The document discusses index hydrogen deficiency (IHD), which is a measure of unsaturation in molecules. IHD is calculated based on the number of hydrogen atoms fewer than would be present in a saturated molecule with the same number of carbon atoms. The document provides examples of calculating IHD for various molecules containing double bonds, rings, and heteroatoms like nitrogen. It also describes how mass spectrometry can be used to determine IHD and identify molecular structures based on their fragmentation patterns.
The Zimmerman-Traxler model is invoked to rationalize the unexpected stereochemical outcomes of certain aldol reactions, such as the Reformatsky and Ivanov reactions. It models the stereochemistry of the products, based on the steric hindrance in the possible six-membered transition states in the aldol condensation reactions.
Created by Alexis Johnson (Undergraduate)
Edited by Margaret Hilton
Honors Organic Chemistry
CHEM 2321 (Sigman), 2013, University of Utah
1) The document discusses different types of elimination reactions, including E1, E2, and E1cB mechanisms.
2) E1 reactions involve the generation of a carbocation intermediate, while E2 reactions occur in one step without intermediates. E1cB reactions first form a carbanion intermediate before the leaving group departs.
3) The mechanism depends on factors like the substrate, leaving group, solvent, and strength of the base used. Zaitsev's, Hofmann, and Bredt's rules also influence the regiochemistry of double bond formation.
- Aromatic compounds are characterized by a cyclic, conjugated ring system with delocalized pi electrons. This allows them to undergo substitution rather than addition reactions.
- Benzene is the prototypical aromatic compound. Its 6 pi electrons are delocalized across the ring, giving it extra stability compared to isolated double bonds. This is explained by molecular orbital theory.
- The Hückel rule states that monocyclic compounds with 4n+2 pi electrons are aromatic. Heterocycles like pyridine and pyrrole can also be aromatic. Polycyclic aromatic compounds have multiple fused rings.
The document summarizes aromaticity and related topics for chemistry students. It discusses:
- Benzenoid and non-benzenoid aromatic compounds, including their properties and reactions.
- Resonance structures of benzene and how it follows Huckel's rule for aromaticity.
- Classification of compounds based on aromaticity and examples of antiaromatic compounds.
- Aromatic ions and heterocyclic aromatic compounds like pyrrole, furan and pyridine.
Aromatic compounds are characterized by planar, conjugated ring structures with delocalized pi-electrons. Benzene, with its cyclic structure of six carbon atoms each bonded to one hydrogen atom, is the simplest aromatic compound. It exhibits atypical stability and undergoes substitution rather than addition reactions. While some aromatic compounds have pleasant smells, aroma is not a requirement - anthracene is aromatic but odorless. The Hückel rule defines a compound as aromatic if it has (4n+2) pi electrons in its conjugated ring system, where n is an integer.
The document discusses the lability and inertness of coordination complexes. It defines labile complexes as those where ligand exchange occurs rapidly, while inert complexes have slow ligand exchange. Lability is determined by factors like the metal ion size, charge, and d-electron configuration, not thermodynamic stability. Smaller or higher charged metal ions and complexes with less than 3 d-electrons tend to be more labile. The rate of ligand substitution depends on both the leaving and entering ligands. Steric effects and solvent also influence the rate. Complexes may undergo dissociative or associative substitution based on their structure.
Nucleophilic Aromatic Substitution of BenzyneAadil Ali Wani
The document discusses the elimination-addition mechanism of nucleophilic aromatic substitution involving benzyne. Aryl halides undergo substitution when treated with strong bases like KNH2 or NH3 at -33°C. The new substituent attaches to either the carbon that bore the leaving group or the adjacent carbon. The mechanism proceeds in three steps: 1) formation of the highly reactive intermediate benzyne, 2) relief of angle strain in benzyne, and 3) addition of the nucleophile to form the substitution product. Benzyne is a reactive dienophile that gives Diels-Alder adducts when generated in the presence of conjugated dienes. Other methods like treating 1-
The Zimmerman-Traxler model is invoked to rationalize the unexpected stereochemical outcomes of certain aldol reactions, such as the Reformatsky and Ivanov reactions. It models the stereochemistry of the products, based on the steric hindrance in the possible six-membered transition states in the aldol condensation reactions.
Created by Alexis Johnson (Undergraduate)
Edited by Margaret Hilton
Honors Organic Chemistry
CHEM 2321 (Sigman), 2013, University of Utah
1) The document discusses different types of elimination reactions, including E1, E2, and E1cB mechanisms.
2) E1 reactions involve the generation of a carbocation intermediate, while E2 reactions occur in one step without intermediates. E1cB reactions first form a carbanion intermediate before the leaving group departs.
3) The mechanism depends on factors like the substrate, leaving group, solvent, and strength of the base used. Zaitsev's, Hofmann, and Bredt's rules also influence the regiochemistry of double bond formation.
- Aromatic compounds are characterized by a cyclic, conjugated ring system with delocalized pi electrons. This allows them to undergo substitution rather than addition reactions.
- Benzene is the prototypical aromatic compound. Its 6 pi electrons are delocalized across the ring, giving it extra stability compared to isolated double bonds. This is explained by molecular orbital theory.
- The Hückel rule states that monocyclic compounds with 4n+2 pi electrons are aromatic. Heterocycles like pyridine and pyrrole can also be aromatic. Polycyclic aromatic compounds have multiple fused rings.
The document summarizes aromaticity and related topics for chemistry students. It discusses:
- Benzenoid and non-benzenoid aromatic compounds, including their properties and reactions.
- Resonance structures of benzene and how it follows Huckel's rule for aromaticity.
- Classification of compounds based on aromaticity and examples of antiaromatic compounds.
- Aromatic ions and heterocyclic aromatic compounds like pyrrole, furan and pyridine.
Aromatic compounds are characterized by planar, conjugated ring structures with delocalized pi-electrons. Benzene, with its cyclic structure of six carbon atoms each bonded to one hydrogen atom, is the simplest aromatic compound. It exhibits atypical stability and undergoes substitution rather than addition reactions. While some aromatic compounds have pleasant smells, aroma is not a requirement - anthracene is aromatic but odorless. The Hückel rule defines a compound as aromatic if it has (4n+2) pi electrons in its conjugated ring system, where n is an integer.
The document discusses the lability and inertness of coordination complexes. It defines labile complexes as those where ligand exchange occurs rapidly, while inert complexes have slow ligand exchange. Lability is determined by factors like the metal ion size, charge, and d-electron configuration, not thermodynamic stability. Smaller or higher charged metal ions and complexes with less than 3 d-electrons tend to be more labile. The rate of ligand substitution depends on both the leaving and entering ligands. Steric effects and solvent also influence the rate. Complexes may undergo dissociative or associative substitution based on their structure.
Nucleophilic Aromatic Substitution of BenzyneAadil Ali Wani
The document discusses the elimination-addition mechanism of nucleophilic aromatic substitution involving benzyne. Aryl halides undergo substitution when treated with strong bases like KNH2 or NH3 at -33°C. The new substituent attaches to either the carbon that bore the leaving group or the adjacent carbon. The mechanism proceeds in three steps: 1) formation of the highly reactive intermediate benzyne, 2) relief of angle strain in benzyne, and 3) addition of the nucleophile to form the substitution product. Benzyne is a reactive dienophile that gives Diels-Alder adducts when generated in the presence of conjugated dienes. Other methods like treating 1-
The document discusses various aromatic electrophilic substitution reactions including Vilsmeier-Haack formylation, Reimer-Tiemann reaction, Gattermann-Koch formylation, and Kolbe-Schmitt reaction. It provides details on the reaction conditions, mechanisms, substrates used, and products formed for each reaction. It also discusses some exceptions and problems related to these reactions.
The document discusses the conjugate base mechanism for the base hydrolysis of cobalt(III) ammine complexes.
1) The complex [Co(NH3)5Cl]2+ acts as a Bronsted acid and loses a proton to form the conjugate base [Co(NH3)4(NH2)Cl]+.
2) The conjugate base is more labile than the original complex and undergoes an SN1 reaction by slowly dissociating chloride, forming a pentacoordinated intermediate.
3) Several experiments provide evidence that the reaction follows a conjugate base mechanism, including second-order kinetics and the rate being independent of hydroxide concentration at high levels.
Chemistry Of Aromatic Compounds By Dr. Gladys Mokua.MathewJude
Slide that venture deep into Benzene, its nomenclature, Its reactions and Benzene substituents reactions. Hope it will be of help to those who want to know about aromaticity.
more chemistry contents are available
1. pdf file on Termmate: https://www.termmate.com/rabia.aziz
2. YouTube: https://www.youtube.com/channel/UCKxWnNdskGHnZFS0h1QRTEA
3. Facebook: https://web.facebook.com/Chemist.Rabia.Aziz/
4. Blogger: https://chemistry-academy.blogspot.com/
Organic Synthesis:
The Disconnection Approach
One Group C-C Disconnection of Alcohol and Alkene
chemical kinetics-kinetic vs thermodynamicFarhadAlsaeid
This document discusses the differences between chemical kinetics and thermodynamics. Thermodynamics deals with whether a reaction can occur based on energy changes and equilibrium, while kinetics is concerned with how fast reactions occur and the rates of change over time. The document provides examples of factors studied in kinetics like reaction mechanisms and rates. While thermodynamics determines reaction spontaneity based on free energy, kinetics is needed to understand how long reactions take to reach equilibrium and what factors influence reaction rates.
For B Pharmacy and M Pharmacy Students
Subscribe to the YouTube Channel
#Professor_Beubenz
https://www.youtube.com/channel/UC84jGf2iRN5VjwnQqi6qmXg?view_as=subscriber
The video lecture for this presentation is available at the following link on YouTube
https://youtu.be/3sxal579RNM
The presenation will be useful for Ug/PG (Chemistry) students
Nucleophilic aromatic substitution reactions follow an addition-elimination mechanism known as SNAr. The rate-determining step is the formation of a cyclohexadienyl anion intermediate through nucleophilic attack. Electron-withdrawing groups stabilize this intermediate through resonance, making the reaction faster. Nucleophilic aromatic substitution is most favorable when the leaving group is fluoride and least with iodide, and occurs readily with strong nucleophiles like hydroxide or cyanide in the presence of electron-withdrawing groups ortho or para to the reaction site.
Bonding and Antibonding interactions; Idea about σ, σ*, π, π *, n – MOs; HOMO, LUMO and SOMO; Energy levels of π MOs of different conjugated acyclic and cyclic systems; Hückel’s rules for aromaticity; Frost diagram
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.
CONTENTS
INTRODUCTION
CONCEPTS OF WALSH DIAGRAM
APPLICATION IN TRIATOMIC MOLECULES
[IN AH₂ TYPE OF MOLECULES(BeH₂,BH₂,H₂O)]
INTRODUCTION
Arthur Donald Walsh FRS The introducer of walsh diagram (8 August 1916-23 April 1977) was a British chemist, professor of chemistry at the University of Dundee . He was elected FRS in 1964. He was educated at Loughborough Grammar School.
Walsh diagrams were first introduced in a series of ten papers in one issue of the Journal of the Chemical Society . Here, he aimed to rationalize the shapes adopted by polyatomic molecules in the ground state as well as in excited states, by applying theoretical contributions made by Mulliken .
Molecular orbital theory(mot) of SF6/CO2/I3-/B2H6sirakash
1) Molecular orbital theory views a molecule as delocalized molecular orbitals formed from linear combinations of atomic orbitals. Bonding molecular orbitals are lower in energy due to constructive interference, while antibonding orbitals are higher in energy due to destructive interference.
2) The document provides examples of applying molecular orbital theory to SF6, CO2, B2H6, and I3- molecules. It describes the atomic orbitals and molecular orbitals formed, including bonding, antibonding, and non-bonding orbitals, and explains how the molecular orbitals rationalize the electronic structures and bonding patterns in these molecules.
Retrosynthes analysis and disconnection approach ProttayDutta1
Retrosynthetic analysis is a technique used to plan organic syntheses by working backwards from the target molecule. It involves mentally deconstructing the target molecule through sequential disconnections and functional group transformations until commercially available starting materials are reached. Each disconnection produces synthons, which are idealized fragments that represent possible reaction precursors. Common types of disconnections include C-X, C-C, and carbonyl bonds. The goal of retrosynthesis is to simplify the target structure and design multiple possible synthesis routes leading from simple starting materials to the target. It helps chemists discover efficient syntheses by considering the reactivity, selectivity, and availability of materials at each step.
The document discusses Hammond's postulates, which state that the transition state of a chemical reaction resembles the structure of the species (reactant or product) that is closer in energy. Specifically:
1) For exothermic reactions, the transition state resembles the reactants more than the products.
2) For endothermic reactions, the transition state resembles the products more than the reactants.
3) Hammond's postulates can be used to predict reaction mechanisms and explain factors that influence reaction rates.
Synthon or Disconnection or Retrosynthesis Approach in Organic Synthesis. This document discusses the key concepts and approaches of retrosynthesis including: 1) Disconnecting a target molecule into logical fragments through breaking bonds to obtain starting materials, 2) It is the reverse of chemical synthesis, 3) Terminologies such as disconnection, synthon, and reagents, 4) Basic rules for preferred disconnections.
This document is a power point presentation on structure and reactivity given by Dr. Gopinath Shirole. It discusses aromaticity based on Huckel's rule and applies the rule to analyze the aromatic, anti-aromatic, and non-aromatic nature of various monocyclic and polycyclic compounds, including benzenoid and non-benzenoid systems as well as annulenes and fused ring compounds like azulenes. Key aspects of aromaticity like planarity, conjugation, and the (4n+2) rule are explained. A total of 34 examples of different compound classes are presented and determined to be aromatic, anti-aromatic, or non-aromatic according to their π
The document discusses character tables and symmetry operations in molecules. It provides examples of determining the point groups and irreducible representations of molecules like water. Character tables are used to predict molecular vibrations that will be active in infrared and Raman spectra. The document also discusses how group theory can be applied to determine hybridization of orbitals and molecular orbitals. Key applications of group theory covered are predicting vibrational modes, hybrid orbitals, and molecular orbitals of different symmetry.
This document discusses coordination chemistry and isomerism in coordination compounds. It defines molecular compounds, complex salts, and double salts formed from combinations of inorganic salts. It also discusses ligands, classifying them based on properties. Coordination number and the resulting geometries for coordination numbers 2 through 9 are described. Finally, it outlines different types of isomerism that can occur in coordination compounds, including structural, spin, and stereo isomerism.
This document summarizes a seminar on group multiplication tables and abelian/non-abelian point groups. It defines groups, subgroups, symmetry operations, and point groups. It provides examples of group multiplication tables for C2v and C3v point groups. Abelian groups have commutative combinations while non-abelian groups like C3v do not. Low, high, and special symmetry molecule types are classified by their point groups. Examples are given throughout to illustrate key concepts.
IB Chemistry on Energetics, Enthalpy Change and ThermodynamicsLawrence kok
1. Heat is the transfer of thermal energy from hot to cold bodies due to a temperature difference. Heat is not a form of energy but rather energy transfer, while temperature is a measure of the average kinetic energy of particles.
2. At the same temperature, different gases have the same average kinetic energy per particle despite differences in mass. Heavier particles move slower than lighter particles at the same temperature.
3. The amount of heat required to change the temperature of a substance depends on its specific heat capacity and mass. Substances with higher specific heat capacity require more heat to change their temperature.
The document discusses various aromatic electrophilic substitution reactions including Vilsmeier-Haack formylation, Reimer-Tiemann reaction, Gattermann-Koch formylation, and Kolbe-Schmitt reaction. It provides details on the reaction conditions, mechanisms, substrates used, and products formed for each reaction. It also discusses some exceptions and problems related to these reactions.
The document discusses the conjugate base mechanism for the base hydrolysis of cobalt(III) ammine complexes.
1) The complex [Co(NH3)5Cl]2+ acts as a Bronsted acid and loses a proton to form the conjugate base [Co(NH3)4(NH2)Cl]+.
2) The conjugate base is more labile than the original complex and undergoes an SN1 reaction by slowly dissociating chloride, forming a pentacoordinated intermediate.
3) Several experiments provide evidence that the reaction follows a conjugate base mechanism, including second-order kinetics and the rate being independent of hydroxide concentration at high levels.
Chemistry Of Aromatic Compounds By Dr. Gladys Mokua.MathewJude
Slide that venture deep into Benzene, its nomenclature, Its reactions and Benzene substituents reactions. Hope it will be of help to those who want to know about aromaticity.
more chemistry contents are available
1. pdf file on Termmate: https://www.termmate.com/rabia.aziz
2. YouTube: https://www.youtube.com/channel/UCKxWnNdskGHnZFS0h1QRTEA
3. Facebook: https://web.facebook.com/Chemist.Rabia.Aziz/
4. Blogger: https://chemistry-academy.blogspot.com/
Organic Synthesis:
The Disconnection Approach
One Group C-C Disconnection of Alcohol and Alkene
chemical kinetics-kinetic vs thermodynamicFarhadAlsaeid
This document discusses the differences between chemical kinetics and thermodynamics. Thermodynamics deals with whether a reaction can occur based on energy changes and equilibrium, while kinetics is concerned with how fast reactions occur and the rates of change over time. The document provides examples of factors studied in kinetics like reaction mechanisms and rates. While thermodynamics determines reaction spontaneity based on free energy, kinetics is needed to understand how long reactions take to reach equilibrium and what factors influence reaction rates.
For B Pharmacy and M Pharmacy Students
Subscribe to the YouTube Channel
#Professor_Beubenz
https://www.youtube.com/channel/UC84jGf2iRN5VjwnQqi6qmXg?view_as=subscriber
The video lecture for this presentation is available at the following link on YouTube
https://youtu.be/3sxal579RNM
The presenation will be useful for Ug/PG (Chemistry) students
Nucleophilic aromatic substitution reactions follow an addition-elimination mechanism known as SNAr. The rate-determining step is the formation of a cyclohexadienyl anion intermediate through nucleophilic attack. Electron-withdrawing groups stabilize this intermediate through resonance, making the reaction faster. Nucleophilic aromatic substitution is most favorable when the leaving group is fluoride and least with iodide, and occurs readily with strong nucleophiles like hydroxide or cyanide in the presence of electron-withdrawing groups ortho or para to the reaction site.
Bonding and Antibonding interactions; Idea about σ, σ*, π, π *, n – MOs; HOMO, LUMO and SOMO; Energy levels of π MOs of different conjugated acyclic and cyclic systems; Hückel’s rules for aromaticity; Frost diagram
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.
CONTENTS
INTRODUCTION
CONCEPTS OF WALSH DIAGRAM
APPLICATION IN TRIATOMIC MOLECULES
[IN AH₂ TYPE OF MOLECULES(BeH₂,BH₂,H₂O)]
INTRODUCTION
Arthur Donald Walsh FRS The introducer of walsh diagram (8 August 1916-23 April 1977) was a British chemist, professor of chemistry at the University of Dundee . He was elected FRS in 1964. He was educated at Loughborough Grammar School.
Walsh diagrams were first introduced in a series of ten papers in one issue of the Journal of the Chemical Society . Here, he aimed to rationalize the shapes adopted by polyatomic molecules in the ground state as well as in excited states, by applying theoretical contributions made by Mulliken .
Molecular orbital theory(mot) of SF6/CO2/I3-/B2H6sirakash
1) Molecular orbital theory views a molecule as delocalized molecular orbitals formed from linear combinations of atomic orbitals. Bonding molecular orbitals are lower in energy due to constructive interference, while antibonding orbitals are higher in energy due to destructive interference.
2) The document provides examples of applying molecular orbital theory to SF6, CO2, B2H6, and I3- molecules. It describes the atomic orbitals and molecular orbitals formed, including bonding, antibonding, and non-bonding orbitals, and explains how the molecular orbitals rationalize the electronic structures and bonding patterns in these molecules.
Retrosynthes analysis and disconnection approach ProttayDutta1
Retrosynthetic analysis is a technique used to plan organic syntheses by working backwards from the target molecule. It involves mentally deconstructing the target molecule through sequential disconnections and functional group transformations until commercially available starting materials are reached. Each disconnection produces synthons, which are idealized fragments that represent possible reaction precursors. Common types of disconnections include C-X, C-C, and carbonyl bonds. The goal of retrosynthesis is to simplify the target structure and design multiple possible synthesis routes leading from simple starting materials to the target. It helps chemists discover efficient syntheses by considering the reactivity, selectivity, and availability of materials at each step.
The document discusses Hammond's postulates, which state that the transition state of a chemical reaction resembles the structure of the species (reactant or product) that is closer in energy. Specifically:
1) For exothermic reactions, the transition state resembles the reactants more than the products.
2) For endothermic reactions, the transition state resembles the products more than the reactants.
3) Hammond's postulates can be used to predict reaction mechanisms and explain factors that influence reaction rates.
Synthon or Disconnection or Retrosynthesis Approach in Organic Synthesis. This document discusses the key concepts and approaches of retrosynthesis including: 1) Disconnecting a target molecule into logical fragments through breaking bonds to obtain starting materials, 2) It is the reverse of chemical synthesis, 3) Terminologies such as disconnection, synthon, and reagents, 4) Basic rules for preferred disconnections.
This document is a power point presentation on structure and reactivity given by Dr. Gopinath Shirole. It discusses aromaticity based on Huckel's rule and applies the rule to analyze the aromatic, anti-aromatic, and non-aromatic nature of various monocyclic and polycyclic compounds, including benzenoid and non-benzenoid systems as well as annulenes and fused ring compounds like azulenes. Key aspects of aromaticity like planarity, conjugation, and the (4n+2) rule are explained. A total of 34 examples of different compound classes are presented and determined to be aromatic, anti-aromatic, or non-aromatic according to their π
The document discusses character tables and symmetry operations in molecules. It provides examples of determining the point groups and irreducible representations of molecules like water. Character tables are used to predict molecular vibrations that will be active in infrared and Raman spectra. The document also discusses how group theory can be applied to determine hybridization of orbitals and molecular orbitals. Key applications of group theory covered are predicting vibrational modes, hybrid orbitals, and molecular orbitals of different symmetry.
This document discusses coordination chemistry and isomerism in coordination compounds. It defines molecular compounds, complex salts, and double salts formed from combinations of inorganic salts. It also discusses ligands, classifying them based on properties. Coordination number and the resulting geometries for coordination numbers 2 through 9 are described. Finally, it outlines different types of isomerism that can occur in coordination compounds, including structural, spin, and stereo isomerism.
This document summarizes a seminar on group multiplication tables and abelian/non-abelian point groups. It defines groups, subgroups, symmetry operations, and point groups. It provides examples of group multiplication tables for C2v and C3v point groups. Abelian groups have commutative combinations while non-abelian groups like C3v do not. Low, high, and special symmetry molecule types are classified by their point groups. Examples are given throughout to illustrate key concepts.
IB Chemistry on Energetics, Enthalpy Change and ThermodynamicsLawrence kok
1. Heat is the transfer of thermal energy from hot to cold bodies due to a temperature difference. Heat is not a form of energy but rather energy transfer, while temperature is a measure of the average kinetic energy of particles.
2. At the same temperature, different gases have the same average kinetic energy per particle despite differences in mass. Heavier particles move slower than lighter particles at the same temperature.
3. The amount of heat required to change the temperature of a substance depends on its specific heat capacity and mass. Substances with higher specific heat capacity require more heat to change their temperature.
IB Chemistry on HNMR Spectroscopy and Spin spin couplingLawrence kok
Spectroscopy measures the interaction of molecules with electromagnetic radiation. Different types of spectroscopy use different regions of the electromagnetic spectrum and provide information about molecular structure. Nuclear magnetic resonance spectroscopy specifically uses radio waves to investigate nuclear spin properties and can determine organic molecular structures. It works by applying a magnetic field to nuclei with an odd number of protons and neutrons, which have a net spin and magnetic moment.
IB Chemistry on Bond Enthalpy and Bond Dissociation EnergyLawrence kok
This document discusses bond enthalpy (BE) and how average BE values are used to calculate enthalpy changes (ΔH) in chemical reactions. It provides examples of calculating ΔH using average BE values for breaking bonds in reactants and forming bonds in products. However, it notes that average BE values are only approximations and ΔHf° (standard enthalpy of formation) and ΔHc° (standard enthalpy of combustion) values provide more accurate determinations of ΔH.
IB Chemistry on Gibbs Free Energy vs Entropy on spontanietyLawrence kok
This document discusses key concepts in thermodynamics including:
1) The first law of thermodynamics states that energy cannot be created or destroyed, only transferred or changed in form. The change in internal energy of a system (ΔE) equals heat transferred (q) plus work done (w).
2) The second law of thermodynamics states that the entropy of the universe always increases for spontaneous processes. Entropy (S) is a measure of disorder or randomness at the molecular level. Spontaneous processes result in increased entropy of the universe (ΔSuni > 0).
3) The third law of thermodynamics states that the entropy of a perfectly crystalline substance is zero at absolute zero temperature
IB Chemistry on ICT, 3D software, Jmol, Pymol, Rasmol and ACD for Internal As...Lawrence kok
The document discusses measuring properties of bonds such as length, angle, and strength using various 3D modeling software. It also covers using these programs to analyze protein and enzyme structures from the Protein Data Bank by inputting four-letter codes. Details are provided on tools for molecular modeling and 3D representation in Jmol, PyMol, RasMol, and ACD Labs. Spectroscopic and chemistry databases are listed for reference.
IB Chemistry on Entropy and Law of ThermodynamicsLawrence kok
This document discusses entropy and the laws of thermodynamics. It defines entropy as a measure of molecular disorder or randomness, and explains that entropy increases as energy and matter disperse and become more randomly distributed. The second law of thermodynamics states that the entropy of the universe always increases for spontaneous processes. Reactions and phase changes that result in higher entropy (more disorder) of the products are spontaneous. The document provides examples and explanations of how entropy changes in different processes.
IB Chemistry on Redox Design and Nernst EquationLawrence kok
The document outlines research questions and procedures to investigate the effect of various factors on the emf and current of voltaic cells. Specifically, it will study how concentration, temperature, electrode size, salt bridge composition, and metal pairs affect measurements in zinc-copper and copper-copper cells. Tests will be conducted by varying one factor at a time while keeping others standard, and measuring the resulting emf and current.
This document provides an overview of analytical techniques used in chemistry, including both classical and instrumental methods. Classical methods involve qualitative and quantitative analysis using chemical tests, flame tests, and titration. Instrumental methods discussed include various types of spectroscopy such as infrared spectroscopy, nuclear magnetic resonance spectroscopy, and chromatography techniques used for separation analysis. Specific analytical techniques are described including their applications and mechanisms. Key concepts covered include electromagnetic radiation, molecular vibration, factors that influence infrared absorption frequencies, and interpreting infrared spectra to determine functional groups in organic compounds.
IB Chemistry on Structural Isomers and Benzene StructureLawrence kok
The document discusses organic functional groups and their naming conventions. It provides examples of common organic compound classes including alkanes, alkenes, alkynes, alcohols, ethers, ketones, aldehydes, carboxylic acids, esters, amides, amines, nitriles, and halogenoalkanes. It also discusses IUPAC nomenclature rules for systematically naming organic molecules based on functional groups, carbon chain length and position of substituents. Additionally, it briefly touches on isomerism, which refers to compounds with the same molecular formula but different structural or spatial arrangements of atoms.
IB Chemistry on ICT, 3D software, Jmol, Pymol and Rasmol for Internal AssessmentLawrence kok
The document discusses using 3D modeling software and databases to collect data on bond angles and lengths of alcohols and haloalkanes. Data was collected from Jmol, Pymol, Rasmol, ACD Lab and databases like CRC and RSC and averaged. Limitations of computational methods are that they assume non-interacting molecules in isolation. Data from multiple sources should be compared and experimental data is most reliable.
IB Chemistry on Gibbs Free Energy, Equilibrium constant and Cell PotentialLawrence kok
The document discusses the relationship between thermodynamic quantities such as Gibbs free energy (ΔG), equilibrium constant (Kc), cell potential (Ecell), and their significance. It provides equations relating these quantities and explains how ΔG and Kc can be used to predict the spontaneity and extent of chemical reactions. Examples are given to show how ΔG decreases as the reaction progresses towards equilibrium, and how the values of ΔG and Kc indicate the position of the reaction mixture between reactants and products.
IB Chemistry on Stereoisomers, E/Z, Cis Trans, Geometric, Optical and Polarim...Lawrence kok
There are two types of isomerism: structural isomerism and stereoisomerism. Structural isomers have the same molecular formula but different structural formulas or arrangements of atoms. Stereoisomers have the same molecular formula and structural formula but different spatial arrangements of atoms. Examples of stereoiosmers include geometric isomers, which require a double bond or ring structure to prevent bond rotation, and optical isomers. The E/Z or Cahn-Ingold-Prelog system is used to name geometric isomers based on atomic mass priorities of substituents.
IB Chemistry on Absorption Spectrum and Line Emission/Absorption SpectrumLawrence kok
Transition metal complexes can have different colors due to the splitting of the metal ion's d orbitals caused by ligands. Ligands of varying strength cause varying degrees of d orbital splitting, represented by ΔE. Stronger ligands cause greater splitting and absorption of higher energy visible light, resulting in colors like violet or blue. Weaker ligands cause less splitting and absorption of lower energy visible light, appearing as colors like yellow or green. The spectrochemical series orders ligands from weakest to strongest field strength based on the color produced.
IB Chemistry on Crystal Field Theory and Splitting of 3d orbitalLawrence kok
The document discusses the properties and behaviors of transition metals. Transition metals are d-block elements that have partially filled d orbitals. They can exist in multiple oxidation states and form colored complexes due to their variable electron configurations. Transition metals are also good catalysts as their partially filled d orbitals allow them to easily gain or lose electrons and form weak bonds with reactants to lower the activation energy of chemical reactions.
IB Chemistry on Gibbs Free Energy and EntropyLawrence kok
This document discusses key concepts in thermodynamics including:
1) The first law of thermodynamics states that energy cannot be created or destroyed, only transferred or changed in form.
2) The second law of thermodynamics states that the entropy of the universe always increases for spontaneous processes. Spontaneous reactions result in an increase in disorder and a more even distribution of energy.
3) Entropy is a measure of molecular disorder/randomness. Higher entropy states correspond to greater dispersal of matter and energy. Phase changes from solid to liquid to gas are accompanied by an increase in entropy.
IB Chemistry on Reactivity Series vs Electrochemical SeriesLawrence kok
The document discusses the reactivity and electrochemical series of group 1 alkali metals lithium, sodium, and potassium. While lithium has the most negative standard reduction potential, indicating it is most easily oxidized, potassium is the most reactive when reacting with water and acids due to lower kinetic barriers. The electrochemical series is a thermodynamic measurement based on standard potentials, while the reactivity series considers reaction kinetics. Thus, there is a correlation but not perfect agreement between the two series.
IB Chemistry on Standard Reduction Potential, Standard Hydrogen Electrode and...Lawrence kok
The document discusses standard electrode potentials and how they are measured. It explains that the standard hydrogen electrode is used as a reference with a potential of 0 V. Other half-cell potentials are measured against this to determine their standard electrode potential. Common half-cells include metal/metal ion, gas/ion, and ion/ion systems. Standard conditions of 1 M concentrations, 1 atm pressure, and 298K temperature must be used. The potentials of zinc/zinc ion, iron III/iron II, and chlorine/chloride ion half-cells are given as examples.
IB Chemistry on Redox, Reactivity Series and Displacement reactionLawrence kok
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The document summarizes elimination reactions, which involve removing two substituents from a molecule in the presence of a base. It describes the E1 and E2 mechanisms, noting that E1 is first order and involves a carbocation, while E2 is second order. E2 requires an anti-coplanar orientation of the leaving groups and occurs more readily with secondary and tertiary substrates. The orientation of elimination is also discussed based on Saytzeff's and Hofmann's rules. Stereochemistry preferences, reactivity factors, and conclusions about elimination versus substitution are provided.
The document provides an introduction to key concepts in electrochemistry including oxidation/reduction reactions, oxidation numbers, and definitions of terms like oxidizing agent and reducing agent. It then discusses rules for assigning oxidation numbers, types of redox reactions like disproportionation, electrochemical cells, and how to determine the potential of a cell.
This document summarizes key reactions of alkenes, including addition reactions and mechanisms. It discusses catalytic hydrogenation, electrophilic additions, hydroboration-oxidation, carbene and radical additions, polymerization, and the roles of alkenes in natural products like pheromones. It also provides examples of alkene reactions in nature, like steroid synthesis, and commercial applications, such as in polyethylene and margarine production.
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This document discusses acid-base physiology and disorders. It provides equations and guidelines for evaluating acid-base disturbances. Some key points:
- The Henderson-Hasselbalch equation relates pH to the ratio of bicarbonate to carbonic acid in the blood.
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The document discusses standard enthalpy of formation (ΔHf°), which is the amount of heat absorbed or released when one mole of a substance is formed from its elements in their standard states. Examples are provided of writing balanced chemical equations for formation reactions and using ΔHf° values to calculate the enthalpy change (ΔH°) of chemical reactions. The standard heat of combustion (ΔHc°) is also introduced, which is the enthalpy change when a substance undergoes complete combustion.
IB Chemistry on Bond Enthalpy, Enthalpy formation, combustion and atomizationLawrence kok
This document discusses several methods to calculate enthalpy change (ΔH) for chemical reactions, including using average bond enthalpies, standard enthalpies of formation (ΔHf), standard enthalpies of combustion (ΔHc), and standard enthalpies of atomization (ΔHa). It provides examples of calculating ΔH for reactions involving CH4, CCl4, S8, carbon polymorphs, and the formation of C5H5N from carbon, hydrogen, and nitrogen. The document emphasizes that while average bond enthalpies can be used, ΔHf, ΔHc, and ΔHa are generally more accurate as they consider the specific bonds in the reaction.
The document discusses several stereoselective and stereospecific reactions:
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5) Titration of chlorine in bleach with sodium thiosulfate after reaction with potassium iodide to determine its molarity.
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1) Free radical substitution, electrophilic addition, nucleophilic substitution, elimination, addition-elimination, electrophilic substitution, esterification, alkaline hydrolysis, nucleophilic addition.
2) Specific mechanisms are described for hydration of alkenes, addition polymerization, bromination of alkenes, nucleophilic substitution, elimination, dehydration, esterification.
3) The formation of polymers like polyamides, polyesters through reactions of dibasic acids and diamines or diols are summarized.
The citric acid cycle (CAC) is the final common pathway for the oxidation of nutrients. It occurs in the mitochondria of cells. Acetyl-CoA from various sources enters the CAC and is oxidized to CO2, producing reduced cofactors that drive ATP synthesis. The 8-step cycle produces ATP, GTP, and reduced cofactors NADH and FADH2. Key enzymes and cofactors regulate the cycle in response to energy demands and product inhibition. Anaplerotic reactions maintain CAC intermediate levels.
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This document contains a chemistry task and solutions from students in class XI IA-6. It includes 17 multiple choice questions related to concepts like the law of conservation of energy, enthalpy changes of reactions, Hess's law, bond enthalpies, and calorimetry. The questions cover topics such as identifying exothermic and endothermic reactions based on enthalpy values, calculating amounts of reactants needed using enthalpy data, determining enthalpy changes using Hess's law, and bond energies.
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Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
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Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
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Chapter 5
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Chapter 6
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2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
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IB Chemistry on Mass Spectrometry, Index Hydrogen Deficiency and Isotopes
1. Index Hydrogen Deficiency (IHD) = Degree unsaturation
H H H H H H
׀ ׀ ׀ ׀ ׀ ׀
H - C - C – C – C – C – C – H
׀ ׀ ׀ ׀ ׀ ׀
H H H H H H
H H H H H H
׀ ׀ ׀ ׀ ׀ ׀
H - C - C = C – C – C – C – H
׀ ׀ ׀ ׀
H H H H
H H H H H H
׀ ׀ ׀ ׀ ׀ ׀
H - C - C – C = C – C – C – H
׀ ׀ ׀ ׀
H H H H
Hexane
C6H14 IHD = 0
Hex-2-ene
C6H12 IHD = 1
Hex-3-ene
C6H12 IHD = 1
Cyclohexane
C6H12 IHD = 1
How many double bonds/rings present
Any double/triple bond/cyclic - number hydrogen atoms decrease
How many H2 need to convert molecule to saturated/noncyclic
Saturatedhydrocarbon = CnH2n+2
Saturated
IDH = 0
Unsaturated
(1 π bond)
2 H deficiency
IHD = 1
H H
׀ ׀
C = C
׀ ׀
H H
Unsaturated
(2 π bond)
4 H deficiency
IHD = 2
Unsaturated
(1 ring)
2 H deficiency
IHD = 1
Unsaturated
(3 π bond) + 1 ring
8 H deficiency
IHD = 4
IHD = 1
1 π bond or 1 ring structure
Unsaturated
(2 π bond) + 1 ring
6 H deficiency
IHD = 3
Unsaturated
(4 π bond) + 1 ring
10 H deficiency
IHD = 5
IHD = 2
2 π bond / 1 π bond + 1 ring
IHD = 3
3 π bond / 2 π bond + 1 ring / 1 π bond+ 2 ring
Unsaturated
(4 π bond) + 1 ring
10 H deficiency
IHD = 5
Unsaturated
(6 π bond) + 2 ring
16 H deficiency
IHD = 8
Click here IHD (Khan Academy)
2.
2
22 yx
IHD
H H H H H H
׀ ׀ ׀ ׀ ׀ ׀
H - C - C – C – C – C – C – H
׀ ׀ ׀ ׀ ׀ ׀
H H H H H H
Hexane
C6H14 IHD = 0
Hex-2-ene
C6H12 IHD = 1
Hex-3-ene
C6H12 IHD = 1
Cyclohexane
C6H12 IHD = 1
2
22 rsyx
IHD
How many double bonds/rings present
Any double/triple bond/cyclic - number hydrogen atoms decrease
How many H2 need to convert molecule to saturated/noncyclic
IHD = 1
1 π bond or 1 ring structure
IHD = 2
2 π bond / 1 π bond + 1 ring
IHD = 3
3 π bond / 2 π bond + 1 ring / 1 π bond+ 2 ring
Molecule with C and H Molecule with N, O, S or Halogen
yx HC srqyx XNOHC
C6H12 C2H2
1
2
)12262(
2
22
IHD
IHD
yx
IHD
or
2
2
)2222(
2
22
IHD
IHD
yx
IHD
(1 π bond / 1 ring) (2 π bond)
C2H3CI C5H7N
1
2
)13222(
2
22
IHD
IHD
syx
IHD
3
2
)17252(
2
22
IHD
IHD
ryx
IHD
H - C = C - CI
׀ ׀
H H
(1 π bond) (3 π bond / 2 π bond + 1 ring)
or
H H H H H H
׀ ׀ ׀ ׀ ׀ ׀
H - C - C = C – C – C – C – H
׀ ׀ ׀ ׀
H H H H
H H H H H H
׀ ׀ ׀ ׀ ׀ ׀
H - C - C – C = C – C – C – H
׀ ׀ ׀ ׀
H H H H
H H H H H H
׀ ׀ ׀ ׀ ׀ ׀
H - C - C = C – C – C – C – H
׀ ׀ ׀ ׀
H H H H
Index Hydrogen Deficiency (IHD) = Degree unsaturation Saturatedhydrocarbon = CnH2n+2
3. Molecule Index H2 Deficiency
C2H2 2
Oxygen and Sulfur - No effect on IHD
Halogen - like H – CHCI3 = CH4 , C2H5CI = C2H6
Nitrogen – add one to C and one to H
- CH5N same IHD as C2H6
Index Hydrogen Deficiency (IHD) = Degree unsaturation
How many double bonds/rings present
Any double/triple bond/cyclic - number hydrogen atoms decrease
Molecule with N, O, S or Halogen
srqyx XNOHC
2
22 rsyx
IHD
Click here IHD video
1
2
)4222(
2
22
yx
IHD
2
2
)2222(
2
22
yx
IHD
1
2
)4222(
2
22
yx
IHD
0
2
)15222(
2
22
syx
IHD
4
2
)6262(
2
22
yx
IHD
Molecule Index H2 Deficiency
C2H4 1
Molecule Index H2 Deficiency
C2H4O 1
Molecule Index H2 Deficiency
C2H5CI 0
Molecule Index H2 Deficiency
C6H6 4
Molecule Index H2 Deficiency
C7H6O2 5
5
2
)6272(
2
22
yx
IHD
Molecule Index H2 Deficiency
C7H9N2CI3 3
1
2
)19242(
2
22
ryx
IHD
Molecule Index H2 Deficiency
C4H9N 1
3
2
)239272(
2
22
rsyx
IHD
Molecule Index H2 Deficiency
C6H9NOCI2 2
2
2
)129262(
2
22
rsyx
IHD
Molecule Index H2 Deficiency
C4H8CIF 0
0
2
)28242(
2
22
syx
IHD
Click here IHD (Khan Academy)
Molecule Index H2 Deficiency
C6H12O6 1
1
2
)12262(
2
22
yx
IHD
Halogen
4. Click here spectroscopy database (NIST)
Weighted average calculationRAM calculationVideo on IsotopesVideo on weighted average
Relative Atomic Mass
Weighted average mass- due to presence of isotopes
RelativeIsotopic Mass, (Ar) of an element:
•Relative isotopic mass = Average mass of one atom of element
1/12 x mass of one carbon-12
• Relative isotopic mass, carbon = 12.01
RAM = 12.01 Relative Abundance
13
Why RAM is not a whole number?
Relative IsotopicMass:
= (Mass 12
C x % Ab) + (Mass 13
C x % Ab)
= (12 x 98.9/100)+ (13 x 1.07/100)= 12.01
Video on Isotopes
12
Isotopes are present
CCC12.01
98.9% 1.07%
Click here spectroscopy database (Ohio State)
5. Mg - 3 Isotopes
24 Mg – (100/127.2) x 100% - 78.6%
25 Mg – (12.8/127.2)x 100% - 10.0%
26 Mg – (14.4/127.2)x 100% - 11.3%
Relative Isotopic Mass:
= (Mass 24
Mg x % Ab) + (Mass 25
Mg x % Ab) + (Mass 26
Mg x % Ab)
= (24 x 78.6/100)+ (25 x 10.0/100) + (26 x 11.3/100) =24.30
Relative Abundance % Abundance
Pb - 4 Isotopes
204Pb – (0.2/10) x 100% - 2%
206Pb – (2.4/10) x 100% - 24%
207Pb – (2.2/10) x 100% - 22%
208Pb – (5.2/10) x 100% - 52%
Relative Isotopic Mass
= (Mass 204Pb x % Ab) + (Mass 206Pb x % Ab) + (Mass 207Pb x % Ab) + (Mass 208Pb x % Ab)
= (204 x 2/100) + (206 x 24/100) + (207 x 22/100)+ (208 x 52/100) = 207.20
Convert relative abundance to % abundance
Convert relative abundance to % abundance
Relative Abundance % Abundance
RelativeIsotopic Mass
24 25 2624 25 26 MgMg
6. Mass Spectrometer
Uses mass spectrometer
Presence of isotopes
and its abundance
Relative atomic mass
of an element
Relative Molecular mass
of a molecule
Structure of organic
compound
Distinguish bet
structural isomers
CH3CH2CH2OH OH
|
CH3CHCH3
CH3
|
CH3C-CH3
|
CH3
CO2
structural
formula
Organic structure
determination
24 25 26Mg
Mg
7. Detail notes from chem msuClick here notes from chemguide
Mass Spectrometer
Parts of Mass Spectrometer
Sample injection
VaporizationChamber
• Sample heat to
vapour state
IonizationChamber
• Molecule bombard with
electron form positive ion
AcceleratorChamber
• M+ ion acceleratedby Electric field
Deflector
• M+ ion deflected by magnetic field
Detector
• Convert amt M+ ion to current.
• M+ ion neutralize by electron (more
e need - higher current –
higher intensity of peak)
• Intensity of peak show -relative
abundanceof ion
Sample X bombard by electron
• Form positive M+ ion
• Accelerated (Electric Field)
• Deflected (Magnetic Field) and Detected
X + e- → X+
+ 2e-
Vaporization Ionization Accelerator Deflector Detector321 54
2
1
3 4
5
8. Click here for simulation
Mass Spectrometer
Parts of Mass Spectrometer
Vaporization Ionization Accelerator Deflector Detector321 54
Vaporization
Injection/ vaporization of sample
liquid state gaseous
Ionization
Form cation, M+
Acceleration
M+ ion accelerate
by Electric field
Deflection
M+ ion deflect
by magnetic field
Deflection depend:
mass/charge (m/z) ratio:
(m/z) ratio HIGH↑ - Deflection LOW↓
Deflection depend:
mass/charge (m/z) ratio:
(m/z) ratio LOW↓- Deflection HIGH ↑
37
CI+
35
CI+
35
CI2+
2
3 4
1
5 Detector
• Convert abundance M+ ion to current.
• M+ ion neutralize by electron (more e need -
high current – high intensity of peak)
• Peak Intensity –relative abundance of ion
9. Video Mass spectrometerVideo Ionization/fragmentation Video how MS works
Excellent Online Spectra Database.Click here to view
Mass Spectra Online Database
1 Search methane molecule, CH4
Video on mass spectrometer
Mass/charge m/z
Relative
abundance
Isotopic peak M+ + 1Molecular ion peak, M+
2 Fragmentation pattern CH4 3 Mass Spectrum CH4
Video how MS works
10. Mg - 3 Isotopes
26 Mg - 11.3% - m/z highest – deflect LEAST
25 Mg - 10.0%
24 Mg – 78.6% - m/z lowest – deflect MOST
Relative Isotopic Mass:
= (24
Mg x % Ab) + (25
Mg x % Ab) + (26
Mg x % Ab)
= (24 x 78.6/100) + (25 x 10.0/100) + (26 x 11.3/100) = 24.30
Mass spectrometry to determine Relative Isotopic Mass
Deflect
MOST
Deflect
LEAST
Pb - 4 Isotopes
208Pb – 52% - m/z highest – deflect LEAST
207Pb - 22%
206Pb - 24%
204Pb – 2% - m/z lowest – deflect MOST
Relative Isotopic Mass
= (204Pb x % Ab) + (206Pb x % Ab) + (207Pb x % Ab) + (208Pb x % Ab)
= (204 x 2/100) + (206 x 24/100) + (207 x 22/100) + (208 x 52/100) = 207.20
Deflect
MOST
Deflect
LEAST
24 Mg 26 Mg
204Pb 208Pb
11. CI - 2 Isotopes
37 CI – 24.5% - m/z highest – deflect LEAST
35 CI – 75.5% - m/z lowest – deflect MOST
Relative Isotopic Mass:
= (35
CI x % Ab) + (37
CI x % Ab)
= (35 x 75.5/100) + (37 x 24.5/100) = 35.5
Deflect
MOST
Deflect
LEAST
Br - 2 Isotopes
81Br – 49.3% - m/z highest – deflect LEAST
79Br – 50.6% - m/z lowest – deflect MOST
Deflect
MOST
Deflect
LEAST
35CI 37CI
Relative Isotopic Mass:
= (79
Br x % Ab) + (81
Br x % Ab)
= (79 x 50.6/100) + (81 x 49.3/100) = 79.9
79Br 81Br
Mass spectrometry to determine Relative Isotopic Mass
35 CI 37 CI
79Br 81Br
12. H - 3 Isotopes
3H – trace amt
2H – 0.015% - m/z highest – deflect LEAST
1H – 99.9% - m/z lowest – deflect MOST
Relative Isotopic Mass:
= (1
H x % Ab) + (2
H x % Ab)
= (1 x 99.9/100) + (2 x 0.015/100) = 1.007
Deflect
MOST
Deflect
LEAST
C - 3 Isotopes
14C- trace amt
13C – 1.1% - m/z highest – deflect LEAST
12C – 98.9% - m/z lowest – deflect MOST
Deflect
MOST
Deflect
LEAST
1H 2H
Relative Isotopic Mass:
= (12
C x % Ab) + (813
Cx % Ab)
= (12 x 98.9/100) + (13 x 1.1/100) = 12.01
12C 13C
3H
14C
Mass spectrometry to determine Relative Isotopic Mass
1H 2H
12C 13C
13. Ionization and Fragmentation
Ionization forming M+
CH3CH2CH2 : CH3 + e → CH3CH2CH2
+
.CH3 + 2e
• Fragmentation of M+
producing 43
CH3CH2CH2
+
·CH3 → CH3CH2CH2
+
+ ·CH3
• Fragmentation of M+
producing 15
CH3CH2CH2
+
·CH3 → CH3CH2CH2· + +
CH3
Ionization and Fragmentation Process- CH3CH2CH2CH3
Ionization Process - CH3CH2CH2CH3
• Bombard by electron form cation
• Molecular ion, M+
= 58
• (CH3CH2CH2CH3)+
= 58
Fragmentation Process CH3CH2CH2CH3
• Molecular ion, M+ undergo fragmentation
• Cation and Radical form
• Cation - Detected
• Radical –Not detected (No charged)
H H
׀ ׀
CH3CH2CH2 C:H + e → CH3CH2CH2C+.H + 2e
׀ ׀
H H
Ionization forming M+
CH3CH2:CH2CH3 + e → CH3CH2
+·CH2CH3 + 2e
• Fragmentation of M+
producing29
CH3CH2
+·CH2CH3 → CH3CH2
+
+ .CH2CH3
Ionization M+
, m/z = 58
CH3CH2CH2CH3 + e → CH3CH2CH2CH3
+
+ 2e
Ionization and Fragmentation of M+
• Form - m/z = 58, 43 and 15
m/z = 58
m/z = 43
m/z = 15
Ionization and Fragmentation of M+
• Form- m/z = 58 and 29
m/z = 58
m/z = 58
m/z = 29
Unpair electronPositively charged
Will ACCELARATED NOT move
cation radical
14. CH3CH2CH2CH3
CH3CH2CH2CH3
+- 58 - m/z highest –deflect LEAST
CH3CH2CH2
+ – 43
CH3CH2
+ – 29
CH3
+ –15 - m/z lowest– deflect MOST
Ionization/ Fragmentationpattern CH3CH2CH2CH3
Deflect
MOST
Deflect
LEAST
CH3CH2CH2CH3
+
CH3CH2CH2
+
ionization
CH3
+
Ionization and FragmentationProcess
Fragmentation
Ionization CH3CH2CH2CH3
CH3CH2CH2CH3 + e → CH3CH2CH2CH3
+
+ 2e → 58
or
CH3CH2:CH2CH3 + e → CH3CH2
+·CH2CH3 + 2e → 58
Mass spectrum CH3CH2CH2CH3IonizationCH3CH2CH2CH3
CH3CH2
+
Fragmentation of M+
CH3CH2CH2
+
·CH3 → CH3CH2CH2
+
- 43
CH3CH2
+·CH2CH3 → CH3CH2
+
– 29
CH3CH2CH2
+
·CH3 → +CH3 - 15
CH3CH2CH2CH3
+- 58
CH3CH2CH2
+ – 43
CH3CH2
+ – 29
CH3
+ – 15
CH3
+ CH3CH2CH2CH3
+
20. Isomers, Propan-1-ol vs Propan-2-ol
Peak 45 is higher
• Loss of methyl radical at both sides produce (CH3CH(OH))+
• No m/z= 29 peak detected – No CH2CH3 found !
Fragmentationpeak
(M - 15)+ = 45 -> (CH2CH2OH)+
(M - 29)+ = 31 -> (CH2OH)+
(M - 31)+ = 29 -> (CH3CH2)+
(M - 45)+ = 15 -> (CH3)+
Isomers of C3H8OH
Fragmentationpeaks
(M - 15)+ = 45 -> (CH3CH(OH))+
(M - 17)+ = 43 -> (CH3CHCH3)+
(M - 33)+ = 27 -> (CH3C)+
Vs
Loss of CH3
Loss of CH3CH2
Loss of CH2OH
Loss of CH2CH2OH
Loss CH3
OH OH
׀ ׀
CH3 C+·CH3 → CH3 C+
+ ·CH3
׀׀
H H
m/z= 45
CH3CH2CH2OH
OH
|
CH3CHCH3
Loss OH
Loss OH, CH3, H
Peak 29 and 31 are found
• Inductive effect of OH cause splitting of CH3CH2-|-CH2OH
• m/z = 29 peak detected – CH2CH3 present
CH3CH2
+
· CH2OH → CH3CH2
+
+ ·CH2OH
m/z= 29
CH3CH2
+
· CH2OH → CH3CH2 · + +
CH2OH
m/z= 31
Propan-1-ol
Propan-2-ol
15
Vs
Molecular Ion, M+
= 60 -> CH3CH2CH2OH+
Molecular Ion, M+
= 60 -> CH3CH(OH)CH3
+
21. Isomers, 2 methylbutanevs 2, 2 dimethylpropane
CH3
׀
CH3CHCH2CH3
CH3
|
CH3C-CH3
|
CH3
Peak 29 absent
• No CH3CH2
Peak 57 is higher
• Loss of methyl radical
produce tertiary carbocation
• Tertiary carbocation – More stable
Fragmentationpeaks
(M - 15)+ = 57 -> CH3CH(CH3)CH2
+
(M - 29)+ = 43 -> CH3CH(CH3)+
(M - 43)+ = 29 -> CH3CH2
+
(M - 57)+ = 15 -> CH3
+
Isomers of C5H12
Fragmentationpeaks
(M - 15)+ = 57 -> C(CH3)3
+
(M - 30)+ = 42 -> C(CH3)2
+
(M - 45)+ = 27 -> CH3C+
(M - 57)+ = 15 -> CH3
+
Vs
Loss of CH3
Loss of CH3CH2
Loss of CH3CH(CH3)
Loss of CH3CH(CH3)CH2
Loss of CH3
Loss of TWO CH3
Loss of THREE CH3
CH3
׀
CH3C+·CH3
׀
CH3
m/z= 57
CH3
׀
CH3 C+
+ ·CH3
׀
CH3
2 methylbutane
2, 2 dimethylpropane
Loss of C(CH3)3
Vs
Peak 29 absent
• CH3CH2 present
Molecular Ion, M+
= 72 -> CH3CH(CH3)CH2CH3
+
Molecular Ion, M+
= 72 -> C(CH3)4
+
22. Normal Vs High ResolutionMass spectrometer
Normal Mass Spectrometer
• Molecular formula by adding all RAM
• RMM for molecule = Sum of all RAM
• RMM O2 = 16 + 16 = 32
• RMM N2H4 = (14 x 2) + (1 x 4) = 32
• RMM CH3OH = (12 + 3 + 16 + 1) = 32
• Molecular ion peak - O2, N2H4, CH3OH - SAME = 32
RAM, O = 16
RAM, N = 14
RAM, H = 1
RAM, C = 12
High ResolutionMass Spectrometer
Measure RMM to 4/5 decimalplaces
• Molecular formula by adding all RAM
• RMM for molecule = Sum of all RAM
• RMM O2 = 15.9949 + 15.9949 = 31.9898
• RMM N2H4 = (14.0031 x 2) + (1.0078 x 4) = 32.0375
• RMM CH3OH = (12.0000 )+ (3 x 1.0078) + 15.9949 = 32.0262
• Molecular ion peak- O2, N2H4, CH3OH is the NOT the same
RAM, O = 15.9949
RAM, N = 14.0031
RAM, H = 1.0078
RAM, C = 12.0000
Vs
Vs
O2, N2H4, CH3OH
Same 32
O2 N2H4 CH3OH
different
Video how MS works
High resolution Mass spectrum
23. 37CI+ 35CI+
CI2 molecule
37CI-37CI - 74 - m/z highest – deflect LEAST
35CI-37CI –72
35CI-35CI –70
37CI –37
35CI –35 - m/z lowest– deflect MOST
Ionization/ Fragmentation pattern CI2
Deflect
MOST
Deflect
LEAST
35CI-35CI+
35CI+
35CI-37CI+
37CI-37CI+
Ionization
37CI+
37CI-37CI+
Fragmentation
Fragmentation of CI2
+
into CI+
CI+
.CI → [35
CI+
+ 35
CI·] + 2e – 35
CI+
.CI → [37
CI+
+ 37
CI·] + 2e –37
Ionization of CI2 to CI2
+
CI:CI + e- →[35
CI+
.35
CI] + 2e – 70
CI:CI + e- →[35
CI+
.37
CI] + 2e – 72
CI:CI + e- →[37
CI+
.37
CI] + 2e – 74
m/z = 37
m/z = 35
Ratio (35
CI : 37
CI) - 3:1
Mass spectrum CI2 / CI atom
Ratio (35
CI35
CI: 35
CI37
CI: 37
CI37
CI) - 9:6:1
IonizationCI2 molecule
37CI-37CI - 74
35CI-37CI – 72
35CI-35CI – 70
37CI – 37
35CI – 35
Ionization and FragmentationProcess
27. TI
IB Questions on Mass Spectrometer
Mass spectrometerused to investigateisotopiccompositionof elements.
Thallium has two isotopes.
1) State symbol of two singly chargedionsform.
2) State which ion will follow path marked X on diagram.
lighter-> DEFLECTED MORE
3) Doublychargedions form. Suggestreason whetherthey wouldbe deflectedless or
more than ions at X and Y.
DEFLECTED MORE. Cause deflectiondependson m/z ratio.
Low Mass + High charge -> m/z ratio is low -> deflectedmore.
Naturally occuringboronhas 2 isotopes.RAM boronis 10.81.
% abundance x% (100 – x)%
Determinepercentageabundanceof these isotopes.
Answer:Let % abundancebe x.
1
TI TI
203 205
81 81
X =
B10 B11
Relative Isotopic Mass:
= (Mass 10
B x % Ab) + (Mass 11
B x % Ab)
= (10 x x/100) + (11 x (100 – x)/100) = 10.81
X = 19%
TI+
81
203
TI+205
81
TI+
203
81
28. IB Questions on Mass Spectrometer
Germaniumis analysedin mass spec. The first and last processesare vaporizationand detection.
1) State the namesof other 3 processesin order in which they occur
Answer:Ionization-> Acceleration-> Deflection
2) For each of processesnamed in a (i), outlinehow processoccur
Ionization-> Sample bombardedwith highenergy/highspeed electrons
Acceleration-> Cations (+ve chargedions) acceleratedby an electricfield
Deflection-> Cations deflectedby a magneticfield
3) Germaniumfoundto have followingcomposition
i)Definerelativeatomic mass.
Average/ weightedmasses of all isotopesof an element.
ii) CalculateRAM, givinganswer to two decimal places.
2
RelativeIsotopicMass
= (Mass 70Ge x % Ab) + (Mass 72Ge x % Ab) + (Mass 74Ge x % Ab) + (Mass 76Ge x % Ab)
= (70 x 22.60/100)+ (72 x 25.45/100)+ (74 x 36.73/100)+ (76 x 15.22/100)= 72.89
29. IB Questions on Mass Spectrometer
Showsa mass spectrometer.
1)Identifythe parts labelledA, B and C.
2)State and explainwhich one will undergogreatest deflection.
Answer : Greatestdeflection-> lowest mass + highestcharged -> m/z -> lowest
3) Mass spectrumshown below:
i) Explainwhy thereis more than one peak.
Existence of isotopes
ii) Calculate RAM.
3
Relative Isotopic Mass
= (Mass 24Y x % Ab) + (Mass25Y x % Ab) + (Mass 26Yx % Ab)
= (24 x 79/100)+ (25 x 10/100)+ (26 x 11/100) = 24.32
• electron gun
• ionisation chamber
• ionizer
• Electric field
• Charged plates
• Potential difference
• Magnetic field
• Magnet
• Electromagnet
greatest deflection – low mass, high charged
smallest deflection – high mass, low charged
A
C
B
Li+
Li2+
7
6
30. IB Questions on Mass Spectrometer
Vaporizedmagnesiumis introducedintomass spec. One of the ionsthat reachesdetectorshown below.
1)Identifynumberof protons,neutronand electrons
Answer: 12 protons,13 neutrons,11 electrons
2) State how ion is acceleratedin mass spectrometer.
Using a strong electricfield/strongoppositechargedplate/potentialdifference
3) The ion is also detected by changingthe magnetic field. Deduceand explainby referenceto
m/z valuesof these two ionsof magnesium,which of the ions and is detectedusing a stronger
magneticfield.
Answer: - due to lower charge -> m/z is higher-> deflectedless -> needsa strongermagneticfield to deflect.
4
Cations (+ve) acceleratedby (-ve) plates
25
12
25Mg 2+
smallest deflection – high mass, low charged
Strong magnet/magnetic field to deflect it to bottom
Mg +
25Mg 2+ 25Mg +
25Mg +
25Mg +
31. Rubidiumcontainstwo stable isotopes.RAM for rubidiumis 85.47
1)Calculate % of each isotopein rubidium.
Answer : Let % abundancebe x %.
% Abundance x% (100 – x)%
76.5% 23.5%
2) Vaporizedsample is ionizedand accelerated.How the use of magneticfieldand detectorenablespercentageof two
isotopesto be determined.
5
85 87
Relative Isotopic Mass:
= (Mass 85
Rb x % Ab) + (Mass 87
Rb x % Ab)
= (85 x x/100) + (87 x (100 – x)/100) = 85.47
X = 76.5%
Rb
Detector
• Convert abundance M+ ions to current.
• M+ ions neutralize by electrons (more
e needed - higher current –
higher intensity of peak)
•Ratio of intensity peaks show
ratio of ions in sample
•Ratio of height of peaks due to
85Rb : 87Rb –> 76.5 : 23.5
Magnetic field/Deflector
• M+ ion deflected by magnetic field
- lighter -> deflectedmore
- heavier -> deflectedless
IB Questions on Mass Spectrometer
Rb Rb
85 Rb 87 Rb
85 Rb 87 Rb
85 Rb
87 Rb