1. Ultraviolet Spectroscopy Chapter 16, Smith (Pages 595-597)

2. What is our approach to spectroscopy? zWe will learn how to get the essential information from four kinds of spectroscopy and combine that information to deduce the structure of a compound. zThe first kind is Ultraviolet Spectroscopy (UV).

3. What is the most important thing to remember about spectroscopy? zThat “spectroscopic data” is a physical property of molecules and that properties of molecules are a direct result of the structure of those molecules. zThus, various forms of spectroscopy will give us “data” that reveals a little bit (i.e., partial structures) about the structure of a compound.

4. How will we use this data? zWe will correlate the spectroscopic data with specific partial structures. zWe will find as many partial structures as possible from the data and then combine all of the partial structures into a complete structure of the only compound whose structure could produce the spectra we interpreted.

5. What kind of data do we get? zIn general, we get numbers (units). zSpecific numbers reveal specific partial structures. zFor example, the number 3400 cm -1 in an IR spectrum reveals the -OH group as a partial structure.  The number 3 over a signal at  = 2.0 in a 1 H NMR spectrum reveals a methyl group next to a carbonyl group.

6. Must I memorize dozens of numbers? zNo, we hope to see enough examples so that you will become so familiar with the numbers that you know them much as you know your telephone number--not because you memorized the numbers but because you use them frequently enough that you simply remember them.

7. What kinds of numbers are important for UV?  A constant with the Greek symbol epsilon (  ), which tells us how much UV light a given compound absorbs.  Epsilon (  ) is the molar absorptivity or molar extinction coefficient.  The value of  can vary from zero (no absorption of UV) to over 10,000 (very strong absorption)

8. How do we characterize various values of epsilon?  Strong (  > 1000)  Weak (  < 100)  End absorption (  can’t be determined)  No absorption (  = 0)

9. How do we use these four classifications of UV? zWe associate or correlate partial structures with each of the four categories. zThe next few slides will show these correlations.

10. Partial structures: Strong UV (  > 1000)  Conjugated  systems--(alternating double bond--single bond--double bond) give  > 1000.

11. If  > 1000, what kind of partial structure is indicated?  The compound MUST CONTAIN a conjugated  system. zIt might be aromatic (like benzene). zIt might be a conjugated polyene (like 1,3-butadiene).

12. If a compound contains a conjugated  system what is  ?   must be > 1000

13. Problem  A compound has a strong UV and the calculation of  + r for the compound is three. zWhat partial structure is present in the compound?

14. Problem  A compound (C 7 H 8 ) has  = 15,000. Draw the structure of the compound.

15. Partial structures: Weak UV (  < 100)  Aldehydes or Ketones give  < 100

16. If  < 100, what kind of partial structure is indicated? zThe compound must have an aldehyde or ketone carbonyl. zThere is no heteroatom next to the carbonyl carbon (only C or H).

17. Given an aldehyde or ketone, what is  ?   < 100

18. Problem  A compound (C 4 H 8 O) has  < 100. Draw two possible structures for the compound.

19. Partial structures: UV End Absorption (No  ) zEsters give end absorption.

20. If UV = end absorption, what partial structure is indicated? zA carbonyl group with an Oxygen atom next to the carbonyl carbon is indicated. zAn ester is a carbonyl with an O but not OH (acid) next to a carbonyl.

21. Problem zA compound (C 2 H 4 O 2 ) shows end absorption in its UV spectrum, what is its structure?

22. Partial structures: No UV (inactive)  For CHM 201: UV = Wavelength  = 200-400 nm, the range of a typical instrument. zThe UV absorption in such compounds as ethene lies outside the above region. zAll partial structures, not covered in our strong, weak or end absorption categories will be considered inactive in the UV. (A ground rule, because of 200-400 nm)

23. How is UV absorption measured?  A sample of a given concentration (C) in moles/liter = molarity, is placed in a 1 cm wide cuvette (pathlength L), and ultraviolet light, starting at a wavelength ( ) of 400 nm and scanning down to 200 nm is passed thru.  The absorbance (A) is plotted vs wavelenth ( ). zA is proportional to C x L for a compound that absorbs UV light.

24. What info is recorded by the analyst?  The plot of A vs. will have one or more maxima or lamda max ( max ).  The A value at each max is recorded.  Since A is proportional to C x L, the proportionality can be made an equation by inserting a proportionality constant .  A =  CL (  is calculated and recorded for each max ).

25. Absorbance zThe incident UV light = 1.00 zThe compound absorbs some of it, say 80%. zThe absorbance A is recorded as 0.80, because the compound absorbed 80% of the incident radiation. zA has no units; it’s a decimal.

26. A typical calculation  Data: A = 0.815, L = 1 cm; C = 5.43 x 10 -5 M; and = 275 nm; solvent = cyclohexane  A =  CL;  = A/CL   = (0.815)/(5.43 x 10 -5 M)(1 cm) = 15,000 (no units); reported as  = 15,000, max = 275 nm (cyclohexane) zWhat kind of partial structure is indicated?

27. How does UV work?  Loosely held  electrons in a given molecular orbital are excited into a higher energy molecular orbital by UV energy.

28.  * Orbitals zAn electron moves (transitions) from one orbital to an empty (unoccupied) orbital that normally is empty.  The name of the orbital where the electron winds up is always called  *.  The name of the orbital where the electron starts out is either a  or an n (n stands for nonbonding)

29. Strong UV vs. Weak UV  Strong UV =  to  * transition  Weak UV = n to  * transition

30. Molecular Orbital Theory zMO theory is a complementary theory to Valence-Shell-Electron-Pair-Replusion or VSEPR theory. zEvery time two atomic orbitals overlap to make a bond, they make two new orbitals—a bonding and an antibonding orbital.

31. Molecular Orbital Theory zElectrons normally fill bonding orbitals. zThe antibonding orbitals (*) are normally empty of electrons, because they are of high energy and there is no net bonding in these orbitals.  The theory is most applicable to  bonds in organic chemistry.

32. Summary  Strong UV,  > 1000, (conj  sys) mostly aromatic (like benzene)  Weak UV,  < 100, (aldehyde or ketone)  End Absorption, no  (ester) zNo UV (everything else)   = constant (defined, no units)