Grade 9
  1. Matter and its nature  1.1. Introduction to matter  1.2. Physical and chemical properties of matter  1.3. States of matter  1.3.1. Solid state  1.3.2. Fluid state  1.3.3. Gaseous state  1.3.4. Plasma and Bose–Einstein condensate  1.4. Changes in the states of matter  1.4.1. Melting and freezing  1.4.2. Evaporation and Condensation  1.4.3. Sublimation and deposition  1.5. Classification of matter  1.6. Elements, Compounds, and Mixtures  1.7. Pure substances and impurities  1.8. Separation Techniques  1.8.1. Filtration  1.8.2. Distillation  1.8.3. Crystallization  1.8.4. Chromatography  1.8.5. Centrifugation  1.8.6. Sublimation  1.8.7. Decantation and sedimentation
  2. Atomic Structure  2.1. Discovery of atoms  2.2. Dalton's atomic theory  2.3. Structure of the atom  2.4. Subatomic particles  2.5. Atomic number and mass number  2.6. Isotopes and Isobars  2.7. Electronic configuration  2.8. Bohr's atomic model  2.9. Modern Atomic Model (Quantum Mechanical Model - Introduction)  2.10. Valency and chemical bonding
  3. C hemical reactions and equations  3.1. Introduction to Chemical Reactions  3.2. Chemical Equation Formulation  3.3. Balancing Chemical Equations  3.4. Types of Chemical Reactions  3.4.1. Combination Reactions  3.4.2. Decomposition reactions  3.4.3. Displacement reactions  3.4.4. Double displacement reactions  3.4.5. Redox reactions  3.4.6. Endothermic and Exothermic Reactions  3.5. Effects of chemical reactions  3.6. Energy Changes in Chemical Reactions  3.7. Catalysts and their role in reactions
  4. Periodic table and periodicity  4.1. History of Periodic Classification  4.2. Mendeleev's periodic table  4.3. Modern Periodic Table  4.4. Periods and groups in the periodic table and periodicity  4.5. Trends in the Periodic Table  4.5.1. Atomic size  4.5.2. Ionization Energy  4.5.3. Electron affinity  4.5.4. Electronegativity  4.5.5. Metallic and Non-Metallic Properties  4.6. Noble gases and their properties
  5. Chemical bond  5.1. Introduction to Chemical Bonding  5.2. Types of chemical bonds  5.2.1. Ionic bond  5.2.2. Covalent bond  5.2.3. Metallic bond  5.2.4. Hydrogen bonding  5.2.5. Van der Waals force  5.3. Properties of Ionic and Covalent Compounds  5.4. Molecular Structure and Geometry (VSEPR Theory - Basics)
  6. Acids, Bases and Salts  6.1. Introduction to Acids and Bases  6.2. Properties of Acids  6.3. Properties of bases  6.4. pH scale and its importance  6.5. Indicators and their uses  6.6. Neutralization reactions  6.7. Strength of Acids and Bases (Strong vs. Weak)  6.8. Preparation of salts  6.9. Uses of acids, bases and salts in daily life
  7. Metals and Nonmetals  7.1. Physical Properties of Metals  7.2. Physical Properties of Nonmetals  7.3. Chemical properties of metals  7.4. Chemical Properties of Nonmetals  7.5. Reactivity Series of Metals  7.6. Extraction of metals  7.7. Corrosion and its prevention  7.8. uses of metals and nonmetals
  8. Carbon and its compounds  8.1. Introduction to Carbon  8.2. Allotropes of carbon (diamond, graphite, fullerene)  8.3. Hydrocarbons  8.3.1. Hydrocarbons  8.3.2. Alkene  8.3.3. Alkynes  8.4. Functional groups in organic chemistry  8.5. Isomerism in organic compounds  8.6. Alcohols and Carboxylic Acids  8.7. Soaps and detergents  8.8. Polymers (Introduction to Natural and Synthetic Polymers)
  9. Solutions and Mixtures  9.1. Types of mixtures  9.2. Homogeneous and Heterogeneous Mixtures  9.3. Concentration of solutions  9.4. Solubility and factors affecting solubility  9.5. Suspensions and Colloids  9.6. Saturated, unsaturated and supersaturated solutions
  10. Air and atmosphere  10.1. Composition of air  10.2. Role of gases in the atmosphere  10.4. Acid rain and its effects  10.5. Greenhouse effect and global warming  10.6. Ozone layer and its depletion  10.7. Air pollution control measures
  11. Water and its importance  11.1. Composition and properties of water  11.2. Hardness of water (temporary and permanent hardness)  11.3. Causes of water pollution  11.4. Effects of Water Pollution  11.5. Water purification methods (filtration, boiling, chlorination)
  12. Industrial Chemistry  12.1. Introduction to Industrial Chemistry  12.2. Important industrial chemicals (sulfuric acid, ammonia, sodium hydroxide)  12.3. Chemical processes in industry  12.4. Uses of Industrial Chemistry in Daily Life  12.5. Environmental impact of industrial chemical processes

Grade 9 → Matter and its nature ↓


Physical and chemical properties of matter


Introduction

Matter is everything that has mass and occupies space. Everything around us is made up of matter, be it the air we breathe or the food we eat. Understanding the properties of matter is very important in the study of chemistry. Broadly, the properties of matter can be classified into physical and chemical properties. In this discussion, we will explore both these categories and their importance in understanding the nature of matter.

Physical properties of matter

Physical properties are characteristics that can be seen or measured without changing the composition of matter. These properties help us identify and classify substances. Physical properties include color, odor, density, melting point, boiling point, and physical state (solid, liquid, gas).

Situation of affairs

Matter exists in different states: solid, liquid, and gas. These states are the physical properties of matter.

  • Solid: It has definite shape and volume. The particles are close to each other and have very little freedom to move.
  • Liquid: It has a definite volume but no definite shape. Liquids take the shape of their container. The particles are loose and can move around.
  • Gas: It has neither a definite shape nor volume. Gases expand to fill the available space. The particles are far apart and move around freely.
SolidLiquidGas

Density

Density is the mass of a substance per unit volume. It is an important physical property that determines whether a substance will float or sink when placed in a fluid. Density is represented mathematically as:

Density (D) = Mass (M) / Volume (V)

For example, the density of water is about 1 g / cm3. Iron, which has a higher density than water, will sink, while oil, which has a lower density, will float on water.

Melting and boiling point

The melting point of a substance is the temperature at which it changes from a solid to a liquid, while the boiling point is the temperature at which it changes from a liquid to a gas. These points are unique to each substance and are used for identification.

Color and smell

Color and odor are obvious physical properties. For example, oxygen is colorless and odorless. Chlorine, on the other hand, is a yellow-green gas with a pungent odor.

Chemical properties of matter

Chemical properties describe the ability of a substance to undergo chemical change. These properties can only be observed during a chemical reaction. Chemical properties include reactivity with other substances, flammability, and acidity.

Jet

Reactivity refers to the nature of a substance to react chemically with other substances. For example, sodium reacts vigorously with water, while gold does not. Here is a simple chemical reaction of sodium with water:

2Na + 2H2O → 2NaOH + H2↑

Flammability

Flammability is the ability of a substance to burn or ignite, causing fire or combustion. Many substances, such as alcohol, gasoline, and natural gas, are highly flammable.

Combustion

Acidity and alkalinity

Acidity and alkalinity refer to a substance's ability to donate or accept protons (H+ ions). Acids such as hydrochloric acid (HCl) have a sour taste and can corrode metals, while bases such as sodium hydroxide (NaOH) feel slippery and are used in cleaning agents.

Importance of physical and chemical properties

Understanding these properties helps scientists and engineers predict behavior and select materials for specific applications. For example:

  • Material selection: Engineers select materials based on physical properties such as tensile strength and thermal conductivity.
  • Safety: Knowing chemical properties, such as reactivity, helps handle chemicals safely.
  • Environmental effects: Chemical properties determine how substances interact with the environment, and affect pollution management and waste disposal.

Conclusion

Understanding physical and chemical properties is essential to the practical application of chemistry. These properties enable us to characterize substances, predict their behavior, and use them effectively in science and industry. By understanding both the visible and intrinsic properties of matter, we broaden our abilities to innovate and solve everyday challenges.


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Physical and chemical properties of matter

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