1 / 28

INTRODUCTION TO

INTRODUCTION TO. SPECTROSCOPY. BY G. RAM KUMAR Department of Chemistry Pydah College P.G. Courses. INTRODUCTION TO SPECTROSCOPY It is the most powerful tool available for the study of atomic and molecular structures. It is used in the analysis of wide range of samples.

kaiya
Download Presentation

INTRODUCTION TO

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. INTRODUCTION TO SPECTROSCOPY BY G. RAM KUMAR Department of Chemistry Pydah College P.G. Courses

  2. INTRODUCTION TO SPECTROSCOPY • It is the most powerful tool available for the study of atomic and molecular structures. • It is used in the analysis of wide range of samples. What is spectroscopy? Spectroscopy may be defined as the study of interactions between the matter and Electro Magnetic Radiations.

  3. TYPES OF SPECTROSCOPY • Atomic Spectroscopy : It is concerned with interactions of Electro Magnetic Radiations with atoms. • Molecular Spectroscopy : It is concerned with interactions of • Electro Magnetic Radiations with molecules . • In general all the Spectroscopic methods are classified into two. • Non-Destructive methods Ex:UV-Visible , IR , NMR. • Destructive methods Ex:FES , AAS , ICP-MS.

  4. ELECTROMAGNETIC RADIAIONS Electromagnetic radiation is an oscillating electric and magnetic disturbance that spreads as a wave through empty space, the vacuum

  5. CHARACTERISTICS OF ELECTROMAGNETIC RADIATIONS • Wave length(λ): It is the distance between two crests or troughs. • Units: Å Angstroms or Nanometers nm • 1 Å=10-8cm=10-10m • 1nm=10 Å=10-9cm • Frequency(υ): It is defined as the number of waves which can pass through a point in one second. • Units: Hertz(Hz); Fresnel • 1Hz = 1cycle/sec; 1Fresnel = 1012 Hz

  6. Wave Number(ΰ): It is the reciprocal of wave length and is defined as the total number of waves which can pass through a space of 1cm. • Units: cm-1 or m-1 • 1cm-1 is sometimes called 1KAYSER(K) • Velocity(v): It is the distance travelled by a wave in 1sec. • Units: cm/sec or m/sec

  7. DISPERSION OF LIGHT When visible light (White light) is passed through prism, it split up into seven colors which corresponds to definite wave lengths.This is known as dispersion of light

  8. Visible and Ultraviolet Spectroscopy

  9. SPECTRUM: The series of color bands obtained by dispersion of light is known as spectrum. In a spectrum all these bands are arranged in the increasing order of wave length

  10. CLASSIFICATION OF SPECTRA: I 1.LINE SPECTRA : Spectrum obtained by interaction of electromagnetic radiations with atoms. Line spectra consists of sharp well defined lines that correspond to a definite frequency 2.BAND SPECTRA: Spectrum obtained by interaction of electromagnetic radiations with molecules.Band spectra consists of different bands just as visible spectrum.

  11. II CONTINUOUS SPECTRUM: In a spectrum, if one color merges into another without a gap, then the spectrum is known as Continuous spectrum. DISCONTINUOUS SPECTRUM: In a spectrum , if one color will not merge into other is known as Discontinuous spectrum.

  12. III ABSORPTION SPECTRUM: If the electromagnetic radiations are passed through a substance, the dark pattern of lines that are obtained corresponding to wave lengths absorbed is known as Absorption spectrum . EMISSION SPECTRUM: If electromagnetic radiations are passed through a substance, the pattern of lines recorded after the emission of the absorbed wave lengths are known as emission spectrum.

  13. ELECTROMAGNETIC SPECTRUM The arrangement of electromagnetic waves or radiations in the order of their increasing wave lengths or decreasing frequencies is called electromagnetic spectrum.

  14. Interactions of Different types of Electromagnetic Radiations produce different types of Spectroscopy Regions of EM spectrum Radio frequency region Microwave region Infrared region UV & Visible region Type of sepctroscopy Nuclear magnetic resonance or electron spin resonance Rotational spectroscopy Vibrational spectroscopy Electronic spectroscopy

  15. Electronic Excitation by UV/Vis Spectroscopy : UV: valance electronic excitation Radio waves: Nuclear spin states (in a magnetic field) IR: molecular vibrations X-ray: core electron excitation

  16. The wavelength and amount of light that a compound absorbs depends on its molecular structure and the concentration of the compound used. The concentration dependence follows Beer’s Law. A=ebc Where A is absorbance (no units, since A = log10P0/ P ) e is the molar absorbtivity with units of L mol-1 cm-1 b is the path length of the sample - that is, the path length of the cuvette in which the sample is contained (typically in cm). c is the concentration of the compound in solution, expressed in mol L-1

  17. Molecules have quantized energy levels: ex. electronic energy levels. hv } energy energy  = hv Q: Where do these quantized energy levels come from? A: The electronic configurations of associated with bonding. Each electronic energy level (configuration) has associated with it the many vibrational energy levels we examined with IR.

  18. max = 135 nm (a high energy transition) Absorptions having max < 200 nm are difficult to observe because everything (including quartz glass and air) absorbs in this spectral region.

  19. = hv =hc/ Example: ethylene absorbs at longer wavelengths: max = 165 nm = 10,000

  20. The n to pi* transition is at even lower wavelengths but is not as strong as pi to pi* transitions. It is said to be “forbidden.” Example: Acetone: n max = 188 nm ; = 1860 n max = 279 nm ; = 15

  21.  135 nm  165 nm n 183 nm weak  150 nm n 188 nm n 279 nm weak 180 nm A 279 nm 

  22. Conjugated systems: Preferred transition is between Highest Occupied Molecular Orbital (HOMO) and Lowest Unoccupied Molecular Orbital (LUMO). Note: Additional conjugation (double bonds) lowers the HOMO-LUMO energy gap: Example: 1,3 butadiene: max = 217 nm ; = 21,000 1,3,5-hexatriene max = 258 nm ; = 35,000

  23. Similar structures have similar UV spectra: max = 240, 311 nm max = 238, 305 nm max = 173, 192 nm

  24. Woodward-Fieser Rules for Dienes   Homoannular Heteroannular Parent l=253 nm l=214 nm =217 (acyclic) Increments for: Double bond extending conjugation +30   Alkyl substituent or ring residue +5   Exocyclic double bond    +5 Polar groupings:   -OC(O)CH3    +0   -OR    +6   -Cl, -Br   +5   -NR2 +60   -SR +30 exocyclic Homoannular heteroannular acyclic For more than 4 conjugated double bonds: max = 114 + 5(# of alkyl groups) + n(48.0-1.7n)

  25. Parent: 214 (heteroannular) 3 alkyls +15 (3x5) +5 (exocyclic) TOTAL 234 nm (Actual = 235 nm) Parent: 253 (homoannular) 3 alkyls +15 (3x5) +5 (exocyclic) TOTAL 273 nm (Actual = 275 nm) Parent: 202 (5-member ring ketone) +35 (alpha hydroxyl) +12 (beta alkyl - note part of ring) Total: 249

  26. max = 114 + 5(8) + 11*(48.0-1.7*11) = 476 nm max(Actual) = 474.

More Related