This document discusses chromophores, which are groups that absorb electromagnetic radiation in the UV or visible region and impart color to compounds. It defines chromophores and provides examples such as C=C and C=O groups. Chromophores can be independent, requiring only one group to impart color, or dependent, requiring more than one group. The document also discusses auxochromes, which are groups that alter the wavelength and intensity of light absorbed by chromophores. It gives examples of how auxochromes can cause bathochromic, hypsochromic, hyperchromic, or hypochromic shifts in absorption.
This document discusses chromophores and how they absorb electromagnetic radiation. It defines a chromophore as a covalently bonded group that absorbs UV or visible light. Common chromophores include C=C, C=O, and NO2 groups. Chromophores can be independent, requiring only one group to impart color, or dependent, requiring more than one group. Auxochromes are groups that alter the wavelength and intensity of absorption when attached to a chromophore. Absorption maxima can be bathochromically or hypsochromically shifted and absorption intensity can be hyperchromically or hypochromically altered.
Optical rotatory dispersion (ORD) is the variation in optical rotation of a substance with changing wavelength of light. ORD can determine the absolute configuration of chiral molecules like metal complexes. It works by measuring how fast left and right circularly polarized light travels through a sample. A polarimeter measures the optical rotation as a function of wavelength in ORD spectroscopy. Key effects seen in ORD spectra include the Cotton effect, where peaks and troughs appear near absorption bands due to differences in how left and right polarized light interact with chiral molecules. ORD can be used to analyze chiral compounds and determine their stereochemistry.
FACTORS AFFECTING IR VIBRATIONAL FREQUENCIES.pdfSudha durairaj
This presentation discuss about he factors affecting IR vibrational frequencies. It discuss about various factors such as Bond Order, Fermi resonance, Inductive effect etc..
This document provides an overview of UV-Visible Spectroscopy. It discusses the basic principles including electromagnetic radiation, interaction of radiation with matter, and electronic transitions. It describes Beer-Lambert's law and how absorbance is directly proportional to concentration and path length. Different types of electronic transitions like σ→σ*, n→σ*, π→π*, and n→π* are explained. Instrumentation components like radiation sources, monochromators, sample holders and detectors are briefly outlined. Key terms like chromophore, auxochrome, bathochromic shift, hypsochromic shift, hyperchromic effect and hypochromic effect are also defined.
IR spectroscopy analyzes the vibrational frequencies of bonds in molecules to determine their structure. It works by measuring the absorption of IR radiation by molecular bonds. Different functional groups absorb at characteristic frequencies, producing a molecular "fingerprint". IR spectroscopy is useful for identification of unknown compounds, analyzing purity, and monitoring chemical reactions through changes in bond absorption. It is a nondestructive technique applied in various fields such as pharmaceutical analysis, biomedical research, forensic science, and atmospheric studies.
This document discusses chromophores and how solvents affect absorption spectra. It defines a chromophore as a covalently bonded group that absorbs UV or visible radiation. Chromophores are classified as independent or dependent based on the number needed to impart color. Absorption maxima can shift to longer (bathochromic) or shorter (hypsochromic) wavelengths due to auxochromes or solvent changes. Solvent polarity also affects absorption based on the type of electronic transition involved. Temperature and solvent interactions determine the fineness of absorption bands.
This document discusses chromophores, which are groups that absorb electromagnetic radiation in the UV or visible region and impart color to compounds. It defines chromophores and provides examples such as C=C and C=O groups. Chromophores can be independent, requiring only one group to impart color, or dependent, requiring more than one group. The document also discusses auxochromes, which are groups that alter the wavelength and intensity of light absorbed by chromophores. It gives examples of how auxochromes can cause bathochromic, hypsochromic, hyperchromic, or hypochromic shifts in absorption.
This document discusses chromophores and how they absorb electromagnetic radiation. It defines a chromophore as a covalently bonded group that absorbs UV or visible light. Common chromophores include C=C, C=O, and NO2 groups. Chromophores can be independent, requiring only one group to impart color, or dependent, requiring more than one group. Auxochromes are groups that alter the wavelength and intensity of absorption when attached to a chromophore. Absorption maxima can be bathochromically or hypsochromically shifted and absorption intensity can be hyperchromically or hypochromically altered.
Optical rotatory dispersion (ORD) is the variation in optical rotation of a substance with changing wavelength of light. ORD can determine the absolute configuration of chiral molecules like metal complexes. It works by measuring how fast left and right circularly polarized light travels through a sample. A polarimeter measures the optical rotation as a function of wavelength in ORD spectroscopy. Key effects seen in ORD spectra include the Cotton effect, where peaks and troughs appear near absorption bands due to differences in how left and right polarized light interact with chiral molecules. ORD can be used to analyze chiral compounds and determine their stereochemistry.
FACTORS AFFECTING IR VIBRATIONAL FREQUENCIES.pdfSudha durairaj
This presentation discuss about he factors affecting IR vibrational frequencies. It discuss about various factors such as Bond Order, Fermi resonance, Inductive effect etc..
This document provides an overview of UV-Visible Spectroscopy. It discusses the basic principles including electromagnetic radiation, interaction of radiation with matter, and electronic transitions. It describes Beer-Lambert's law and how absorbance is directly proportional to concentration and path length. Different types of electronic transitions like σ→σ*, n→σ*, π→π*, and n→π* are explained. Instrumentation components like radiation sources, monochromators, sample holders and detectors are briefly outlined. Key terms like chromophore, auxochrome, bathochromic shift, hypsochromic shift, hyperchromic effect and hypochromic effect are also defined.
IR spectroscopy analyzes the vibrational frequencies of bonds in molecules to determine their structure. It works by measuring the absorption of IR radiation by molecular bonds. Different functional groups absorb at characteristic frequencies, producing a molecular "fingerprint". IR spectroscopy is useful for identification of unknown compounds, analyzing purity, and monitoring chemical reactions through changes in bond absorption. It is a nondestructive technique applied in various fields such as pharmaceutical analysis, biomedical research, forensic science, and atmospheric studies.
This document discusses chromophores and how solvents affect absorption spectra. It defines a chromophore as a covalently bonded group that absorbs UV or visible radiation. Chromophores are classified as independent or dependent based on the number needed to impart color. Absorption maxima can shift to longer (bathochromic) or shorter (hypsochromic) wavelengths due to auxochromes or solvent changes. Solvent polarity also affects absorption based on the type of electronic transition involved. Temperature and solvent interactions determine the fineness of absorption bands.
INSTRUMENTAL METHODS OF ANALYSIS, B.PHARM 7TH SEM. AND FOR BSC,MSC CHEMISTRY. This is Geeta prasad kashyap (Asst. Professor), SVITS, Bilaspur (C.G) 495001
This document discusses Beer's law and Lambert's law, which describe how the intensity of light passing through an absorbing medium decreases exponentially with increasing thickness and concentration of the medium. It states that Beer's law relates the decrease in intensity to both the thickness and concentration, while Lambert's law relates it only to thickness. The document also describes deviations from the linear relationship predicted by these laws that can occur, including positive deviations where concentration changes have a greater than expected effect, and negative deviations where changes have a smaller effect. Possible causes of deviations, both instrumental and physicochemical, are outlined.
This document provides an overview of the principles of UV-visible spectroscopy. It discusses how UV-visible spectroscopy involves exciting electrons from lower to higher orbital energies using electromagnetic radiation between 200-800nm. The absorption of radiation is dependent on the structure of the compound and type of electron transition. The main types of electron transitions are σ->σ*, n->π*, π->π*, and n->σ*. Selection rules determine which transitions are allowed. UV-visible spectroscopy is used in pharmaceutical analysis for qualitative, quantitative, and structural analysis of compounds in solution.
UV-visible spectroscopy is a technique that uses light in the visible and adjacent ranges. It works by measuring how much light is absorbed by a sample at each wavelength.
The document discusses the basic principles of spectroscopy, including how electromagnetic radiation interacts with matter. It describes the laws of absorption, specifically Beer's law, which states that absorbance is proportional to concentration.
The key aspects of instrumentation are outlined, including light sources, wavelength selectors like monochromators, sample holders, and detection devices. Single beam and double beam spectrophotometers are explained as the main types of instruments used in UV-visible spectroscopy.
This document discusses absorption laws, chromophores, and limitations in ultraviolet-visible spectroscopy. It describes Beer's law and Lambert's law, which state that absorbance is directly proportional to concentration and path length. Deviations from these laws can occur. Chromophores are groups that absorb specific wavelengths, while auxochromes induce bathochromic shifts. Substituents can cause bathochromic, hypsochromic, hyperchromic, or hypochromic shifts in absorption. UV-Vis spectroscopy has many applications in qualitative and quantitative analysis.
Beer's law and Lambert's law describe the absorption of light in materials. Beer's law states that absorbance is directly proportional to concentration, while Lambert's law states absorbance is directly proportional to path length. Beer and Lambert combined their laws into the Beer-Lambert law, which states absorbance is equal to the molar absorptivity (a constant for a given substance and wavelength) multiplied by the path length and concentration. The Beer-Lambert law is commonly used for quantitative analysis but has limitations at very high concentrations due to interactions between molecules.
The Beer-Lambert Law describes how the intensity (I) of monochromatic light is attenuated when passing through a solution due to absorption. I decreases exponentially with increasing concentration (c) of the absorbing material, according to Beer's Law, and with increasing path length (l) through the material, according to Lambert's Law. The relationship can be expressed as: A (or extinction, E) = kcl, where k is the material's molar extinction coefficient and c and l have the above definitions. A plot of E versus c at constant l will yield a straight line passing through the origin.
This document discusses adsorption chromatography, which involves the adsorption of solutes onto the surface of a stationary phase. Key points include:
- Adsorption is a surface phenomenon where interaction occurs only on the surface of one substance, unlike absorption.
- Common stationary phases used in adsorption chromatography include silica gel, alumina, charcoal, and kieselguhr. Silica gel is the most widely used, with hydroxyl groups facilitating hydrogen bonding.
- Forces between solutes and the adsorbent like dipole-dipole interactions, hydrogen bonding, and van der Waals forces determine how strongly compounds are retained on the stationary phase. Mobile phase composition impacts the balance of
The document discusses how solvents and chromophores affect UV-visible spectroscopy. It states that the solvent exerts influence on the absorption spectrum, with the same drug showing different absorption maxima in different solvents. Common solvents used are water, methanol, ethanol, ether, and cyclohexane. The solvent should not absorb in the region studied and have minimum interaction with solute. Chromophores like conjugated systems, carbonyls, and metal complexes determine absorption. Factors like conjugation, auxochromes, and solvent polarity can shift absorption maxima.
Introduction,Instrumentation, Classification of electronic transitions, Substituent and solvent effects, Classification of electronic transitions
Substituent and solvent effects
Applications of UV Spectroscopy
UV spectral study of alkenes
UV spectral study of poylenes
UV spectral study of α, β-unsaturated carbonyl
UV spectral study of Aromatic compounds
Empirical rules for calculating λmax.
Applications of UV Spectroscopy, Empirical rules for calculating λmax.
The document summarizes infrared (IR) spectroscopy, including its principle, instrumentation, applications, and interpretation of spectra. IR spectroscopy works by detecting the vibrational and rotational absorption frequencies of molecules when exposed to IR radiation. The spectrum produced provides information on molecular structure and bonding. Key regions of the IR spectrum correspond to common functional groups like C=O, N-H, and O-H. Analysis of peak positions and relative intensities allows identification of compounds and detection of impurities.
Introduction to Spectroscopy,
Introduction to UV, electronic transitions, terminology, chromophore, Auxochrome, Examples and Applications.
Introduction to IR, Fundamental vibrations, Types of Vibrations, Factors affecting the vibrational freaquencies, Group frequencies, examples and applications.
This document provides an overview of the key components and operating principles of mass spectrometry. It discusses the inlet system, ion sources, mass analyzers, detectors, and vacuum system. Common types of ion sources like electron impact and chemical ionization are described. Popular mass analyzers such as quadrupole, time-of-flight, ion trap, and double focusing are explained. The document also covers the theory behind how mass spectrometry separates ions based on their mass-to-charge ratio and discusses the need for high vacuum levels in mass spectrometers.
The document discusses fluorescence spectroscopy. It defines fluorescence as emission of light that occurs when a substance absorbs light and returns to its ground state, emitting photons. Factors that affect fluorescence include the molecular structure, substituents, concentration, pH, temperature, and viscosity. Instrumentation for fluorescence spectroscopy includes a light source, filters, sample cells, and detectors such as photomultiplier tubes. Applications of fluorescence spectroscopy include determination of inorganic substances, use as fluorescent indicators, pharmaceutical analysis, and liquid chromatography.
This document discusses using infrared spectroscopy to determine the structure of organic compounds. It begins by explaining electromagnetic radiation and the infrared region. It describes the different types of molecular vibrations that can be observed in an infrared spectrum. The document then explains how to interpret an infrared spectrum, noting the functional group and fingerprint regions. It provides examples of interpreting spectra for specific functional groups such as alkenes, alkynes, alcohols, aldehydes, ketones, carboxylic acids, amines and amides. Key absorption bands that identify each functional group are highlighted.
- The document is a presentation on ultraviolet spectroscopy submitted by Moriyom Akhter and Md Shah Alam from the Department of Pharmacy at World University of Bangladesh.
- It defines ultraviolet spectroscopy and discusses key concepts like absorption spectra, types of electronic transitions that can occur, Beer's and Lambert's absorption laws, instrumentation components, and applications in qualitative and quantitative analysis.
- The presentation also examines effects of chromophores and auxochromes on absorption spectra and maximum wavelengths, and how solvents can shift absorption peaks.
This document discusses Beer's law, which states that absorbance of a solution is directly proportional to the concentration of the absorbing material in the solution. It defines Beer's law, derives the mathematical equation, and lists some limitations and sources of deviation from the law, including high concentrations, dissociation/association reactions, use of polychromatic radiation, stray light, and mismatched sample cells. The derivation shows how the Beer's law equation is obtained based on probability of photon absorption in thin sections of the sample.
Fluorimetry involves measuring fluorescence intensity at a particular wavelength using a fluorimeter or spectrofluorimeter. Fluorescence occurs when molecules absorb radiation and electrons are excited to a higher energy state. As electrons return to the ground state, they emit radiation. Factors like concentration, pH, and temperature can affect fluorescence intensity. Instrumentation includes a light source, filters/monochromators, sample cells, and detectors. Applications include determining inorganic/organic substances and compounds in pharmaceutical analysis.
LEC 1 Dyestuff and Colour Science. pptx.pptxNasirSarwar5
Dyestuffs and dyes impart color to substrates like textiles, paper, and plastics. Dyes contain aromatic compounds that absorb certain wavelengths of light, appearing colored. Chromophores are structures within dyes that are responsible for light absorption by altering the energy levels of delocalized electrons. Auxochromes intensify dye color by further modifying electron energies. Factors like hue, strength, and bathochromic/hypsochromic shifts describe dye color properties. Photochromism causes reversible color changes in dyes under light due to cis-trans isomerization of azobenzene structures.
The current presentation explains basics of chromophore and auxochrome concept, types of absorption shift, effect of solvent, its polarity and effect of conjugation on absorption in uv-visible spectroscopy.
INSTRUMENTAL METHODS OF ANALYSIS, B.PHARM 7TH SEM. AND FOR BSC,MSC CHEMISTRY. This is Geeta prasad kashyap (Asst. Professor), SVITS, Bilaspur (C.G) 495001
This document discusses Beer's law and Lambert's law, which describe how the intensity of light passing through an absorbing medium decreases exponentially with increasing thickness and concentration of the medium. It states that Beer's law relates the decrease in intensity to both the thickness and concentration, while Lambert's law relates it only to thickness. The document also describes deviations from the linear relationship predicted by these laws that can occur, including positive deviations where concentration changes have a greater than expected effect, and negative deviations where changes have a smaller effect. Possible causes of deviations, both instrumental and physicochemical, are outlined.
This document provides an overview of the principles of UV-visible spectroscopy. It discusses how UV-visible spectroscopy involves exciting electrons from lower to higher orbital energies using electromagnetic radiation between 200-800nm. The absorption of radiation is dependent on the structure of the compound and type of electron transition. The main types of electron transitions are σ->σ*, n->π*, π->π*, and n->σ*. Selection rules determine which transitions are allowed. UV-visible spectroscopy is used in pharmaceutical analysis for qualitative, quantitative, and structural analysis of compounds in solution.
UV-visible spectroscopy is a technique that uses light in the visible and adjacent ranges. It works by measuring how much light is absorbed by a sample at each wavelength.
The document discusses the basic principles of spectroscopy, including how electromagnetic radiation interacts with matter. It describes the laws of absorption, specifically Beer's law, which states that absorbance is proportional to concentration.
The key aspects of instrumentation are outlined, including light sources, wavelength selectors like monochromators, sample holders, and detection devices. Single beam and double beam spectrophotometers are explained as the main types of instruments used in UV-visible spectroscopy.
This document discusses absorption laws, chromophores, and limitations in ultraviolet-visible spectroscopy. It describes Beer's law and Lambert's law, which state that absorbance is directly proportional to concentration and path length. Deviations from these laws can occur. Chromophores are groups that absorb specific wavelengths, while auxochromes induce bathochromic shifts. Substituents can cause bathochromic, hypsochromic, hyperchromic, or hypochromic shifts in absorption. UV-Vis spectroscopy has many applications in qualitative and quantitative analysis.
Beer's law and Lambert's law describe the absorption of light in materials. Beer's law states that absorbance is directly proportional to concentration, while Lambert's law states absorbance is directly proportional to path length. Beer and Lambert combined their laws into the Beer-Lambert law, which states absorbance is equal to the molar absorptivity (a constant for a given substance and wavelength) multiplied by the path length and concentration. The Beer-Lambert law is commonly used for quantitative analysis but has limitations at very high concentrations due to interactions between molecules.
The Beer-Lambert Law describes how the intensity (I) of monochromatic light is attenuated when passing through a solution due to absorption. I decreases exponentially with increasing concentration (c) of the absorbing material, according to Beer's Law, and with increasing path length (l) through the material, according to Lambert's Law. The relationship can be expressed as: A (or extinction, E) = kcl, where k is the material's molar extinction coefficient and c and l have the above definitions. A plot of E versus c at constant l will yield a straight line passing through the origin.
This document discusses adsorption chromatography, which involves the adsorption of solutes onto the surface of a stationary phase. Key points include:
- Adsorption is a surface phenomenon where interaction occurs only on the surface of one substance, unlike absorption.
- Common stationary phases used in adsorption chromatography include silica gel, alumina, charcoal, and kieselguhr. Silica gel is the most widely used, with hydroxyl groups facilitating hydrogen bonding.
- Forces between solutes and the adsorbent like dipole-dipole interactions, hydrogen bonding, and van der Waals forces determine how strongly compounds are retained on the stationary phase. Mobile phase composition impacts the balance of
The document discusses how solvents and chromophores affect UV-visible spectroscopy. It states that the solvent exerts influence on the absorption spectrum, with the same drug showing different absorption maxima in different solvents. Common solvents used are water, methanol, ethanol, ether, and cyclohexane. The solvent should not absorb in the region studied and have minimum interaction with solute. Chromophores like conjugated systems, carbonyls, and metal complexes determine absorption. Factors like conjugation, auxochromes, and solvent polarity can shift absorption maxima.
Introduction,Instrumentation, Classification of electronic transitions, Substituent and solvent effects, Classification of electronic transitions
Substituent and solvent effects
Applications of UV Spectroscopy
UV spectral study of alkenes
UV spectral study of poylenes
UV spectral study of α, β-unsaturated carbonyl
UV spectral study of Aromatic compounds
Empirical rules for calculating λmax.
Applications of UV Spectroscopy, Empirical rules for calculating λmax.
The document summarizes infrared (IR) spectroscopy, including its principle, instrumentation, applications, and interpretation of spectra. IR spectroscopy works by detecting the vibrational and rotational absorption frequencies of molecules when exposed to IR radiation. The spectrum produced provides information on molecular structure and bonding. Key regions of the IR spectrum correspond to common functional groups like C=O, N-H, and O-H. Analysis of peak positions and relative intensities allows identification of compounds and detection of impurities.
Introduction to Spectroscopy,
Introduction to UV, electronic transitions, terminology, chromophore, Auxochrome, Examples and Applications.
Introduction to IR, Fundamental vibrations, Types of Vibrations, Factors affecting the vibrational freaquencies, Group frequencies, examples and applications.
This document provides an overview of the key components and operating principles of mass spectrometry. It discusses the inlet system, ion sources, mass analyzers, detectors, and vacuum system. Common types of ion sources like electron impact and chemical ionization are described. Popular mass analyzers such as quadrupole, time-of-flight, ion trap, and double focusing are explained. The document also covers the theory behind how mass spectrometry separates ions based on their mass-to-charge ratio and discusses the need for high vacuum levels in mass spectrometers.
The document discusses fluorescence spectroscopy. It defines fluorescence as emission of light that occurs when a substance absorbs light and returns to its ground state, emitting photons. Factors that affect fluorescence include the molecular structure, substituents, concentration, pH, temperature, and viscosity. Instrumentation for fluorescence spectroscopy includes a light source, filters, sample cells, and detectors such as photomultiplier tubes. Applications of fluorescence spectroscopy include determination of inorganic substances, use as fluorescent indicators, pharmaceutical analysis, and liquid chromatography.
This document discusses using infrared spectroscopy to determine the structure of organic compounds. It begins by explaining electromagnetic radiation and the infrared region. It describes the different types of molecular vibrations that can be observed in an infrared spectrum. The document then explains how to interpret an infrared spectrum, noting the functional group and fingerprint regions. It provides examples of interpreting spectra for specific functional groups such as alkenes, alkynes, alcohols, aldehydes, ketones, carboxylic acids, amines and amides. Key absorption bands that identify each functional group are highlighted.
- The document is a presentation on ultraviolet spectroscopy submitted by Moriyom Akhter and Md Shah Alam from the Department of Pharmacy at World University of Bangladesh.
- It defines ultraviolet spectroscopy and discusses key concepts like absorption spectra, types of electronic transitions that can occur, Beer's and Lambert's absorption laws, instrumentation components, and applications in qualitative and quantitative analysis.
- The presentation also examines effects of chromophores and auxochromes on absorption spectra and maximum wavelengths, and how solvents can shift absorption peaks.
This document discusses Beer's law, which states that absorbance of a solution is directly proportional to the concentration of the absorbing material in the solution. It defines Beer's law, derives the mathematical equation, and lists some limitations and sources of deviation from the law, including high concentrations, dissociation/association reactions, use of polychromatic radiation, stray light, and mismatched sample cells. The derivation shows how the Beer's law equation is obtained based on probability of photon absorption in thin sections of the sample.
Fluorimetry involves measuring fluorescence intensity at a particular wavelength using a fluorimeter or spectrofluorimeter. Fluorescence occurs when molecules absorb radiation and electrons are excited to a higher energy state. As electrons return to the ground state, they emit radiation. Factors like concentration, pH, and temperature can affect fluorescence intensity. Instrumentation includes a light source, filters/monochromators, sample cells, and detectors. Applications include determining inorganic/organic substances and compounds in pharmaceutical analysis.
LEC 1 Dyestuff and Colour Science. pptx.pptxNasirSarwar5
Dyestuffs and dyes impart color to substrates like textiles, paper, and plastics. Dyes contain aromatic compounds that absorb certain wavelengths of light, appearing colored. Chromophores are structures within dyes that are responsible for light absorption by altering the energy levels of delocalized electrons. Auxochromes intensify dye color by further modifying electron energies. Factors like hue, strength, and bathochromic/hypsochromic shifts describe dye color properties. Photochromism causes reversible color changes in dyes under light due to cis-trans isomerization of azobenzene structures.
The current presentation explains basics of chromophore and auxochrome concept, types of absorption shift, effect of solvent, its polarity and effect of conjugation on absorption in uv-visible spectroscopy.
This document discusses the classification of dyes. It begins by explaining Witt's theory of color, which states that dyes contain chromophores that produce color and auxochromes that intensify color. The document then discusses various dye classifications including by color theory, chemical structure, and application method. The main chemical structures of dyes discussed are azo dyes, which are the most important class, and anthraquinone dyes. Dye application methods covered are direct dyes, mordant dyes, vat dyes, and disperse dyes. Examples are provided for many different dye types and classes.
This document discusses chromophores, auxochromes, and spectral shifts in organic chemistry. It defines chromophores as the part of a molecule responsible for its color and absorption spectrum. Auxochromes are substituents that modify a chromophore's absorption by increasing conjugation. There are two types of spectral shifts: bathochromic shifts move absorption to longer wavelengths (red shift) while hypsochromic shifts move it to shorter wavelengths (blue shift). Hyperchromic effects increase absorption intensity while hypochromic effects decrease it. Examples like phenol and nitrobenzene are provided.
1) The absorption of light by organic compounds involves the promotion of electrons from ground state to excited state molecular orbitals. Sigma electrons undergo σ-σ* transitions at shorter wavelengths while pi and non-bonding electrons undergo π-π* and n-π* transitions at longer wavelengths.
2) Chromophores are functional groups responsible for electronic transitions, imparting color. Auxochromes enhance absorption by chromophores through resonance. Conjugation and pH can shift absorption to longer wavelengths while dilution, solvents, and temperature can affect absorption spectra.
3) Spectrophotometry is widely used for quantitative analysis due to its sensitivity, selectivity, accuracy and ease. Both absorbing and non-absorbing
Spectroscopic methods in inorganic Chemistry: Fluorescence spectroscopy Chris Sonntag
Fluorescence spectroscopy involves absorption of UV or visible light by a molecule, promoting electrons to an excited state. The molecule then relaxes and emits light of a longer wavelength. It has many applications, including determination of organic and some inorganic substances at low concentrations in areas like food analysis, pharmaceuticals, and clinical samples. Factors like conjugation, substituents, temperature, and oxygen presence can influence fluorescence intensity. It is a sensitive and specific technique compared to absorption spectroscopy.
1. Color is an attribute resulting from light reflected, transmitted, or emitted from objects that causes visual sensations dependent on wavelength.
2. Theories of color include chromophore-auxochrome theory, which proposes unsaturated groups called chromophores impart color, and auxochromes intensify it.
3. Modern theories include valence bond theory, where excited states resemble less stable, charge-separated forms, and molecular orbital theory, where π→π* transitions in conjugated systems cause visible absorption.
DYES part I ( intrduction, chromophore n auxochrome and classification.pptxDrAparanaDighade1
This document discusses the key properties and components of dyes. It defines chromophores as the part of a molecule responsible for its color, and notes that chromophores undergo π-π* or n-π* electronic transitions. Auxochromes are groups that intensify a dye's color by extending conjugation with the chromophore. Common auxochromes include -OH, -NH2, and -COOH groups. The document also classifies dyes based on their structure, application method, and presence of acidic or basic auxochrome groups.
UV-visible spectroscopy involves using electromagnetic radiation to obtain information about atoms and molecules. It is based on electronic excitation of molecules that causes promotion of an electron from a ground state to an excited state. Factors like conjugation, solvents, and pH can affect the position and intensity of UV absorption. Applications of UV spectroscopy include determining molecular weight, identifying impurities, and characterizing aromatic compounds and conjugation.
This document discusses UV-visible spectroscopy. It begins by introducing spectroscopy and the different types, including UV, IR, NMR, and mass spectrometry. It then explains the principles of UV light absorption and Beer-Lambert's law. Factors that affect the position and intensity of UV absorption peaks are described, such as chromophores, auxochromes, pH, solvents, and conjugation. Finally, some applications of UV-visible spectroscopy are mentioned, such as determining molecular weight, impurities, concentrations, and characterizing aromatic compounds.
This document provides an overview of spectroscopy. It discusses topics like electromagnetic radiation, photons, wavelength, frequency, the electromagnetic spectrum, absorption spectroscopy, emission spectroscopy, Lambert's law, Beer's law, chromophores, auxochromes, shifts in absorption spectra, and components of a visible spectrophotometer like sources, filters, and monochromators.
This document discusses ultraviolet-visible spectroscopy and its principles. It covers the electromagnetic spectrum, units used, absorption laws including Lambert's law and Beer's law. It describes chromophores and auxochromes, types of electronic transitions, factors affecting absorption bands, and solvent effects. Different types of absorption bands and applications of UV-Vis spectroscopy are also summarized.
Solvents and solvent effect in UV - Vis Spectroscopy, By Dr. Umesh Kumar sh...Dr. UMESH KUMAR SHARMA
This document discusses solvent effects on UV-visible spectroscopy. It begins by explaining that UV spectra are usually measured in dilute solutions using solvents that are transparent in the wavelength range and do not interact strongly with the solute. Common solvents mentioned are ethanol, hexane, and water. The document then discusses various solvent effects including bathochromic shifts, hypsochromic shifts, hyperchromic shifts, and hypochromic shifts. It provides examples of how solvents can alter absorption wavelengths and intensities. The document concludes by mentioning several reference texts on this topic.
Uv absorption spectra arise from electronic transitions in molecules where electrons move from lower to higher energy levels. The amount of energy absorbed is proportional to the concentration of the solution based on Beer-Lambert's law. Uv-visible spectroscopy can be used to determine structural information about organic compounds, identify additional impurities, and perform quantitative analysis of compounds that absorb uv radiation.
this slides contains information about UV Visible spectroscopy and how we can demonstrate its applications in our daily life as it also contains visible region and all the wavelengths includes in this region and why substances appears colored
ENERGY CONSERVATION IN PLANTS TO PERFORM THEIR LIFE PROCESS.pptshikshaclinic
- Photosynthesis is the process by which plants convert carbon dioxide and water into oxygen and energy-rich carbohydrates like glucose, using sunlight as an energy source. It takes place in two stages - the light-dependent reactions and the light-independent reactions.
- The light reactions convert solar energy to chemical energy in the form of ATP and NADPH. These products are used in the Calvin cycle during the light-independent reactions to reduce carbon dioxide into carbohydrates like glucose.
- Chlorophyll is the main photosynthetic pigment found in plant chloroplasts. It absorbs blue and red light for photosynthesis while reflecting green light, giving leaves their green color. Carotenoids and phyc
Spectroscopy involves the absorption of electromagnetic radiation by molecules. This document discusses various spectroscopy techniques including UV-visible spectroscopy and infrared (IR) spectroscopy. UV-visible spectroscopy measures absorption in the ultraviolet and visible wavelength regions and can identify functional groups that undergo π-π* or n-π* transitions. IR spectroscopy detects molecular vibrations between 2.5-40 micrometers and is useful for determining functional groups. The document provides examples of instrumentation, sample preparation methods, and spectra for various compounds analyzed by these techniques.
UV/Visible spectroscopy involves electronic transitions that absorb light in the ultraviolet-visible region. There are several types of transitions including n→π*, π→π*, and σ→σ* transitions. The energy and wavelength of absorbed light depends on the difference between molecular orbital energies. Chromophores and auxochromes determine absorption properties, and solvents, concentration, and temperature can affect observed spectra. UV/Vis spectrometers contain a light source, monochromator, sample holder, and detector to measure absorption of light by a sample.
The document discusses UV spectroscopy and the different types of bands that can be observed. It explains that compounds with higher conjugation absorb at lower wavelengths due to a smaller energy gap between orbitals. Four main bands are described: K-band observed in conjugated double bonds with high intensity; R-band in carbonyl compounds with low intensity as it is a forbidden transition; B-band in aromatic/heteroaromatic compounds typically between 230-270nm; and E-band in benzenoid systems where benzene shows a strong band at 184nm.
This document discusses ultraviolet-visible (UV-Vis) spectroscopy. It begins by defining spectroscopy and describing the electromagnetic radiation spectrum. It then focuses on UV-Vis spectroscopy, explaining that it involves electronic transitions in molecules caused by the absorption of ultraviolet or visible light. The major electronic transitions that can occur are defined, including σ → σ*, n → σ*, π → π*, and n → π* transitions. Factors that affect these transitions, such as conjugation, are also discussed. Real-world examples of molecular structures and the transitions they undergo are provided.
The document discusses various spectroscopic methods used in organic chemistry including UV-Visible, Infrared, Nuclear Magnetic Resonance, and Mass Spectroscopy. It explains the basic principles of spectroscopy such as how electromagnetic radiation interacts with molecules by absorption or emission of energy. The document also provides details on the instrumentation used in spectroscopy including spectrophotometers and spectrographs.
The document discusses green chemistry as a remedy for environmental pollution. It defines green chemistry as the generation of new products and processes that reduce or eliminate hazardous materials. The need for green chemistry is explained by new environmental problems, harmful side effects of some chemicals like DDT, and accidents. Advantages of green chemistry include being eco-friendly, energy efficient, producing less waste and safer products. The principles of green chemistry focus on preventing waste, improving atom economy in synthesis, using safer solvents and feedstocks, and designing for energy efficiency and degradation. Examples are given around safer chemical design and replacing hazardous solvents.
The document discusses chemistry problems and solutions presented by B.Sateesh Kumar, an assistant professor of chemistry at GDC(M)-SKLM. It includes 3 chemistry problems involving the products of reactions and Kumar's explanations of the major products formed. Specifically, it discusses hydrogenolysis to deprotect functional groups on amino acids, the reduction of an epoxide to an alcohol using LAH, and a two-step reaction sequence involving a Schmidt reaction and Boc protection.
DIBAL-H is a commercially available selective reducing agent that can reduce esters and nitriles to the corresponding aldehydes. It is prepared by heating triisobutylaluminum, which induces beta hydride elimination to form DIBAL-H and isobutene. DIBAL-H selectively reduces esters to aldehydes at low temperatures through a tetrahedral intermediate. Hydrolytic workup of this intermediate then yields the desired aldehyde products. The document provides an introduction to DIBAL-H including its preparation, applications in organic synthesis, and how it differs from other reducing agents like LiAlH4.
The document discusses sodium cyanoborohydride (NaBH3CN), including its preparation from sodium borohydride and hydrogen cyanide, properties such as being a less reactive reducing agent than sodium borohydride, solubility in solvents like THF and methanol, and ability to reduce protonated aldehydes and ketones at pH 3 but not neutral aldehydes and ketones. Main applications of sodium cyanoborohydride include its use as a reducing agent in organic synthesis reactions.
This slide is special for master students (MIBS & MIFB) in UUM. Also useful for readers who are interested in the topic of contemporary Islamic banking.
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.
বাংলাদেশের অর্থনৈতিক সমীক্ষা ২০২৪ [Bangladesh Economic Review 2024 Bangla.pdf] কম্পিউটার , ট্যাব ও স্মার্ট ফোন ভার্সন সহ সম্পূর্ণ বাংলা ই-বুক বা pdf বই " সুচিপত্র ...বুকমার্ক মেনু 🔖 ও হাইপার লিংক মেনু 📝👆 যুক্ত ..
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A review of the growth of the Israel Genealogy Research Association Database Collection for the last 12 months. Our collection is now passed the 3 million mark and still growing. See which archives have contributed the most. See the different types of records we have, and which years have had records added. You can also see what we have for the future.
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
Exploiting Artificial Intelligence for Empowering Researchers and Faculty,
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at Integral University, Lucknow, 06.06.2024
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A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.
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Main Java[All of the Base Concepts}.docxadhitya5119
This is part 1 of my Java Learning Journey. This Contains Custom methods, classes, constructors, packages, multithreading , try- catch block, finally block and more.
How to Make a Field Mandatory in Odoo 17Celine George
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
How to Build a Module in Odoo 17 Using the Scaffold MethodCeline George
Odoo provides an option for creating a module by using a single line command. By using this command the user can make a whole structure of a module. It is very easy for a beginner to make a module. There is no need to make each file manually. This slide will show how to create a module using the scaffold method.
7. Chromophore
• Isolated covalent bonded groups that shows a
characteristic absorption in UV-Visible region, those
are called Chromophore.
In the case of multiple bonded compounds, the π-electrons are responsible for
absorption and electronic excitation.
Chromophore must contains
-N=N-
Ethylenic, acetylenic, carbonyls, acids, esters, nitrile group etc.
8. Auxochromes
• The groups does not show any characteristic
absorption in UV-Visible region, those groups are
called Auxochromes.
• These are electron-donating groups and are known
as auxochromes.
• Examples of auxochrome groups are: -NH2, -OR, -
NHR, -SH, -OH ..Etc.
auxochrome (from Ancient
Greek αὐξάνω (auxanō) 'increase',
and χρῶμα (chrōma) 'colour')
9. Auxochrome
• An auxochrome is a functional group of atoms with
one or more lone pairs of electrons when attached
to a chromophore, alters both the wavelength and
intensity of absorption.
@DrBSK
10. • An auxochrome can be defined as any group which does not itself act
as a chromophore but whose presence in a compound brings about a
shift of the absorption band towards the red of the spectrum (i.e.
longer wavelength)
Benzene shows an absorption at 255nm whereas aniline
absorbs at 280 nm. Thus amino group is an auxochrome
11. • There are mainly two types of auxochromes:
• Acidic: −COOH, −OH, −SO3H
• Basic: −NH2, −NHR, −NR2
@DrBSK
12. Effects on chromophore
• It increases the color of any organic compound
• Nitrobenzene is pale yellow colorbecause of the presence of a nitro
group (−NO2) which acts as a chromophore.
• But p-hydroxynitrobenzene exhibits a deep yellow color, in which the −OH group
acts as an auxochrome. Here the auxochrome (−OH) is conjugated with the
chromophore −NO2.
• Similar behavior is seen in azobenzene which has a red color, but p-
hydroxyazobenzene is dark red in color.
@DrBSK