Chapter 3: Metals and Non-Metals

Chapter 3: Metals and Non-Metals ATOM BOMB

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Chapter 3: Metals and Non-Metals

Properties of Metals

Physical: Malleable, ductile, shiny, high melting points, good conductors of heat and electricity.
Chemical: React with oxygen to form basic oxides (e.g., 2Mg + O₂ → 2MgO), react with

water to release hydrogen (e.g., 2Na + 2H₂O → 2NaOH + H₂).

Properties of Non-Metals

Physical: Brittle, dull, poor conductors of heat and electricity.
Chemical: React with oxygen to form acidic oxides (e.g., CO₂ + H₂O → H₂CO₃), react with hydrogen to form hydrogen compounds (e.g., Cl₂ + H₂ → 2HCl).

Reactivity Series

Metals are arranged based on their reactivity.

Example: Potassium (K) > Calcium (Ca) > Magnesium (Mg) > Zinc (Zn) > Iron (Fe) > Copper (Cu).

Corrosion

Definition: The gradual destruction of metals due to chemical reactions with their environment (e.g., rusting of iron).
Prevention:
- Galvanization: Coating metal with zinc to prevent rusting.
- Alloying: Mixing metals to form alloys (e.g., stainless steel).
- Chapter 4: Carbon and Its Compounds

Chapter 2: Acids, Bases, and Salts

Chapter 2: Acids, Bases, and Salts ATOM BOMB

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Chapter 2: Acids, Bases, and Salts

Acids

Definition: Substances that release hydrogen ions (H⁺) when dissolved in water.
Properties: Sour taste, turn blue litmus red, conduct electricity, react with metals to release hydrogen.
Examples: Hydrochloric acid (HCl), Sulfuric acid (H₂SO₄), Nitric acid (HNO₃).

Bases

Definition: Substances that release hydroxide ions (OH⁻) in water.
Properties: Bitter taste, slippery feel, turn red litmus blue, neutralize acids to form salt and water.
Examples: Sodium hydroxide (NaOH), Potassium hydroxide (KOH).

Salts

Definition: A product of the reaction between an acid and a base.
Formation:

HCl+NaOH→NaCl+H2OHCl+NaOH→NaCl+H2O (Sodium chloride is formed).

Types of Salts:

Normal Salts: Completely neutralized acids (e.g., NaCl).
Acidic Salts: Formed by partial neutralization (e.g., NaHSO₄).
Basic Salts: Formed by partial neutralization of a base (e.g., Fe(OH)₂SO₄).

pH Scale

Measures the acidity or basicity of a solution (scale 0 to 14).
- pH = 7: Neutral (pure water).
- pH < 7: Acidic (e.g., lemon juice, vinegar).
- pH > 7: Basic (e.g., soap solution, NaOH).

Neutralization

The reaction between an acid and a base to form salt and water.

Example: HCl+NaOH→NaCl+H2OHCl+NaOH→NaCl+H2O

Chapter 3: Metals and Non-Metals

Chapter 1: Chemical Reactions and Equations

Chapter 1: Chemical Reactions and Equations ATOM BOMB

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Chapter 1: Chemical Reactions and Equations

What is a Chemical Reaction?

A chemical reaction is a process where reactants transform into products, accompanied by energy changes. These changes can be observed as:

Change in color: (e.g., burning of magnesium ribbon).
Formation of a precipitate: (e.g., mixing of solutions of barium chloride and sodium sulfate).
Evolution of gas: (e.g., reaction between acids and metals).
Change in temperature: (e.g., combustion of fuels).

Types of Chemical Reactions

Combination Reaction: Two or more substances combine to form a single product.
- Example:

2H2+O2→2H2O2H2+O2→2H2O (Hydrogen combines with oxygen to form water).

Decomposition Reaction: A single reactant breaks down into two or more products.
- Example:

2KClO3→2KCl+3O22KClO3→2KCl+3O2 (Potassium chlorate decomposes into potassium chloride and oxygen).

Displacement Reaction: A more reactive element displaces a less reactive one from its compound.
- Example:

Zn+CuSO4→ZnSO4+CuZn+CuSO4→ZnSO4+Cu (Zinc displaces copper from copper sulfate).

Double Displacement Reaction: The ions of two compounds exchange to form new compounds.
- Example:

NaCl+AgNO3→NaNO3+AgClNaCl+AgNO3→NaNO3+AgCl (Formation of silver chloride from sodium chloride and silver nitrate).

Redox Reactions: Simultaneous oxidation and reduction processes. Example: 2Na+Cl2→2NaCl2Na+Cl2→2NaCl (Sodium is oxidized, chlorine is reduced).

Balancing Chemical Equations

Law of Conservation of Mass: Matter is neither created nor destroyed in a chemical reaction. The mass of reactants equals the mass of products.
Steps to Balance Equations:
- Count the number of atoms of each element on both sides.
- Add coefficients to balance the number of atoms.

Energy in Reactions

Exothermic Reactions: Release energy (usually heat). Example: C+O2→CO2C+O2→CO2
Endothermic Reactions: Absorb energy (usually heat). Example: Photosynthesis in plants: