infrared spectroscopy dr. milkevitch organic chem ii lab spring 2010 feb 11 & 13, 2010
TRANSCRIPT
Introduction
The purpose of this experiment
To introduce the student to spectroscopy
Discuss the specific technique of Infrared Spectroscopy Which is used to acquire
structural information on organic molecules
Use this technique in the laboratory
First: In order to Understand Spectroscopy Must understand electromagnetic
radiation (EMR)
EMR is a form of energy
Has a particle and wave nature
Examples: Light, microwaves, radiowaves
We Use Symbols to Designate Properties of
Waves λ is the wavelength of the waves
ν is the frequency of the waves
c is the speed of light of all EMR actually
Relationships Between These Variables
Speed = wavelength x frequency
Therefore: c = λν λ = c/ν ν = c/λ
For electromagnetic waves, the speed (c) is constant 3 x 108 m/s
What This Means
Wavelength has a direct, inverse relationship with frequency: λ ∝ 1/ν The higher the frequency, the
shorter the wavelength The longer the wavelength, the
smaller the frequency
Wavenumbers
When the wavelength is measured in centimeters: the reciprocal of the wavelength (1/cm)
Is directly proportional to the frequency
1/cm Is called the wavenumber and is a commonly used term in spectroscopy
Spectroscopy Is the Study of the
Interaction of Matter andElectromagnetic Radiation
In Organic Chemistry, the common techniques include: Infrared Spectroscopy Nuclear Magnetic Resonance
Spectroscopy UV/Visible Spectroscopy
What Spectroscopy Tells Us
Specific information on the structural features of the molecules being studied
The presence or absence of specific patterns of chemical bonding in a molecule
Infrared Spectroscopy: The use of infrared radiation to determine the presence or absence of specific patterns of bonding in a molecule (i.e., functional groups)
When IR Radiation is Applied to a Molecule
Some passes through it, but some does not
Some of it is absorbed
All bonds in a molecule have a vibrational frequency
If the frequency of the IR energy matches the specific vibrational frequency of a bond in a molecule The molecule will absorb the IR radiation at that
frequency
The bond is excited from a lower to a higher vibrational state Amplitude of vibration increases dramatically
We can measure this absorbance of IR radiation
We can come up with a graph of absorbance intensity vs. Wavelength
What an IR Spectrum Looks Like
E = hv = hc
λ
Graph of absorption intensity vs. radiation frequencyGiven as % transmittanceUnits are in wavenumbers (cm-1), (sometimes microns)
Now, Organic Molecules are Quite Diverse
Millions of organic compounds exist Remember the 12 families of organic compounds?
Structurally different molecules can have different functional groups Do not absorb exactly the same frequencies of IR
radiation Therefore, give different patterns of absorption Specific bonds and functional groups in a molecule
Have specific vibrational frequencies Therefore, will absorb characteristic frequency
ranges of IR radiation
This means: IR spectroscopy is a valuable tool for identifying
different functional groups Also, a valuable tool for helping identify the
structure of an organic compound
Ways Molecules Vibrate: Vibrational
Modes Vibrational Modes: Fancy way to describe the ways a molecule can vibrate 2 most important vibrational modes in IR spectroscopy:
Stretching: involves a change in interatomic distance Bending: involves a change in bond angles
Change in bond anglesChange in interatomic distance
IR-Active and Inactive Bonds
Stretching and bending must: Change the molecule’s dipole moment in
order to be IR active Large changes in dipole moment: very
intense IR absorption This is really important
Polar bonds will absorb strongly Does a polar bond have a dipole moment?
A nonpolar bond will absorb weakly or not at all Does a nonpolar bond have a dipole
moment?
Some Trends in Vibrational Frequency
The smaller the atoms in a bond, frequency increases
Larger the atoms in a bond, frequency decreases
Bond strength also effects frequency of absorption Stronger bonds, higher frequency of
absorption
Alkyne 2250 – 2100 cm-1
Alkene 1680 – 1600 cm-1
Alkane 1200 – 800 cm-1
Trends: Carbon-Hydrogen Stretching
Bonds with more s character absorb at a higher frequency
More s character, shorter and stronger bond
sp3 C-H, just below 3000 cm-1 (to the right)
sp2 C-H, just above 3000 cm-1 (to the left) sp C-H, at 3300 cm-1
The Three Most Important Regions of the IR Spectrum
3600 – 3100 cm-1 Where OH and NH stretching occur
Region around 1700 cm-1
Where C=O stretching occurs
Region around 1650 cm-1
Where C=C stretching occurs
Many of the important functional classes are identified by the presence (or absence) of absorptions in these regions
FT-IR Spectrometer “The modern IR spectrometer”
Small and compact Computer controlled
Has better sensitivity than dispersive instruments
Irradiate the sample with all IR frequencies at the same time
Does multiple scans quickly Averages the results
CorrelationTable:Summary of Notable IR absorbances for the functional Groups
Very importantFor the organicChemist
Procedure
Each group should choose one of the following compounds:
Chlorooctane Dodecane ChlorodecaneCyclohexaneCyclohexene3,3-dimethyl-1-buteneHeptaneHexane1-heptyne1-hexene
Procedure (2)
Obtain an IR spectrum See Dr. M in the instrument lab
Interpret major absorption frequencies Using tables in this handout Annotate the spectrum with your
interpretations
Your Report
Your introduction should include a discussion of IR spectroscopy Your textbook also has a chapter on IR
Spectroscopy, use it if necessary No reaction mechanism or balanced equation in this
experiment Physical properties section should be the relevant
physical properties of your chosen compound
Your results section should include the spectrum of your chosen compound Annotated
What do the peaks correspond to? If it’s not annotated, it is meaningless Make a table of relevant absorbances, along with their identity
Conclusions: Things to think about Did you successfully obtain your IR spectrum?
Is the spectrum clean? Crappy? Easy to obtain? What does your IR spectrum look like?
What major peaks do you have? What stretches do these peaks correspond to?
Do the peaks correspond to what type of compound you have (alkane, alkene or alkyne)?
Prove this: correlate your peaks to what peaks these compounds should have in an IR spectrum
Prove it further: find an IR spectrum of the compound and compare it to your spectrum
Overall, what did you learn about IR spectroscopy?
Additional Questions to answer:
1. Which absorbs at a higher frequency: a C-H bond or a C-D bond? Explain.
2. Why does H2 not have an IR spectrum?
3. Explain why the C=C stretch for a trans-disubstituted alkene is weaker than for a cis-disubstituted alkene.