Grade 7
  1. Introduction to Chemistry  1.1. What is Chemistry?  1.2. Importance of chemistry in daily life  1.3. Branches of chemistry  1.4. Scientific Method in Chemistry  1.5. Laboratory Safety Rules and Precautions  1.6. Common Laboratory Equipment and Their Uses  1.7. Units of measurement in chemistry
  2. Matter and its properties  2.1. Definition of Matter  2.2. Classification of matter  2.3. Properties of matter  2.3.1. Physical properties  2.3.2. Chemical properties  2.4. States of matter  2.4.1. Solid state  2.4.2. Fluid state  2.4.3. Gaseous state  2.4.4. Plasma and Bose–Einstein condensates  2.5. Changes in the states of matter  2.5.1. Melting and freezing  2.5.2. Evaporation and Condensation  2.5.3. Sublimation and deposition  2.6. Density and its applications  2.7. Diffusion and its importance
  3. Elements, Compounds, and Mixtures  3.1. Definition of the element  3.2. Classification of elements  3.3. Metals, Nonmetals and Metalloids  3.4. Noble gases and their properties  3.5. Introduction to the Periodic Table  3.6. Definition of Compound  3.7. Properties of Compounds  3.8. Introduction to Chemical Formulas  3.9. Definition of Mixture  3.10. Types of mixtures  3.10.1. Homogeneous mixture  3.10.2. Heterogeneous mixtures  3.11. Difference Between Compounds and Mixtures  3.12. Solutions, Colloids and Suspensions
  4. Separation of mixtures  4.1. Need for separation of mixtures  4.2. Separation methods  4.2.1. Filtration  4.2.2. Sedimentation and decantation  4.2.3. Evaporation  4.2.4. Crystallization  4.2.5. Distillation  4.2.6. Chromatography  4.2.7. Magnetic Separation  4.2.8. Centrifugation
  5. Atomic Structure  5.1. Introduction to Atoms  5.2. Structure of the atom  5.2.1. Nucleus and electron cloud  5.3. Subatomic particles  5.3.1. Proton  5.3.2. Neutron  5.3.3. Electrons  5.4. Atomic number and mass number  5.5. Isotopes and their uses  5.6. Ions and ion formation
  6. Periodic table  6.1. Introduction to the Periodic Table  6.2. Groups and periods  6.3. Trends in the Periodic Table  6.3.1. Atomic Size  6.3.2. Metallic and non-metallic character  6.3.3. Electronegativity  6.3.4. Reactivity of the elements  6.4. Alkali metals and their properties
  7. Chemical bond  7.1. Why do atoms form bonds?  7.2. Types of chemical bonds  7.2.1. Ionic bond  7.2.2. Covalent bond  7.2.3. Metal Bond  7.3. Properties of Ionic and Covalent Compounds  7.4. Intermolecular forces
  8. Chemical reactions  8.1. Introduction to Chemical Reactions  8.2. Signs of a chemical reaction  8.3. Types of Chemical Reactions  8.3.1. Combination Reactions  8.3.2. Decomposition reactions  8.3.3. Displacement reactions  8.3.4. Double displacement reactions  8.3.5. Combustion reactions  8.4. Law of conservation of mass  8.5. Balancing simple chemical equations
  9. Acids, Bases and Salts  9.1. Definition of Acid and Base  9.2. Properties of Acids  9.3. Properties of bases  9.4. pH Scale and Indicators  9.5. Neutralization reactions  9.6. Common Acids and Bases in Everyday Life  9.7. Preparation and use of salts  9.8. Strong and weak acids and bases
  10. Solutions and Solubility  10.1. Definition of Solution  10.2. Components of the solution  10.2.1. Solvent  10.2.2. solute  10.3. Factors Affecting Solubility  10.4. Concentration of solutions  10.5. Saturated and unsaturated solutions  10.6. Colloids and suspensions  10.7. Solubility curve and its interpretation
  11. Air and atmosphere  11.1. Composition of air  11.2. Properties of gases in the air  11.3. Importance of Oxygen and Carbon Dioxide  11.4. Air pollution and its effects  11.5. Greenhouse effect and global warming  11.6. Ways to reduce air pollution  11.7. Ozone layer and its importance
  12. Water and its importance  12.1. Properties of Water  12.2. Water as the universal solvent  12.3. Importance of water for life  12.4. Water pollution and its effects  12.5. Water Purification  12.5.1. Filtration  12.5.2. boil  12.5.3. Chlorination in water purification  12.5.4. reverse osmosis  12.6. Hard and soft water  12.7. Water cycle and its importance
  13. Fuel and energy  13.1. Types of fuel  13.1.1. Fossil fuels  13.1.2. Renewable energy sources  13.2. Combustion and energy release  13.3. Global warming and its effects  13.4. Alternative sources of energy  13.5. Ways to conserve energy
  14. Metals and Nonmetals  14.1. Physical and chemical properties of metals  14.2. Physical and Chemical Properties of Non-Metals  14.3. Difference Between Metals and Nonmetals  14.4. Uses of metals and nonmetals  14.5. Corrosion of metals and its prevention  14.6. Alloys and their importance
  15. Plastics and polymers  15.1. Natural and synthetic polymers  15.2. Properties of plastics  15.3. Biodegradable and Non-Biodegradable Plastics  15.4. Environmental impact of plastic  15.5. Recycling and waste management in plastics and polymers  15.6. Daily Uses of Polymers
  16. Introduction to Organic Chemistry  16.1. Basic definitions of organic chemistry  16.2. Carbon Compounds in Daily Life  16.3. Hydrocarbons  16.4. Simple functional groups (alcohols and carboxylic acids)  16.5. Importance of organic compounds in industry

Grade 7 ↓


Introduction to Chemistry


What is chemistry?

Chemistry is a branch of science that studies matter, its properties, the way it interacts, combines, and changes. Chemistry helps us understand the world around us and is often referred to as the "central science" because it connects the physical sciences with the life sciences and applied sciences.

What is the matter?

Matter is anything that has mass and takes up space. Everything around you is made of matter. You can hold it in your hands, see it with your eyes, or even smell it with your nose.

Case occupies space

Imagine a wooden chair. The chair is made of matter. It has mass, so it feels heavy when you try to pick it up. It takes up space because you can't walk over it.

States of matter

Matter can exist in different states. The three most common states of matter are solid, liquid, and gas. Each state has its own distinct properties.

Solid

Solids have definite shape and volume. The particles in solids are tightly bound to each other and move very little.

Solid particles

Liquid

Liquids have a fixed volume but take the shape of their container. The particles in a liquid are close to each other but can move freely.

Liquid particles

Gas

Gases have no definite shape or volume. Gas particles are far away from each other and move very fast.

Gas particles

Elements, compounds, and mixtures

All substances are made up of elements, compounds, or mixtures. Let's learn about each one.

Elements

An element is a pure substance that cannot be broken down into simpler substances by chemical means. Elements are made up of only one type of atom.

H is the chemical symbol for hydrogen, and O is the chemical symbol for oxygen.

Compounds

A compound is a pure substance made from two or more different elements that are chemically combined. Compounds contain a fixed ratio of elements.

For example, water is a compound made of hydrogen and oxygen. Its chemical formula is:

H 2 O

Mixture

A mixture is a combination of two or more substances that are not chemically combined. Mixtures can be separated by physical means.

Sand and salt when mixed together form a mixture, as they can be easily separated by adding water and filtering.

Atoms and molecules

Atoms are the basic building blocks of matter. They are the smallest units of an element that retain the properties of that element.

Atom

Molecules are groups of two or more atoms that are linked together. They can be made of the same type of atom or different types of atoms. For example, the air we breathe contains oxygen in the form of molecules.

O 2

This represents two oxygen atoms bonded together.

Chemical reactions

Chemical reactions occur when substances interact to form new substances. In a chemical reaction, the atoms in the reactants rearrange to form different molecules in the products.

An example of a simple chemical reaction is the reaction between hydrogen and oxygen to form water:

2H 2 + O 2 → 2H 2 O

In this reaction, two molecules of hydrogen gas react with one molecule of oxygen gas to form two molecules of water.

Periodic table

The periodic table is a chart that arranges all known elements based on their properties. It is structured in such a way that it predicts the properties of the elements and their compounds.

Periodic table

Each box on the periodic table represents an element with its symbol, atomic number, and atomic mass. Elements are arranged in rows called periods and columns called groups based on similar properties.

Acids and bases

Acids and bases are two special types of chemicals. Nearly all liquids are acids or bases to some degree. Acidic substances taste sour and can be corrosive. Basic substances, also called alkalis, taste bitter and feel slippery.

A common acid is hydrochloric acid, HCl, and a common base is sodium hydroxide, NaOH.

Conclusion

Chemistry is a fascinating and amazing field that touches every part of our lives. It helps us understand how different substances come together, react and change to form new substances. By studying chemistry, we gain a better understanding of the world around us and how matter behaves.


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Introduction to Chemistry

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