Covalent Bonding

HideShow resource information
View mindmap
  • Covalent Bonding
    • 2 Non-Metals
      • The atoms/single elements share electrons
        • Each shared pair of electrons strongly attract the atoms together - A Covalent Bond
          • However atoms of some elements can form several covalent bonds
            • Called Giant Covalent Structures
              • There ae no intermolecular forces just covalent bonds
                • So they have a very high melting and boiling point. A lot of energy is needed to break down the lattice
              • Diamond
                • Each carbon atom forms four covalent bonds
                  • Very hard
                • 3-D so is transparent
              • Silicon Doxide (Similar properties to diamond)
                • Diamond
                  • Each carbon atom forms four covalent bonds
                    • Very hard
                  • 3-D so is transparent
              • Graphite
                • Covalently bonded to three other carbon atoms
                • Flat 2-D layers that slide
                  • No covalent bonds between layers: Weak intermolecular
                    • They slide over each other
                      • Used in pencils as layers slide to leave a mark and in lubricants
                • Has one delocalised electron so can conduct heat and electricity
                  • This is because it bonds covalently 3 times so has a spare electron (delocalised) to carry a charge
              • Fullerenes
                • Large molecules formed from £-D hexagonal rings of carbon
                  • Some are nano-sized and used for drug delivery in the body, lubricants, reinforcing metals

Comments

No comments have yet been made

Similar Chemistry resources:

See all Chemistry resources »See all Structure and bonding resources »