Is a cyclic tertiary amine, such as the one shown in the attachment, chiral? If so, would it be counted in the 2^n rule?
Is a cyclic tertiary amine, such as the one shown in the attachment, chiral? If so, would it be counted in the 2^n rule?
Not sure what you mean by a 2^n rule, but the nitrogen in that molecule is a chiral center. It has 4 unique substituents - build a model and it should be pretty obvious that its mirror image is non-superimposable.
It only has 3, if the nitrogen had four substituents it would be charged.
I had forgotten about this, but I suspect that the reason that TPR isn't calling it a chiral center or including it in your rule is because of nitrogen inversion. At normal temperatures, nitrogen compounds actually invert themselves, which is why the drawing you posted earlier doesn't indicate any chirality. Without really low temperatures, it's probably not possible to isolate an R or S variant.I'm referring to the formula that determines the number of possible stereoisomers by raising 2 to the nth power where n is the number of stereocenters.
This is somewhat similar to how molecules undergo conformational changes at normal temperatures, although it is different in that the actual structure changes. One way to think about it is that it is in equilibrium with its stereoisomer at room temperatures.
There's a lone pair on the nitrogen, which gives that particular molecule a trigonal pyramidal shape, so the methyl group winds up being either above the ring or below it. That's why it's a chiral center. However, it's not permanent, due to nitrogen inversion (see my next statement).
There's a lone pair on the nitrogen, which gives that particular molecule a trigonal pyramidal shape, so the methyl group winds up being either above the ring or below it. That's why it's a chiral center. However, it's not permanent, due to nitrogen inversion (see my next statement).
I had forgotten about this, but I suspect that the reason that TPR isn't calling it a chiral center or including it in your rule is because of nitrogen inversion. At normal temperatures, nitrogen compounds actually invert themselves, which is why the drawing you posted earlier doesn't indicate any chirality. Without really low temperatures, it's probably not possible to isolate an R or S variant.
This is somewhat analagous to how molecules undergo conformational changes at normal temperatures, although it is different in that the actual structure changes. One way to think about it is that it is in equilibrium with its stereoisomer at room temperatures.
There's a lone pair on the nitrogen, which gives that particular molecule a trigonal pyramidal shape, so the methyl group winds up being either above the ring or below it. That's why it's a chiral center. However, it's not permanent, due to nitrogen inversion (see my next statement).
I had forgotten about this, but I suspect that the reason that TPR isn't calling it a chiral center or including it in your rule is because of nitrogen inversion. At normal temperatures, nitrogen compounds actually invert themselves, which is why the drawing you posted earlier doesn't indicate any chirality. Without really low temperatures, it's probably not possible to isolate an R or S variant.
This is somewhat analagous to how molecules undergo conformational changes at normal temperatures, although it is different in that the actual structure changes. One way to think about it is that it is in equilibrium with its stereoisomer at room temperatures.