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 → Matter and its properties ↓


Physical and chemical properties of matter


Matter is everything that has mass and occupies space. Everything around us is made of matter, whether it is solid, liquid or gas. To understand how matter behaves and interacts with other types of matter, it is important to know about its properties. These properties can be classified into two main types: physical properties and chemical properties.

Physical properties of matter

Physical properties are characteristics of matter that can be observed or measured without changing the substance's composition or identity. These properties are more about the appearance or state of matter. Here are some important physical properties with examples and visual explanations:

1. Colour

The color of a substance is a physical property because it can be observed without any change in the substance. For example, sulfur is yellow, while copper is reddish-brown. You can visualize this concept like this:

2. Smell

A substance can be quickly identified by its smell. For example, hydrogen sulfide is known to smell like rotten eggs. Like color, smell can also be identified without changing the substance.

3. Density

Density is the mass per unit volume of a substance. It is calculated using the formula:

Density = Mass / Volume

Gold has a very high density, so it feels heavier than the same size piece of aluminum. Imagine a small piece of gold and a large piece of aluminum. The gold will still weigh more.

4. Melting point and boiling point

These points represent the temperatures at which a substance changes its state. The melting point is where a solid becomes a liquid, and the boiling point is where a liquid turns into a gas.

Solid Gas Melting point Boiling point

5. Solubility

Solubility is the ability of a substance to dissolve in a solvent. For example, sugar is soluble in water, while sand is not.

Example: Dissolving a teaspoon of salt in a glass of water shows the solubility of salt in water.

6. Rigidity

This property measures a material's resistance to scratching. Diamonds are highly valued because of their hardness.

7. Electrical conductivity

The ability of a substance to conduct electricity. Metals such as copper and aluminum are good conductors.

Chemical properties of matter

Chemical properties describe the ability of a substance to undergo a specific chemical change. Seeing these properties often means that the substance has changed into something else. Here are some essential chemical properties:

1. Reactivity

It determines how a substance reacts with other substances. For example, sodium reacts explosively with water, while gold does not react with water at all.

reactive substance

2. Flammability

The ability of a substance to burn in the presence of oxygen. Gasoline is highly flammable, while water is not.

3. pH

This property tells how acidic or alkaline a substance is. Lemon juice has a low pH, which makes it acidic, while soap has a high pH, which makes it alkaline.

4. Combustion

The process of burning can be a chemical property that results in the emission of heat and light. The combustion of methane is a classic example of this:

CH4 + 2O2 → CO2 + 2H2O + energy

5. Corrosion

This property refers to the gradual destruction of substances, usually metals, by chemical reactions with environmental elements, such as oxygen. An example of this is the rusting of iron.

Comparison of physical and chemical properties

Understanding the difference between these two types of properties is essential to predict the behavior of matter under different conditions. For example, physical properties can be used to identify substances without changing their nature, while chemical properties can predict how a substance will react with others.

Identifying a substance often requires observing both physical and chemical properties. For example, to identify an unknown metal, you could measure its density (a physical property) and then test its reactivity with acids (a chemical property).

Conclusion

Understanding the physical and chemical properties of matter helps us describe, classify and predict how different substances interact and change. This fundamental knowledge is vital for further studies in chemistry and helps solve practical problems in engineering, environmental science and everyday life. By recognising these properties, we can harness the true potential of different materials, contributing to scientific progress and technological innovation.


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States of matter
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Physical and chemical properties of matter

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