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Bonding (Intermolecular (London Dispersion Forces (It is the weakest of…

- - - - Always between a metal and a non-metal
      - Bond is formed when the metals "give up" electrons, in order to pair unparied electrons. And non-metals gain electrons in this process.
      - Bond is formed due to electrostatic attractions between oppositely charged ions.
      - Are usually solids with lattice structures under normal conditions. As hard as different types of cheeses.
  - - - Single bonds= one pair of shared electrons
      - Double bonds= two pairs of shared electrons
      - Triple bonds= three pairs of shared electrons
      - The more bonds there are the shorter they get.
        
        The shorter a bond is the stronger they get
    - - Occurs when atoms with different electronegativity are bonded together
        
        In some situations the bonds can cancel out it they have different polarities. However, it depends on the molecule's structure
        
        Usually molecules that are polar consist of fluorine, oxygen, nitrogen, or chlorine are in a bond with something else
      - Video
    - - Exceptions to this "rule" are Boron(B) and Beryllium(Be). They are able to form stable bonds without, having a full octet.
  - - - Conduct heat and electricity due to the mobile electrons within a metal's structure.
      - They are malleable due to their lattice structure. They have metal ions in a sea of electrons. Therefore the ions can pass by one another when moved.
      - They make a metallic sound
    - - They are a mixture of metals.
        
        For example: Copper + Zinc forms Brass
        
        Copper + Tin forms Bronze
      - They have enhanced properties. They are stronger, harder, and are better conductors of electricity.
- - - - This is due to the presence of highly electronegative elements such as, Flourine, Nitrogen, Oxygen, and Chlorine
  - - - Especially with polar bonds because the nucleus is exposed when bonding with hydrogen
- - - - Three main examples of resonance structures are C6H6, CO3^2- and O3.
    - - Valence Shell Electron Pair Repulsion:
        
        1) All valence electrons for the central atom are shown.
        
        2) The valence electrons are kept in pairs
        
        3) The pairs of valence electrons will repel each other and be as far apart in space as possible
        
        4) Double and triple bonds count as a single "pair".
        
        5) The number of pairs around the central atom determine it's shape.
        
        6) Non bonded pairs repel each other more than bonded pairs.