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Is 1 whole molecule an induced dipole?

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Why bother with a post grad? Are they even worth it? Have your say! 26-10-2016
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    Unfortunately this is not very clear in the book. Is an instantaneous dipole one part of a molecule e.g. a C-H bond or is the whole molecule?

    And I know that when you are talking about hydrocarbons, you refer to surface area of contact between molecules which increases London forces. I also remember learning about how the number of electrons also affects London forces.Does that also apply to hyrdocarbon chains or is that only for molecules such as S8.

    The number of electrons i.e. the bigger the molecule means that the induced dipoles created are stronger. But how would that work if only one part of the molecule is the induced dipole and not the whole molecule?i.e. in terms of hyrdocarbons the same C-H bond would be the induced dipoles so surely a bigger chain would have no difference to a smaller chain as only the C-H bonds would induce each other. So I guess this is where the surface area of contact come in to play, so the longer the carbon chain length, the more induced dipoles there are between 2 molecules. So if this is the case, why does the number of electrons matter at all? Shouldn't the number of induced dipoles determine the stength of the inter molecular force.

    Im so confused.

    EDIT: Ultimately what I am asking is why does more electrons mean a stronger London force?

    Answering your edit, basically London forces refer to the temporary dipoles occuring between molecules due to the distribution of charge in a particle and the attraction between the partial charges. If you have more electrons and more uneven distribution of charge, you're going to have more electrostatic attraction, and overall a larger van der Waals force.
    Hope this helps
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