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OCR B (Salters) F332 Tuesday 4th June 2013 Exam Discussion (Now Closed) watch

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    (Original post by krisshP)
    Do we have to know how to name phenols?
    No, that's F334


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    (Original post by abzy1234)
    You're correct, remember to show all the lone pairs as well
    Thank you I just thought it was weird that the central nitrogen has 3 bonds and a dative bond whilst the oxygen keeps all its electrons. Doesn't seem fair really :rolleyes:
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    What does the dot and cross diagram look like for a dative covalent bond?
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    can someone please give me links to any good revision places or any other good ways of revising? or could someone just send me links of revision notes would really appreciate it? many thanks
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    (Original post by King Hotpie)
    Thank you I just thought it was weird that the central nitrogen has 3 bonds and a dative bond whilst the oxygen keeps all its electrons. Doesn't seem fair really :rolleyes:
    Yah, dative structures can get a bit weird tbh. Oxygen's a boss
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    (Original post by wizardlad)
    can someone please give me links to any good revision places or any other good ways of revising? or could someone just send me links of revision notes would really appreciate it? many thanks
    http://www.chemguide.co.uk/index.html#top
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    Aaaaaahhhhhh the exam is getting closer and closer :eek: !!!
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    cheers could you be more specific on which bits to revise so i dont end up revising the wrong stuff haha ?
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    (Original post by tasnimc)
    What does the dot and cross diagram look like for a dative covalent bond?
    Instead of a dot and a cross
    The covalent bond would be 2 dots or 2 crosses showing one atom provides both of the electrons
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    (Original post by wizardlad)
    cheers could you be more specific on which bits to revise so i dont end up revising the wrong stuff haha ?
    Go see the spec
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    (Original post by super121)
    Where are you getting the 4f from? Iodine is nowhere near the f block.
    true, but i am still confused do we just skip out 4f and jump straight onto 5s2 5p6? ... ugghh !!!!
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    (Original post by nksunny)
    true, but i am still confused do we just skip out 4f and jump straight onto 5s2 5p6? ... ugghh !!!!
    Yeah, I advice you to follow this: https://www.youtube.com/watch?v=lqWL0WMtlYk
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    (Original post by tigerz)
    Yeah, I advice you to follow this: https://www.youtube.com/watch?v=lqWL0WMtlYk
    AHHHH ... thanks a lot ... makes so much more sense now ... PANIC over
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    (Original post by nksunny)
    true, but i am still confused do we just skip out 4f and jump straight onto 5s2 5p6? ... ugghh !!!!
    The f block comes last (we don't even need to know about it).
    This may help:
    http://www.google.co.uk/search?safe=...s%3B1438%3B952

    You can see that iodine is in the p-block, and is 5p^5. But because its and iodide ion, you need an extra electron so it 5p^6
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    (Original post by nksunny)
    AHHHH ... thanks a lot ... makes so much more sense now ... PANIC over
    Haha no problem I quite like electronic config, out of all the past papers Chlorine always gets asked and Iodines outer sub-shell has only been asked once!
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    can anyone explain how a double bond can be nucleophilic if it has got plenty of electrons ( shouldn't it just be electrophilic? ) i'm getting this from the revision guide page 95 by the way.
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    (Original post by tigerz)
    Haha no problem I quite like electronic config, out of all the past papers Chlorine always gets asked and Iodines outer sub-shell has only been asked once!
    yeah it was the iodine one which i was stuck on ... i didn't knw how to work it out cause the mark scheme said 5p6 and i ended up with 4f8 because i went up the spdf scale thing, only knw we could jump from 3p-4s-3d and no more jumping further on, obviously i was wrong -_- ... but this had made things very clear now
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    (Original post by madrevision)
    can anyone explain how a double bond can be nucleophilic if it has got plenty of electrons ( shouldn't it just be electrophilic? ) i'm getting this from the revision guide page 95 by the way.
    Neucleophiles are electron pair donors - so they have many electrons i.e. a lone pair or in this case an electron dense area like a double bond. Electrophiles do not have enough electrons they are electron pair acceptors.
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    (Original post by madrevision)
    can anyone explain how a double bond can be nucleophilic if it has got plenty of electrons ( shouldn't it just be electrophilic? ) i'm getting this from the revision guide page 95 by the way.
    It bonds by donating a pair of lone electrons in a dative covalent bond so a double bond is kind of like a nucleophile.

    Although you will be more asked about an electrophile bonding with the double bond not the other way round.
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    How would you draw the monomer of 1,3-butadiene?

    It's on June 2011 pre release
 
 
 
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