guys theres an exam q 4b(ii) of unit 4 jan 2012, it asks "suggest how well these four compounds would be separated using alkane stationary phase, in your answers include indication of retention times" the stationary phase is a liquid alkane and the compounds are; 2 esters, an alkane and an alcohol. im confused dont really understand the question? help pls!
Basically, the more similar a molecule is to the stationary phase, the more it will interact with it, so the alkane has the longest retention time, but it will have the most interactions with an alkane stationary phase. The alcohol will have a short retention time because only a small promotion of the molecule will be able to for van der waals with the alkane stationary phase due to the OH group. The esters will have similar retention times because they have the same functional group, and there for have very similar interactions with the stationary phase.
Basically, the more similar a molecule is to the stationary phase, the more it will interact with it, so the alkane has the longest retention time, but it will have the most interactions with an alkane stationary phase. The alcohol will have a short retention time because only a small promotion of the molecule will be able to for van der waals with the alkane stationary phase due to the OH group. The esters will have similar retention times because they have the same functional group, and there for have very similar interactions with the stationary phase.
Can someone please clarify this because I've seen it different on 2 different markschemes Is it that benzene cannot induce a dipole in Br2 but phenol can or induces a dipole less than phenol in Br 2 - confused which is correct Also would it be correct to say pi-electrons or pi-bonds when describing the bonding in benzene?
Can someone please clarify this because I've seen it different on 2 different markschemes Is it that benzene cannot induce a dipole in Br2 but phenol can or induces a dipole less than phenol in Br 2 - confused which is correct Also would it be correct to say pi-electrons or pi-bonds when describing the bonding in benzene?
probably that benzene can induce a dipole less than phenol but not strong enough to polarise br2.
Can someone please clarify this because I've seen it different on 2 different markschemes Is it that benzene cannot induce a dipole in Br2 but phenol can or induces a dipole less than phenol in Br 2 - confused which is correct Also would it be correct to say pi-electrons or pi-bonds when describing the bonding in benzene?
You can say either I think, for the newer papers it says benzene polarises bromine less and then it has Allow benzene cannot polarise bromine/cannot induce a dipole. I just did a 2010 paper again and it didn't have polarises bromine less on the ms but I assume that was because it's old? I think you can say pi-electrons or pi-bonds it doesn't matter either
Hey does anyone know if we can access the specimen papers for other years? I ran out of F324 papers and just found a specimen paper but there's only one on the website. Idk if they produce them every year or just when the spec changed in 2010? Thanks
It would be G and F alternating but with H's in between them since G and F are Di carboxylic acids so they can't bond to each other only to H? So GHFHGHFHGHFH. What paper is that question from?
It would be G and F alternating but with H's in between them since G and F are Di carboxylic acids so they can't bond to each other only to H? So GHFHGHFHGHFH. What paper is that question from?
Hey does anyone know if we can access the specimen papers for other years? I ran out of F324 papers and just found a specimen paper but there's only one on the website. Idk if they produce them every year or just when the spec changed in 2010? Thanks