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Greater the Van der Waal's force lower the melting point. Watch

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    Am I right?

    Melting point of chlorine is lower than sulphur because Van der Waal's forces increases..

    but the next point in the mark scheme states ' e'/size/Mr is smaller for Cl molecules'
    looking at the periodic table the Mr is going up?
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    I thought it would be the other way round :/

    Stronger Van der Waals = stronger bonds = more energy needed to break the bond = higher melting point?
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    No.. Chlorine has a lower melting point then Sulphur and it has a greater van der waal's force.
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    (Original post by yaya1)
    No.. Chlorine has a lower melting point then Sulphur and it has a greater van der waal's force.
    Chlorine has a higher electronegativity than sulphur yes. But it does not have stronger intermolecular forces.

    The stronger the intermolecular forces the higher the melting point.
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    Chlorine exists as Cl2, but sulphur exists as S8, hence the smaller Mr and weaker van der Waal's force
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    (Original post by nkvuong)
    Chlorine exists as Cl2, but sulphur exists as S8, hence the smaller Mr and weaker van der Waal's force
    Thank You.
 
 
 
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