Bonding and shapes of molecules

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  • Bonding
    • Metals
      • Makes a lattice work of positive ions surrounded by negative electrons
      • Conducts electricity because the electrons are free to move about through the metal.(delocalised)
      • Because the atoms are in sheets, this makes metallic bonds very durable and can slide over each other easily when not alloyed
    • Metal + Non-metals
      • Generally forms giant ionic lattices
        • These lattices comprise of positive ions surrounded by negative ions in a regular pattern
      • Conducts electricity when molten
        • This is because the ions are free to move about in the melted "soup"
    • Non-metal
      • Bonds between non-metals are described as covalent bonds
        • This is the sharing of electrons and therefore means that no ions are formed
      • Can be giant macromolecules
        • Examples are diamond, Graphite and silicon dioxide
        • Because the bonds are all covalent there are no intermolecular forces.
          • This means that they has an extremely high melting/boiling point
      • Or simple molecules
        • These generally have very little forces of attraction between them unless they at polar
          • Examples include CH4 and HCl
          • Polarity
            • A molecule is polar when there is a large difference in the electronegativity
              • The electronegativity of an element is a measure of the attraction between the electrons and the highly positive nucleus
      • Dative covalent bonds
        • Bonds whereupon the electrons are donated by only one of the atoms
          • E.G. NH4
        • E.G. NH4
    • Types of attraction
      • Permanant dipole-dipole
        • Where the molecule is simple and has a delta negative part and a delta positive point. E.G. HCl
      • Temporary dipole-dipole
        • Happens when electrons randomly get close to each other in the orbit and therefore create and temporary delta positive and delta negative part
      • Hydrogen Bonding
        • Only happens when hydrogen is bonded to Nitrogen, Oxygen and Fluorine
        • The end hydrogen of on molecule is delta positive so is attracted to the delta negative part of another molecule creating a strong bond of attraction
    • Polarity
      • A molecule is polar when there is a large difference in the electronegativity
        • The electronegativity of an element is a measure of the attraction between the electrons and the highly positive nucleus
    • Shape of molecules
      • Molecule shapes are defined by the number of bonds they make
      • Bond angles are defined by the number of bonds and if there are any lone pairs
        • Lone pairs are unused electrons that are in the outermost shell of the atoms that contains them

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