Grade 10
  1. Matter and its properties  1.1. States of matter  1.2. Physical and chemical properties of matter  1.3. Classification of substances (elements, compounds, mixtures)  1.4. Changes in Matter (Physical and Chemical Changes)  1.5. Law of conservation of mass and law of definite proportions
  2. Atomic Structure  2.1. Historical development of the atomic model  2.2. Subatomic particles (protons, neutrons, electrons)  2.3. Atomic number, mass number and isotopes  2.4. Electronic Configuration and Energy Levels  2.5. Valency, ion formation and oxidation state
  3. Periodic table  3.1. History and Development of the Periodic Table  3.2. Modern Periodic Law and Periodic Trends  3.3. Groups and Periods in the Periodic Table  3.4. Trends in the Periodic Table  3.5. Metals, non-metals, metalloids and their properties  3.6. Noble gases and their chemical inertness
  4. Chemical bond  4.1. Formation of Chemical Bonds (Octet Rule)  4.2. Ionic Bonding and Properties of Ionic Compounds  4.3. Covalent Bond and Properties of Covalent Compounds  4.4. Metallic bond and its properties  4.5. Molecular geometry and VSEPR theory  4.6. Polarity and dipole moment of molecules  4.7. Intermolecular forces
  5. Chemical Reactions and Equations  5.1. Types of Chemical Reactions  5.2. Writing and balancing chemical equations  5.3. Law of conservation of mass in chemical reactions  5.4. Factors Affecting Chemical Reactions  5.5. Catalysts and their role in chemical reactions  5.6. Exothermic and Endothermic Reactions
  6. Stoichiometry and Chemical Calculations  6.1. Mole concept and Avogadro number  6.2. Molar Mass and Gram-Mole Conversions  6.3. Empirical and molecular formula  6.4. Stoichiometric calculations and chemical yield  6.5. Limiting and Excess Reactants
  7. Acids, Bases and Salts  7.1. Properties and Definitions of Acids and Bases (Arrhenius, Bronsted-Lowry, Lewis)  7.2. pH Scale, pOH, and Indicators  7.3. Neutralization reactions and salt formation  7.4. Strength of Acids and Bases (Strong vs. Weak Acids and Bases)  7.5. Common Acids and Bases in Daily Life  7.6. Salts, their solubility and applications
  8. Metals and Nonmetals  8.1. Physical and chemical properties of metals  8.2. Physical and Chemical Properties of Non-Metals  8.3. Reactivity Series of Metals and Displacement Reactions  8.4. Extraction of metals from ores  8.5. Corrosion, its causes and prevention  8.6. Alloys, their composition and uses
  9. Carbon and its compounds  9.1. Allotropes of Carbon  9.2. Hydrocarbons and their classification (alkanes, alkenes, alkynes)  9.3. Functional groups in organic compounds  9.4. Nomenclature of organic compounds (IUPAC system)  9.5. Isomerism in organic chemistry (structural and geometrical)  9.6. Important organic reactions (combustion, addition, substitution, polymerization)  9.7. Applications of organic compounds in industry and daily life
  10. Environmental Chemistry  10.1. Air Pollution (Sources, Effects and Control)  10.2. Water Pollution (Causes, Effects and Remedies)  10.3. Greenhouse effect and global warming  10.4. Ozone layer depletion and its effects  10.5. Green Chemistry and Its Applications  10.6. sustainable chemistry practice
  11. Thermochemistry  11.1. Heat and Energy Changes in Chemical Reactions  11.2. Exothermic and Endothermic Reactions  11.3. Enthalpy, enthalpy change, and heat of reaction  11.4. Specific heat capacity and calorimetry  11.5. Energy Changes in Combustion Reactions
  12. Electrochemistry  12.1. Electrolytes and non-electrolytes  12.2. Electrolysis and its applications (electroplating, extraction of metals)  12.3. Redox reactions (oxidation and reduction)  12.4. Galvanic cell and electrochemical series  12.5. Corrosion and electrochemical prevention methods
  13. Chemical kinetics and equilibrium  13.1. Rate of chemical reactions and its measurement  13.2. Factors affecting the reaction rate (catalyst, temperature, concentration)  13.3. Reversible and irreversible reactions  13.4. Dynamic equilibrium and equilibrium constant  13.5. Le Chatelier's principle and its applications
  14. Gases and Gas Laws  14.1. Properties of gases and kinetic molecular theory  14.2. Boyle's Law (Pressure-Volume Relation)  14.3. Charles's Law  14.4. Gay-Lussac's Law  14.5. Combined Gas Law and Ideal Gas Law  14.6. Real Gases vs Ideal Gases
  15. Nuclear Chemistry  15.1. Introduction to Radioactivity and Nuclear Reactions  15.2. Types of radioactive decay (alpha, beta, gamma)  15.3. Half-life and applications of radioactive isotopes  15.4. Nuclear fission and fusion reactions  15.5. Nuclear power generation and its environmental impact

Grade 10 → Environmental Chemistry ↓


Green Chemistry and Its Applications


Green chemistry, also known as sustainable chemistry, is a field of chemistry that focuses on the design of products and processes that reduce the use and production of hazardous substances. It is a field of chemistry dedicated to finding ways to reduce the environmental impact of conventional chemical processes and make them more sustainable.

Principles of green chemistry

Green chemistry is based on twelve fundamental principles that guide chemists in designing safer chemicals and processes. These principles are:

  1. Prevention: It is better to prevent waste than to treat or clean it after it has been generated.
  2. Atom economy: Synthetic methods should be designed to maximize the incorporation of all materials used in the process into the final product.
  3. Less hazardous chemical synthesis: Wherever possible, synthetic methods should be designed to use and produce substances that have little or no toxicity to human health and the environment.
  4. Design of safer chemicals: Chemical products must be designed to perform their intended function while also being as non-toxic as possible.
  5. Safe solvents and excipients: The use of excipients (such as solvents) should be made unnecessary wherever possible, and they should be harmless when used.
  6. Design for energy efficiency: Energy requirements should be identified for their environmental and economic impacts and minimized. Synthetic methods should be operated at ambient temperature and pressure whenever possible.
  7. Use of renewable feedstock: Whenever technically and economically feasible, the raw material or feedstock should not be exhaustible but renewable.
  8. Minimize derivatization: Unnecessary derivatization (use of blocking groups, protection/deprotection, temporary modification of physical/chemical processes) should be minimized or avoided if possible.
  9. Catalysis: Catalytic reagents (as selective as possible) are superior to stoichiometric reagents.
  10. Design for degradation: Chemical products should be designed so that at the end of their life they decompose into harmless degradation products and do not persist in the environment.
  11. Real-time analysis for pollution prevention: Analytical methods need to be further developed to monitor and control the process in real time before hazardous substances are formed.
  12. Inherently safe chemicals for accident prevention: The materials and nature of substances used in the chemical process should be selected in such a way that the probability of chemical accidents, including emissions, explosions and fires, is minimized.

Applications of green chemistry

Green chemistry is used in many areas and can have benefits for both the environment and human health. Here are some examples of its applications:

Green chemistry in industrial production

Manufacturers of industrial products are focusing on using greener processes to reduce waste and reduce energy consumption. For example, the manufacture of Nylon-6 is being improved by using water instead of hazardous organic solvents in some processes.

        Nylon-6: A tough, synthetic polymer used for manufacturing fibers, molded products, and films.

Biodegradable plastic

Conventional plastics are known for their durability and resistance to decomposition, but these properties also make them a serious concern for the environment. Green chemistry promotes the development of biodegradable plastics that break down easily in the environment. These are made using natural materials such as starch and cellulose, providing a more sustainable alternative.

Green hydrogen production

Hydrogen is a clean energy source that produces only water when burned. Using innovative methods like solar and wind energy, scientists are producing hydrogen from water in a green way. This method reduces dependence on fossil fuels.

Medicines with fewer side effects

The aim of green chemistry is to design medicines that produce fewer harmful byproducts and have fewer side effects. One way to achieve this is to use more efficient synthetic routes that eliminate or reduce the use of toxic solvents and hazardous reagents.

Illustrating the principles of green chemistry

To understand the essence of green chemistry, let's visualize these concepts:

Green Chemistry Principles Waste prevention Nuclear Economy

Conclusion

The concept of green chemistry is fundamental to creating a sustainable future. By adopting these principles, the chemical industry can develop processes and products that are not only economically viable but also beneficial to the environment. Although we have highlighted just a few practices and applications of green chemistry, its scope is vast and constantly growing. As we continue to innovate and adopt more sustainable methods, green chemistry offers a path to reduce the ecological footprint of chemical processes and ensure a healthy planet.

Further study

Students are encouraged to delve deeper into the practical applications and innovations emerging from green chemistry. Understanding and applying these principles at an early stage will foster a new generation of environmentally conscious chemists who are prepared to tackle future environmental challenges.


Grade 10 → 10.5


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Green Chemistry and Its Applications

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