ATAR Notes: Forum
Archived Discussion => 2010 => Mid-year exams => Exam Discussion => Victoria => Chemistry => Topic started by: joocoobpootooloo on June 09, 2010, 08:57:58 pm
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Question 9C).....
if i forgot to mention hydrogen bonding in regards to propan-1-ol but mentioned its polarity and dipole dipole bonds and that butane is non polar and has dispersion forces i might get the 3 marks? :S
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Question 9C).....
if i forgot to mention hydrogen bonding in regards to propan-1-ol but mentioned its polarity and dipole dipole bonds and that butane is non polar and has dispersion forces i might get the 3 marks? :S
same with me, but i also stated that dispers Forces are weaker... i think wed get the marks
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Didn't see the bloody negative.
FML.
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i talked about:
the electronegativity of oxygen (dont know why)
the dispersion forces are weak in butane
the dispersion forces in butane are weaker then that of those in propan-1-ol..
hopefully i get at least 1 mark....
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Question 9C).....
if i forgot to mention hydrogen bonding in regards to propan-1-ol but mentioned its polarity and dipole dipole bonds and that butane is non polar and has dispersion forces i might get the 3 marks? :S
same with me, but i also stated that dispers Forces are weaker... i think wed get the marks
i mentioned that too.. i talked about absolutely everything you could talk about except hydrogen bonding :S
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Question 9C).....
if i forgot to mention hydrogen bonding in regards to propan-1-ol but mentioned its polarity and dipole dipole bonds and that butane is non polar and has dispersion forces i might get the 3 marks? :S
same with me, but i also stated that dispers Forces are weaker... i think wed get the marks
i mentioned that too.. i talked about absolutely everything you could talk about except hydrogen bonding :S
lol exactly tha same....i think dipole dipole should do it imo
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hmm i feel slightly better now :D. wow going on vcenotes was the worst thing i could do for my confidence, i thought i mightve gotten full marks.. now il be happy with 71+.
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hmm i feel slightly better now :D. wow going on vcenotes was the worst thing i could do for my confidence, i thought i mightve gotten full marks.. now il be happy with 71+.
i would die for a 71! haha
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Didn't see the bloody negative.
FML.
same -.- i was reading my response and i knew it made no sense at all. but ceebs reading the question again.
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hydrogen bonding is a special case of dipole dipole. You probably would get away with it..
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fingers crossed :P i went through thinking it was hydrogen bonding in my head in the exam but i convinced myself it wasnt somehow :S
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hmm i feel slightly better now :D. wow going on vcenotes was the worst thing i could do for my confidence, i thought i mightve gotten full marks.. now il be happy with 71+.
you=me.
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hydrogen bonding is a special case of dipole dipole. You probably would get away with it..
I think that if you mentioned that propanol was polar due to the presence of the OH group, and could therefore form dipole-dipole bonds, then I think you might get away with not saying the words hydrogen bonding - but I think it's risky!
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Not sure if you need to say polar but its mainly due to strong hydrogen intermolecular bonding which requires high energy (temperature) to break
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Not sure if you need to say polar but its mainly due to strong hydrogen intermolecular bonding which requires high energy (temperature) to break
Yessum, but I was suggesting that IF you forgot to say hydrogen bonding, then "very polar" would maybe make up for it?
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Really have no idea but I just think polarity doesn't really have much to do with this? I thought polarity is mainly to describe solubility. But I am not 100% sure. Essentially polarity is determined by hydrogen bonding though...
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Really have no idea but I just think polarity doesn't really have much to do with this? I thought polarity is mainly to describe solubility. But I am not 100% sure. Essentially polarity is determined by hydrogen bonding though...
Hydrogen bonding is determined by polarity, not the other way around.
Polarity does indeed have a lot to do with solubility, but it also has a lot to do with intermolecular bonding and therefore melting and boiling points. Non-polar molecules can form only dispersion forces between molecules, so the molecules are relatively easy to separate i.e. low boiling point. Polar molecules, depending on how polar, can form dipole-dipole bonds, which are stronger than regular dispersion forces, and if the molecules are polar enough, (NOF) then they can form hydrogen bonds, a particularly strong version of dipole-dipole attractions... and thus the more polar, the stronger the intermolecular forces, the higher the boiling point...
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Yea I guess your correct.
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Get the methods book going andrew.........:P