Grade 11
  1. Basic concepts of chemistry  1.1. Importance of Chemistry  1.2. Nature and scope of chemistry  1.3. laws of chemical combination  1.3.1. Law of conservation of mass  1.3.2. Law of definite proportions  1.3.3. Law of multiple proportions  1.3.4. Law of gaseous volume  1.3.5. Avogadro's Law  1.4. Dalton's atomic theory  1.5. Mole concept and molar mass  1.6. Percent composition  1.7. Empirical and molecular formula  1.8. Stoichiometry and Stoichiometric Calculations  1.9. Limiting reagent concept
  2. Structure of the atom  2.1. Discovery of the electron, proton, and neutron  2.2. Atomic Model  2.2.1. Thomson's model  2.2.2. Rutherford's model  2.2.3. Bohr's model  2.3. Quantum mechanical model of the atom  2.4. Dual nature of matter and radiation  2.5. Heisenberg's uncertainty principle  2.6. Quantum numbers  2.7. Atomic orbitals and their shapes  2.8. Electronic configuration of elements  2.9. Aufbau principle  2.10. Pauli's exclusion principle  2.11. Hund's maximum multiplicity rule  2.12. de Broglie's hypothesis  2.13. Photoelectric effect
  3. Classification of elements and periodicity in properties  3.1. Historical development of the periodic table  3.2. Modern Periodic Law and Periodic Table  3.3. Periodic trends in properties  3.3.1. Atomic and Ionic Radius  3.3.2. Ionization enthalpy  3.3.3. Electron gain enthalpy  3.3.4. Electronegativity  3.3.5. Valency  3.3.6. Metallic and Non-Metallic Properties  3.3.7. Oxidation states  3.4. Unusual Properties of the First Elements
  4. Chemical Bonding and Molecular Structure  4.1. Kossel–Lewis approach to chemical bonding  4.2. Ionic or electrovalent bond  4.3. Covalent bond and its features  4.4. Bond parameters  4.5. VSEPR Theory  4.6. Valence bond theory  4.7. Hybridization and its types  4.8. Molecular orbital theory  4.8.1. Bond order and stability  4.9. Hydrogen bonding
  5. States of matter  5.1. Intermolecular forces  5.2. Gas Laws  5.2.1. Boyle's law  5.2.2. Charles's Law  5.2.3. Avogadro's Law  5.2.4. Dalton's law of partial pressure  5.2.5. Graham's law of spread  5.3. Ideal Gas Equation and Applications  5.4. Real gases and deviations from ideal behaviour  5.5. Kinetic molecular theory of gases  5.6. Liquefaction of gases  5.7. Properties of Liquids  5.8. Surface tension and viscosity
  6. Thermodynamics  6.1. System and environment  6.2. Types of systems in thermodynamics  6.3. Types of procedures  6.4. First law of thermodynamics  6.5. Internal energy and enthalpy  6.6. Heat capacity and specific heat  6.7. Hess's law of constant heat summation  6.8. Bond dissociation enthalpy  6.9. Enthalpy of formation and combustion  6.10. Enthalpy of solution and neutralization  6.11. Spontaneity and the second law of thermodynamics  6.12. Gibbs free energy and its applications
  7. Balance  7.1. The concept of balance  7.2. Equilibrium constant and its applications  7.3. Le Chatelier's principle  7.4. Ionic equilibrium in solutions  7.5. Acid and Base Theory  7.5.1. Arrhenius concept  7.5.2. Bronsted-Lowry concept  7.5.3. Lewis concept  7.6. pH Scale and pOH  7.7. Common ion effect  7.8. Hydrolysis of salts  7.9. Buffer solutions and their mechanism of action  7.10. Solubility equilibrium of sparingly soluble salts
  8. Redox reactions  8.1. Oxidation and reduction concepts  8.2. Oxidation number and its applications  8.3. Redox reactions in terms of electron transfer  8.4. Balancing redox reactions (oxidation number and ion-electron methods)  8.5. Types of redox reactions  8.6. Electrochemical Cells and Redox Reactions
  9. Hydrogen  9.1. Position of Hydrogen in the Periodic Table  9.2. Isotopes of hydrogen  9.3. Preparation of Hydrogen  9.4. Properties of Hydrogen  9.5. Hydrides and their classification  9.6. Water and heavy water  9.7. Hydrogen peroxide and its properties  9.8. Uses of Hydrogen and Its Compounds
  10. S-block elements (alkali and alkaline earth metals)  10.1. Group 1 Elements - Properties and Trends  10.2. Group 2 Elements - Properties and Trends  10.3. Unusual properties of lithium and beryllium  10.4. Important compounds of sodium and their uses  10.5. Important Compounds of Magnesium and Calcium
  11. Some p-block elements  11.1. General Introduction to p-Block Elements  11.2. Group 13 Elements  11.2.1. Boron and its compounds  11.3. Group 14 Elements  11.3.1. Carbon and its allotropes  11.3.2. Important Compounds of Carbon and Silicon
  12. Organic Chemistry - Some Basic Principles and Techniques  12.1. Classification and Nomenclature of Organic Compounds  12.2. Structural representation of organic compounds  12.3. Classification of organic reactions  12.4. Electronic Effects in Organic Chemistry  12.4.1. Inductive effect  12.4.2. Resonance effect  12.4.3. Hyperconjugation  12.5. Reaction mechanism and intermediate species  12.6. Purification and qualitative analysis of organic compounds
  13. Hydrocarbons  13.1. Hydrocarbons  13.1.1. Preparation and Properties of Alkenes  13.2. alkene  13.2.1. Preparation and Properties of Alkenes  13.2.2. Electrophilic addition reactions  13.3. Alkynes  13.3.1. Preparation and Properties of Alkynes  13.4. Aromatic hydrocarbons  13.4.1. Structure and properties of benzene  13.4.2. Electrophilic substitution reactions of benzene
  14. Environmental Chemistry  14.1. Environmental Pollution  14.2. Atmospheric pollution and the greenhouse effect  14.3. Water pollution and treatment methods  14.4. Soil pollution and its effects  14.5. Industrial waste and its treatment  14.6. Strategies for pollution control

Grade 11 → Basic concepts of chemistry ↓


Nature and scope of chemistry


Chemistry is the branch of science that studies the composition, structure, properties, and transformation of matter. It provides a basis for understanding the physical and biological world in which we live. This field of study is fundamental to many scientific disciplines, and has wide applications in industries, medicine, environmental science, and everyday life.

What is chemistry?

Chemistry is often called the "central science" because it connects other natural sciences such as physics, geology, and biology. It is essential for understanding various phenomena and processes around us. At its core, chemistry is about the following:

  • Structure: What the matter is made of, such as elements and compounds.
  • Structure: How the parts of matter are arranged, such as atomic and molecular structure.
  • Properties: Characteristics of matter, including physical and chemical properties.
  • Transformation: How matter changes from one form to another, such as through chemical reactions.

Visual example: structure of water molecule

O H H

Diagram showing the structure of the water molecule, H2O.

Branches of chemistry

There are several branches of chemistry, each focusing on different aspects of chemistry and chemical reactions:

1. Organic chemistry

This branch deals with the study of compounds containing carbon. Organic chemistry explores the various structures, properties, and reactions of carbon-containing compounds, which often contain hydrogen, oxygen, nitrogen, and other elements.

2. Inorganic chemistry

Inorganic chemistry focuses on compounds that do not contain carbon-hydrogen bonds. This branch studies metals, minerals, and organometallic compounds. It is important for understanding different materials and their properties.

3. Physical chemistry

Physical chemistry combines chemistry with physics. It investigates how matter behaves at the molecular and atomic level and how chemical reactions occur. It involves concepts such as thermodynamics and quantum mechanics.

4. Analytical chemistry

This branch of chemistry analyzes substances to determine their composition and quantity. Analytical chemistry is important in fields such as forensics, environmental science, and quality control in manufacturing.

Visual example: separation technique

Liquid Mixture Part 1 Part 2

Diagram showing a basic technique in analytical chemistry - chromatography, used to separate mixtures.

5. Biochemistry

Biochemistry is the study of the chemical processes within and related to living organisms. It is a laboratory-based science that combines biology and chemistry to try to understand how living systems work.

Importance and applications of chemistry

Medicine

Chemistry plays a vital role in medicine and pharmaceuticals. It helps understand the biochemical nature of the human body and enables the design and synthesis of drugs that can cure diseases and alleviate symptoms.

Food industry

In the food industry, chemistry ensures food safety by enabling the analysis of nutritional content, preservatives and artificial flavors. It also plays an important role in the development of new food products.

Agriculture

Chemistry contributes significantly to agriculture by developing fertilizers, pesticides and herbicides to increase crop yields and protect crops. Understanding soil chemistry helps in choosing appropriate treatments to increase fertility.

Environmental science

Chemistry helps us understand environmental issues such as pollution. It is important in developing solutions to environmental problems such as waste management and the creation of sustainable energy sources.

Everyday life

Chemistry plays a vital role in the manufacture of everyday products such as soaps, plastics, clothes and cosmetics. This science explains everyday phenomena, such as why iron rusts, how food is cooked and why leaves change colour.

Chemical reactions

Chemical reactions are processes in which one or more substances, the reactants, are transformed into one or more different substances, the products. They involve the formation and breaking of chemical bonds and the rearrangement of atoms. Here are some examples:

2H2 + O2 → 2H2O

This is the chemical equation for the formation of water from hydrogen and oxygen.

CH4 + 2O2 → CO2 + 2H2O

This equation shows the combustion of methane in oxygen to produce carbon dioxide and water.

NaCl → Na+ + Cl-

This simple decomposition reaction shows the dissociation of sodium chloride in solution.

Conclusion

Chemistry, as the study of matter and its transformations, is integral to understanding the world around us. Its branches cover a wide range of topics and applications, from microscopic interactions in biochemistry to large-scale processes in industrial chemistry. The principles of chemistry enable innovation, which impacts a variety of fields such as healthcare, manufacturing, and environmental science. Through its study, it allows us to solve problems, develop new materials, and progress scientifically and technologically. In short, chemistry is both a fundamental science and an essential tool for progress in many fields.


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Nature and scope of chemistry

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