Structural isomers, stereoisomers, geometric isomers, cis-trans isomers, and enantiomers.
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- So just to be clear, it looks like you can just flip an Enantiomer over and it would be the same (aka, fold at the dotted line). But since it's a 3 dimensional structure it wouldn't work like that, correct?(47 votes)
- Just to add, the "3D structure" that the original post referred to is the thick green line connecting C to Cl. This means that Cl is not on the page, but is "popping out at you."
This is why you simply cannot rotate the enantiomer to make them equal. If you try to rotate the left enantiomer 180 degrees, the Cl will be into the page, while the Cl on the right enantiomer will be out of the page.(14 votes)
- How can a different molecule have the same atoms?(13 votes)
- In Biology and Chemistry, it's important to realize that Shape Affects Function. Different configurations of a molecule (isomers) are what gives that molecule different properties. Let's use a perfectly fictional example of Hydrogen bonding. In Hydrogen bonding, a water molecule can bond with three other neighbors due to partial negative and positive charges with its atoms (which is caused by water being a polar covalent bond). If in some fictional reality, H2O was arranged differently, the Hydrogen bonds wouldn't occur between water molecules.
Hope that made sense!(22 votes)
- Why can't you rotate with a double bond? Does this mean you can't rotate at all if you were working with longer chains and had only one carbon double bond?(11 votes)
- The reason for it is that double bonds have pi bonds which kind of "restrain" or "fix it" the atoms as they have overlapping above and below the bond(sigma) axis which "locks" them and constricts rotation.
For a better understanding of this watch the videos on hybridization in the organic chem playlist.(15 votes)
- Do isomers only occur with hydrocarbon compounds?(8 votes)
- No, isomers are defined as molecules that have the same elemental composition, but different structures. This in no way limits the types of elements involved.
For example there are many biologically significant organic molecules that contain elements other than carbon and hydrogen such as amino acids and sugars that have enantiomers (a type of isomer), only one of which can be metabolized. For example, D-glucose and L-glucose.
In addition, carbon doesn't need to be involved at all since silicon based molecules can also have isomers -- https://en.wikipedia.org/wiki/Silanes#Isomerism.(3 votes)
- In structural isomers there is no double bonds, there is only single bond in video example , so why they can not rotate and change their shape to get a identical molecule(3 votes)
- This is because a structural bond involves changes in the types of bonds, no matter if you rotate the second carbon molecule on the bottom is still going to have 3 bonds.(3 votes)
- If you have more carbon atoms in a molecule, does that increase or decrease the number of isomers possible for that molecule?(4 votes)
- Generally the number of isomers increases. You can demonstrate this to yourself by drawing all possible structures for propane (1), butanes (2), pentanes (3), and hexanes (5).
One way to think about this is as follows: Each carbon you add can attach to any of the carbons already present in any isomer of the molecule. Some of these will make unique structures, so you will get more possible structures as you add more carbons.
Of course, the types of bonding among the carbons matter, for example adding a double bond to butane gives you butene, which has three isomers.
A detailed listing for alkane structural isomers can be found at: http://www.cpp.edu/~psbeauchamp/pdf/314_supp_6_isom_form.pdf.(1 vote)
- why double bonds do not allow rotation?(3 votes)
- Double bonds do not allow rotation as in the double bonds, the p-orbitals also overlap along with s-orbitals. And, as soon as you (obviously not you, but something else :) ) try/tries to rotate the dumbbell shaped p-orbitals, the amount of overlap decreases and that is in a way, breaking of a bond which requires a lot of energy and hence the rotation is not allowed.
The single bonds formed by the overlap of s-orbitals, however, are allowed to overlap as s-orbitals are spherical in shape, and on rotation the sphere-sphere overlap, perhaps, remains the same.(2 votes)
- Why does the single bond allow rotation and not a double bond? Is that just the way it is or is there a particular reason for it because I do not quite grasp that concept.(3 votes)
- It has to do with where the electrons are in the bond.
I don't know how much you already know, so I will start with one way of describing what bonds are.
Bonds are formed when there are electrons between two atoms, and these are attracted to both nuclei. However, to explain this rotation, don't think of this as two little particles sat still at the middle between two nuclei. Electrons can actually be thought of as having a probability of being at different positions. Depending on what 'orbital' is in, the electron is more or less likely to be in different positions. In a single bond, the electrons in the bond have a distribution that is rotationally symmetric around the axis between the two atoms, so it is a bit like a cylinder. This can rotate without changing energy. In a double bond, the second pair of electrons are more likely to be above/below the line between the atoms than to the sides. This bond is able to be formed because the orbitals of the bonded atoms line up a certain way, and so twisting this bond would bring them out of alignment. That requires energy, and prevents rotation.
I am sorry this is not very clear, and isn't even a full explanation of why you would need energy to rotate the bond. But there is more info about double bonds here https://www.chemguide.co.uk/atoms/bonding/doublebonds.html(2 votes)
- Why do we take 1 degree 2 degree and 3 degree amines as different fucntional groups and classify them under fuctional isomers although it's the same functional group that is amine?(3 votes)
- Many times in chemistry we'll see different molecules that have the same constituent atoms. For example, these two molecules here, they both have four carbons. One, two, three, four. One, two, three, four. So if I were to write their chemical formula, it would be C4 and then they both have, one, two, three, four, five, six, seven, eight, nine, ten. One, two, three, four, five, six, seven, eight, nine, ten hydrogens. So both of them, both of them have the chemical formula C4H10. C4H10, but they're still fundamentally different molecules and you can see that because they have different bonding. For example, over here we have a carbon that is bonded to three other carbons and a hydrogen. Over here I can't find any carbon that's bonded to three other carbons. I can find ones that are bonded to two other carbons, but not one that's bonded to three other carbons. So, how we've put the atoms together, is actually different. They're bonded to different things. And so when we have the situation where you have the same constituent atoms, where you have the same chemical formula, but you're still dealing with different molecules because either how their bonds are made or what their shape is, we call those isomers. So an isomer, isomer, you have the same chemical formula, same chemical formula. But you could have different bonding but different, different bonding, bonding or shape, bonding, shape or orientation. Orientation. So over here you have just different bonding and this type of isomer is called a structural isomer. So these characters are structural isomers, same constituent atoms, but different bonding. Structural isomers. So that's structural isomers right over there. Now when you look at this pair or this pair, you'll say those don't look like structural isomers. Not only do they have the same constituents, both of these for example have four carbons, four carbons and they both have one, two, three, four, five, six, one, two, three, four, five, six, seven, eight, and they both have eight hydrogens. So these are both C4H8, it's looks like they're bonded similarly. For example, I mean the left hand side here, these look identical and one the right hand side, you have a carbon bonded to another carbon that's bonded to three hydrogens, carbon bonded to another carbon that's bonded to three hydrogens. Carbon bonded to a hydrogen, carbon bonded to a hydrogen, so it looks like the structure of the bonding, everything's bonded to the same things, but you might notice a difference. Over here, on the right hand side, this CH3 is on the bottom right, while over here it's on the top right and you might say okay well we know, what's the big deal there, these, you know, all these molecules, they're all moving around, maybe they're rotating with respect to each other and these things could, this thing could have rotated down to become what we have up here. If this was a single bond. A single bond would allow for that type of rotation, it would allow for these things to rotate around each other. For the molecule to rotate around that bond, but a double bond does not allow that rotation. So this fixes these two things, this fixes these two things in place. And because of that, these are actually two different molecules. Over here on the top, you have the CH3 groups, they're both, they're both, I guess you could say, facing down or their both on the same side of the double bond, while over here they're on different sides of the double bond and so this type of isomerism, where you have the same constituents and you even have the same bonding, this is called stereoisomerism. So over here we're caring much more about how things sit in three dimensions. We don't just care about what's bonded to what or the constituents and actually this one is, as we'll see, is also a stereoisomer because this carbon is bonded to the same things in either case. So these are both, these are both situations, there are both stereoisomers, stereoisomers, and this particular variation of stereoisomer is called a cis trans isomer. Cis is when you have the two groups on the same side, cis, and trans is when you have the two groups on the opposite sides of the double bond. Cis trans isomers. Cis trans isomers. Isomers, and these are often called geometric isomers. Geometric, geometric isomers. So that's a subset, so when I'm talking about cis trans or geometric, I'm talking about these two characters over here. They are a subset of the stereoisomers. Now what's going on over here? I have no double bond, I'm not talking about cis and trans. The carbon, as I've just said, is bonded to fluorine, chlorine, bromine, and a hydrogen, fluorine, chlorine, bromine, and a hydrogen. How are these two things different? And the way that they're different is if you were to actually try to superimpose them on each other. You will see that it is impossible. There are mirror images of each other and because there's four different constituents here, you can actually not superimpose this molecule onto this molecule over here and actually because of that, they actually have different chemical properties, and so this over here, these two characters, which is a subset of stereoisomers. Stereoisomers are concerned with how things are positioned in three dimensions, not just how their bonding is different, but this subset where you have these mirror images that cannot be superimposed, we call these enantiomers. So these two characters, these are enantiomers. Enantiomers, and enantio comes from Greek, the Greek word or the Greek root opposite. So these are opposites of each other, they cannot be superimposed, they're mirror, they're mirror images. So all of these are different variations of isomers and once again, you might say, okay theses are clearly two different molecules that have different bonding, but even cis trans isomer will have different chemical properties. These two in particular, they aren't that different but they do have different chemical properties, but sometimes they're so different that one might be able to exist in a biological system while the other is not. One might be okay for your health, and the other might not be okay for your health. Same thing for enantiomers. One might be biologically active in a certain way and the other one might not be biologically active in that same way.