London Forces Watch

khalilbigboy
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Report Thread starter 9 months ago
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Why doesnt Silicone dioxide have london forces (induced dipole dipole interactions)? Can you explain why and maybe list other compunds
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James_m1
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(Original post by khalilbigboy)
Why doesnt Silicone dioxide have london forces (induced dipole dipole interactions)? Can you explain why and maybe list other compunds
Silicon dioxide is a giant covalent structure, meaning it has many covalent bonds holding it together. As covalent bonds are way stronger than London forces, and the outer electrons of the silicon and oxygen atoms are in covalent bonds, London forces aren't really significant

Another example of a giant covalent structure is diamond, with 4 covalent bonds connected to each carbon atom.
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giraffe30
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I agree with James. Absolutely everything will generate London forces, because they arise from the uneven distribution of the electrons in each atom. They are only significant if that's all you've got. So in a plain hydrocarbon, the London forces are significant, because there's nothing else. Hence the trend from gas to liquid to solid as chain length increases. But if you introduce a polar group like an OH, you've put in hydrogen bonding and your London forces suddenly strike you as trivial.
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