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    Came across these questions about boiling and melting points and am a bit stuck... any help would be appreciated!

    1. How do you explain the fact that, although the boiling point of silicon is very high (2360 deg. C), the percentage increase in temperature from melting point to boiling point is less for silicon than for most of the other elements?

    Might it be because silicon forms a giant covalent compound? Although I'm unsure why that would help, if indeed it does.

    2. Why is the boiling point of argon (-186 deg. C) only slightly higher than its melting point?

    Again a guess, but is it due to the fact that argon only has van der Waals forces? I'm not really sure how it relates though.
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    You're right. It's all bwt the intermolecular force crap
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    1. I'd hazard a guess that's because you need to break all the very strong covalent bonds to make it a liquid; after that, there's not much left, so most of the work has been done.
    2. The only type of intermolecular forces in Argon (and all Noble gases) are id-id, and those are the weakest type, so it'd be a case of breaking them, then there being little else to break.
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    correct, these questions are really very much logical and you can bet that you will know how to answer them if you think about it, along the basic chemical rules.
 
 
 
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