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 → Chemical Reactions and Equations ↓


Types of Chemical Reactions


Chemical reactions are processes where reactants are transformed into products. Understanding the type of reaction can help predict products and understand the conditions necessary for a reaction to occur. Here, we explore the four main types of chemical reactions: combination, decomposition, displacement, and double displacement.

1. Combination reactions

Combination reactions, also called synthesis reactions, occur when two or more reactants combine to form a single product. The general form of a combination reaction is:

A + B → AB

Examples of combination reactions:

Example 1: Formation of water from hydrogen and oxygen:

2H 2 + O 2 → 2H 2 O
H H , Hey , H Hey H

Example 2: Formation of carbon dioxide from carbon and oxygen:

C + O 2 → CO 2
C , Hey Hey , Hey Hey C

2. Decomposition reactions

A decomposition reaction occurs when a single compound breaks down into two or more simpler substances. Its general form is:

AB → A + B

Examples of decomposition reactions:

Example 1: Decomposition of water into hydrogen and oxygen:

2H 2 O → 2H 2 + O 2
HHeyH H H Hey

Example 2: Decomposition of calcium carbonate to calcium oxide and carbon dioxide:

CaCO 3 → CaO + CO 2
CA , CHey Hey CA Hey

3. Displacement reactions

Displacement reactions, also called single displacement or substitution reactions, occur when one element displaces another element in a compound, forming a new compound. Its general form is:

A + BC → AC + B

Examples of displacement reactions:

Example 1: Displacement of copper by zinc in copper sulphate solution:

Zn + CuSO 4 → ZnSO 4 + Cu
Zinc , Cube SHey Hey ZincHey so

Example 2: Iron displaces hydrogen from hydrochloric acid:

Fe + 2HCl → FeCl 2 + H 2
Fe , H Chlorine Fe Chlorine Chlorine

4. Double displacement reactions

A double displacement reaction, also known as a metathesis reaction, involves the exchange of ions between two compounds to form two new compounds. Its general form is:

AB + CD → AD + CB

Examples of double displacement reactions:

Example 1: The reaction of barium chloride with sodium sulfate forms barium sulfate and sodium chloride:

BaCl 2 + Na 2 SO 4 → BaSO 4 + 2NaCl
B. A Chlorine Chlorine , No No S Hey B. A S Hey

Example 2: The reaction of hydrochloric acid with silver nitrate produces silver chloride and nitric acid:

HCl + AgNO 3 → HNO 3 + AgCl
H Chlorine , AG N Hey H N Hey

Understanding these fundamental types of chemical reactions provides a solid foundation for further study in chemistry. By recognizing patterns of interaction of atoms and molecules, we can predict reaction outcomes, design new compounds, and appreciate the dynamic nature of chemical systems.


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Types of Chemical Reactions

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