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Why are some elements like Ge and Si have liquids denser than their solids? In water it is explainable by H bonding, but no H bonds or such are there in Ge and Si. Well, I want an explanation about the structure formed by Ge and Si in their solid state which makes them less dense than their liquids, and also the bonds formed

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    $\begingroup$ If this helps, (I have taken this from @matt_black answer here.) "There isn't really a simple single explanation of why some solids are less dense than their associated liquids. The general explanation (which doesn't really explain much) is that the solid has a structure and, sometimes, that structure takes us more space than the average structure that occurs in the liquid." $\endgroup$
    – Zenix
    Commented Mar 1, 2020 at 15:03
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    $\begingroup$ Thanks for that Zenix, but I wanted a more detailed answer, so I modified the question accordingly as well. $\endgroup$ Commented Mar 1, 2020 at 15:29
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    $\begingroup$ Si and Ge are 4-fold coordinated diamond structure semiconducting solids. Their liquids are 8 to 12-fold coordinates metallic phases. The diamond crystal structure is fairly open. $\endgroup$
    – Jon Custer
    Commented Mar 1, 2020 at 17:28
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    $\begingroup$ Gallium and bismuth are also more dense, as liquids near their melting points, than are their respective solids at room temperature. $\endgroup$
    – Ed V
    Commented Mar 1, 2020 at 18:50
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    $\begingroup$ Don’t forget antimony as well... $\endgroup$
    – Jon Custer
    Commented Mar 2, 2020 at 3:07

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