions
    • Covalent bonding - non metal + non metal
      Electrostatic attraction between a shared pair of electrons + two nuclei
    • Metallic bonding - two metals
    • Ionic compound structure
      Giant ionic lattice
    • Mp + Bp of giant ionic lattices
      High
    • Electric conductivity of giant ionic lattices
      Only when molten or aqueous as ions are able to move around and carry a charge. Ions are fixed in place during solid form.
    • Solubility of giant ionic lattices
      Often soluble
    • Higher charge = higher mp and bp in giant ionic lattices
    • Most covalent bonds are simple molecular structures
    • Are covalent bones strong or weak?
      Strong
    • Are intermolecular forces in covalent bonds strong or weak?
      Weak
    • Where are intermolecular forces found? (covalent bonding)
      Between adjacent molecules
    • Melting and boiling points of simple covalent substances
      Low - intermolecular forces are weak and little energy is needed to overcome them
    • Electricity conductivity of simple molecular substances
      Insulator - can't conduct - no ions or delocalised electrons
    • Solubility of simple covalent substances
      Insoluble -molecules are neutral so water molecules aren't attracted to them
    • Giant covalent exceptions:
      • Diamond
      • Graphite
      • Silicon dioxide
    • Structure of metallic bonding
      Giant metallic lattices
    • Metallic bonding
      Electrostatic attraction between the metal cations and the delocalised electrons
    • Metallic bonding:
      A) delocalised electrons
      B) metal ions
    • Covalent bonding:
    • Ionic bonding:
    • Density of metallic bonds
      High - particles are closely packed together in a regular arrangement
    • Mp + Bp of metals
      High - a lot of energy is required to break the strong electrostatic attractions between the cations and delocalised electrons.
    • What is an alloy?
      A mixture of two or more elements, at least one of which is a metal.
    • Metal conductivity
      Good conductor - lots of delocalised electrons to move around and carry a charge
    • Why are metals malleable?
      Layers of cations can slide over each other
    • What happens to substances when they are heated?
      They expand (gases can also increase pressure)
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