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CHEM 344

CHEM 344. Spectroscopy of Organic Compounds Lecture 1 4th and 5 th September 2007. Modern Spectroscopic Methods. Revolutionized the study of organic chemistry Can determine the exact structure of small to medium size molecules in a few minutes

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CHEM 344

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  1. CHEM 344 Spectroscopy of Organic Compounds Lecture 1 4th and 5th September 2007

  2. Modern Spectroscopic Methods • Revolutionized the study of organic chemistry • Can determine the exact structure of small to medium size molecules in a few minutes • Nuclear Magnetic Resonance (NMR) and Infrared Spectroscopy (IR) are particularly powerful techniques which we will focus on and use in this course

  3. Interaction of Light and MatterThe Physical Basis of Spectroscopy • Spectroscopy: the study of molecular structure by the interaction of electromagnetic radiation with matter • Electromagnetic spectrum is continuous and covers a very wide range of wavelengths • Wavelengths (l) range from 103to 10-15 meters

  4. The Electromagnetic Spectrum

  5. Relationship Between Wavelength, Frequency and Energy • Speed of light (c) is constant for all wavelengths • Frequency (n), the number of wavelengths per second, is inversely proportional to wavelength: n = c/l • Energy of a photon is directly proportional to frequency E = hc/l = hn (where h = Plank’s constant)

  6. Energy Levels in Molecules • Energy levels within a molecule are discrete (quantized) • Transitions between various energy levels occur only at discrete energies • Transition caused by subjecting the molecule to radiation of an energy that exactly matches the difference in energy between the two levels Eupper – Elower = ΔE = hn

  7. Wavelength/Spectroscopy Relationships

  8. Nuclear Spins • Spin ½ atoms: mass number is odd 1H, 13C, 19F, 29Si, 31P • Spin 1 atoms: mass number is even 2H, 14N • Spin 0 atoms: mass number is even 12C, 16O, 32S NO NMR SIGNAL

  9. Magnetic Properties of the Proton Related to Spin

  10. Energy States of Protons in a Magnetic Field No External Mag. Field External Mag. Field Bo Spin states degenerate Random orientations Two allowed orientations (2I+1) = 2 Aligned with or against direction of Bo

  11. Nuclear Magnetic Resonance (NMR) • Nuclear – spin ½ nuclei (e.g. protons) behave as tiny bar magnets • Magnetic – a strong magnetic field causes a small energy difference between + ½ and – ½ spin states • Resonance – photons of radio waves can match the exact energy difference between the + ½ and – ½ spin states resulting in absorption of photons as the protons change spin states

  12. The NMR Experiment • The sample, dissolved in a suitable NMR solvent (e.g. CDCl3, CCl4, C6D6), is placed in the strong magnetic field of the NMR spectrometer • The sample is bombarded with a series of radio frequency (Rf) pulses and absorption of the radio waves is monitored • The data are collected and manipulated on a computer to obtain an NMR spectrum

  13. An NMR Spectrometer

  14. Our NMR Spectrometer

  15. PNNL NMR Spectrometer

  16. The NMR Spectrum • The vertical axis shows the intensity of Rf absorption • The horizontal axis shows relative energy at which the absorption occurs (parts per million, ppm) • Tetramethylsilane (TMS, SiMe4) is included as a standard zero point reference (0.00 ppm) • The area under any peak corresponds to the number of hydrogens represented by that peak

  17. NMR Spectrum of p-Xylene

  18. Chemical Shift (d) • The chemical shift (d) in units of ppm is defined as: d =shift from TMS (in Hz) radio frequency (in MHz) • A standard notation is used to summarize NMR spectral data. For example p-xylene: d 2.3 (6H, singlet) d 7.0 (4H, singlet) • Hydrogen atoms in identical chemical environments have identical chemical shifts

  19. Shielding – The Reason for Chemical Shift Differences • Circulation of electrons within molecular orbitals results in local magnetic fields that oppose the applied magnetic field • The greater this “shielding” effect, the greater the applied field needed to achieve resonance, and the further to the right (“upfield”) the NMR signal

  20. Structural Effects on Shielding • Electron donating groups increase the electron density around nearby hydrogen atoms resulting in increased shielding, shifting peaks to the right. • Electron withdrawing groups decrease the electron density around nearby hydrogen atoms resulting in decreased shielding, (deshielding) shifting peaks to the left (downfield).

  21. Structural Effects on Shielding The deshielding effect of an electronegative substituent can be seen in the 1H-NMR spectrum of 1-bromobutane: Br – CH2-CH2-CH2-CH3 d (ppm): 3.4 1.8 1.5 0.9 No. of H’s: 2 2 2 3

  22. Some Specific Structural Effects on NMR Chemical Shift

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