12 structure determination mass spectrometry and infrared spectroscopy
Download
1 / 62

12. Structure Determination: Mass Spectrometry and Infrared Spectroscopy - PowerPoint PPT Presentation


  • 89 Views
  • Uploaded on
  • Presentation posted in: General

12. Structure Determination: Mass Spectrometry and Infrared Spectroscopy. Based on McMurry’s Organic Chemistry , 7 th edition. Determining the Structure of an Organic Compound.

loader
I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
capcha

Download Presentation

12. Structure Determination: Mass Spectrometry and Infrared Spectroscopy

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.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -

Presentation Transcript


12 structure determination mass spectrometry and infrared spectroscopy
12. Structure Determination: Mass Spectrometry and Infrared Spectroscopy

Based on

McMurry’sOrganic Chemistry, 7th edition


Determining the structure of an organic compound
Determining the Structure of an Organic Compound Spectroscopy

  • 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


Determining the structure of an organic compound1
Determining the Structure of an Organic Compound Spectroscopy

  • 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


12 1 mass spectrometry ms
12.1 Mass Spectrometry (MS) Spectroscopy

  • Sample vaporized and bombarded by energetic electrons that remove an electron, creating a cation-radical

  • Bonds in cation radicals begin to break (fragment)


Mass spectrometer
Mass Spectrometer Spectroscopy


Mass spectrometer1
Mass Spectrometer Spectroscopy


The mass spectrum
The Mass Spectrum Spectroscopy

  • 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+)


Ms examples methane and propane
MS Examples: Methane and Propane Spectroscopy

  • Methane produces a parent peak (m/z = 16) and fragments of 15 and 14


Ms examples methane and propane1
MS Examples: Methane and Propane Spectroscopy

  • The Mass Spectrum of propane is more complex (Figure 12-2 ) since the molecule can break down in several ways



12 2 interpreting mass spectra
12.2 Interpreting Mass Spectra Spectroscopy

  • 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


Other mass spectral features
Other Mass Spectral Features Spectroscopy

  • 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


Interpreting mass spectral fragmentation patterns
Interpreting Mass-Spectral Fragmentation Patterns Spectroscopy

  • 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


2 2 dimethylpropane mm 72 c 5 h 12
2,2-Dimethylpropane: SpectroscopyMM = 72 (C5H12)


Mass spectral fragmentation of hexane
Mass Spectral Fragmentation of Hexane Spectroscopy

Hexane (m/z = 86 for parent) has peaks at m/z = 71, 57, 43, 29


Hexane
Hexane Spectroscopy


Worked example 12 1 methylcyclohexane or ethylcyclopentane
Worked example 12.1: Spectroscopymethylcyclohexane or ethylcyclopentane?


Mass spectral cleavage reactions of alcohols
Mass Spectral Cleavage Reactions of Alcohols Spectroscopy

  • Alcohols undergo -cleavage (at the bond next to the C-OH) as well as loss of H-OH to give C=C


Mass spectral cleavage of amines
Mass Spectral Cleavage of Amines Spectroscopy

  • Amines undergo -cleavage, generating radicals


Fragmentation of ketones and aldehydes
Fragmentation of Ketones and Aldehydes Spectroscopy

  • 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



12 4 mass spec in biochemistry tof
12.4 Mass Spec. in Biochemistry: SpectroscopyTOF

  • ESI and MALDI are techniques to produce charged molecules at relatively low energy, to minimize fragmentation.

  • The large biological molecules are separated by Time of Flight analysis (TOF) in a drift tube without a magnetic field imposed.


Maldi tof spectrum of chicken egg white lysozyme
MALDI-TOF Spectroscopy spectrum of chicken egg-white lysozyme




Absorption spectra
Absorption Spectra Spectroscopy

  • 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)



12 6 infrared spectroscopy of organic molecules
12.6 Infrared Spectroscopy of Organic Molecules Spectroscopy

  • 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



Infrared energy modes
Infrared Energy Modes Spectroscopy

  • 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


Infrared energy modes1
Infrared Energy Modes Spectroscopy


12 7 interpreting infrared spectra
12.7 Interpreting Infrared Spectra Spectroscopy

  • 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)


Regions of the infrared spectrum

4000-2500 cm Spectroscopy-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



Differences in infrared absorptions
Differences in Infrared Absorptions Spectroscopy

  • Molecules vibrate and rotate in normal modes, which are combinations of motions (relates to force constants)

  • Bond stretching dominates higher energy (frequency) modes


Differences in infrared absorptions1
Differences in Infrared Absorptions Spectroscopy

  • 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


12 8 infrared spectra of hydrocarbons

C-H, C-C, C=C, C Spectroscopyº C have characteristic peaks

12.8 Infrared Spectra of Hydrocarbons


Hexane1
Hexane Spectroscopy


Alkenes
Alkenes Spectroscopy


1 hexene
1-Hexene Spectroscopy


Alkynes
Alkynes Spectroscopy


12 8 infrared spectra of some common functional groups
12.8 SpectroscopyInfrared Spectra of Some Common Functional Groups

  • Spectroscopic behavior of functional groups is discussed in later chapters

  • Brief summaries presented here


Aromatic compounds
Aromatic compounds: Spectroscopy


Phenylacetylene
Phenylacetylene Spectroscopy


Ir alcohols
IR: Alcohols Spectroscopy

Cyclohexanol


Amines
Amines Spectroscopy


Ir carbonyl compounds
IR: Carbonyl Compounds Spectroscopy

  • 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



Phenylacetaldehyde
Phenylacetaldehyde Spectroscopy


C o in ketones
C=O in Ketones Spectroscopy

  • 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


C o in esters
C=O in Esters Spectroscopy

  • 1735 cm1 in saturated esters

  • 1715 cm1 in esters next to aromatic ring or a double bond


Chromatography purifying organic compounds
Chromatography: Purifying Organic Compounds Spectroscopy

  • Chromatography : a process that separates compounds using adsorption and elution

    • Mixture is dissolved in a solvent (mobile phase) and placed into a glass column of adsorbent material (stationary phase)

    • Solvent or mixtures of solvents passed through

    • Compounds adsorb to different extents and desorb differently in response to appropriate solvent (elution)

    • Purified sample in solvent is collected from end of column

    • Can be done in liquid or gas mobile phase


Principles of liquid chromatography
Principles of Liquid Chromatography Spectroscopy

  • Stationary phase is alumina (Al2O3) or silica gel (hydrated SiO2)

  • Solvents of increasing polarity are used to elute more and more strongly adsorbed species

  • Polar species adsorb most strongly to stationary phase

    • For examples, alcohols adsorb more strongly than alkenes


High pressure or high performance liquid chromatography hplc
High-Pressure (or High-Performance) Liquid Chromatography (HPLC)

  • More efficient and complete separation than ordinary LC

  • Coated silica microspheres (10-25 µm diameter) in stationary phase

  • High-pressure pumps force solvent through tightly packed HPLC column

  • Detector monitors eluting material

  • Figure 12.18: HPLC analysis of a mixture of ten fat-soluble vitamins, using acetonitrile as the mobile phase


Hplc of fat soluble vitamins
HPLC (HPLC) of Fat Soluble Vitamins


Prob 12 32 cyclohexane or cyclohexene
Prob. 12.32: (HPLC)Cyclohexane or Cyclohexene?




Some useful websites
Some Useful Websites: (HPLC)

  • Interpretation of IR spectra (CSU Stanislaus): http://wwwchem.csustan.edu/Tutorials/INFRARED.HTM

  • IR Spectroscopy Tutorial (CU Boulder): http://orgchem.colorado.edu/hndbksupport/irtutor/tutorial.html

  • NIST Chemistry WebBook: http://webbook.nist.gov/chemistry/

  • SDBS Data Base: http://www.aist.go.jp/RIODB/SDBS/menu-e.html


ad
  • Login