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19 Cards in this Set
- Front
- Back
Spectroscopy
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Interaction of nuclei, atoms, ions, or molecules with electromagnetic radiation.
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Electromagnetic radiation (EM)
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- a sinusoidal electric and magnetic wave traveling through the space
- a discrete series of “particles” that have a specific energy but have no mass, photons |
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Wave Properties of EM Radiation: wavelength
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Linear distance between two equivalent points on successive waves.
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Wave Properties of EM Radiation: amplitude (A)
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The length of electric vector at a maximum
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Wave Properties of EM Radiation: frequency
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The number of oscillations occurred per sec.
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Wave Properties of EM Radiation: period (T)
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Time for 1 wavelength to pass a fixed point; =1/freq
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Wave Properties of EM Radiation: velocity (V)
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vi=wavelentghi * freq (c=2.99792x10^8 m/s)
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Wave Properties of EM Radiation: Diffraction
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Parallel electromagnetic wave can be bend when passing through a narrow opening (width ~ wavelength).
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Wave Properties of EM Radiation: Constructive interference (intense band)
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can be observed when the difference in path length from two slits is equal to wavelength (first order interference), or 2wavelength, 3 wavelength... corresponding to difference between two phase angles = 2nPi, n is an integral 1,2,3...
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Wave Properties of EM Radiation: Transmission
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Velocity of wave propagation (m/s) = wavelength(m) x frequency (s^-1).
- In a vacuum: electromagnetic wave travels at the speed of light, c = 3.00 x108 m/s - In other media, frequency remains constant, wavelength and thus v decreases vi=c/ni ni: the medium refractive index >=1 (liquids 1.3-1.8, solids >=1.3) see lecture 3! |
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Particle Description of Radiation: Particle Properties
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According to Photoelectric Effect experiment:
- energy of a photon can be related to its frequency E (J) = h * freq where h is Planck's constant 6.6254x10^-34 J*s energy is inversely proportional to the wavelength freq= c/wavelength -> E=hc/wavelength |
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Commonly Used Units (Wavelength units vary with spectral region)
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X-ray & short UV: Angstrom = 10^-10m
UV/Visible range: nm=10^-9m µm=10^-6 Infrared range: µm Photon energy: - X-ray region: eV 1J = 6.24x10^18 eV - Visible region: kJ/mol = J/photon x 6.02x10^23 photon/mol x10^-3 kJ/J |
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Interaction with Matter: Postulates of Quantum Mechanics
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Atoms, ions and molecules exist in discrete energy states only -- quantized.
E0: ground; E1 E2 E3 exited states. Exitation can be electronic, vibrational or rotational. Enegery levels of atoms, ions or molecules all different -> measuring energy levels gives means of identification of chemical species - spectroscopy |
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Interaction with Matter: Absorption spectra - Atoms
(Just as in emission spectra an atom, ion or molecule can only absorb radioation if energy matches separation between two energy states) |
Atoms: No vibrational or rotation energy levels - sharp line spectra with few features
Na 3s->3p 589.0, 589.6 nm (yellow) For valence excitation, visible energy. For core (inner) excitation, UV and X-ray energy. For absorption to occur, the energy of incident beam must correspond to one of the energy difference. Measurement of the amount of light absorbed as a function of wavelength. |
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Interaction with Matter: Absorption spectra - Molecules
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Electronic, vibrational and rotational energy levels all involved.
Each electronic state – many vibrational states Each vibrational states – many rotational states E = Eelec + Evib + Erot -> broad band spectra with many features |
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Interactions with Matter: Photoluminescence Spectra
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- Photoluminescence methods (fluorescence and phosphorescence)
- Fluorescence: prompt emission - Phosphorescence: delayed emission |
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Interactions with Matter: Relaxation Process
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Lifetime of excited state is short (fs->ms)
Nonradiative relaxation: loss of energy by collisions, happpens in a series of small steps. Tiny temperature rise of surrounding species. Radiative relaxation (emission): Fluorescence (<10^-5s) |
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Stokes shift:
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Emission has a lower frequency than the radiation (due to vibrational relaxation occurs before fluorescence)
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Major Classes of Spectrochemical Methods
see lecture! |
- Emission (Method: Atomic emission)
- Luminescence (Method: Atomic and molecular fluorescence, phosphorescence and chemiluminescence) - Scattering (Method: Raman scattering, turbidimetry, and particle sizing) - Absorption (Method: Atomic and molecular absorption) |