Grade 9
  1. Matter and its nature  1.1. Introduction to matter  1.2. Physical and chemical properties of matter  1.3. States of matter  1.3.1. Solid state  1.3.2. Fluid state  1.3.3. Gaseous state  1.3.4. Plasma and Bose–Einstein condensate  1.4. Changes in the states of matter  1.4.1. Melting and freezing  1.4.2. Evaporation and Condensation  1.4.3. Sublimation and deposition  1.5. Classification of matter  1.6. Elements, Compounds, and Mixtures  1.7. Pure substances and impurities  1.8. Separation Techniques  1.8.1. Filtration  1.8.2. Distillation  1.8.3. Crystallization  1.8.4. Chromatography  1.8.5. Centrifugation  1.8.6. Sublimation  1.8.7. Decantation and sedimentation
  2. Atomic Structure  2.1. Discovery of atoms  2.2. Dalton's atomic theory  2.3. Structure of the atom  2.4. Subatomic particles  2.5. Atomic number and mass number  2.6. Isotopes and Isobars  2.7. Electronic configuration  2.8. Bohr's atomic model  2.9. Modern Atomic Model (Quantum Mechanical Model - Introduction)  2.10. Valency and chemical bonding
  3. C hemical reactions and equations  3.1. Introduction to Chemical Reactions  3.2. Chemical Equation Formulation  3.3. Balancing Chemical Equations  3.4. Types of Chemical Reactions  3.4.1. Combination Reactions  3.4.2. Decomposition reactions  3.4.3. Displacement reactions  3.4.4. Double displacement reactions  3.4.5. Redox reactions  3.4.6. Endothermic and Exothermic Reactions  3.5. Effects of chemical reactions  3.6. Energy Changes in Chemical Reactions  3.7. Catalysts and their role in reactions
  4. Periodic table and periodicity  4.1. History of Periodic Classification  4.2. Mendeleev's periodic table  4.3. Modern Periodic Table  4.4. Periods and groups in the periodic table and periodicity  4.5. Trends in the Periodic Table  4.5.1. Atomic size  4.5.2. Ionization Energy  4.5.3. Electron affinity  4.5.4. Electronegativity  4.5.5. Metallic and Non-Metallic Properties  4.6. Noble gases and their properties
  5. Chemical bond  5.1. Introduction to Chemical Bonding  5.2. Types of chemical bonds  5.2.1. Ionic bond  5.2.2. Covalent bond  5.2.3. Metallic bond  5.2.4. Hydrogen bonding  5.2.5. Van der Waals force  5.3. Properties of Ionic and Covalent Compounds  5.4. Molecular Structure and Geometry (VSEPR Theory - Basics)
  6. Acids, Bases and Salts  6.1. Introduction to Acids and Bases  6.2. Properties of Acids  6.3. Properties of bases  6.4. pH scale and its importance  6.5. Indicators and their uses  6.6. Neutralization reactions  6.7. Strength of Acids and Bases (Strong vs. Weak)  6.8. Preparation of salts  6.9. Uses of acids, bases and salts in daily life
  7. Metals and Nonmetals  7.1. Physical Properties of Metals  7.2. Physical Properties of Nonmetals  7.3. Chemical properties of metals  7.4. Chemical Properties of Nonmetals  7.5. Reactivity Series of Metals  7.6. Extraction of metals  7.7. Corrosion and its prevention  7.8. uses of metals and nonmetals
  8. Carbon and its compounds  8.1. Introduction to Carbon  8.2. Allotropes of carbon (diamond, graphite, fullerene)  8.3. Hydrocarbons  8.3.1. Hydrocarbons  8.3.2. Alkene  8.3.3. Alkynes  8.4. Functional groups in organic chemistry  8.5. Isomerism in organic compounds  8.6. Alcohols and Carboxylic Acids  8.7. Soaps and detergents  8.8. Polymers (Introduction to Natural and Synthetic Polymers)
  9. Solutions and Mixtures  9.1. Types of mixtures  9.2. Homogeneous and Heterogeneous Mixtures  9.3. Concentration of solutions  9.4. Solubility and factors affecting solubility  9.5. Suspensions and Colloids  9.6. Saturated, unsaturated and supersaturated solutions
  10. Air and atmosphere  10.1. Composition of air  10.2. Role of gases in the atmosphere  10.4. Acid rain and its effects  10.5. Greenhouse effect and global warming  10.6. Ozone layer and its depletion  10.7. Air pollution control measures
  11. Water and its importance  11.1. Composition and properties of water  11.2. Hardness of water (temporary and permanent hardness)  11.3. Causes of water pollution  11.4. Effects of Water Pollution  11.5. Water purification methods (filtration, boiling, chlorination)
  12. Industrial Chemistry  12.1. Introduction to Industrial Chemistry  12.2. Important industrial chemicals (sulfuric acid, ammonia, sodium hydroxide)  12.3. Chemical processes in industry  12.4. Uses of Industrial Chemistry in Daily Life  12.5. Environmental impact of industrial chemical processes

Grade 9 → Carbon and its compounds ↓


Alcohols and Carboxylic Acids


Carbon and its compounds have a very important place in the world of chemistry. Two important classes of organic compounds derived from carbon are alcohols and carboxylic acids. These compounds play important roles in both nature and industry. In this explainer, we will delve into the fascinating world of alcohols and carboxylic acids, along with their properties, uses, and more.

Alcohol

Alcohols are a class of organic compounds characterized by the presence of one or more hydroxyl (-OH) groups attached to a carbon atom. The general formula for alcohols is C n H 2n+1 OH, where n is the number of carbon atoms.

A visual example of an alcohol molecule would be:


    
    
    
    
    
    
    H
    
    
    C
    
    
    C

    
    C

    
    Hey
    
    
    H


This is a simplified model of the butanol molecule which is an alcohol.

Naming of alcohols

The name of an alcohol is derived from the name of the corresponding alkane (base hydrocarbon). The ending -e in the name of the alkane is replaced with -ol. For example, if the alkane is methane, the corresponding alcohol is methanol.

  • methanol ( CH 3 OH )
  • Ethanol ( C 2 H 5 OH)
  • Propanol ( C 3 H 7 OH )
  • Butanol ( C 4 H 9 OH )

Properties of alcohol

Alcohols have unique properties that make them versatile for a variety of applications:

1. Physical properties

Alcohols are known for their ability to form hydrogen bonds due to the hydroxyl group. This causes alcohols to have higher boiling points than their corresponding alkanes. They are also soluble in water, and the solubility decreases as the length of the carbon chain increases.

2. Chemical properties

Alcohol undergoes several chemical reactions such as:

  • Combustion: Alcohols burn in air to release carbon dioxide and water.
  • Oxidation: Alcohols can be converted into aldehydes, ketones, or carboxylic acids depending on their structural positions.
  • Esterification: Alcohols react with carboxylic acids to form esters, this reaction is called esterification.

Uses of alcohol

Alcohol is widely used in everyday life and in industrial processes:

  • Methanol: It is used in the manufacture of formaldehyde and as a solvent.
  • Ethanol: It is widely used in alcoholic beverages and as a biofuel.
  • Isopropanol: Commonly used in disinfectants and hand sanitizers.

Carboxylic acid

Carboxylic acids are organic compounds that contain a carboxyl group ( -COOH ). The general formula for a carboxylic acid is R-COOH, where R represents a hydrocarbon chain.

Here's a basic diagram of a carboxylic acid:


    
    
    
    
    
    
    
    R
    
    
    C
    
    
    Hey

    
    Hey

    
    H


The above picture is the symbol of carboxyl group present in carboxylic acid.

Nomenclature of carboxylic acids

Carboxylic acids are named based on the longest carbon chain containing the carboxyl group. The suffix -oic acid is used. Examples include:

  • Formic acid ( HCOOH )
  • Acetic acid ( CH 3 COOH )
  • Propionic acid ( C 2 H 5 COOH )
  • Butanoic acid ( C 3 H 7 COOH )

Properties of carboxylic acids

Carboxylic acids are known for their unique properties, which are listed below:

1. Physical properties

Carboxylic acids have higher boiling points than alcohols, ketones, or ethers of similar molecular weight. This is due to strong hydrogen bonding between the acid molecules. They are generally soluble in water, although solubility decreases as the length of the carbon chain increases.

2. Chemical properties

Some of the major chemical reactions involving carboxylic acids are:

  • Acidic nature: They release hydrogen ions ( H + ) in aqueous solution, making them acidic.
  • Esterification: Carboxylic acids react with alcohols in the presence of an acid catalyst to form esters.
  • Saponification: It is the alkali-catalyzed hydrolysis of an ester to form an alcohol and a carboxylate salt.

Uses of carboxylic acid

Carboxylic acids have diverse uses in industries and everyday life:

  • Acetic acid: It is used in the production of vinegar, synthetic fibres and plastics.
  • Formic acid: Used in leather production and as a preservative.
  • Citric acid: A common substance used to add a sour taste to foods and beverages.

Conclusion

The study of alcohols and carboxylic acids opens up a world of interesting chemical behavior and practical applications. Understanding these compounds equips us with the knowledge to harness their properties for innovative uses in industry, medicine, and daily life. From simple alcoholic beverages to complex pharmaceuticals, the importance of alcohols and carboxylic acids in our world is clearly profound.

As you learn about more organic compounds, remember that the carbon atom plays a central role in forming the vast array of molecules that make up our universe. Whether through their basic chemical properties or through their important applications, alcohols and carboxylic acids are as versatile and essential as nature itself.


Grade 9 → 8.6


U
username
0%
completed in Grade 9

← Prev (8.5)
Isomerism in organic compounds
Next (8.7) →
Soaps and detergents

Comments 



Alcohols and Carboxylic Acids

https://www.chemistryelite.com/g9/8.6?ceal=en