1 / 42

Organic Mass Spectrometry

Organic Mass Spectrometry. Interpretation of Mass Spectra. Basic Interpretation. Most mass spectra are not trivial to decipher due to: – interferences complexities of fragmentation (exception: some elemental analysis cases)

manon
Download Presentation

Organic Mass Spectrometry

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Organic Mass Spectrometry Interpretation of Mass Spectra

  2. Basic Interpretation • Most mass spectra are not trivial to decipher due to: • – interferences • complexities of fragmentation • (exception: some elemental analysis cases) • Instead, MS Interpretation is problem solving, ‘playing chess’, or ‘cracking a code’

  3. Basic Interpretation • Use all available information in a logical and organized manner • Our focus: EI spectra of “small” organic molecules • but interpretation techniques are applicable to spectra obtained with other ionization techniques (homework, examples…)

  4. References on MS Interpretation • McLafferty & Turecek, Interpretation of Mass Spectra, 4th Ed., 1993. • Best book on the subject • We will follow it closely • Smith & Busch,Understanding Mass Spectra, 1999. • Alternative to McLafferty, somewhat easier to read

  5. References on MS Interpretation • Lee, A beginner’s Guide to Mass Spectral Interpretation, 1998. • More basic, easy to read. Useful introduction before tackling McLafferty. • Sorrell, Interpreting Spectra of Organic Molecules, 1988. • Older and more general.

  6. MS Interpretation: First Steps • You have a sample to be analyzed. How do you proceed? • Three steps: 1. Run the spectra you get against a database (if available) 2. Obtain a high resolution spectrum if possible This will help constrain the elemental compositions 3. Follow the standard interpretation procedure (SIP) and make sure that your identification is self-consistent

  7. Standard Interpretation Procedure • Ask questions in a logical order • Big picture questions first • E.g. which elements are present • Avoid “blind alleys” • More detailed questions later • E.g. molecular substructures • Put it all together at the end • Postulate a molecule that is consistent with all previous information

  8. Standard Interpretation Procedure • (1) Study all available information (spectroscopic, chemical, sample history). Give explicit directions for obtaining spectrum (better yet, do it yourself). • Verify the m/z assignments. Use calibrants if needed. • (2) Using isotopic abundances (where possible) deduce the elemental composition of each peak in the spectrum; calculate rings plus double bonds.

  9. Standard Interpretation Procedure • (3) Test molecular ion identity; must be the highest mass peak in spectrum, odd-electron ion, and give logical neutral losses. Check with CI or other soft ionization. • (4) Mark ‘important’ ions: odd-electron and those of highest abundance, highest mass, and/or highest in a group of peaks.

  10. Standard Interpretation Procedure (5) Study general appearance of the spectrum: molecular stability, labile bonds, etc. • (6) Postulate and rank possible sub-structural assignments for: a) Important low-mass ion series b) Important primary neutral fragments from M+. indicated by high-mass ions (loss of largest alkyl favored) plus those secondary fragmentations indicated by MS/MS spectra. c) Important characteristic ions.

  11. Standard Interpretation Procedure • (7) Postulate molecular structures; test against a reference spectrum, against spectra of similar compounds, or against spectra predicted from mechanisms of ion decompositions Remember to follow SIP step-by-step in order.

  12. Library Databases • Databases are critical for even the most grizzled MS veterans • EI databases • NIST’s Chemistry WebBook @ • http://webbook.nist.gov/chemistry • 6000 molecules, but free and on the web • NIST off-line, Wiley, Palisades • • Hundreds of thousands of molecules, $2k-$8k

  13. Reproducibility of Spectra

  14. Reproducibility of Spectra • Be aware that database (and other) spectra have limited signal-to-noise and reproducibility • McLafferty examples: • +/- for each peak 10% relative to itself • +/- 0.2 absolute (base peak = 100) • Library spectra depend on instrument used, how long ago, etc.

  15. Reproducibility of Spectra • Be aware that background/leak/contaminant peaks may be present that are not related to the molecule of interest. • Take a “background” spectrum just before your analysis • Make sure m/z values are correct!

  16. High Resolution Information

  17. High Resolution Information

  18. Elemental Composition • Reminder: use high resolution spectra (if at all possible) and always attempt to identify the peaks of every fragment. • Even with unit resolution, the presence of isotopes of known natural abundances provides a useful & simple method.

  19. Isotopic Abundances Note that the isotope of lowest mass is the most abundant for all of these elements. – “A”, “A+1”, and “A+2” elements

  20. A + 2 Elements: Cl, Br, O, S, and Si • Especially prominent in the spectrum • Look for these first!

  21. A + 2 Elements • Linear superposition of isotopic patterns • If there is more than one atom in the molecule of one of the A+2 elements, the result is even more striking

  22. Structural Isomers vs. MS

  23. A + 2 Elements • Oxygen isotopes • The A+2 abundance of O is low (0.2%) • Need high abundance accuracy • Other isotopic patterns can interfere (C), thus estimate number of oxygen after A+1 and other A+2 elements • Absence of A+2 elements • Often they are not there. Value of negative info • If [(X+2)]/[X] < 3%, the peak X cannot contain the most abundant isotope of Si, S, Cl, or Br

  24. A + 1 Elements • 2H/1H is so small that it is considered “A” • Increasing number of C atoms linearly increases the probability that one of them is a 13C (see table 2.2) • A way to deduce the number of carbon atoms • 1.1% of 13C changes ~2% with source • • Don’t worry about N for now (next class) • “Nitrogen Rule” will come to our rescue

  25. Unknown 2.4 • Check for A+2 elements • • Isotopic composition of 43 and 58? • • Loss between 58 and 43? • • Identity of the molecule?

  26. Note about Unknown 2.4 • Note the many small peaks below the major ones, due to neutral losses of H and H2 • If you don’t see those, the molecule likely has no H • Also note that those peaks are less important in determining the structure • Start with the higher m/z (overall and in each group of peaks)

  27. Unknown 2.5 • Is 0.2% at m/z 80 due to an oxygen atom? • Elemental formula of base peak? • Identity of the molecule?

  28. Unknown 2.6

  29. A Elements: H, F, P, and I • After the number of A+1 and A+2 elements have been assigned, A elements should provide the balance of the mass • Use number of atoms consistent with rules of bonding (no CH6 please!) • Note that only H can be used until we need to add 19 (F)

  30. Example 1: • Example 2:

  31. Unknown 2.7

  32. Unknown 2.8

  33. Rings + Double Bonds • Because of the valences, the total number of rings and double bonds in a molecule of the formula CxHyNzOn will be: • Calculate: C4H10 , C6H6 , C5H5N , C7H5O • For ions, the value may end in 0.5 (‘even electron ion’) • More general case AyBnCzDx, where A = H, F, Cl, Br, I; B = O, S; C = N, P; and D = C, Si • Does not count double bonds to elements in higher valence states

More Related