The molecular formula of an unknown compound is C10H12O2. The compound gives strong peak at 1745cm-1 in IR spectrum The NMR details are 7.55∆(5H,m),1.4∆(6H,d),5.2∆(1H,septet) identify the unknown organic compound
Answers
Answer:
McMaster University - Chem3D03
Problem Set #1 ANSWERS January 12, 1998
1. Fill in the boxes in the reaction sequences below.
PS1-1a
PS1-1b
PS1-1c
PS1-1d
PS1-1e
PS1-1f
PS1-1g
2. Show with equations how the molecule on the left could be converted to the molecule on the right. You may use any other reagents you need. Draw the structures of all intermediate compounds in each sequence. Mechanisms are not required.
PS1-2a
PS1-2b
PS1-2c
PS1-2d
PS1-2e
3. Propose mechanisms for the following reactions.
PS1-3a
PS1-3b
PS1-3c
PS1-3d
PS1-3e
4. The infrared and 1H nmr spectra of a compound with molecular formula C10H12O2 are shown below. Deduce the structure of the compound from these data. Note that in the nmr spectrum, the integration has been done for you; the number of protons responsible for each of the "signals" is indicated right above it in the spectrum.
C10H12O2 - IR Spectrum
C10H12O2 - NMR Spectrum
Answer
1. Molecular Formula C10H12O2 -> 5 sites of unsaturation. For a molecule this size, (i.e., only ten carbons), such a large number of sites of unsaturation is usually due to the presence of a phenyl ring (which provides 4 sites on its own). For a quick proof, take a quick glance at the 1H nmr spectrum, and look for signals in the 7-8 ppm (aromatic proton) region. No question, they're there! This leaves only one site unaccounted for.
2. Infrared Spectrum - strong peak at ~1700 cm-1 -> C=O (this accounts for the other site of unsaturation!)
- nothing at ~3500 cm-1 -> no OH, so a carboxylic acid or alcohol can be ruled out.
- weak absorption in the 3000-3100 cm-1 region indicative of sp2 C-H stretches, in addition to prominent bands in the 2800-3000 cm-1 range due to sp3 C-H. There is lots more information here, but this is the easiest to pull out, and all we need for the present.
1H NMR spectrum - 6 types of H's:
- singlet at 9.8 ppm (1H) -> aldehyde or carboxylic acid proton. The ir spectrum rules out a carboxylic acid, so this must be an aldehyde. The absence of coupling indicates that the -CHO group is bonded to an atom with no protons attached to it.
- two doublets at ~6.9 and ~7.7 ppm (4H) -> aromatic protons; symmetrical pattern of two doublets suggests a 1,4-disubstituted benzene. Each doublet corresponds to 2 equivalent protons, each of which has one nearest neighbour:
Note that the two doublets are skewed towards one another and that the magnitude of the splitting is the same for both - this verifies that the two doublets "belong together"; i.e., they represent a pair of protons coupled to each other.
We've accomplished alot; check the molecular formula to see what's left! We've accounted for a -CHO group and a -C6H4-. All that's left is three carbons bearing 7 hydrogens and an oxygen. Since all sites of unsaturation are accounted for, the seven H's must all be bound to sp3 carbons.
- triplet at ~4 ppm (2H) -> two equivalent protons with 2 nearest neighbours. With only 3 carbons left, this must be due to a CH2 attached to a CH2!
- triplet at 1 ppm (3H) -> three equivalent protons with 2 nearest neighbours. This must be due to a methyl group attached to a CH2.
The last two bits of information, coupled with the fact that we have only C3H7 left, are only consistent with one structure - CH2CH2CH3!
- sextet at ~1.8 ppm (2H) -> two equivalent protons with 5 nearest neighbours. This is the middle CH2 in the -CH2CH2CH3 chain.
Let's take stock of what we have:
There are only TWO possible ways that these fragments can be put together:
To choose between the two, we need to take a closer look at the nmr spectrum and ask "how will the spectra of these two compounds differ?" One set of protons will have a significantly different chemical shift in the two structures. (Sometimes, more than one set can be identified as being significantly different; sometimes none can, in which case we would need more data). This is the terminal CH2 group in the CH2CH2CH3 chain. In A, it's attached to oxygen and should come at around 4 ppm. In B, it's attached to an sp2 carbon and should come at 2-2.5 ppm. Clearly, structure A is the one that fits the spectrum the best.
5. The highest molecular weight ions in the mass spectrum of an unknown compound arise at 150 and 152 amu, in the intensity ratio 3:1. Its infrared and 1H nmr spectra are shown below. Deduce the structure of the compound from these data.
Answer
Mass Spectrum
The highest molecular weight ion usually corresponds to the molecular ion, and hence gives the molecular weight of the compound. A pair of peaks separated by 2 amu with an intensity ratio of 3:1 indicates that the molecule contains a single chlorine atom. This would normally be verified by looking elsewhere in the spectrum for similar pairs of peaks representing Cl-containing fragment ions. Thus, the true molecular weight of the compound R-Cl is 150.5. The fragment R will have a weight of 115 amu, and thus contains zero or an even number of nitrogen atoms. Without the full mass spectrum, this is all we can use for now.