Chemical properties of alcohols
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Explain chemical properties of alcohols by various chemical reactions Define and explain preparation of ethers from alcohols by using chemical equations
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Alkene
Alkenes are hydrocarbons containing at least one carbon-carbon double bond. They have lower melting and boiling points than alkanes due to weaker intermolecular forces. The number of carbons determines an alkene's name and formula. Alkenes undergo addition reactions, combustion reactions, polymerization reactions, and can be used to test for double bonds. They differ from alkanes in bonding, reactivity and ability to cause soot during combustion. Isomers are compounds with the same molecular formula but different structural formulas, resulting in different physical but same chemical properties.
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Chapter 3 ketone
Here are the answers:
a)
i) K (2-methyl-1-propanol):
CH3
|
CH3-C-CH2-CH2-OH
|
CH3
L (2-methyl-2-propanol):
CH3
|
CH3-C-CH(OH)-CH3
ii) K can be prepared by reacting propanone with methylmagnesium bromide, a Grignard reagent:
CH3COCH3 + CH3MgBr → CH3C(OCH3)(CH3) → CH3C(OH)(CH3)CH3 + MgBr
iii) M
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2) Alkenes undergo characteristic reactions such as addition of halogens, hydrogenation to form alkanes, hydration and polymerization. Many of these reactions follow Markovnikov's rule.
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This chapter discusses alkynes, carbon-carbon triple bonds. Alkynes contain two pi bonds and have the general formula CnH2n-2. They can be named using IUPAC nomenclature by changing the -ane ending of the parent alkane to -yne. Alkynes undergo addition reactions like alkenes but also have unique reactions like forming acetylide ions. They can be synthesized through elimination and by reactions of acetylide ions. Oxidation and ozonolysis reactions of alkynes cleave the triple bond.
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Here are the answers:
a)
i) K (2-methyl-1-propanol):
CH3
|
CH3-C-CH2-CH2-OH
|
CH3
L (2-methyl-2-propanol):
CH3
|
CH3-C-CH(OH)-CH3
ii) K can be prepared by reacting propanone with methylmagnesium bromide, a Grignard reagent:
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2) Alkenes undergo characteristic reactions such as addition of halogens, hydrogenation to form alkanes, hydration and polymerization. Many of these reactions follow Markovnikov's rule.
3) Alkenes are industrially important as monomers for polymers like polyethylene, polypropylene, PVC and polystyrene. Ethylene and propylene are the largest volume organic chemicals produced.
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Weak acids are acids that dissociate partially in water. The extent of dissociation is given by the equilibrium constant.
Note:
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The document discusses several topics related to chemistry:
1) The voltage needed to create an electron is about one million volts, the same voltage as lightning. This high voltage accelerates electrons from the sky to the ground.
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The document summarizes key information about carboxylic acids from their general formula of RCOOH to their characteristic properties and reactions. It discusses (1) the nomenclature and structures of carboxylic acids, (2) their higher boiling points and water solubility compared to similar molecules due to hydrogen bonding, (3) their acidity stemming from ionization of the carboxyl group, and (4) several important reactions including preparation by oxidation, esterification, and formation of derivatives like acid chlorides, anhydrides, salts, and amides.
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Esters have the general formula RCOOR'. They are formed by the reaction of carboxylic acids with alcohols, which is called esterification. Esters can also be prepared from acyl chlorides or acid anhydrides. Esters undergo various reactions including hydrolysis, aminolysis, reactions with Grignard reagents, and transesterification. Hydrolysis converts esters back into carboxylic acids and alcohols. Transesterification involves exchanging one alkoxy group in an ester for another.
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Strong weak acids and bases
Acids are divided into two categories based on the ease with which they can donate protons to the solvent: i) strong acids and ii) weak acids
Strong acids are acids that completely dissociate in water. The reaction of an acid with its solvent (typically H2O) is called an acid dissociation reaction.
Weak acids are acids that dissociate partially in water. The extent of dissociation is given by the equilibrium constant.
Note:
A measure of the relative strength of an acid is: i) the equilibrium constant ka of the dissociation reaction of the acid in water (depends on temperature) ii) the degree of dissociation α of the acid in water (depends on the concentration of the acid an on temperature).
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Ethers are named based on the groups bonded to oxygen, with the common system naming the two groups followed by "ether". The IUPAC system names the larger alkyl group as a suffix and the smaller group with oxygen as a prefix like "methoxy". Ethers can be prepared through Williamson's synthesis using alcohols and alkyl halides, by reacting alkyl halides with silver oxide, or by dehydrating two alcohols with sulfuric acid. Ethers are colorless, inflammable compounds that are good solvents and lighter than water. They react with acids like HI and HBr, with HI cleaving the ether bond to form an alcohol and alkyl iodide.
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This document discusses relative atomic mass and relative molecular mass. It provides examples to calculate these values.
The key points are:
1. Relative atomic mass (Ar) is the average mass of a single atom of an element compared to 1/12 the mass of one carbon-12 atom.
2. The relative molecular mass (Mr) of a molecule is the sum of the relative atomic masses of all the atoms in the molecule.
3. Examples are provided to calculate relative atomic masses and relative molecular masses using atomic mass values and molecular formulas. Formulas, atomic masses, and molecular masses are compared to calculate unknown values.
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Alkanes are saturated hydrocarbons whose general formula is CnH2n+2. Their names are derived from their molecular formula. Structural formulas show how atoms are bonded. Physical properties of alkanes include being soluble in organic solvents but not water, and existing as gases at low carbon numbers and liquids or solids at higher numbers. Melting and boiling points increase with more carbon atoms as intermolecular forces strengthen. Alkanes undergo combustion and halogenation reactions. Complete combustion produces CO2 and H2O while incomplete produces CO and H2O. Halogenation is a substitution reaction that occurs in sunlight, breaking C-H bonds and forming C-X bonds to produce chlorometh
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Learning Objectives
1. Know that Carboxylic acids contain the functional group -COOH
2. Understand how to draw structural and displayed formulae for Carboxylic Acids
3. 3. Predict physical properties of Carboxylic Acids
Alkenes ppt slides
Alkenes readily undergo addition reactions where carbon-carbon double bonds become single bonds. Common addition reactions include bromination, hydrogenation, and combustion. Alkenes are manufactured through cracking of petroleum, which involves breaking down long-chain hydrocarbons into smaller molecules like alkenes over a catalyst at high temperatures. Cracking provides important products for fuels and materials.
Tang 01d bond energy
This document discusses bond energy and how it relates to chemical reactions. It states that bond breaking is endothermic while bond formation is exothermic. Bond energies can be used to calculate the change in enthalpy (ΔH°) of a reaction. A table of average bond energies is provided. Examples are given showing how to use bond energies to calculate ΔH° for different reactions, recognizing that bond energies may vary depending on neighboring bonds. Bond dissociation energy is also introduced as another measure of bond strength.
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Carboxylic acids have the general formula R-COOH. They can be synthesized through oxidation of alcohols and arenes, carbonation of Grignard reagents, and hydrolysis of nitriles. As acids, they ionize in water and react with bases. They can be converted to functional derivatives like acid chlorides, esters, and amides. They undergo reactions such as reduction, alpha-halogenation, and electrophilic aromatic substitution. Spectroscopically, they show a C=O stretch around 1700 cm-1 and a COOH proton around 12 ppm.
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II. It describes isomerism including chain isomerism, position isomerism, and geometric isomerism that can occur when compounds have the same molecular formula. It also discusses stereoisomerism including enantiomers and diastereomers.
III. Reaction pathways are outlined for functional group interconversions including oxidation, reduction, hydration, halogenation, and saponification. Tests for identifying organic compound classes are also referenced.
F.Sc.Part.2 Ch.08 Exercise Solved by Malik Xufyan
Three alkenes can be hydrogenated to form 2-methylbutane. The three alkenes are: 3-methyl-1-butene, 2-methyl-2-butene, and 2-methyl-1-butene. Ethane can be converted to ethene, which can then be converted to ethyne and back to ethane through a series of reactions involving halogenation, hydrolysis, and hydrogenation. Starting from ethyne, many compounds can be synthesized including acetaldehyde, benzene, chloroprene, glyoxal, oxalic acid, acrylonitrile, ethane, and acetonitrile.
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This document discusses alcohols, including their structure, nomenclature, classification, physical properties, acidity and basicity, and methods of preparation. Key points covered include that alcohols contain an -OH functional group, can be classified as primary, secondary or tertiary based on carbon atom bonding, associate through hydrogen bonding affecting physical properties, and can be prepared through fermentation, hydration of alkenes, nucleophilic substitution, and reduction of carbonyl compounds.
Chapter 11 carbon compound
1. The document discusses various topics related to carbon compounds including hydrocarbons, alkenes, isomers, homologous series, functional groups, and reactions such as fermentation, oxidation, esterification, and dehydration of alcohols.
2. An experiment is described to prepare the ester ethyl ethanoate from ethanol and ethanoic acid using concentrated sulfuric acid. Upon mixing and warming the reactants, a sweet smell is observed and an insoluble product forms in water.
3. Differences between alkanes and alkenes are compared, including molecular structure, physical properties, reactivity, and chemical tests. Alkenes contain carbon-carbon double bonds and
Alcohols.ppt
Alcohols can undergo several chemical reactions:
1) They act as both acids and bases due to the hydroxyl group and can form alkoxides or accept protons.
2) The hydroxyl group can be replaced by halides using reagents like phosphorus pentachloride or thionyl chloride.
3) Alcohols can undergo esterification when reacted with carboxylic acids to form esters.
oc-ch7 Aldehyde and ketone.ppt
Procedure for test of aldehydes and ketones:
Dissolve the given organic compound in ethanol.
To this solution, add an alcoholic solution of 2,4-dinitrophenyl hydrazine.
Shake the mixture well.
If there is a formation of yellow to orange precipitate then the given compound is an aldehyde or ketone.
Synthesis via enolates
Enolates are formed as intermediaes in reactions of active methylene compounds with aldehydes or ketones
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Chemical properties of alcohols
- 1. Chemical Properties of Alcohols D.M S.H. K.M
- 2. Contents Introduction: Learning Objectives Alcohols' Combustion Alcohols' Dehydration Alcohols' Oxidation Preparation of Ethers 2 Examples and Questions
- 3. Introduction: Learning Objectives 2. Define and explain preparation of ethers from alcohols by using chemical equations 1. Explain chemical properties of alcohols by various chemical reactions
- 4. Alcohols' Combustion Reactions Combustion What is Combustion?
- 5. Example and Questions Let's Practice and Revise! ___ C3H7OH + ___ O2 → ___ CO2 + ___ H2O Propanol: C3H7OH or C3H8O reactants products C C H H O O = a d c b Coefficients: a = b = c = d =
- 6. Alcohols' Combustion Reactions 2C3H7OH + 9O2 6CO2 + 8H2O Tips for Balancing: 1) If number of H atoms in alcohol molecule completely divide to 4, so the coefficient of alcohol molecule should be 2. Then start equalizing number of C, H, then O atoms. 2) If number of H atoms in alcohol molecule do not divide to 4, so the coefficient of alcohol molecule should be 1. Then start equalizing number of C, H, then O atoms.
- 7. Alcohols' Combustion Reactions 4. ___ C7H16O + ___ O2 → ___ CO2 + ___ H2O 3. ___ C6H13OH + ___ O2 → ___ CO2 + ___ H2O 1. ___ C4H9OH + ___ O2 → ___ CO2 + ___ H2O 2. ___ C5H11OH + ___ O2 → ___ CO2 + ___ H2O 5. ___ C8H18O + ___ O2 → ___ CO2 + ___ H2O 6. ___ C9H20O + ___ O2 → ___ CO2 + ___ H2O Balance the combustion reaction of an alcohol:
- 8. Alcohols' Dehydration Conditions: t > 140 °C → ALKENE t < 140 °C → ETHER
- 9. Alcohols' Dehydration Dehydration of Primary alcohols: CH3 – CH2 – CH(CH3) – CH2OH CH3 – CH2 – C(CH3) = CH2 +H2O 2-methylbutan-1-ol 2-methylbut-1-ene 2 CH3 – CH2OH CH3 – CH2 – O – CH2 - CH3 + H2O t < 140 °C ethanol diethylether CH3 – CH2OH CH2 = CH2 + H2O t > 140 °C ethanol ethene Preparation of Ethers Preparation of Alkenes
- 11. Alcohols' Dehydration Dehydration of Secondary alcohols: CH3 – CHOH – CH2 – CH3 CH3 - CH = CH – CH3 + H2O butan-2-ol but-2-ene
- 13. Preparation of Ethers What were the ethers? General Formula? Functional Group? CH3CH2OH + HOCH2CH3 → CH3CH2OCH2CH3 + H2O Preparation of Ethers from Alcohols:
- 16. Examples and Questions Let’s practice: CH3-CH2-OH CH3-CH(CH3)-CH2OH CH3-CH2-CH2-OH CH3-CH(OH)-CH3 CH3-CH2-CH(OH)-CH(CH3)-CH3
- 17. Examples and Questions – HomeWork 5. 6. 7.