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    Can anyone help I was doing some revision and came across this question draw a diagram showing hydrogen bonding for 2 molecules of CH3CH2OH I understand that the bond is from the oxygen to the hydrogen to join the molecules together but why is the H-C-H bond not electronegetive as stated on a youtube tutorial as I would of thought that there would be a small + charge on the hydrogen I checked the values of carbon and hydrogen and there is a difference in electronegtive values of about 0.3 so very close to being completely covlant but still should be a charge
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    (Original post by Daz0101)
    Can anyone help I was doing some revision and came across this question draw a diagram showing hydrogen bonding for 2 molecules of CH3CH2OH I understand that the bond is from the oxygen to the hydrogen to join the molecules together but why is the H-C-H bond not electronegetive as stated on a youtube tutorial as I would of thought that there would be a small + charge on the hydrogen I checked the values of carbon and hydrogen and there is a difference in electronegtive values of about 0.3 so very close to being completely covlant but still should be a charge
    The electronegativity of carbon and hydrogen is so close as to consider the bond virtually non-polar. You are, however, correct in what you have surmised. This is responsible for the +I effect of the alkyl groups. The relative electropositivity of the hydrogen atoms allows other, more electronegative, groups to draw electron density from alkyl groups, even though it is usually described the other way round.
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    (Original post by Daz0101)
    Can anyone help I was doing some revision and came across this question draw a diagram showing hydrogen bonding for 2 molecules of CH3CH2OH I understand that the bond is from the oxygen to the hydrogen to join the molecules together but why is the H-C-H bond not electronegetive as stated on a youtube tutorial as I would of thought that there would be a small + charge on the hydrogen I checked the values of carbon and hydrogen and there is a difference in electronegtive values of about 0.3 so very close to being completely covlant but still should be a charge
    Carbon isn't electronegative enough to command the pair of electrons in the C-H bond towards it to a significant degree. Remember hydrogen bonding only occurs between hydrogen and Nitrogen, Oxygen and Fluorine
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    (Original post by Daz0101)
    Can anyone help I was doing some revision and came across this question draw a diagram showing hydrogen bonding for 2 molecules of CH3CH2OH I understand that the bond is from the oxygen to the hydrogen to join the molecules together but why is the H-C-H bond not electronegetive as stated on a youtube tutorial as I would of thought that there would be a small + charge on the hydrogen I checked the values of carbon and hydrogen and there is a difference in electronegtive values of about 0.3 so very close to being completely covlant but still should be a charge
    I think the hydrogen has to be bonded to F, N or O. Also, there aren't lone pairs on the carbons.
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    Hydrogen bonds only occur when H is bonded to either nitrogen, oxygen or fluorine as these atoms are the only ones electronegative enough. So the carbon chain wouldn't form H bonds


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