Grade 7
  1. Introduction to Chemistry  1.1. What is Chemistry?  1.2. Importance of chemistry in daily life  1.3. Branches of chemistry  1.4. Scientific Method in Chemistry  1.5. Laboratory Safety Rules and Precautions  1.6. Common Laboratory Equipment and Their Uses  1.7. Units of measurement in chemistry
  2. Matter and its properties  2.1. Definition of Matter  2.2. Classification of matter  2.3. Properties of matter  2.3.1. Physical properties  2.3.2. Chemical properties  2.4. States of matter  2.4.1. Solid state  2.4.2. Fluid state  2.4.3. Gaseous state  2.4.4. Plasma and Bose–Einstein condensates  2.5. Changes in the states of matter  2.5.1. Melting and freezing  2.5.2. Evaporation and Condensation  2.5.3. Sublimation and deposition  2.6. Density and its applications  2.7. Diffusion and its importance
  3. Elements, Compounds, and Mixtures  3.1. Definition of the element  3.2. Classification of elements  3.3. Metals, Nonmetals and Metalloids  3.4. Noble gases and their properties  3.5. Introduction to the Periodic Table  3.6. Definition of Compound  3.7. Properties of Compounds  3.8. Introduction to Chemical Formulas  3.9. Definition of Mixture  3.10. Types of mixtures  3.10.1. Homogeneous mixture  3.10.2. Heterogeneous mixtures  3.11. Difference Between Compounds and Mixtures  3.12. Solutions, Colloids and Suspensions
  4. Separation of mixtures  4.1. Need for separation of mixtures  4.2. Separation methods  4.2.1. Filtration  4.2.2. Sedimentation and decantation  4.2.3. Evaporation  4.2.4. Crystallization  4.2.5. Distillation  4.2.6. Chromatography  4.2.7. Magnetic Separation  4.2.8. Centrifugation
  5. Atomic Structure  5.1. Introduction to Atoms  5.2. Structure of the atom  5.2.1. Nucleus and electron cloud  5.3. Subatomic particles  5.3.1. Proton  5.3.2. Neutron  5.3.3. Electrons  5.4. Atomic number and mass number  5.5. Isotopes and their uses  5.6. Ions and ion formation
  6. Periodic table  6.1. Introduction to the Periodic Table  6.2. Groups and periods  6.3. Trends in the Periodic Table  6.3.1. Atomic Size  6.3.2. Metallic and non-metallic character  6.3.3. Electronegativity  6.3.4. Reactivity of the elements  6.4. Alkali metals and their properties
  7. Chemical bond  7.1. Why do atoms form bonds?  7.2. Types of chemical bonds  7.2.1. Ionic bond  7.2.2. Covalent bond  7.2.3. Metal Bond  7.3. Properties of Ionic and Covalent Compounds  7.4. Intermolecular forces
  8. Chemical reactions  8.1. Introduction to Chemical Reactions  8.2. Signs of a chemical reaction  8.3. Types of Chemical Reactions  8.3.1. Combination Reactions  8.3.2. Decomposition reactions  8.3.3. Displacement reactions  8.3.4. Double displacement reactions  8.3.5. Combustion reactions  8.4. Law of conservation of mass  8.5. Balancing simple chemical equations
  9. Acids, Bases and Salts  9.1. Definition of Acid and Base  9.2. Properties of Acids  9.3. Properties of bases  9.4. pH Scale and Indicators  9.5. Neutralization reactions  9.6. Common Acids and Bases in Everyday Life  9.7. Preparation and use of salts  9.8. Strong and weak acids and bases
  10. Solutions and Solubility  10.1. Definition of Solution  10.2. Components of the solution  10.2.1. Solvent  10.2.2. solute  10.3. Factors Affecting Solubility  10.4. Concentration of solutions  10.5. Saturated and unsaturated solutions  10.6. Colloids and suspensions  10.7. Solubility curve and its interpretation
  11. Air and atmosphere  11.1. Composition of air  11.2. Properties of gases in the air  11.3. Importance of Oxygen and Carbon Dioxide  11.4. Air pollution and its effects  11.5. Greenhouse effect and global warming  11.6. Ways to reduce air pollution  11.7. Ozone layer and its importance
  12. Water and its importance  12.1. Properties of Water  12.2. Water as the universal solvent  12.3. Importance of water for life  12.4. Water pollution and its effects  12.5. Water Purification  12.5.1. Filtration  12.5.2. boil  12.5.3. Chlorination in water purification  12.5.4. reverse osmosis  12.6. Hard and soft water  12.7. Water cycle and its importance
  13. Fuel and energy  13.1. Types of fuel  13.1.1. Fossil fuels  13.1.2. Renewable energy sources  13.2. Combustion and energy release  13.3. Global warming and its effects  13.4. Alternative sources of energy  13.5. Ways to conserve energy
  14. Metals and Nonmetals  14.1. Physical and chemical properties of metals  14.2. Physical and Chemical Properties of Non-Metals  14.3. Difference Between Metals and Nonmetals  14.4. Uses of metals and nonmetals  14.5. Corrosion of metals and its prevention  14.6. Alloys and their importance
  15. Plastics and polymers  15.1. Natural and synthetic polymers  15.2. Properties of plastics  15.3. Biodegradable and Non-Biodegradable Plastics  15.4. Environmental impact of plastic  15.5. Recycling and waste management in plastics and polymers  15.6. Daily Uses of Polymers
  16. Introduction to Organic Chemistry  16.1. Basic definitions of organic chemistry  16.2. Carbon Compounds in Daily Life  16.3. Hydrocarbons  16.4. Simple functional groups (alcohols and carboxylic acids)  16.5. Importance of organic compounds in industry

Grade 7 → Introduction to Organic Chemistry ↓


Simple functional groups (alcohols and carboxylic acids)


Entering the world of organic chemistry is like embarking on a new adventure where we explore the basic building blocks of life. In this journey, it is important to understand simple functional groups such as alcohols and carboxylic acids. These are not just scientific terms; they also represent compounds that play important roles in everyday life.

What are functional groups?

Functional groups are specific groups of atoms within molecules that have certain properties and chemical behavior. When we look at larger organic compounds, these groups determine how the compound reacts in chemical reactions. In short, functional groups are responsible for the specific chemical behavior of organic molecules.

Alcohol: simple group containing hydroxyl (-OH)

Alcohols are one of the simplest examples of functional groups. The defining characteristic of alcohols is the presence of a hydroxyl group, represented as –OH. This hydroxyl group is composed of an oxygen atom bonded to a hydrogen atom. It is attached to a carbon atom in the hydrocarbon chain.

        Methanol: CH3OH
        Ethanol: C 2 H 5 OH
        Propanol: C 3 H 7 OH

Methanol is the simplest alcohol, containing one carbon atom. Its formula is CH 3 OH. It is widely used as a solvent and antifreeze.

Ethanol, or grain alcohol, is commonly found in alcoholic beverages. Its formula is C 2 H 5 OH. In addition to beverages, ethanol is used as a fuel, disinfectant, and industrial solvent.

Propanol has three carbon atoms. Propanol prepared as C 3 H 7 OH is used in the synthesis of other chemicals.

Oh C H

This diagram shows the basic structure of an alcohol molecule. Note -OH group attached to the carbon.

Carboxylic acid: carboxyl (-COOH) group

Carboxylic acids are another important functional group in organic chemistry. What makes them unique is the presence of a carboxyl group, represented as -COOH. This group contains a carbon atom that is double bonded to an oxygen atom and is also bonded to a hydroxyl group.

        Formic acid: HCOOH
        Acetic acid: CH3COOH
        Propionic acid: C 2 H 5 COOH

Formic acid is the simplest carboxylic acid having the chemical formula HCOOH. It is found naturally in the venom of ant stings.

Acetic acid, which is known for giving vinegar its sour taste and strong odor, has the formula CH3COOH. It is used extensively in the food industry as a preservative.

Propionic acid or propanoic acid is used in baking and food preservation. Its formula is C 2 H 5 COOH.

C Hey Oh

Here, the structure of a carboxylic acid is shown, with -COOH group clearly shown.

How do these functional groups react?

Both alcohols and carboxylic acids exhibit unique reactivity due to their functional groups. These reactions are essential in organic synthesis and industrial applications.

Reactions to alcohol

Alcohols can participate in a variety of reactions, some of which are important in the manufacture of everyday products:

  • Dehydration: Alcohols can lose a water molecule to form an alkane. For example, ethanol can dehydrate to form ethene.
  • Oxidation: When alcohols are oxidized, they can become aldehydes, ketones, or carboxylic acids. Ethanol is oxidized to form acetic acid.
  • Esterification: Alcohols react with carboxylic acids to form esters, which have wide applications in fragrances and flavors.

Reactions of carboxylic acids

Carboxylic acids also have specific reactions that contribute significantly to industrial processes:

  • Neutralization: Carboxylic acids can react with bases to form salts and water. Acetic acid reacts with sodium hydroxide to form sodium acetate.
  • Esterification: As mentioned, they react with alcohols to form esters. This reaction is very important in the manufacture of fragrances and flavors.
  • Reduction: Carboxylic acids can be reduced to alcohols, reversing the oxidation process of alcohols.

The role of alcohols and carboxylic acids in everyday life

Alcohols and carboxylic acids aren't just confined to chemistry textbooks; they play important roles in our daily lives, in areas ranging from cooking to healthcare.

Everyday uses of alcohol

Ethanol is probably the most well-known alcohol because it is found in alcoholic beverages. However, its usefulness extends beyond beverages:

  • It is used as a fuel and a fuel additive, increasing its combustibility.
  • It acts as a disinfectant and antiseptic, and is often present in sanitizers and hand rubs.
  • It serves as a solvent in the production of various items, such as perfumes and essences.

Daily uses of carboxylic acid

Carboxylic acids are equally important in practical applications:

  • Acetic acid: Found primarily in vinegar, it is used for flavoring and food preservation.
  • Citric acid: Commonly used in soft drinks and carbonated beverages, providing a tart taste.
  • Lactic acid: Used in dairy products, especially during the fermentation of foods such as yogurt and sauerkraut.

Conclusion

Understanding the basics of alcohols and carboxylic acids explains many aspects of organic chemistry. These simple functional groups not only help define chemical reactions, but also many applications that impact daily life. From the ethanol in our hand sanitizer to the acetic acid in our pantry, these compounds illustrate how chemistry is woven into the fabric of our existence.

As you continue to explore these fascinating molecules, remember that the world of organic chemistry is vast and there are many discoveries yet to be made. By using alcohols and carboxylic acids as bases, the path is paved for the future exploration of more complex chemical structures and their versatile uses.


Grade 7 → 16.4


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