Hyperconjugation is the donation of a sigma bond into an adjacent empty or partially filled p orbital, which results in an increased stability of the molecule.
Contributed by: Samuel Redstone (Undergraduate), University of Utah, 2016
This presentation describes the concept of Hyperconjugation in simple words, gives definition of hyperconjugation, explains why it is called as 'No bond Resonance' and gives the effects of hyperconjugation on the chemical properties of compounds: alkyl cations and their relative stability, alkyl radicals and their relative stability, alkenes and their relative stability, bond length, anomeric effect and Baker - Nathan effect.
This document discusses the concept of hyperconjugation, which involves the delocalization of sigma electrons from an adjacent C-H bond into an empty p-orbital of an unsaturated system like an alkene or benzene ring. This effect increases the stability of alkenes and carbocations with more alkyl substituents by allowing for additional no bond resonance structures. The stability of alkenes and carbocations increases with the number of alkyl groups due to greater hyperconjugative stabilization from more C-H bonds. Hyperconjugation is an important effect that helps explain the observed stability and reactivity patterns of unsaturated organic compounds.
Dr. Neelam from the Department of Chemistry presented on the topic of hyperconjugation. Hyperconjugation is the delocalization of σ-electrons from a C-H bond into an adjacent unsaturated system. It can occur in alkenes, alkynes, carbocations, and carbon radicals. The number of possible hyperconjugative structures equals the number of alpha hydrogens on sp3 hybridized carbon atoms. Hyperconjugation explains trends in stability and heats of hydrogenation between different alkenes. It is a permanent effect that does not change hybridization and is distance independent.
This document discusses inductive effect and mesomeric (or resonance) effect, including their definitions, types, and applications. The key points are:
1. Inductive effect is the polarization of a sigma bond due to electron donating or withdrawing groups, transmitted through sigma bonds. It influences chemical and physical properties.
2. Mesomeric effect is polarity produced between pi bonds or a pi bond and lone pair, leading to electron delocalization. Groups like -NO2 show negative mesomeric effect while -OH shows positive effect.
3. Applications include reactivity patterns of aromatic compounds affected by activating or deactivating groups, stability of carbocations/carbanions, and acid/base
Conjugation involves the overlap of p-orbitals across intervening sigma bonds, creating a system of delocalized electrons within alternating single and multiple bonds. This conjugated system can be cyclic, linear, or mixed and increases stability compared to non-conjugated systems. Hyperconjugation also stabilizes compounds through the interaction of sigma bonds with adjacent empty or partially filled p-orbitals, without actual bond resonance. Both conjugation and hyperconjugation extend molecular orbitals to increase stability.
The document discusses organic reactions and reaction mechanisms. It defines nucleophiles and electrophiles, and provides examples of each. It then summarizes several common types of organic reactions including addition reactions, substitution reactions, elimination reactions, and aromatic substitutions. The mechanisms and examples of nucleophilic addition, electrophilic addition, nucleophilic substitution, and electrophilic aromatic substitutions like nitration, sulfonation, and halogenation are described in detail.
This is a presentation file on Inductive Effect, Bond Length, Bond Energy, Bond Angle for the course Organic Pharmacy I, course code is PHAR-1105 specially for the pharmacy students. Also it can be used for the Biochemistry students and other like as HSC level in Bangladesh or another country. We are the students of Mawlana Bhashani Science and Technology University, department of pharmacy which is located in Tangail.
Thank you for your patient.
This document discusses aromaticity, including its introduction, criteria for aromatic compounds, Hückel's rule, examples of aromatic and anti-aromatic compounds, and non-aromatic compounds. Aromatic compounds are cyclic, planar, and have delocalized pi electrons that follow Hückel's rule of 4n+2 pi electrons. Benzene is used to originally define aromaticity. Resonance contributes greatly to aromatic stability. Anti-aromatic compounds have 4n pi electrons and are destabilized by cyclic pi electron delocalization. Cyclooctatetraene is provided as an example of a non-aromatic compound for not being planar.
This presentation describes the concept of Hyperconjugation in simple words, gives definition of hyperconjugation, explains why it is called as 'No bond Resonance' and gives the effects of hyperconjugation on the chemical properties of compounds: alkyl cations and their relative stability, alkyl radicals and their relative stability, alkenes and their relative stability, bond length, anomeric effect and Baker - Nathan effect.
This document discusses the concept of hyperconjugation, which involves the delocalization of sigma electrons from an adjacent C-H bond into an empty p-orbital of an unsaturated system like an alkene or benzene ring. This effect increases the stability of alkenes and carbocations with more alkyl substituents by allowing for additional no bond resonance structures. The stability of alkenes and carbocations increases with the number of alkyl groups due to greater hyperconjugative stabilization from more C-H bonds. Hyperconjugation is an important effect that helps explain the observed stability and reactivity patterns of unsaturated organic compounds.
Dr. Neelam from the Department of Chemistry presented on the topic of hyperconjugation. Hyperconjugation is the delocalization of σ-electrons from a C-H bond into an adjacent unsaturated system. It can occur in alkenes, alkynes, carbocations, and carbon radicals. The number of possible hyperconjugative structures equals the number of alpha hydrogens on sp3 hybridized carbon atoms. Hyperconjugation explains trends in stability and heats of hydrogenation between different alkenes. It is a permanent effect that does not change hybridization and is distance independent.
This document discusses inductive effect and mesomeric (or resonance) effect, including their definitions, types, and applications. The key points are:
1. Inductive effect is the polarization of a sigma bond due to electron donating or withdrawing groups, transmitted through sigma bonds. It influences chemical and physical properties.
2. Mesomeric effect is polarity produced between pi bonds or a pi bond and lone pair, leading to electron delocalization. Groups like -NO2 show negative mesomeric effect while -OH shows positive effect.
3. Applications include reactivity patterns of aromatic compounds affected by activating or deactivating groups, stability of carbocations/carbanions, and acid/base
Conjugation involves the overlap of p-orbitals across intervening sigma bonds, creating a system of delocalized electrons within alternating single and multiple bonds. This conjugated system can be cyclic, linear, or mixed and increases stability compared to non-conjugated systems. Hyperconjugation also stabilizes compounds through the interaction of sigma bonds with adjacent empty or partially filled p-orbitals, without actual bond resonance. Both conjugation and hyperconjugation extend molecular orbitals to increase stability.
The document discusses organic reactions and reaction mechanisms. It defines nucleophiles and electrophiles, and provides examples of each. It then summarizes several common types of organic reactions including addition reactions, substitution reactions, elimination reactions, and aromatic substitutions. The mechanisms and examples of nucleophilic addition, electrophilic addition, nucleophilic substitution, and electrophilic aromatic substitutions like nitration, sulfonation, and halogenation are described in detail.
This is a presentation file on Inductive Effect, Bond Length, Bond Energy, Bond Angle for the course Organic Pharmacy I, course code is PHAR-1105 specially for the pharmacy students. Also it can be used for the Biochemistry students and other like as HSC level in Bangladesh or another country. We are the students of Mawlana Bhashani Science and Technology University, department of pharmacy which is located in Tangail.
Thank you for your patient.
This document discusses aromaticity, including its introduction, criteria for aromatic compounds, Hückel's rule, examples of aromatic and anti-aromatic compounds, and non-aromatic compounds. Aromatic compounds are cyclic, planar, and have delocalized pi electrons that follow Hückel's rule of 4n+2 pi electrons. Benzene is used to originally define aromaticity. Resonance contributes greatly to aromatic stability. Anti-aromatic compounds have 4n pi electrons and are destabilized by cyclic pi electron delocalization. Cyclooctatetraene is provided as an example of a non-aromatic compound for not being planar.
1. Electrochemistry deals with the transformation of electrical energy to chemical energy and vice versa. It involves the chemical applications of electricity.
2. An electrolytic cell converts electrical energy to chemical energy, while an electrochemical cell converts chemical energy to electrical energy.
3. Arrhenius' theory of electrolytic dissociation states that when an electrolyte dissolves in water, it breaks up into ions. There is a dynamic equilibrium between the ionized and non-ionized molecules. The degree of ionization depends on factors like the ionization constant.
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.
1. Carbenes are neutral molecules containing a divalent carbon atom with two unshared valence electrons. They exist in both singlet and triplet states depending on the electronic spin.
2. Carbenes undergo insertion reactions into X-H and C-C bonds. They also add across double bonds, with singlet carbenes preserving alkene stereochemistry and triplet carbenes losing it.
3. Carbenes are generated by reactions such as α-elimination of halogenated compounds with base or decomposition of diazo compounds. They can rearrange through migrations such as the Wolff or Arndt-Eistert reactions.
1) α,β-Unsaturated carbonyl compounds contain a carbonyl group and a conjugated carbon-carbon double bond separated by one carbon-carbon single bond.
2) These compounds undergo both electrophilic and nucleophilic addition reactions due to the conjugation between the carbonyl and double bond.
3) Common reactions include the Michael addition, in which a carbanion adds to the β-carbon, and the Diels-Alder reaction, where a conjugated diene adds to form a six-membered ring.
1) The document summarizes aromaticity and anti-aromaticity, discussing the key criteria for aromatic compounds including being cyclic, conjugated, planar, and having 4n+2 π electrons.
2) It provides examples of aromatic compounds like benzene and non-aromatic compounds that do not meet the criteria. Anti-aromatic compounds are also discussed.
3) NMR spectroscopy is discussed as a way to distinguish aromatic protons from other types of protons based on chemical shift values.
This document discusses organic reactions and mechanisms. It defines key terms like substrate, reagent, products, and mechanism. It describes how factors like inductive and mesomeric effects can influence reactions by altering electron density. It also discusses different types of reaction intermediates that can form, such as carbonium ions, carbanions, free radicals, and carbenes. The document classifies reagents as electrophiles or nucleophiles and describes their behaviors. It explains concepts like activation energy and the transition state that systems must go through for a reaction to occur.
Hybridization is the idea that atomic orbitals fuse to form newly hybridized orbitals, which in turn, influences molecular geometry and bonding properties. Hybridization is also an expansion of the valence bond theory.
An organic species which has a carbon atom bearing only six electrons in its outermost shell and has a positive charge is called carbocation.
The positively charged carbon of carbocation is sp2 hybridized.
The unhybridized p-orbital remains vacant.
They are highly reactive and act as reaction intermediate.
They are also called carbonium ion.
Inductive Effect is the important topic in organic chemistry that gives us idea about electron withdrawing and accepting module of the specific group that determines the reactivity of the molecule or compound.
This document discusses different electronic effects in organic chemistry. It describes inductive effect as a permanent polarization of electron density between two unlike atoms in a bond. Electron-withdrawing and electron-releasing groups are discussed. Mesomeric effect allows for resonance stabilization through delocalization of charge in conjugated systems. Electromeric effect involves the temporary shift of a pi bond electron pair to one atom upon reaction with an electrophile. The order of effects from strongest to weakest is given as mesomeric, electromeric, and inductive. Applications to stability of ions and carbocations are outlined.
This document discusses carbanions, which are negatively charged organic species where carbon carries three bond pairs and one lone pair. Carbanions are stabilized through conjugation, resonance effects, field effects, and aromaticity. They are generated through heterolytic bond cleavage or addition of a negative ion to a carbon-carbon multiple bond. As nucleophiles, carbanions undergo reactions such as alpha-halogenation of ketones, additions to carbonyls, nucleophilic acyl substitutions, substitutions with alkyl halides, and Michael additions.
Resonance occurs when a molecule can be represented by multiple Lewis structures and the actual structure is a hybrid of all the contributing structures. A resonance hybrid is the average structure between all the canonical or contributing Lewis structures. Delocalization of electrons through resonance leads to decreased potential energy and increased stability compared to any single contributing structure. Electron donating groups cause positive resonance or inductive effects while electron withdrawing groups cause negative resonance or inductive effects. Resonance and inductive effects influence acidity, basicity, and reactivity.
This presentaion describes about the basic principle effects in organic chemistry like inductive,mesomeric,electromeric, resonance and hyperconjugation. this presentation contains some JAM competitive questions.
Mesomeric (or resonance) effect refers to the polarity produced in a molecule through delocalization of pi electrons between bonds or a bond and lone pair. This effect can increase or decrease electron density in different parts of a molecule. Negative mesomeric effects are shown by groups like nitro (-NO2) that withdraw electron density, while positive effects are shown by groups like hydroxyl (-OH) that release electron density. Understanding mesomeric effects helps explain a molecule's reactivity toward electrophiles and nucleophiles by determining where electron density is increased or decreased.
This document discusses electronic displacement in organic compounds. It describes two types of electronic displacement: permanent displacement including inductive, resonance, and mesomeric effects; and temporary displacement through electromeric effects. Inductive effects are further broken down into +I effects where groups donate electron density and -I effects where groups withdraw electron density. Examples of inductive effects include their impact on acid/base strength, stability of carbocations/carbanions, and dipole moments.
Cyclohexane exists in different conformations viz chair, boat, twist boat and half chair. These conformations possess different energies. Therefore they differ in energy.
Resonance structures represent different arrangements of electrons in a molecule that have the same positions of nuclei but different bonding patterns. Resonance contributes to the stability of molecules like benzene by delocalizing electrons across multiple equivalent structures. The actual structure of a molecule represented by resonance is a hybrid of the contributing structures, with bond lengths intermediate between single and double bonds. Delocalization of electrons is depicted using curved arrows between resonance structures.
Resonance effect occurs when a compound can be represented by two or more Lewis structures with the same arrangement of atoms. These contributing structures are called resonance structures.
The resonance structures are hypothetical and do not represent real molecules individually. Together they contribute to a resonance hybrid structure that is more stable than any individual resonance structure. The most stable contributing structure contributes the most to the resonance hybrid.
Conditions for resonance include sp or sp2 hybridized atoms involved, overlapping parallel p-orbitals to form a conjugated system. The sigma bond framework remains the same between structures, atomic positions do not change, and electron counts are equal.
This document discusses inductive effect, which is the permanent displacement of a carbon chain's shared electron pair towards the more electronegative atom or group. It describes the negative inductive effect caused by electron-withdrawing groups and the positive inductive effect of electron-donating groups. Finally, it explains how inductive effect influences the strength of organic acids and bases, with acid strength decreasing as positive inductive effect or negative inductive effect decreases.
Infrared spectroscopy involves using infrared radiation to analyze materials. Molecules absorb specific infrared frequencies that are characteristic of their structure, such as bond vibrations and stretches. There are two main methods for infrared spectroscopy - scanning monochromator which analyzes one wavelength at a time, and Fourier transform infrared spectroscopy which uses interferometry to measure all infrared wavelengths simultaneously. Fourier transform then converts this raw interferogram data into the infrared spectrum. Infrared spectroscopy can be used to identify functional groups and molecular structures in compounds like 1-Hexene, Toluene, and Cyclohexanol based on their characteristic absorption peaks.
1. Electrochemistry deals with the transformation of electrical energy to chemical energy and vice versa. It involves the chemical applications of electricity.
2. An electrolytic cell converts electrical energy to chemical energy, while an electrochemical cell converts chemical energy to electrical energy.
3. Arrhenius' theory of electrolytic dissociation states that when an electrolyte dissolves in water, it breaks up into ions. There is a dynamic equilibrium between the ionized and non-ionized molecules. The degree of ionization depends on factors like the ionization constant.
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.
1. Carbenes are neutral molecules containing a divalent carbon atom with two unshared valence electrons. They exist in both singlet and triplet states depending on the electronic spin.
2. Carbenes undergo insertion reactions into X-H and C-C bonds. They also add across double bonds, with singlet carbenes preserving alkene stereochemistry and triplet carbenes losing it.
3. Carbenes are generated by reactions such as α-elimination of halogenated compounds with base or decomposition of diazo compounds. They can rearrange through migrations such as the Wolff or Arndt-Eistert reactions.
1) α,β-Unsaturated carbonyl compounds contain a carbonyl group and a conjugated carbon-carbon double bond separated by one carbon-carbon single bond.
2) These compounds undergo both electrophilic and nucleophilic addition reactions due to the conjugation between the carbonyl and double bond.
3) Common reactions include the Michael addition, in which a carbanion adds to the β-carbon, and the Diels-Alder reaction, where a conjugated diene adds to form a six-membered ring.
1) The document summarizes aromaticity and anti-aromaticity, discussing the key criteria for aromatic compounds including being cyclic, conjugated, planar, and having 4n+2 π electrons.
2) It provides examples of aromatic compounds like benzene and non-aromatic compounds that do not meet the criteria. Anti-aromatic compounds are also discussed.
3) NMR spectroscopy is discussed as a way to distinguish aromatic protons from other types of protons based on chemical shift values.
This document discusses organic reactions and mechanisms. It defines key terms like substrate, reagent, products, and mechanism. It describes how factors like inductive and mesomeric effects can influence reactions by altering electron density. It also discusses different types of reaction intermediates that can form, such as carbonium ions, carbanions, free radicals, and carbenes. The document classifies reagents as electrophiles or nucleophiles and describes their behaviors. It explains concepts like activation energy and the transition state that systems must go through for a reaction to occur.
Hybridization is the idea that atomic orbitals fuse to form newly hybridized orbitals, which in turn, influences molecular geometry and bonding properties. Hybridization is also an expansion of the valence bond theory.
An organic species which has a carbon atom bearing only six electrons in its outermost shell and has a positive charge is called carbocation.
The positively charged carbon of carbocation is sp2 hybridized.
The unhybridized p-orbital remains vacant.
They are highly reactive and act as reaction intermediate.
They are also called carbonium ion.
Inductive Effect is the important topic in organic chemistry that gives us idea about electron withdrawing and accepting module of the specific group that determines the reactivity of the molecule or compound.
This document discusses different electronic effects in organic chemistry. It describes inductive effect as a permanent polarization of electron density between two unlike atoms in a bond. Electron-withdrawing and electron-releasing groups are discussed. Mesomeric effect allows for resonance stabilization through delocalization of charge in conjugated systems. Electromeric effect involves the temporary shift of a pi bond electron pair to one atom upon reaction with an electrophile. The order of effects from strongest to weakest is given as mesomeric, electromeric, and inductive. Applications to stability of ions and carbocations are outlined.
This document discusses carbanions, which are negatively charged organic species where carbon carries three bond pairs and one lone pair. Carbanions are stabilized through conjugation, resonance effects, field effects, and aromaticity. They are generated through heterolytic bond cleavage or addition of a negative ion to a carbon-carbon multiple bond. As nucleophiles, carbanions undergo reactions such as alpha-halogenation of ketones, additions to carbonyls, nucleophilic acyl substitutions, substitutions with alkyl halides, and Michael additions.
Resonance occurs when a molecule can be represented by multiple Lewis structures and the actual structure is a hybrid of all the contributing structures. A resonance hybrid is the average structure between all the canonical or contributing Lewis structures. Delocalization of electrons through resonance leads to decreased potential energy and increased stability compared to any single contributing structure. Electron donating groups cause positive resonance or inductive effects while electron withdrawing groups cause negative resonance or inductive effects. Resonance and inductive effects influence acidity, basicity, and reactivity.
This presentaion describes about the basic principle effects in organic chemistry like inductive,mesomeric,electromeric, resonance and hyperconjugation. this presentation contains some JAM competitive questions.
Mesomeric (or resonance) effect refers to the polarity produced in a molecule through delocalization of pi electrons between bonds or a bond and lone pair. This effect can increase or decrease electron density in different parts of a molecule. Negative mesomeric effects are shown by groups like nitro (-NO2) that withdraw electron density, while positive effects are shown by groups like hydroxyl (-OH) that release electron density. Understanding mesomeric effects helps explain a molecule's reactivity toward electrophiles and nucleophiles by determining where electron density is increased or decreased.
This document discusses electronic displacement in organic compounds. It describes two types of electronic displacement: permanent displacement including inductive, resonance, and mesomeric effects; and temporary displacement through electromeric effects. Inductive effects are further broken down into +I effects where groups donate electron density and -I effects where groups withdraw electron density. Examples of inductive effects include their impact on acid/base strength, stability of carbocations/carbanions, and dipole moments.
Cyclohexane exists in different conformations viz chair, boat, twist boat and half chair. These conformations possess different energies. Therefore they differ in energy.
Resonance structures represent different arrangements of electrons in a molecule that have the same positions of nuclei but different bonding patterns. Resonance contributes to the stability of molecules like benzene by delocalizing electrons across multiple equivalent structures. The actual structure of a molecule represented by resonance is a hybrid of the contributing structures, with bond lengths intermediate between single and double bonds. Delocalization of electrons is depicted using curved arrows between resonance structures.
Resonance effect occurs when a compound can be represented by two or more Lewis structures with the same arrangement of atoms. These contributing structures are called resonance structures.
The resonance structures are hypothetical and do not represent real molecules individually. Together they contribute to a resonance hybrid structure that is more stable than any individual resonance structure. The most stable contributing structure contributes the most to the resonance hybrid.
Conditions for resonance include sp or sp2 hybridized atoms involved, overlapping parallel p-orbitals to form a conjugated system. The sigma bond framework remains the same between structures, atomic positions do not change, and electron counts are equal.
This document discusses inductive effect, which is the permanent displacement of a carbon chain's shared electron pair towards the more electronegative atom or group. It describes the negative inductive effect caused by electron-withdrawing groups and the positive inductive effect of electron-donating groups. Finally, it explains how inductive effect influences the strength of organic acids and bases, with acid strength decreasing as positive inductive effect or negative inductive effect decreases.
Infrared spectroscopy involves using infrared radiation to analyze materials. Molecules absorb specific infrared frequencies that are characteristic of their structure, such as bond vibrations and stretches. There are two main methods for infrared spectroscopy - scanning monochromator which analyzes one wavelength at a time, and Fourier transform infrared spectroscopy which uses interferometry to measure all infrared wavelengths simultaneously. Fourier transform then converts this raw interferogram data into the infrared spectrum. Infrared spectroscopy can be used to identify functional groups and molecular structures in compounds like 1-Hexene, Toluene, and Cyclohexanol based on their characteristic absorption peaks.
The anomeric effect was discovered in 1955 with the work of J.T. Edward, N.-J. Chu, and R.U. Lemieux.
Contributed by: Cody F. Bender, Charles E. Price (Undergraduates), University of Utah, 2016
Investigation of one compound effect on main neuronal properties in a native ...NEUROSERVICE
The document reports on an investigation of the effects of Compound A on neuronal properties in rat hippocampal slices. The study evaluated the effects of Compound A on input/output properties, paired-pulse facilitation, basal synaptic transmission, long-term potentiation, long-term depression, and paired-pulse inhibition. The results showed that Compound A slightly decreased basal synaptic transmission but did not modify other properties like paired-pulse facilitation or long-term potentiation and depression. The conclusion is that Compound A does not significantly affect the main neuronal properties evaluated in the study.
Steric Effects on the Configuration of the Nitrogen In PiperidineTruongan Nguyen
The document discusses steric effects on the configuration of nitrogen in piperidine. Specifically, it summarizes that:
1) The nitrogen proton in piperidine prefers the axial conformation due to an attractive interaction between the NH and CH groups, rather than solely repulsive steric interactions.
2) Piperidine exists as two conformational isomers in equilibrium.
3) NMR spectroscopy can be used to measure the conformation of the nitrogen proton, with axial protons giving larger coupling constants.
Optically active compounds and their effect on and importance in biological s...Sabrina Lee
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive function. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
B.tech. ii engineering chemistry unit 4 B organic chemistryRai University
Organic reactions and their mechanisms are described. Key topics covered include nucleophiles and electrophiles, reaction types (addition, elimination, substitution), and organic intermediates. Electron displacement effects such as inductive, mesomeric, electromeric and inductometric effects are also discussed. Common organic reactions like nitration, halogenation and nucleophilic aromatic substitution are summarized.
This document contains 60 questions related to organic chemistry concepts like alcohols, phenols, ethers, aldehydes, ketones, carboxylic acids, amines, etc. The questions cover topics like relative acidities, reactivities, mechanisms of reactions, effect of substituents, physical properties and their relationship to molecular structure. Answers provided explain the concepts in brief.
Hydrogen bonding occurs between polar molecules where a hydrogen atom is bonded to a highly electronegative atom like oxygen or nitrogen. This partial positive charge on the hydrogen allows it to form an attractive force with another partially negatively charged atom. Water exhibits strong hydrogen bonding between its molecules, giving rise to properties like its high boiling point. Ethanol also exhibits hydrogen bonding between its -OH groups, allowing it to have a higher boiling point than similar sized molecules without this bonding, like methoxymethane. This hydrogen bonding also allows ethanol to be soluble in water whereas non-polar molecules cannot disrupt the water's hydrogen bonding network.
This document discusses aromatic compounds and Hückel's rule for aromaticity. It defines aromatic compounds as cyclic, planar and fully conjugated compounds that have 4n + 2 π electrons according to Hückel's rule. These compounds are highly stable due to delocalization of π electrons over the whole ring. They undergo substitution rather than addition reactions and have intermediate bond lengths and diatropic NMR properties. Anti-aromatic compounds have 4n π electrons and show the opposite NMR characteristics. Molecular orbital theory is used to explain the stability and properties of aromatic compounds.
This document discusses the concept of resonance in organic chemistry. Resonance describes when the bonding in a molecule cannot be accurately represented by a single Lewis structure, and instead requires multiple structures that depict the delocalized electrons. Ozone is provided as an example where two resonance structures are needed to represent its true structure with equal bond lengths and partial charges on the outer oxygens. Benzene is also described as having two resonance structures, and its hexagonal structure with a circle inside represents the delocalized pi electrons in the ring.
Organic compounds can exist as isomers - compounds with the same molecular formula but different structural formulas or spatial arrangements. There are two main types of isomerism: structural isomerism and stereoisomerism. Structural isomerism includes six sub-types based on differences in carbon chain structure, functional groups, or ring formations. Stereoisomerism involves two sub-types, geometric isomers which differ in spatial arrangements around double bonds, and optical isomers which are non-superimposable mirror images called enantiomers.
This document discusses various concepts in organic chemistry related to alcohols, phenols, ethers, aldehydes, ketones, carboxylic acids, amines and aromatic compounds. Some key points covered include:
1. The bond angle in alcohols is less than tetrahedral due to repulsion between oxygen's lone pairs. Branched alcohols have lower boiling points than straight-chain alcohols due to decreased intermolecular forces.
2. Phenol is a stronger acid than alcohols due to resonance stabilization of the phenoxide ion. Ethers have lower boiling points than alcohols due to the absence of hydrogen bonding.
3.
The document discusses different types of substitution reactions including nucleophilic substitution, electrophilic substitution, and free radical substitution. It provides details on the mechanisms, kinetics, stereochemistry and factors affecting the rate of nucleophilic substitution reactions SN1 and SN2. SN1 follows a unimolecular mechanism involving a carbocation intermediate while SN2 follows a bimolecular mechanism with a single concerted transition state. The document also discusses electrophilic aromatic substitution reactions and addition and elimination reactions of alkenes and alkynes.
The document discusses the concept of resonance through examples such as bridges and mechanical systems. It explains that resonance occurs when an object vibrates at greater amplitudes due to another source emitting its natural frequency. Specifically, it discusses how the Tacoma Narrows Bridge collapsed in 1940 due to wind-induced oscillations resonating with the structure of the bridge. It also summarizes the collapse of the Nimitz Freeway in 1989, which was caused by an earthquake matching the bridge's resonant frequency. The document provides background on concepts like kinetic energy, potential energy, amplitude, and frequency to explain the physics of resonance.
1. Hydrogen bonding occurs between hydrogen atoms attached to electronegative atoms like oxygen, fluorine, and nitrogen of one molecule and an electronegative atom of another molecule.
2. Water is able to form extensive hydrogen bonding networks between molecules due to each water molecule having two hydrogen atoms and two lone pairs of electrons on the oxygen atom.
3. The hydrogen bonding network in liquid water is responsible for its unique properties, while hydrogen bonding in ice forms its crystalline lattice structure.
This document discusses conjugation, hyperconjugation, and cross-conjugation. Conjugation involves the overlap of p-orbitals across sigma bonds, resulting in alternating single and multiple bonds that increase stability. Hyperconjugation stabilizes molecules through interactions between sigma bonds and empty or partially filled orbitals. It increases stability in carbocations, radicals, and alkenes. Cross-conjugation involves the exclusion of one pi bond from conjugative interactions. Hyperconjugation disperses charge and stabilizes molecules. More substituted systems experience greater hyperconjugation and stability.
This document summarizes different types of electron displacement effects including permanent polarization effects like inductive effect, mesomeric effect, and hyperconjugation, as well as temporary polarization effects like electromeric effect. It describes the inductive effect as the displacement of electron density in a covalent bond towards the more electronegative atom. The mesomeric effect involves resonance stabilization of molecules through pi electron delocalization. Hyperconjugation refers to sigma electron delocalization between C-H bonds and adjacent pi systems. The electromeric effect temporarily polarizes multiple bonds during reaction with electrophiles.
This document discusses various types of electron displacement effects that can occur in covalent bonds, including permanent polarization effects like inductive effect, mesomeric effect, and hyperconjugation, as well as temporary polarization like electromeric effect. It provides examples and explanations of each type of effect, such as how inductive effect involves the displacement of electrons towards the more electronegative atom in a bond. It also discusses applications of these effects, such as explaining relative stabilities of carbocations and carbanions.
This document discusses various types of organic reaction intermediates. It explains that reaction intermediates are transient chemical species that are formed in one step of a reaction mechanism and consumed in a subsequent step. Common types of intermediates discussed include radicals, carbocations, and carbanions. The document compares the stability of primary, secondary, and tertiary carbocations and carbanions based on factors like inductive effects, hybridization, and resonance. It also provides examples and structures of different organic reaction intermediates.
Isotopes are two atoms of the same element that have the same number of protons but different numbers of neutrons. Isotopes are specified by the mass number.
Chemical Bonding
Ionic bonds form when electrons are transferred from a metal to a nonmetal, creating oppositely charged ions. Covalent bonds form when atoms share electrons. Ionic bonds are generally stronger than covalent bonds. The strength of an ionic bond depends on the charge and size of the ions - higher charges and smaller sizes result in stronger bonds. Ionic solids form crystalline structures with repeating patterns of ions. Lattice energy is required to separate ions in an ionic solid into gaseous ions.
1. Organic reaction mechanisms involve the reaction of a substrate with a reagent, forming intermediates and ultimately products.
2. Bond cleavage can occur through either a heterolytic or homolytic process. Heterolytic cleavage leads to the formation of ions while homolytic cleavage leads to free radicals.
3. Electrophiles are electron seeking species that attack nucleophilic centers, while nucleophiles are electron pairing species that attack electrophilic centers. Common electrophiles include carbocations and carbonyl groups, while common nucleophiles include carbanions.
This document discusses structural theory in organic chemistry. It covers topics like bond fission and its types (homolysis and heterolysis), organic reagents (electrophiles, nucleophiles, free radicals), types of organic reactions (substitution, elimination, addition, rearrangement), inductive effect and its applications, and mesomeric effect and its applications. Examples are provided to illustrate key concepts. Essay and short answer questions are also included at the end to test understanding of topics covered.
Introduction to Foundation of Chemistry 1M.T.H Group
This document provides an introduction to foundational concepts in organic chemistry. It begins with learning outcomes focusing on orbitals, bonding structures, and the periodic table. It then reviews electron configuration, atomic structure including shells and subshells. The document discusses hybridization and molecular shapes for sp, sp2, and sp3 including examples. It introduces ionic and covalent bonding, and how atoms bond to attain stable electron configurations. Key concepts are defined such as line angle formulas, Hund's rule, and octet rule. Exercises are provided to identify bonding types and draw Lewis structures.
1) Alkenes are hydrocarbons containing a carbon-carbon double bond. They include many naturally occurring compounds like flavors and fragrances.
2) This chapter focuses on the general reaction of alkenes, which is electrophilic addition. It examines the consequences of alkene stereoisomerism and how double bonds are present in most organic molecules.
3) Electrophilic addition of alkenes involves the attack of an electrophile like HBr on the pi bond, forming a carbocation intermediate that then reacts with the bromide ion. This two-step process allows preparations using HCl or HI as well.
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2. Hyperconjugation: Definitions
1. J. Chem. Soc., 1935, 1844-1847.
Hyperconjugation is the donation of a sigma bond into an adjacent empty or
partially filled p orbital, which results in an increased stability of the molecule.
Hyperconjugation contributes to the resonance stabilization
of this tertiary carbocation, where electrons from the C-H
sigma bonding orbital are donated to the empty p orbital of
the cation.
Hyperconjugation was first described by Baker and Nathan in 1935 to describe the
“abnormal behavior” of alkyl-substituted compounds.1
3. Trends in Hyperconjugation
1. Less electronegative atoms make for better sigma bond
donors. This is because more electronegative atoms have
lower lying HOMOs, which have poor overlap with the LUMO
of the electron acceptor.
>
In other words, less electronegative atoms are more willing to share there
electrons with the carbocation. Therefore, the 2-methyl butane is more
stabilized through hyperconjugation than the 3-fluoro 2-methyl butane.
4. Trends in Hyperconjugation
3. The greater the number of substituents on a carbocation, the
more stabilized it will be through hyperconjugation.
2. Lower lying LUMOs make for better electron acceptors, as there is better
orbital overlap with the HOMO of the electron donor.
> > >Atomic orbital sp π* sp2 π*
sp3 π*
> >
Therefore, tertiary carbocations are more stable than secondary or primary.
5. Other types of Hyperconjugation
Occasionally, electron density will be donated from a filled 𝜋 or p orbital into
an adjacent σ* orbital. This is known as negative hyperconjugation.
Other times, electron density will be donated from a p orbital into an adjacent
𝜋* orbital; the result is an overall neutral charge on the molecule. This is
known as neutral hyperconjugation.
6. Consequences of Hyperconjugation
2. Chem. Phys. Lett., 1981, 84, 267.
1. Conformational Preferences of Esters
(E) Conformer
(Z) Conformer
ΔG=+4.8 kcal/mol
Esters exist in two
conformers, E and Z.
(E) Conformer (Z) Conformer
Because the Z conformation
allows for the overlap of the
lone pair with the C—O σ* it
is favored over the E
conformation, where the
lone pair is aligned with the
C—R σ*.2
No resonance, poor orbital overlap!
7. Consequences of Hyperconjugation
J. Chem. Phys., 1951, 19, 342.
2. The Secondary Kinetic Isotope Effect
The kinetic isotope effect (KIE) is the change in rate of a reaction when an atom is replaced with a heavier
isotope. A secondary KIE is when the isotope substitution occurs at an atom where a bond is not being broken
or formed.
Because heavier atoms form stronger bonds, they are less willing to contribute to hyperconjugation. Therefore,
reactions that require the elimination of a leaving group proceed more slowly.
For example:
*Note: TsO, or tosylate, is a leaving group.
1.
2.
Due to the weaker C—H bond, Reaction 1 proceeds faster than
Reaction 2. This is because the C—H σ bond is more willing to push
electrons into the empty orbital of the carbocation and contribute to
hyperconjugation.
KH/KD is the ratio of the rates of the individual reactions. A KH/KD >1
suggests that the reaction occurs more slowly with the isotopic
substitution.
KH/KD = 1.15, as found by Streitwieser, et al.3
8. Problems
1. Rank the ability of the following bonds to contribute to hyperconjugation: C—F, C—O, C—N, C—H.
A. C—F > C—O > C—N > C—H
B. C—H > C—N > C—O > C—F
C. C—H > C—O > C—N > C—F
D. C—F > C—H > C—N > C—O
2. The following molecule will not experience hyperconjugation. Why is that?
A. The hybridization of the molecule does not permit proper orbital overlap.
B. The deuterium does not contribute hyperconjugation very well.
C. There is poor overlap between the LUMO of the N—Me bond and HOMO of the N—D bond.
D. Hyperconjugation does not occur on heteroatoms such as nitrogen.
3. Which of the following most readily ionizes?
A. B. C. D.
4. Identify whether the following molecules have positive, negative, or neutral hyperconjugation.
i.
A. Positive
B. Negative
C. Neutral
ii.
A. Positive
B. Negative
C. Neutral
A. Positive
B. Negative
C. Neutral
iii.
10. This work is licensed under a
Creative Commons Attribution-
ShareAlike 4.0 International
License.
Contributed by:
Samuel Redstone (Undergraduate)
University of Utah, 2016