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 ↓


sustainable chemistry practice


Sustainable chemistry practices are important in today's world to ensure that the chemical processes and products we use do not harm our environment and are available for future generations. This subject is an integral part of environmental chemistry, which focuses on the chemical aspects of environmental issues. In this lesson, we will explore what sustainable chemistry practices are, why they are important, and how they are applied in various industries.

What is sustainable chemistry?

Sustainable chemistry, often referred to as green chemistry, is a field of chemistry that aims to design chemical products and processes that reduce or eliminate the use and production of hazardous substances. The goal is to create processes that are not only efficient and economical but also environmentally friendly. It involves every stage of a chemical's life cycle, from its manufacture to its disposal.

Why is sustainable chemistry important?

There are several reasons why sustainable chemistry practices are important:

  • Environmental protection: Sustainability reduces pollutants that can harm air, water, and soil.
  • Resource efficiency: By using resources more efficiently, sustainable practices can help conserve non-renewable resources.
  • Economic benefits: Sustainable chemistry can lead to cost savings through improved efficiency and reduced waste.
  • Health and safety: Reducing the use of harmful substances helps protect human and animal health.

Twelve principles of green chemistry

Green chemistry is guided by twelve principles, which provide a framework for innovation and creativity in the field.

  1. Prevention: It is better to prevent waste than to treat or clean it after it has been generated.
  2. Atom economy: This principle focuses on incorporating all the materials used in the process into the final product. An example of poor atom economy is when a large amount of reagents are used in a chemical reaction and only a small portion ends up in the final product.
  3. Less hazardous chemical synthesis: Designing chemical syntheses to use and produce substances with low 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. Safer solvents and excipients: Avoid using excipients (e.g., solvents, separating agents) whenever possible, and render them harmless when they must be used.
  6. Design for energy efficiency: Minimize energy requirements, and if possible, operate synthetic methods at ambient temperature and pressure.
  7. Use of renewable feedstocks: Raw materials should be renewable wherever technically and economically feasible.
  8. Minimize derivatization: Reduce or avoid unnecessary derivatization (use of blocking groups, protection/deprotection) in chemical synthesis.
  9. Catalysis: Catalytic reagents (as selective as possible) are superior to stoichiometric reagents.
  10. Design for degradation: Chemical products should be designed to degrade into harmless substances after use, so that they do not accumulate in the environment.
  11. Real-time analysis for pollution prevention: Developing methods that allow process monitoring and control in real time before hazardous substances are created.
  12. Inherently safer chemistry for accident prevention: Designing chemicals and their transformation processes to minimize the potential for chemical accidents, including emissions, explosions, and fires.

Examples and applications of sustainable chemistry

There are many real-world examples where sustainable chemistry practices are applied:

Use of renewable feedstocks

One of the principles of green chemistry is to use renewable materials. For example, bio-based plastics are made from renewable resources such as corn starch or sugar cane. These plastics are designed to be biodegradable, meaning they can decompose naturally in the environment.

Case study: Bioplastics from corn

Let's look at an example of bioplastic production from corn:

C 6 H 12 O 6 + 2 ADP + 2 Pi + 2 NAD + → 2 CH 3 CHOHCOOH + 2 ATP + 2 NADH

This process converts glucose (from corn starch) into lactic acid through fermentation, which can then be converted into polylactic acid (PLA), a biodegradable plastic.

Safe solvent

Traditionally, some solvents used in chemical processes can be harmful to both the environment and human health. Sustainable chemistry focuses on finding safer alternatives. For example, replacing toxic organic solvents with water, supercritical CO2 or ionic liquids can substantially reduce the environmental impact.

Educational initiatives in sustainable chemistry

Incorporating sustainable chemistry into education is important to build a better future. Schools and universities are now offering courses and programs specifically focused on this area. These programs teach students how to develop sustainable solutions by applying the principles of green chemistry.

For example, chemistry students may be given the task of developing a laboratory experiment that uses non-toxic materials or finding a way to reduce waste in the school laboratory.

Challenges and future prospects

Although sustainable chemistry practices have significant benefits, they also pose challenges:

  • Cost: Initially, sustainable chemistry practices may be more expensive due to research and development costs. However, they can lead to long-term savings.
  • Technical limitations: Sustainable alternatives are not yet available for some chemical processes, which will require further innovation and research.
  • Regulatory issues: Regulatory barriers may need to be resolved to widely implement new sustainable chemistry solutions.

The future of sustainable chemistry is promising. Advances in technology and growing awareness of environmental issues are fueling the development of new methods and materials. Governments and industry are investing more in research and development to overcome existing barriers. As these advances continue, sustainable chemistry will likely become an integral part of all chemical processes.

Conclusion

Sustainable chemistry practices are vital to ensuring a safe, efficient, and environmentally responsible approach to chemistry. By following the principles of green chemistry, we can reduce the negative impact of chemical processes on our planet and take important steps toward a sustainable future. Education, innovation, and policy support will be key factors in advancing these practices in industries around the world.


Grade 10 → 10.6


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sustainable chemistry practice

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