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A201 Molecular Interactions, Strength 1) Ion-dipole 2) Hydrogen bonds …

- - - - Electron in a polar molecule shift towards the more electronegative end
        
        Creates a permanent positive charge (low electronegativity) & negative charge (low electronegativity)
        
        Partial positive charge of one end attracts to another molecule Partial negative charge (vice-versa)
  - - - Electron in polar molecule shift towards the more electronegative end (electronegativity difference is so huge, it creates a super-strong bond)
        
        This creates a permanent positive (H+) & negative end (F,O,N)
        
        The positive end interacts with the negative end of another molecule (vice-versa)
  - - - Electrons in non-polar molecules are constantly moving around (Low electronegativity difference)
        
        Any instance, electrons shift, creating a temporary partial positive charge and temp negative charge
        
        Temp partial positive charge attract to temp negative charge of another molecule (vice-versa)
  - - - Ions are positively or negatively charged
        The cation is attracted to the permanent negative end of a polar molecule
        Anion attracted to the permanent positive end of a polar molecule
- - - - 1) Solvent-Solvent interactions must broken
        2) Solute-Solute interactions must be broken
        3) Solvent-Solute interactions must occur
        
        The energy released from forming Solvent-Solute interaction must be greater or equal to the energy needed to break the Solvent-Solvent & Solute-Solute interactions
        To overcome the energy required to separate solute & solvent in the dissolution process
        
        Dissolution usually when interactions before & after mixing are similar in polarity and strength