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CHEMISTRY BONDING - Coggle Diagram

- - - - contain hexagonal rings in a cylindrical tube shape
      - have very high length to diameter ratios
      - each carbon is ended to 3 others
      - can conduct electricity as the free electron can carry charge and flow through the structure
      - can be used in computers or wiring in aircrafts, tennis rackets and bike frames
- - - - diamond - very hard as it has a giant elastic structure with 4 covalent bonds between carbon atoms. there are no free elections and can't conduct electricity
      - graphite - each carbon atoms forms 3 covalent bonds which forms layers of hexagonal rings that have weak forces of attraction between them. the means that the layers can slide over each other. graphite is soft and slippery and can conduct electricity as there are free/delocalised electrons
      - Silicon dioxide (silica) - hard due to its giant lattice structure an death silicon atoms is bonded to 2 oxygen atoms and can't conduct electricity due to no free electrons
      - all 3 have high melting and boiling point as they are all joined by covalent bonds which require lots of energy to break
- - - - this is a bond between one metal and a non-metal and involves the sharing of electrons and are bonded together due to the oppositely charges ions pulling each other together
      - electrons are transferred from the metal atom and given to the non metal. metal becomes a positive charged ion while the non metal becomes a negative charged ion
      - these bonds are held together by the opposites charges producing an electrostatic force of attraction
      - show these bonds by drawing the new electron configuration and put square brackets around them with the charge at the top right
      - .
        
        structure snd properties
        
        ionic compounds are giant lattice structures that are held together by strong electrostatic forces of attraction between oppositely charges molecules and this acts in all directions
        
        they have a high melting point and boiling point as lots of energy is needed to break these bonds apart
        
        they can't conduct electricity when solid as the ions are in a fixed position and cannot more (no free electrons)
        
        if molten or dissolved in water they can conduct electricity as the ions are free to move and allow for the flow of charge
    - - this is a bond between a non metal and a non metal and involves sharing pairs of electrons nd both the atoms being attached together
      - these bond are strong and molecules are covalent bonds
      - examples of the is H2O where hydrogen has one electron and oxygen have 6 on its outer shell and needs one more os it bonds with 2 hydrogen. both hydrogen share its electron with oxygen and become attached together
      - a single bond is when one pair of electrons are shared, a double bond is when 2 pairs of electrons are shared (e.g O2) and a triple bond is when 3 pairs of electron are shared (e.g N2)
    - - metals are giant structures of ions and atoms and electrons in the outer shell are delocalised and free to move which forms a sea of delocalised electrons which holds the metal ions together and makes strong metallic bonds
      - they can conduct electricity as the free electrons can carry charge through the metal
      - good conductors of heat energy as the energy is transferred through the free electrons
      - in pure metals, the atoms are arranged in layers so they can slide over which means they can be bend and change in shape
      - alloys
        
        harder than pure metals
        
        can be a mixture of metals or a mixture of a metal and a non metal
        
        layer are distorted by other atoms so they can't slide over each other