nmr
DESCRIPTION
LecutrerTRANSCRIPT
Lab Work for This Week
•Finish recrystallization of any of the unknowns. Ifany of your compounds are not dry, see next page.
•Take melting points of the minilab unknown andmain lab unknowns
•Take IR of main lab unknowns
•Take TLC, uses methylene chloride to dissolveyour samples and as eluent, of main lab unknowns(one plate for both). Calculate Rf’s of any spots.Turn this in in a baggie (provided) with your labreport)
If any of the melting points, IR’s, or TLC’s are notcompleted by the time you finish in lab this week, thelabs will be open this Saturday and Sunday, bothfrom 1-4pm. You may not do any wet chemistry(separations, recrystallizations, filtrations). Dress asyou would normally come to lab. Enter HutchisonHall on the Plaza level (second floor).
Lab reports due next week
•Discuss the solubility data you collected the firstweek of the experiment
•Discuss what techniques were employed to decidewhich unknowns you have. You do not (cannot)decide the structure of the minilab compound. Justreport it’s slow melting point range.
•Calculate the recrystallized yield of the minilabunknown and the main two main lab unknowns
•Discuss the IR’s taken
•Discuss the TLC taken
•Answer questions from website posted last week.
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Nuclear Magnetic Resonance
Introduction
This introduction is designed to explain Nuclear Magnetic Resonance Spectroscopy
(NMR), which is now the main structure determination tool used by organic chemists.
This technique can be used to determine the structures of virtually all organic compounds,
no matter how complex. It is even being used to determine very complex structures such as
enzymes and proteins.
NMR produces a spectrum containing a number of peaks. The heights and positions of
these peaks enable a chemist to very accurately determine what the carbon-
hydrogen framework of an organic molecule is.
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NMR Introduction
What is Nuclear Magnetic
Resonance Spectroscopy?
NMR is a spectroscopic technique which uses electromagnetic radiation and magnetic fields
to determine the structure of organic compounds.
Radio-frequency radiation is used to stimulate
nuclei present within the molecule and from the information we obtain from doing this we
can very accurately determine where the carbon atoms are located and where hydrogen
atoms are located.
Basics: Nuclei with an odd mass or odd atomic number have
"nuclear spin" (in a similar fashion to the spin of
electrons). This includes 1H and 13C (but not 12C). The
spins of nuclei are sufficiently different that NMR
experiments can be sensitive for only one particular
isotope of one particular element. The NMR behavior of 1H and 13C nuclei has been exploited by organic chemist
since they provide valuable information that can be used
to deduce the structure of organic compounds. These will
be the focus of our attention.
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Since a nucleus is a charged particle in motion, it will
develop a magnetic field. 1H and 13C have nuclear spins of
1/2 and so they behave in a similar fashion to a simple,
tiny bar magnet. In the absence of a magnetic field,
these are randomly oriented but when a field is applied
they line up parallel to the applied field, either spin
aligned or spin opposed. The more highly populated state
is the lower energy spin state spin aligned situation. Two
schematic representations of these arrangements are
shown below:
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In NMR, EM radiation is used to
"flip" the alignment of nuclear spins from the low energy spin
aligned state to the higher energy spin opposed state. The
energy required for this transition depends on the
strength of the applied magnetic field (see below) but
in is small and corresponds to the radio frequency range of the
EM spectrum.
As this diagram shows, the energy required
for the spin-flip depends on the magnetic field strength at the nucleus. With no
applied field, there is no energy difference between the spin states, but as the field
increases so does the separation of energies of the spin states and therefore so
does the frequency required to cause the spin-flip, referred to as resonance.
The basic arrangement of an
NMR spectrometer is shown
to the left. The sample is
positioned in the magnetic
field and excited via
pulsations in the radio
frequency input circuit. The
realigned magnetic fields
induce a radio signal in the
output circuit which is used
to generate the output
signal. Fourier analysis of
the complex output produces
the actual spectrum. The
pulse is repeated as many
times as necessary to allow
the signals to be identified
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from the background noise.
Types of Nuclei
There are many nuclei which are NMR active. The table below shows some of the more common ones. Despite this, most NMR data are collected for 1H and 13C since they are so important in organic chemistry.
Isotope % abund Nuclear spin 1H 99.985 1/2 13C 1.108 1/2 2H 0.015 1 11B 80.42 3/2 14N 99.63 1 19F 100 1/2 31P 100 1/2
NMR Active Isotopes
NMR sample preparation:
NMR tube: usually 5mm across and 5 or 7 inches in
length.
In the NMR tube goes an approximate 1% solution of the
compound under investigation and a solvent. But not any
solvent!
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If one had a 1% solution of cyclohexane in chloroform, the
proton in chloroform would overwhelm the signal for
cyclohexane. Thus, one uses a deutersolvent, like CDCl3,
aka deuterochloroform or chloroform-d.
In the complete interpretation of an NMR, there are
four questions to answer:
1) How many unique observations are there? 2) Where are these unique observations located? 3) What are the nearby neighbors of the
observations in question? 4) How many H’s of each unique observation are
there?
We will answer the first two questions this week, and the last two questions we’ll answer in the next
two weeks.
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1) How many unique observations are there?
Let’s look at a few examples:
CH3CH3 HH
HHH
H
CH3CH2CH3 CH3CH2CH2CH3
CH3 C
CH3
H
CH2CH3 CH3 C
CH3
CH3
CH2CH3
C
H
H
C
H
H
C
H
H
C
CH3
H
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How many unique observations are there?
Let’s look at a few examples:
one
two two
four three
One four
CH3CH3 HH
HHH
H
CH3CH2CH3 CH3CH2CH2CH3
CH3 C
CH3
H
CH2CH3 CH3 C
CH3
CH3
CH2CH3
C
H
H
C
H
H
C
H
H
C
CH3
H
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2) Where are these unique observations
located?
Chemical Shift
• An NMR spectrum is a plot of the radio frequency applied against absorption.
• A signal in the spectrum is referred to as a resonance. • The frequency of a signal is known as its chemical shift.
The chemical shift in absolute terms is defined by the frequency of the resonance expressed with reference to a standard compound which is defined to be at 0 ppm. The scale is made
more manageable by expressing it in parts per million (ppm) and is indepedent of the spectrometer frequency.
It is often convienient to describe the relative positions of the resonances in an NMR spectrum. For example, a peak at a
chemical shift, δ, of 10 ppm is said to be downfield or deshielded with respect to a peak at 5 ppm, or if you prefer, the peak at 5 ppm is upfield or shielded with respect to the peak at 10 ppm.
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NMR spectra usually are displayed like the one below
with the applied field strength increasing from left to right
and the intensity of absorption plotted on the vertical
axis.
Cl CH2 C
O
CH3
Chloropropanone
In order that we get consistent positions for absorptions
we add an internal standard, usually TMS
(tetramethylsilane, (CH3)4Si). The protons in this
compound are all identical and are assigned a chemical
shift of zero. It is selected for both 1H and 13C spectra
because its single peak occurs upfield of almost all other
absorptions. The chemical shift is the name given to the
position in the spectrum at which an absorption occurs.
The horizontal scale is measured in delta or parts per
11
million (ppm), 1 ppm is 1 part per million of the
spectrometer frequency. For example, if we used a 200
MHz spectrometer, we would have each ppm would be
equal to a separation of 200 Hz. The reason for this is
that there are many different spectrometers available,
operating at many different frequencies, and so to
eliminate any variability from one instrument to another
this system is used.
So what causes chemical shift?
Shielding in H-NMR
The magnetic field experienced by a proton is influenced by various structural factors. Since the magnetic field strength dictates the energy separation
of the spin states and hence the radio frequency of the resonance, the structural factors mean that different types of proton will occur at different chemical shifts. This is what makes NMR so useful for structure determination, otherwise all protons would
have the same chemical shift.
The various factors include:
• inductive effects by electronegative groups • magnetic anisotropy • hydrogen bonding
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Electronegativity
The electrons around the proton create a magnetic field that
opposes the applied field. Since this reduces the field experienced at the nucleus, the electrons are said to shield the proton. It can be useful to think of this in terms of vectors....
Since the field experienced by the proton defines the energy difference between the two spin
states, the frequency and hence the chemical shift, δ /ppm, will change depending on the electron
density around the proton. Electronegative groups attached to the C-H system decrease the electron density around the
protons, and there is less shielding (i.e. deshielding) so the chemical shift increases. This is reflected by the plot shown in the graph to the
left which is based on the data shown below.
Compound, CH3X CH3F CH3OH CH3Cl CH3Br CH3I CH4 (CH3)4Si X F O Cl Br I H Si
Electronegativity of X 4.0 3.5 3.1 2.8 2.5 2.1 1.8 Chemical shift, δ / ppm 4.26 3.4 3.05 2.68 2.16 0.23 0
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These effects are cumulative,
so the presence of more electronegative groups produce more deshielding and
therefore, larger chemical shifts.
Compound CH4 CH3Cl CH2Cl2 CHCl3 δ / ppm 0.23 3.05 5.30 7.27
These inductive effects are not just
felt by the immediately adjacent protons as the disruption of
electron density has an influence further down the chain. However,
the effect does fade rapidly as you move away from the
electronegative group. As an example, look at the chemical shifts
for part of a primary bromide
H signal -CH2-CH2-CH2Br δ / ppm 1.25 1.69 3.30
This is known as the β effect
Magnetic Anisotropy
The word "anisotropic" means "non-uniform". Magnetic anisotropy means that there is a "non-uniform magnetic field".
Electrons in p systems (e.g. aromatics, alkenes, alkynes, carbonyls etc.) interact with the applied field which induces a magnetic field that causes the anisotropy. As a result, the nearby protons will experience 3 fields: the applied field, the shielding
field of the valence electrons and the field due to the p system. Depending on the position of the proton in this third field, it can be either shielded (smaller δ) or deshielded (larger δ), which implies that the energy required for, and the frequency of the absorption
will change.
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Hydrogen Bonding
Protons that are involved in hydrogen bonding (this usually means -OH or -NH) are typically observed over a large range of chemical
shift values. The more hydrogen bonding there is, the more the proton is deshielded and the higher its chemical shift will be. However, since the amount of hydrogen bonding is susceptible to factors such as solvation, acidity, concentration and temperature,
it can often be difficult to predict.
HINT : It is often a good idea to leave assigning -OH or -NH
resonances until other assignments have been made.
Experimentally, -OH and -NH protons can be identified by carrying out a simple D2O (deuterium oxide, also known as heavy water)
exchange experiment.
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• Run the regular H-NMR experiment • Add a few drops of D2O
• Re-run H-NMR experiment • Compare the two spectra a look for peaks that have
"disappeared"
Why would a peak disappear?
Consider the alcohol case for example:
R-OH + D2O <=> R-OD + HOD During the hydrogen bonding, the alcohol and heavy water can "exchange" -H and -D each other, so the alcohol becomes R-OD.
Although D is NMR active, its’ signals are of different energy and are not seen in the H-NMR, hence the peak due to the -OH disappears. (Note that the HOD will appear...)
The range in which NMR absorptions occurs is quite
narrow. 1H absorptions occur normally in the range 0 - 12
ppm downfield from TMS.
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Aromatic
Protons
Vinylic
Protons
Protons on C
Attached to
Electronegative
atoms
Allylic Alkanes
Saturated
Alkanes
8.0 6.5 4.5 2.5 1.5 0
0-1.5 H on a sp3 C next to a sp3 C.
1.5-2.5 H on a sp3 C next to a sp2 C.
2.5-4.5 H on a sp3 C next to a heteroatom (w/ lone pair of electrons)
4.5-6.5 H on a sp2 C
6.5-8.0 H on an aromatic (benzene) ring
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β-effect – Add 0.5 ppm to the expected range (0-1.5); now 0.5-2.0.
CH3CH2CH3 CH3CH2CH2CH3
C
H
H
C
H
H
C
H
H
C
CH3
H
H
H
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