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 → Metals and Nonmetals ↓


Reactivity Series of Metals and Displacement Reactions


The study of reactivity series and displacement reactions is an essential part of understanding chemistry, especially when dealing with the behavior of metals. This explanation will highlight the concepts related to these two fundamental topics.

Understanding the reactivity series

The reactivity series is a way of arranging metals (and hydrogen) in order of their reactivity from highest to lowest. This order helps predict the behavior of metals in a reaction. The more reactive the metal, the more vigorous its reactivity will be.

Order of metals in reactivity series

Here is a commonly used reactivity series, listed from most reactive to least reactive:

Potassium (K) > Sodium (Na) > Calcium (Ca) > Magnesium (Mg) > Aluminium (Al) > Zinc (Zn) > Iron (Fe) > Tin (Sn) > Lead (Pb) > (Hydrogen) > Copper (Cu) > Mercury (Hg) > Silver (Ag) > Gold (Au)

Note that hydrogen is included in the series for reference to help predict reactions involving acids.

Examples of reactivity

Reactivity can be observed through various experiments, such as observing bubbles in an acid or how quickly a metal corrodes when exposed to oxygen.

Visual explanation example

Reactivity of Metals with WaterPotassiumSodiumCalciumMagnesiumAluminium

In this example, as you move down the list, the reactivity with water decreases.

Factors affecting reactivity

  • Atomic structure: Valency and number of losing electrons are important for stability.
  • Electron shielding: More electron shells means less friction force between the nucleus and the valence electrons.
  • Nuclear force: Metals with lower atomic number have lower nuclear force, which makes them more reactive.

Displacement reactions

Displacement reactions occur when a more reactive metal displaces a less reactive metal from its compound. This is a common chemical reaction seen in metals and tells us about the strength and power of different metals.

General equations and examples:

Metal A + Salt solution (of metal B) → Salt solution (of metal A) + Metal B

If metal A is more reactive than metal B, it will "pull" metal B out of the compound, and take its place.

Textual examples

Zinc + Copper sulphate → Zinc sulphate + Copper

The above equation can be expressed as:

Zn(s) + CuSO 4 (aq) → ZnSO 4 (aq) + Cu(s)

Why do displacement reactions happen?

Displacement occurs due to differences in the reactivity of the metals. If a metal is higher up in the reactivity series, it can displace another metal with lower reactivity. Essentially, the reaction is driven by energy mobility, where the more reactive metal will more easily give up electrons, thus leaving another metal in a position.

Visual example of a displacement reaction

Displacement reaction visualizationZincqueso 4ZnSO 4Cube

Other examples of displacement reactions

Iron + Copper sulphate → Iron sulphate + Copper

Fe (s) + CuSO 4 (aq) → FeSO 4 (aq) + Cu (s)
  • Aluminum and Lead Nitrate:
    2Al (s) + 3Pb(NO 3 ) 2 (aq) → 2Al(NO 3 ) 3 (aq) + 3Pb (s)
  • Magnesium and Silver Nitrate:
    Mg (s) + 2AgNO 3 (aq) → Mg(NO 3 ) 2 (aq) + 2Ag (s)

Applications of reactivity series and displacement reactions

Understanding these reactions has practical applications in real-world scenarios, including:

  1. Extraction of metals: Metals are often extracted from their ores via displacement reactions.
  2. Corrosion prevention: Knowledge of the reactivity of metals helps in designing better corrosion resistant materials.
  3. Electroplating: Electroplating uses displacement reactions to coat one metal with another less reactive metal.

Summary

The study of reactivity series and displacement reactions sheds light on the nature and behaviour of metals. It helps in predicting the outcomes of chemical reactions, thereby enriching our understanding of chemical processes. By analysing these fundamental principles, students can better understand the intricacies of chemistry.


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Physical and Chemical Properties of Non-Metals
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Reactivity Series of Metals and Displacement Reactions

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