Download
12 structure determination mass spectrometry and infrared spectroscopy n.
Skip this Video
Loading SlideShow in 5 Seconds..
12. Structure Determination: Mass Spectrometry and Infrared Spectroscopy PowerPoint Presentation
Download Presentation
12. Structure Determination: Mass Spectrometry and Infrared Spectroscopy

12. Structure Determination: Mass Spectrometry and Infrared Spectroscopy

554 Vues Download Presentation
Télécharger la présentation

12. Structure Determination: Mass Spectrometry and Infrared Spectroscopy

- - - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript

  1. 12. Structure Determination: Mass Spectrometry and Infrared Spectroscopy

  2. Determining the Structure of an Organic Compound • The analysis of the outcome of a reaction requires that we know the full structure of the products as well as the reactants • In the 19th and early 20th centuries, structures were determined by synthesis and chemical degradation that related compounds to each other

  3. Determining the Structure of an Organic Compound • Physical methods now permit structures to be determined directly. We will examine: • mass spectrometry (MS)—this chapter • infrared (IR) spectroscopy—this chapter • nuclear magnetic resonance spectroscopy (NMR)—Chapter 13 • ultraviolet-visible spectroscopy (VIS)—Chapter 14

  4. 12.1 Mass Spectrometry (MS) • Sample vaporized and bombarded by energetic electrons that remove an electron, creating a cation-radical • Bonds in cation radicals begin to break (fragment)

  5. Mass Spectrometer

  6. The Mass Spectrum • Plot mass of ions (m/z) (x-axis) versus the intensity of the signal (corresponding to the number of ions) (y-axis) • Tallest peak is base peak (100%) • Other peaks listed as the % of that peak • Peak that corresponds to the unfragmented radical cation is parent peak or molecular ion (M+)

  7. MS Examples: Methane and Propane • Methane produces a parent peak (m/z = 16) and fragments of 15 and 14 (See Figure 12-2 a)

  8. MS Examples: Methane and Propane • The Mass Spectrum of propane is more complex (Figure 12-2 b) since the molecule can break down in several ways

  9. 12.2 Interpreting Mass Spectra • Molecular weight from the mass of the molecular ion • Double-focusing instruments provide high-resolution “exact mass” • 0.0001 atomic mass units – distinguishing specific atoms • Example MW “72” is ambiguous: C5H12 and C4H8O but: • C5H12 72.0939 amu exact mass C4H8O 72.0575 amu exact mass • Result from fractional mass differences of atoms 16O = 15.99491, 12C = 12.0000, 1H = 1.00783

  10. Other Mass Spectral Features • If parent ion not present due to electron bombardment causing breakdown, “softer” methods such as chemical ionization are used • Peaks above the molecular weight appear as a result of naturally occurring heavier isotopes in the sample • (M+1) from 13C that is randomly present

  11. 12.3 Interpreting Mass-Spectral Fragmentation Patterns • The way molecular ions break down can produce characteristic fragments that help in identification • Serves as a “fingerprint” for comparison with known materials in analysis (used in forensics) • Positive charge goes to fragments that best can stabilize it

  12. 2,2-Dimethylpropane: MM = 72 (C5H12)

  13. Mass Spectral Fragmentation of Hexane • Hexane (m/z = 86 for parent) has peaks at m/z = 71, 57, 43, 29

  14. Hexane

  15. Practice Problem 12.2: methylcyclohexane or ethylcyclopentane?

  16. Mass Spectral Cleavage Reactions of Alcohols • Alcohols undergo -cleavage (at the bond next to the C-OH) as well as loss of H-OH to give C=C

  17. Mass Spectral Cleavage of Amines • Amines undergo -cleavage, generating radicals

  18. Fragmentation of Ketones and Aldehydes • A C-H that is three atoms away leads to an internal transfer of a proton to the C=O, called the McLafferty rearrangement • Carbonyl compounds can also undergo  cleavage

  19. Fragmentation of Ketones and Aldehydes

  20. 12.5 The Electromagnetic Spectrum

  21. Wavelength and Frequency

  22. Absorption Spectra • Organic compounds exposed to electromagnetic radiation can absorb photons of specific energies (wavelengths or frequencies) • Changing wavelengths to determine which are absorbed and which are transmitted produces an absorption spectrum • Energy absorbed is distributed internally in a distinct and reproducible way (See Figure 12-11)

  23. Infrared Absorption Spectrum of Ethanol

  24. 12.6 Infrared Spectroscopy of Organic Molecules • IR region is lower in photon energy than visible light (below red – produces heating as with a heat lamp) • 2.5  106 m to 2.5  105 m region used by organic chemists for structural analysis • IR energy in a spectrum is usually measured as wavenumber (cm-1), the inverse of wavelength and proportional to frequency: • Wavenumber (cm-1) = 1/l(cm) • Specific IR absorbed by organic molecule is related to its structure

  25. IR region and vicinity

  26. Infrared Energy Modes • IR energy absorption corresponds to specific modes, corresponding to combinations of atomic movements, such as bending and stretching of bonds between groups of atoms called “normal modes” • Energy is characteristic of the atoms in the group and their bonding • Corresponds to molecular vibrations

  27. Infrared Energy Modes

  28. 12.7 Interpreting Infrared Spectra • Most functional groups absorb at about the same energy and intensity independent of the molecule they are in • Characteristic IR absorptions in Table 12.1 can be used to confirm the existence of the presence of a functional group in a molecule • IR spectrum has lower energy region characteristic of molecule as a whole (“fingerprint” region)

  29. 4000-2500 cm-1 N-H, C-H, O-H (stretching) 3300-3600 N-H, O-H 3000 C-H 2500-2000 cm-1 CºC and C º N (stretching) 2000-1500 cm-1 double bonds (stretching) C=O 1680-1750 C=C 1640-1680 cm-1 Below 1500 cm-1 “fingerprint” region Regions of the Infrared Spectrum

  30. Regions of the Infrared Spectrum

  31. Differences in Infrared Absorptions • Molecules vibrate and rotate in normal modes, which are combinations of motions (relates to force constants) • Bond stretching dominates higher energy (frequency) modes

  32. Differences in Infrared Absorptions • Light objects connected to heavy objects vibrate fastest (at higher frequencies): C-H, N-H, O-H • For two heavy atoms, stronger bond requires more energy (higher frequency): C º C, C º N > C=C, C=O, C=N > C-C, C-O, C-N, C-halogen

  33. 12.8 Infrared Spectra of Hydrocarbons • C-H, C-C, C=C, C º C have characteristic peaks

  34. Hexane

  35. Alkenes

  36. 1-Hexene

  37. Alkynes

  38. 12.9 Infrared Spectra of Some Common Functional Groups • Spectroscopic behavior of functional groups is discussed in later chapters • Brief summaries presented here

  39. IR: Alcohols

  40. Amines

  41. IR: Aromatic Compounds • Weak C–H stretch at 3030 cm1 • Weak absorptions 1660 - 2000 cm1 range • Medium-intensity absorptions 1450 to 1600 cm1

  42. Phenylacetylene

  43. IR: Carbonyl Compounds • Strong, sharp C=O peak 1670 to 1780 cm1 • Exact absorption characteristic of type of carbonyl compound • 1730 cm1 in saturated aldehydes • 1705 cm1 in aldehydes next to double bond or aromatic ring

  44. Practice problem 12.7:

  45. Phenylacetaldehyde

  46. C=O in Ketones • 1715 cm1 in six-membered ring and acyclic ketones • 1750 cm1 in 5-membered ring ketones • 1690 cm1 in ketones next to a double bond or an aromatic ring