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Chemical Bonds - Coggle Diagram

- - - - Each Carbon forms 4 STRONG covalent bonds to other atoms
        
        Strong bonds in all directions
        
        Very Hard
        
        Very high melting (+ boiling) point
        
        Used for: cutting tools + drill bits
      - All Electrons Used to bond
        
        No free electrons
        
        Does NOT conduct heat/electricity
    - - Each Carbon forms 3 STRONG covalent bonds to other atoms
        
        1 other electron in each atom (not used for covalent bonding)
        
        lost to a SEA OF DELOCALISED ELECTRONS
        
        SEA OF DELOCALISED ELECTRONS present
        
        very good electrical conductor
        
        Used for: Electrodes
        
        (As only 3 covenant bonds)
        
        Contrast - 4 in diamond - where all electrons are used in covalent bonding
      - Forms HEXAGONAL LAYERS
        
        Strong bonds in layers
        
        High melting (+ Boiling) point
      - WEAK FORCES BETWEEN LAYERS
        
        Layers can slide over each other
        
        Soft
        
        Used for: Lubricant + Pencils
    - - Large CLASS of allotropes of Carbon
      - Made of balls/cages/tubes of carbon atoms
      - Carbon nano-tubes - type of Fullerene
    - - Layers of graphite rolled into a tube
        
        1 free electron per carbon because of the rolled up structure
        
        Very good electrical conductor
      - Extremely strong
      - Seethrough
      - Light
    - - Single layer of a Graphite molecule
        
        Thinnest material (currently known)
      - Bonded together in HEXAGONAL HONEYCOMB LATTICE
      - Best (currently known) conductor of heat + electricity
      - Unreactive
      - Very strong 100x-300x stronger than steel)
    - - e.g. diamond, graphite, fullerenes, carbon nanotubes are allotropes of Carbon
  - - - Easy to break
        
        Low melting + boiling point
        
        Usually liquids/gas at room temp.
        
        LOW density
    - - DOES NOT conduct electricity
  - - - (As no METALS)
    - - 1 PAIR of shared electrons
        
        Drawn as: X-X
    - - 2 PAIRS of shared electrons
        
        Drawn as: X=X
    - - 3 PAIRS of shared electrons
- - - - STRONG ATTRACTION between POSITIVE IONS and the DELOCALISED ELECTRONS
        
        By sharing delocalised electrons - strong metallic
        bonds are formed between metal atoms
  - - - Electrons in sea - can move freely carrying ELECTRICTY + HEAT ENERGY
        
        Conducts heat
        
        Conducts electricty
      - Layers of ions - can slide over each other when hammered or stretched
        
        (Electrons 'moved/displaced' by this can still bond)
        
        doesn't cause ions to repell
        
        like what happens in IONIC BONDS
        
        Malleable
        
        Ductile
  - - - MELTING POINT increases as GROUP increases
        
        Group 2
        
        2 Outer electrons
        
        each atom releases 2 electrons into sea of delocalised electrons
        
        Metal ions: 2+ charge
        
        Attraction between:
        
        2 more items...
        
        Group 1
        
        1 Outer electron
        
        each atom releases 1 electron into sea of delocalised electrons
        
        Metal ions: 1+ charge
        
        Metal - Higher group
        
        Metal - must lose more electrons to gain full outer shell
        
        Each atom has a greater positive charge - greater number of electrons, so greater difference between number of protons and electrons
        
        More electrons in sea of electrons - release more electrons into sea of electrons per atom
        
        Attraction - between greater number of electrons, and Metal ions with a greater charge
        
        Metallic bond - much stronger here
        
        1 more item...
- - - - Form positive ions
    - - Form negative ions
        
        Ions - OPPOSITE CHARGES
        
        ATTRACT each other
  - - - Atoms BEFORE
      - Electrons transfer
      - Ions formed
  - - - Ionic lattice
        
        the regular arrangement of the ions in ionic structures
      - The oppositely charged ions attract each
        other in a regular pattern
      - SOLID
        
        Ions - fixed in position + cannot move
        
        Doesn't Conduct Electricity
      - DISSOLVED/MOLTEN
        
        Ions - free to move/carry charge
        
        Conducts Electricity
      - Free Ions - can bond with water molecules
        
        Soluble in water
      - External force applied
        
        Layers slide past one another
        
        same charges repel each other
        
        Brittle
      - Orderly array of oppositely charged ions