So, this is a picture of the test and I think the ClF3 answer is right :/, and as you can see on the left I was gonna draw a trigonal bipyramidal but the scribbled it off cause I thought if there is lone pairs so each must've pushed 5 degrees more meaning it will not be a straight line, and btw also the ms says allow any 3 bp and Lp but the teacher is being too stubborn about it probably cause I already got 64/70 and he doesn't want me to get higher lol. This is AQA June 2010 Chem 1 Markscheme
On question 1b for CCl2F2 you have drawn a displayed formula. I think what the question is asking is for you to draw the shape meaning using Wedges, broken lines etc and indicated the lone pairs on there. Reason being this is a Shapes of Molecules Question. But the one on the right is correct. So I can check this can you post a picture of the complete question and the mark scheme for this? Alternatively tell me what exam board and what exam you are doing.
The issue with your structure for ClF3 is that it's not obviously T-shaped; you should have stuck with your first attempt! On the bright side, you will probably not make this mistake again.
The fundamental shape for a five-bond centre is a trigonal bipyramid — three bonds around the middle, one at the top and one at the bottom. Although the markscheme says to award marks for a structure with 3 BPs and 2 LPs, I can understand why your teacher has not credited you. Your diagram looks like a pentagonal planar structure, which is definitely wrong.
The fundamental shape for a five-bond centre is a trigonal bipyramid — three bonds around the middle, one at the top and one at the bottom. Although the markscheme says to award marks for a structure with 3 BPs and 2 LPs, I can understand why your teacher has not credited you. Your diagram looks like a pentagonal planar structure, which is definitely wrong.
Yeah that's exactly what he told me today, he did end up giving me the mark though however sadly turns out the 1)a)ii) question is wrong hahahah it has to be Cl2 and F2, oh well thank you everyone
So, this is a picture of the test and I think the ClF3 answer is right :/, and as you can see on the left I was gonna draw a trigonal bipyramidal but the scribbled it off cause I thought if there is lone pairs so each must've pushed 5 degrees more meaning it will not be a straight line, and btw also the ms says allow any 3 bp and Lp but the teacher is being too stubborn about it probably cause I already got 64/70 and he doesn't want me to get higher lol. This is AQA June 2010 Chem 1 Markscheme
I would not credit that answer either. You're expected to know the shapes of molecules and yours is not the correct arrangement for 3Bp & 2Lp.
I would not credit that answer either. You're expected to know the shapes of molecules and yours is not the correct arrangement for 3Bp & 2Lp.
EQUATION: 0.5Cl2+1.5F2------> ClF3
remember cl2 and f2 (diatomic molecules)
For shape of ClF3:
Cl is central atom Using the rules: 7+3=10e =5 pairs hence 3 bp and 2 lp
NOW BE CAREFUL HERE
The lone pairs here have no effect, as the repulsion from one lone pair cancels out the repulsion from the other hence shape is trigonal planar and bond angle=120
So, this is a picture of the test and I think the ClF3 answer is right :/, and as you can see on the left I was gonna draw a trigonal bipyramidal but the scribbled it off cause I thought if there is lone pairs so each must've pushed 5 degrees more meaning it will not be a straight line, and btw also the ms says allow any 3 bp and Lp but the teacher is being too stubborn about it probably cause I already got 64/70 and he doesn't want me to get higher lol. This is AQA June 2010 Chem 1 Markscheme
EQUATION: 0.5Cl2+1.5F2------> ClF3
remember cl2 and f2 (diatomic molecules)
For shape of ClF3:
Cl is central atom Using the rules: 7+3=10e =5 pairs hence 3 bp and 2 lp
NOW BE CAREFUL HERE
The lone pairs here have no effect, as the repulsion from one lone pair cancels out the repulsion from the other hence shape is trigonal planar and bond angle=120
So, this is a picture of the test and I think the ClF3 answer is right :/, and as you can see on the left I was gonna draw a trigonal bipyramidal but the scribbled it off cause I thought if there is lone pairs so each must've pushed 5 degrees more meaning it will not be a straight line, and btw also the ms says allow any 3 bp and Lp but the teacher is being too stubborn about it probably cause I already got 64/70 and he doesn't want me to get higher lol. This is AQA June 2010 Chem 1 Markscheme
Also your teacher is a clear moron- mark scheme awards marks for 3 bond pairs an 2 lone pairs regardless of the shape, as long as you have 3 BOND PAIRS AND 2 LONE PAIRS, you should get the marks regardless of whether the structure exists like that in 3 dimensional space
as I said before you would have got both marks for the shapes when applying the mark scheme however you should not have got the mark for the equation since chlorine and fluorine are diatomic
The lone pairs here have no effect, as the repulsion from one lone pair cancels out the repulsion from the other hence shape is trigonal planar and bond angle=120
This would only be true if the two lone pairs occupied the axial positions, which they don't.
as I said before you would have got both marks for the shapes when applying the mark scheme however you should not have got the mark for the equation since chlorine and fluorine are diatomic
Oh yeah never noticed that, that's bad marking haha
Cl is central atom Using the rules: 7+3=10e =5 pairs hence 3 bp and 2 lp
NOW BE CAREFUL HERE
The lone pairs here have no effect, as the repulsion from one lone pair cancels out the repulsion from the other hence shape is trigonal planar and bond angle=120
Or..... I could know what I was on about and draw the 'seesaw' shape