Chapter 17 spectroscopy
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Spectroscopy involves the interaction of electromagnetic radiation with matter. Spectroscopic methods are used to elucidate molecular structure and quantify inorganic and organic compounds. There are several regions of the electromagnetic spectrum used including X-ray, UV, visible, and IR. Important concepts include Beer's law, which states absorbance is proportional to concentration, molar absorptivity, and path length. Spectrophotometry is used for qualitative and quantitative analysis in areas such as determining unknown concentrations. Fluorescence also provides a sensitive technique where molecules emit light at longer wavelengths after absorbing radiation.
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Absorbance powerpoint
1) Spectrophotometry is a technique used to measure how much light of varying wavelengths is absorbed by a substance.
2) The document outlines procedures for using a spectrophotometer to determine the wavelength of maximum absorbance (lambda max) of a basic fuchsin dye solution.
3) It then discusses how to use the Beer-Lambert law to determine the relationship between absorbance and concentration by measuring absorbance values of serial dilutions of the dye solution.
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Spectroscopy is the science dealing with interactions of radiation with matter. The most widely used spectroscopic methods are based on electromagnetic radiation like light, gamma rays, X-rays, UV, microwave, and radio-frequency. When radiation passes through matter, certain frequencies may be absorbed, transferring electromagnetic energy to the sample. Absorption promotes particles from their ground state to higher-energy excited states. Beer's law states that absorbance depends on the total quantity of an absorbing compound in the light path, and absorbance is directly proportional to concentration, path length, and molar absorptivity. Atomic absorption spectroscopy is a quantitative technique applicable to many metals. It works by heating metals so they absorb light at characteristic frequencies, and
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Absorbance powerpoint
1) Spectrophotometry is a technique used to measure how much light of varying wavelengths is absorbed by a substance.
2) The document outlines procedures for using a spectrophotometer to determine the wavelength of maximum absorbance (lambda max) of a basic fuchsin dye solution.
3) It then discusses how to use the Beer-Lambert law to determine the relationship between absorbance and concentration by measuring absorbance values of serial dilutions of the dye solution.
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Based on the information provided, the compound is likely acrylonitrile. Some key points:
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UV-Vis spectrophotometer measure absorption of UV radiation (200-400 nm) and visible light (400-800 nm) by molecule.
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Based on the information provided, the compound is likely acrylonitrile. Some key points:
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This document provides an overview of spectroscopy and its applications. It discusses the basic principles of spectroscopy including how electromagnetic radiation interacts with matter and is detected. It describes different types of spectroscopy including UV-Visible spectroscopy and infrared spectroscopy. It explains concepts such as electronic transitions, chromophores, auxochromes, and how they relate to absorption spectra. Examples are provided to illustrate these concepts and spectroscopy techniques.
Photochemistry
Photochemistry is the study of the interaction of electromagnetic radiation with matter, which can result in physical or chemical changes. Key aspects of photochemistry include that a molecule must absorb light for a reaction to occur, and that the radiation energy must match the energy difference between the ground and excited electronic states. There are two main types of photochemical processes: photophysical processes involve light absorption but no chemical reaction, while photochemical or photochemical reactions are brought about by light absorption in the visible and UV regions.
Uv-visible spectroscopy
This document provides an overview of UV-visible spectroscopy. It discusses the electromagnetic spectrum and how light exhibits both wave and particle properties. It explains the basic components and principles of UV-visible spectrometers, including sources such as tungsten lamps and lasers, wavelength selectors like monochromators, sample containers, and various types of detectors. It also covers important concepts such as Beer's law, deviations from Beer's law, and the factors that affect spectroscopic measurements.
UV-VIS Spectroscopy
UV-VIS spectroscopy involves using ultraviolet or visible light to illuminate a sample and analyzing the light that is absorbed. Electronic transitions in molecules can be detected by observing which wavelengths of light are absorbed. This provides information about functional groups and conjugated systems present in the sample. A UV-VIS spectrophotometer directs light from a source through the sample solution and a monochromator selects wavelengths, which are then measured by a detector. The amount of light absorbed at each wavelength follows Beer's Law, allowing for determination of concentrations from a calibration curve.
Spectroscopy.PPT
Colorimeter and Spectrophotometer
Electromagnetic Radiation
EMR
THE ELECTROMAGNETIC SPECTRUM
Interaction of e.m.r. with Matter
Molecular Spectra
Spectrophotometry
Principles OF Spectrophotometry
uv.pptx
Ultraviolet-visible spectroscopy involves promoting electrons from the highest occupied molecular orbital to the lowest unoccupied molecular orbital when molecules absorb electromagnetic radiation. This causes different types of electronic transitions that can be observed based on wavelength shifts. The technique follows Beer's law where absorbance is directly proportional to concentration and path length. It is used to determine conjugation and identify functional groups in molecules.
UV / Visible Spectroscopy
This document discusses UV/Visible spectroscopy. It begins by defining spectroscopy as the study of interaction between electromagnetic radiation and matter. It then discusses the different types of spectroscopy including UV spectroscopy, IR spectroscopy, NMR spectroscopy, and emission spectroscopy. The document focuses on UV/Visible spectroscopy. It discusses electromagnetic radiation, including frequency, wavelength, and the relationship between them. It also discusses how electromagnetic radiation interacts with matter through electronic, vibrational, and rotational energy levels. The document then explains the principles of spectroscopy including Lambert's law and Beer's law. It discusses terms such as chromophores and auxochromes as they relate to UV/Visible spectroscopy.
Spectropotometer.08.20 - Copy.ppt
Here are the answers to your questions:
1. To determine molar absorptivity (ε) and specific absorbtivity (A), measure the absorbance (A) of solutions with known concentrations (c) and pathlengths (l). Molar absorptivity is calculated as ε = A/cl. Specific absorbtivity is calculated as A = εcl.
2. The grating in a spectrophotometer functions to separate polychromatic light into its component wavelengths (monochromatic light). It does this via the principle of diffraction - the grating grooves act like multiple slits that diffract light at different angles depending on the wavelength.
3. The main parts of a mon
Colorimetry B.Sc.III
1. Colorimetry uses the measurement of light absorption to determine the concentration of colored compounds in solution.
2. Lambert's law and Beer's law describe the relationship between light absorption and characteristics of the absorbing medium like concentration and path length.
3. Beer's law states that absorbance remains constant when concentration and path length are changed in inverse proportion, allowing for determination of unknown concentrations.
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Ultraviolet spetroscopy by Dr. Monika Singh part-1 as per PCI syllabus
Ultraviolet spetroscopy by Dr. Monika Singh part-1 as per PCI syllabus
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Here are the steps to solve this problem:
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Moles of Ag+ = (0.0100 M) * (0.025 L) = 2.5 x 10-5 moles
2) Volume of EDTA solution = 15 mL
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4) Kf' = α * Kf
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* HCl is a strong acid and will titrate first
* Its equivalence point was at 35.00 mL of NaOH
* NaOH concentration is 0.100 M
* Moles of NaOH used = Volume x Concentration
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* Moles of HCl = Moles of NaOH used = 0.003500 mol
* H3PO4 is a weak acid and will titrate second
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* Moles of additional Na
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Chapter 17 spectroscopy
- 1. Chapter 17-18: Spectrophotometry Spectroscopy – the interaction of radiation and matter Spectroscopic methods measure the amt of radiation produced or absorbed Elucidation of molecular structure Qual./Quant. Detn. of inorganic and organic compds Classify Region of the electromagnetic spectrum X-ray UV Visible IR
- 2. Electromagnetic radiation – as a wave Waves – properties of wavelength, frequency, velocity, amplitude Particles – discrete packets of energy called photons
- 4. Important Equations E = hν νλ= c V = 1/λ E = hc/λ E = hcV c = 2.998 x 1010 cm/s h = 6.626 x 10-34 Js UV: 180- 380 nm Vis: 380 – 780 nm Near IR: 0.78 – 2.5 µm Far IR: 2.5 – 50 µm Memorize Memorize wavenumber
- 5. What happens when a molecule absorbs a photon of light? Energy increases GS ES E = hc/λ M + hν M* Energy absorbed = exactly the energy difference between those states
- 6. Three Basic Transitions 1- rotational (lower energy) 2- vibrational 3- electronic (higher energy) Pure Vibrational IR region Pure Rotational Microwave UV-Vis: move bonding (outer valence electrons)
- 8. σ σ* ∆E large (λ<150 nm) nσ* (halogens, N, O, S) ∆E smaller (λ=150-250 nm) ππ* nπ* ∆E small (λ=200-700 nm) UV-Vis: move bonding (outer valence electrons) GS ES E = hc/λ M + hν M* Know this.
- 9. Organic Chromophores From Skoog, West, Holler
- 10. Clicker questions If E = 600 KJ/mol , what is the wavelength in nm? If E = 160 KJ/mol , what is the wavelength in nm? Hint: 6.023 x 1023 photons/mol
- 11. Instrumentation
- 12. Basis Radiation goes through the sample, certain frequencies are removed via absorption Plot A vs λ determine what frequencies are absorbed A λ Broad: why?
- 13. From Skoog, West, Holler Why are lines narrower in vapor phase?
- 14. When radiation interacts with matter 1. Some transmitted through sample 2. Some absorbed by the sample 3. Some reflected at each surface 4. Some scattered by dust…. Absorption - Transmission P0 P T = P/P0 %T = P/Po x 100% A = -log T A = 2 – Log %T Memorize
- 15. Quantitative Chemical Analysis Beer’s Law: A = abc a = absorptivity b = pathlength c = concentration If C has units of M and b has units of cm, A = εbc ε = molar absorptivity (M-1 cm-1 ) Memorize Beer’s Law is additive:
- 16. 1. Chemical A. Dilute Solutions B. Analyte dissociates/associates…. HIn = H+ + In- color 1 color 2 Limitations of Beer’s Law 1. Instrumental 2. Chemical
- 17. 2. Instrumental A. Polychromatic radiation Beer’s law valid for monochromatic radiation From Skoog, West, Holler
- 18. B. Stray light Scattered radiation… “stray” Usually a different λ and may not have passed through the sample
- 19. Example A solution contains 1.00 mg of K3Fe(CN)6 (FW 328.26) in 100.0 mL. It transmits 70.0% of incident light compared to a blank in a 1.00 cm cell. Calculate molar absorptivity? Clicker Question:
- 20. Applications and Fluorescence Qualitative Analysis Supplemental to other techniques (lacks structure) Detect certain chromophoric group Compare to other spectra Quantitative Analysis Molecule must absorb UV-Vis radiation Beers Law must be obeyed Moderately sensitive, 10-4 – 10-6 M Moderately selective Good accuracy Relatively easy, convenient, rapid
- 21. Details of Analysis Properly select wavelength Properly clean and handle sample cells Chose standard solutions carefully Proper concentration and composition
- 22. Standard Addition Method Match the overall composition of the samples keep the matrix constant Impt for solns with complex composition C A Single Point Method Multiple additions Extension of the calibration curve method Involves addition of known quantity of std to unk
- 23. Photometric Titrations S + t = P εs εt εp εs = 0 εt > 0 εp = 0 A Vol Used to locate equiv. Point Beers Law must be obeyed Correct A for volume changes Know how sketch these for different species S= substrate, analyte T = titrant P = product
- 24. Fluorescence Emission process Molecules excited by absorption of electromagnetic radiation, lose excess energy via photon emission Very sensitive (ppb) Limited number of compds fluoresce (aromatic) M + hν → M* M* → M + heat M* → M + hν Emits at a longer wavelength than it absorbs
- 25. Energy level Diagram Vibrational relaxation Internal conversion Intersystem crossing Fluorescence Phosphorescence Fluorescence
- 28. Instrument components Source (mercury arc lamp) Monochromator Sample (right angles) Photomultiplier tube 900 : why?
- 29. Quantitative Chemical Analysis F = kC (at constant P0) Linear at low concentrations Why drop in I ?
- 30. A compound with a molecular weight of 125.0 has a molar absorptivity of 2.5 x 105 M-1 cm-1 . How many grams of this compound should be dissolved in 1.00 L such that after a 200-fold dilution the resulting solution will give an absorbance of 0.60 in a 1.0 cm cell Clicker question
- 31. Cytochrome c has a molar absorptivity of 106,000 M-1 cm-1 . 100 uL of a solution cyt. C is diluted to 1.00 mL. The Absorbance of the diluted solution is 0.30 in a 1.0 mm cell. Calculate the concentration of cyt. C in the original soln.
- 32. A 2.00 mL specimen was treated with reagents to generate color with phosphate following which the sample was diluted to 100.0 mL. Photometric measurement for the phosphate in a 25.0 mL aliquot yielded an absorbance of 0.428. Addition of 1.00 mL of a solution containing 0.0500 mg of phosphate to a second 25.0 mL aliquot resulted in an absorbance of 0.517. Calculate the mgs of phosphate in each milliliter of the specimen. Clicker question
- 33. Quinine in a 1.664 g antimalarial tablet was dissolved in sufficient 0.10 M HCL to give 500.0 mL of solution. A 15.00 mL aliquot was then diluted to 100.0 mL with the acid. The fluorescent intensity for the diluted sample at 347 nm provided a reading of 288 on an arbitrary scale. A standard 100.0-ppm Quinine solution registered 180 when measured under identical conditions. Calculate the mgs of quinine in the tablet Clicker question (fluorescence)