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Chemical Bonding (Metallic Bonding (Strength of bond (-Charge of ion…

- - - - Nucleus charged higher, attracts electrons-stronger
    - - Smaller radius, attracts electrons-stronger
    - - Smaller amount of electrons, attracts electrons-stronger
- - - - .
  - - - .
  - - - .
  - - - .
  - - - .
  - - - .
- - - - Strength-minimum
      - Length-longest
    - - Strength-medium
      - Length-shorter
    - - Strength-maximum
      - Length-shortest
  - - - C.B share electrons
      - I.B give/receive e
    - - C.B between non-metals/low electronegativity exchane
      - I.B between metals and non-metals/high electronegative exchange
    - - I.B high
      - C.B low
    - - C.B low
      - I.B high
  - - - Exothermic
      - Electrons follow octet rule to be stable
        
        Lewis Structure
  - - - Double bond- bond order 2
      - Line Names-
        Sigma
        Pi
    - - Triple bond- bond order 3
      - Line Names-
        Sigma
        Pie
        Pie
    - - Single Bond- bond order 1
      - Line Name-
        Sigma
  - - - Difference in electronegativity-below 1.8 and above 0
      - Look at structure
      - Presence of lone pairs
    - - No difference in electronegativity
      - Can have polar bonds (electronegativity difference)
        
        must balance and be symmetrical
- - - - Oxidised
        -When an atom loses electrons, it becomes oxidised
        -In ionic bonds, the metals lose electrons, becoming oxidised
      - Reduced
        -When an atom gains electrons, it becomes reduced
        -In ionic bonds, the non-metals gain electrons, becoming reduced
      - One or more electrons tranfer
        
        To achieve noble gas e configuration
    - - Non-Metals
      - Metals
    - - Formed by metals losing e
    - - Formed by non-metals gaining e
- - - - London Dispersion Forces
        
        All particles
        
        Weakest force
        
        Increase by
        
        Larger Radius
        more electrons (more chance of uneven)
        
        Size of electron cloud
        e.g. long molecules
        (interacts with each other
        
        Less Branching
        allows to line easilier
    - - Dipole-Dipole Forces
        
        London forces are also present
        
        More stable-more strong than L.D.F
        
        Only present with polar covalent molecules
      - Hydrogen Bonds
        
        Strongest intermolecular force
        
        Only forms when hydrogen is covalently
        bonded with N, O or F
        
        London forces ALWAYS present
  - - - Polar covalent
      - Non-polar covalent