Writing molecular formula for alcohols and carboxylic acids
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This document discusses how to write molecular formulas for alcohols and carboxylic acids. It provides the general formulas, examples for propanol and butanol, and practice problems for writing formulas for butanol, hexanol, butanoic acid and propanoic acid.
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Carbonyl compounds contain a carbon=oxygen double bond. They are divided into two types: aldehydes and ketones. Both have the general formula CnH2nO. Carbonyl compounds can be prepared through oxidation of alcohols, dehydrogenation of alcohols, distillation of carboxylate salts, decarboxylation/dehydration of carboxylic acids, hydrolysis of geminal dihalides, ozonolysis of alkenes, and through processes like the oxo and Wacker processes that start with alkenes.
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This document provides answers to questions about organic chemistry concepts related to carboxylic acids and their derivatives. Key points covered include:
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This document discusses carbon, hydrogen, oxygen and organic compounds. It states that carbon, hydrogen and oxygen are common elements that form compounds by chemically bonding together. Carbon forms many compounds that are essential to life, such as those found in living things like diamond, graphite, chalk, coal and wood. Organic compounds specifically contain carbon and hydrogen, and sometimes other elements. There are over 10 million known organic compounds, and thousands more are created each year. Organic chemistry studies the structure, properties and reactions of carbon-containing compounds.
Alcohol and carboxylic acid
1) Alcohols and carboxylic acids are organic compounds that contain functional groups (-OH for alcohols, -COOH for carboxylic acids).
2) Alcohols include methanol, ethanol, and are named based on the carbon chain with the suffix -ol. They undergo combustion, oxidation, and reactions with sodium and carboxylic acids.
3) Carboxylic acids have the general formula R-COOH and are named by identifying the parent hydrocarbon chain and replacing the ending with -oic acid, like ethanoic acid. They lose hydrogen ions and dissociate in water.
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Hydrocarbons1_grade_9_science lesson_detailed
This document provides an overview of carbon and organic compounds containing carbon. It discusses that carbon is tetravalent and can form single, double, and triple bonds with other elements like hydrogen, oxygen, nitrogen and others. Organic chemistry is the study of carbon compounds, which includes hydrocarbons that contain only carbon and hydrogen. Hydrocarbons are classified as aliphatic or aromatic, with aliphatic hydrocarbons further divided into saturated and unsaturated types like alkanes, alkenes, and alkynes. Alkanes are saturated and have the general formula CnH2n+2. Alkenes contain carbon-carbon double bonds and have the formula CnH2n. Alkynes have a
images_organic_1st_year__2014.pdf
This document discusses carbon and its importance in living things. Carbon is uniquely able to form long chains and complex molecules through strong covalent bonds between carbon atoms. While not the most abundant element in living things, carbon is essential as the backbone of organic compounds. The chemistry of living things is based on carbon, and organic chemistry studies carbon-containing molecules, whether found in living things or not. Carbon's ability to form stable chains and complex structures through bonding makes it well-suited to form the compounds that make up living things.
TOPIC 10 : ORGANIC CHEMISTRY
- Alcohols contain an -OH functional group which makes them polar and soluble in water. They can be classified as primary, secondary, or tertiary based on the number of carbon atoms bonded to the carbon attached to the OH group.
- Primary alcohols can be oxidized to aldehydes then carboxylic acids using oxidizing agents like acidified dichromate or manganate. Secondary alcohols oxidize to ketones. Tertiary alcohols do not oxidize.
- Burning alcohols releases energy with the amount increasing with the alcohol chain length due to more carbon dioxide produced. In limited oxygen, carbon monoxide is formed instead of carbon
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ALKANES.ppt hydrocarbons most commonly found in nature
ALKANES.ppt hydrocarbons most commonly found in nature
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Alkanes and their reactions
Alkanes are saturated hydrocarbons that contain only carbon-carbon single bonds. They have the general formula CnH2n+2 and include common fuels like methane, ethane, propane and butane. Alkanes are nonpolar and insoluble in water, making them float on surfaces. While generally nonreactive, alkanes readily undergo combustion reactions, releasing energy. Incomplete combustion produces hazardous byproducts like carbon monoxide. Alkanes also react through halogenation reactions where halogens replace hydrogen atoms.
Esters
Esters are compounds formed from an organic acid and alcohol. They have a distinctive fruity smell and can be natural or man-made. Natural esters include fats, oils, and aromas in fruits. Man-made esters are used in perfumes, solvents, paints, varnishes, and biodiesel. Esters have lower boiling points than acids and are more soluble in organic solvents. They are formed via the reaction of a carboxylic acid and alcohol, producing an ester and water. Esters can also be hydrolyzed back into an acid and alcohol using acid or base catalysts.
Reactions of carboxylic acids
Carboxylic acids have the general formula CnH2n+1COOH. They are weak acids that can undergo acid-base reactions with metals and metal oxides/hydroxides to form salts and water. These neutralization reactions produce metal carboxylates. Carboxylic acids also react with carbonates and hydrogen carbonates to form metal carboxylates, carbon dioxide, and water. Additionally, carboxylic acids undergo esterification reactions with alcohols where they lose a water molecule to form an ester.
Reactions of alcohols
Alcohols undergo several characteristic reactions: combustion produces carbon dioxide and water; reaction with sodium forms sodium alkoxides and hydrogen; oxidation converts alcohols like ethanol to carboxylic acids using oxidizing agents; esterification reacts alcohols and carboxylic acids to form esters and water; and dehydration removes a water molecule and forms an alkene. Ethanol specifically burns with a blue flame due to its low carbon-to-hydrogen ratio, and it oxidizes to ethanoic acid when heated with acidified potassium manganate or dichromate solutions.
Reactions of alkenes
Alkenes undergo addition reactions with halogens, hydrogen, and oxygen. When bromine is added to ethene, it produces dibromoethane by adding one bromine atom to each carbon in the double bond. Alkenes also react with hydrogen through hydrogenation, where hydrogen is added across the carbon-carbon double bond at 1500C with a nickel catalyst under pressure to produce the saturated alkane. When pentene undergoes hydrogenation, it forms pentane by adding hydrogen across the carbon-carbon double bond.
Uses of hydrocarbons
Hydrocarbons can be separated from crude oil using fractional distillation based on their different boiling points. Long chain hydrocarbons can be cracked into shorter chains through thermal or catalytic cracking. Thermal cracking uses high temperature and pressure while catalytic cracking uses lower temperature, pressure and a zeolite catalyst. Alkanes have various uses as fuels, solvents, and in biogas production where bacteria convert organic waste into methane gas. Alkenes are used to produce important polymers like polyethylene, polypropylene, and PVC.
Distinguishing between alkanes and alkenes
Alkanes and alkenes can be distinguished using bromine water and acidified potassium manganate (VII) solutions. Bromine water will remain red-brown when added to alkanes, but turns colorless rapidly when added to alkenes, indicating an addition reaction. Acidified potassium manganate (VII) solution will remain purple when added to alkanes, but is rapidly reduced to a colorless solution when added to alkenes. These tests allow alkenes to be identified based on their reactions with bromine water and acidified potassium manganate (VII) solutions.
Organic nomenclature
The document provides an overview of IUPAC nomenclature rules for naming organic compounds. It explains that organic compound names have three parts: a prefix, root, and suffix. The prefix indicates functional groups, the root name comes from the number of carbon atoms in the main chain, and the suffix denotes the type of compound. It provides examples of applying the rules to name alkanes, alkenes, alcohols, carboxylic acids, and cyclic and branched compounds.
Redox reactions at electrodes
During electrolysis, redox reactions occur where ions are reduced or oxidized at the electrodes. At the cathode, ions gain electrons through reduction reactions and at the anode, ions lose electrons through oxidation reactions. The overall reactions in electrolysis depend on the electrolyte, with common products including hydrogen, oxygen, chlorine and metals.
Redox in everyday life
Everyday activities involve many redox reactions. Metals corrode through oxidation when exposed to oxygen and moisture. Bleach removes color through redox reactions that oxidize dyes. Breathalyzer tests use the oxidation of ethanol to change a solution from orange to green. Cut fruits brown through enzymatic oxidation reactions with oxygen in the air. Respiration, combustion, photosynthesis, and photography all involve important redox reactions as well.
Distinguishing between oxidizing and reducing agents
Oxidizing agents are substances that accept electrons in redox reactions, becoming reduced. They tend to have high oxidation states and strong electron affinity. Fluorine is the strongest oxidizing agent due to its high electronegativity. Common oxidizing agents include oxygen, chlorine, and ozone.
Reducing agents are substances that donate electrons in redox reactions, becoming oxidized. Metals in the alkali group are good reducing agents as they have low ionization energies and electronegativity. Lithium is the strongest reducing agent due to its small standard reduction potential. Some substances can act as both oxidizing and reducing agents depending on the reaction.
Redox reactions using oxidation numbers
This document discusses identifying redox reactions using oxidation numbers. It provides examples of assigning oxidation numbers to determine if a reaction is redox. A redox reaction is identified when oxidation numbers change for an element. The first reaction provided is a redox reaction where bromine is oxidized and chlorine is reduced. The second reaction shown is determined to not be a redox reaction because no oxidation numbers change. Multiple choice questions are given at the end to test identifying redox reactions.
Oxidation- reduction reactions
Introduction to redox reactions
References
Tindale, Ritchie et al, 2014, Chemistry for CSEC 2nd Edition, Nelson Thornes. p156-159
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Writing molecular formula for alcohols and carboxylic acids
- 1. Writing molecular formula for Alcohols and Carboxylic Acids
- 2. Alcohols • Alcohols have the general formula CnH2n+1OH • Example: propanol ( C3H5OH) By using the general formula we know that a compound with 3C’s would have 7 hydrogens. We also know the compound’s molecular formula ends in OH
- 3. Practice • Using the general formula of alcohols, write the molecular formula of 1. Butanol-4 carbons 2. Hexanol-6 carbons
- 4. Carboxylic acids • Carboxylic acids have the general formula CnH2n+1COOH In carboxylic acids the CnH2n+1COOH accounts for one of the carbon atoms and one of the hydrogen atoms. So in writing molecular formula we must remember to deduct one carbon and Hydrogen from the root formula CnH2n+1COOH Writing the molecular formula for a carboxylic acid with 3 Carbons C2H5COOH
- 5. Practice • Using the general formula of carboxylic acids, write the molecular formula of; 1. Butanoic acid-4 carbons 2. Propanoic acid-5 carbons