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 ↓


Introduction to matter


Matter is all around us. Everything you can see, touch and feel is made of matter. For example, the phone or computer you are using to read this, the food you eat and even the air you breathe are all forms of matter. In this introduction, we will explore what matter is, how it behaves and why it is important to our world and to our understanding of chemistry.

What is the matter?

Matter is everything that has mass and occupies space. It is made up of tiny particles called atoms. Atoms are the basic building blocks of all matter. They are so small that they cannot be seen with ordinary microscopes, but they make up everything around us.

Atom

States of matter

There are three primary states of matter - solid, liquid and gas. Let us discuss each of them.

Solids

The particles in solids are tightly packed together in a certain structure. This means that solids have a definite shape and volume. An example of a solid is a piece of rock or ice.

Solid

Liquids

The particles in fluids are not as tightly packed as those in solids. They can move past one another, allowing fluids to flow and take the shape of their container, although they have a fixed volume. Examples of fluids are water and oil.

Liquid

Gases

The particles in gases are far apart and move around freely. Gases have no definite shape or volume. An example of a gas is the air we breathe, which contains gases such as oxygen and nitrogen.

Gas

Change in state of matter

Matter can change from one state to another when heated or cooled. These changes are called physical changes and include melting, freezing, evaporation, condensation, and sublimation.

Melting: Change from a solid to a liquid. Example: Ice melting into water.

Freezing: Change from a liquid to a solid. Example: Water freezing into ice.

Vaporization: Change from a liquid to a gas. This includes both boiling and evaporation.

Condensation: Change from a gas to a liquid. Example: Formation of water droplets on a cold surface.

Sublimation: Change from solid state to gas state directly, without going through the liquid state. Example: Dry ice changing into carbon dioxide gas.

Chemical composition of the substance

In addition to the physical state, matter can also be classified based on its chemical composition. There are two main types: elements and compounds.

Elements

Elements are pure substances made up of only one type of atom. Each element is unique and is represented on the periodic table. Examples include hydrogen (H), oxygen (O), and gold (Au).

Gold (Australia)

Compounds

Compounds are substances made up of two or more different types of atoms. Compounds have properties that differ from the individual elements they are made of. A common example of a compound is water (H2O), which is made up of hydrogen and oxygen.

Water (H2O)

Mixture

In addition to elements and compounds, substances can also exist as mixtures. A mixture is a combination of two or more substances where each substance maintains its chemical identity. There are two types of mixtures: homogeneous and heterogeneous mixtures.

Homogeneous mixture

Homogeneous mixtures have the same composition. Often, these are solutions. An example of this is salt water, where the salt is evenly distributed throughout the water.

Heterogeneous mixtures

Heterogeneous mixtures have uneven structure, meaning that different parts of the mixture can be seen. An example of this would be a salad, where you can see and identify the different ingredients.

Physical and Chemical Properties

Every substance has properties that help identify or describe it. These properties are classified into physical properties and chemical properties.

Physical properties

These are characteristics that can be seen or measured without changing the matter into another substance. Examples include color, melting point, boiling point, and density.

Chemical properties

These describe the ability of a substance to undergo a particular chemical change. Examples include reactivity with acids, flammability, and the ability to rust.

Conclusion

Understanding matter and its nature is essential, as it is the basic foundation of chemistry. Matter makes up everything in the universe, from the smallest atoms to the vastness of galaxies. By studying matter, scientists can unravel the mysteries of how substances interact, change, and create the world we experience. Keep the basic concepts of matter in mind as you progress in chemistry, as they will serve as important building blocks for more complex topics.


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Introduction to matter

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