Covalent Bonding

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  • Covalent Bonding
    • Enthalpy
      • + nuclei are attracted to e- densite. + nuclei also repel each other
      • The distance between the 2 nuclei is where attractive and repulsive forces are balances
      • Higher electron density = stronger attraction between atoms & lower bond length
    • Evidence
      • Good thermal conductors = vibrations easily travel through lattice
      • Often very hard = strong bonds in the lattice
      • Insoluble = covalent bonds mean atoms are more attracted to atoms in the lattice than the solvents
      • High melting points = need to break a lot of bonds to melt it
      • Can't conduct electricity = no free charged ions or electrons
    • Bonding
      • 2 atoms share electrons so they both have full outer shells
      • The strong electrostatic attraction between the bonding nuclei and the electrons in the bonds
    • Giant Structures
      • Each atom is covalently bonded to other atoms in the structure
      • Have a network of covalently bonded atoms = high electrostatic attraction
      • Covalent bonding can form simple structures or giant lattices
    • Dative Bonds
      • One atom donates both electrons to a bond
      • Ammonium ions are formed by dative covalent bonds. Nitrogen atom donates a pair of e- to H+
    • Graphite
      • Carbon atoms form sheets
      • Each carbon atom shares 3 e- with other atoms in structure, 4th can move between sheets
      • One sheet = joined in hexagons & 1 atom thick
      • Can conduct as delocalised electrons can move along the sheet
      • Incredibly strong, transparent and light

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