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Why are diamond and graphite insoluble in water? Watch

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    (Original post by Lunch_Box)
    I am unsure whether it is because of:

    a) both have very strong covalent bonds, or

    b) both are non-polar, so cannot form bonds with water


    Help appreciated.


    edit: just realised that both are insoluble in organic solvents which are non-polar too, so im assuming it is the first.
    Both giant covalent lattices ...
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    Yeah, its definitely the first one. Diamond is a covalent network structure so I doubt it'll dissolve in anything.
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    (Original post by Lunch_Box)
    I am unsure whether it is because of:

    a) both have very strong covalent bonds, or

    b) both are non-polar, so cannot form bonds with water


    Help appreciated.


    edit: just realised that both are insoluble in organic solvents which are non-polar too, so im assuming it is the first.
    As it is apolar, and I we consider an apolar organic solvent we could assume that the interactions between the solvent and the solute is unimportant (or rather the enthalpy of solvation is zero, i.e. the interactions between two solvent molecules is the same as the interaction between a solvent molecule and a carbon.). This is the condition for what is known as an ideal solution......
    Therefore any solvation of the carbons will be due to entropic factors.

    These are only weak forces at room temperature, and to dissolve the lattice must first 'melt', which in the case of graphite and diamond is VERY disfavourable as reflected by their insanely high melting points.
 
 
 
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