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 ↓


Periodic table


The periodic table is a chart that arranges the elements in a way that highlights their common properties. This table allows scientists and students to quickly find and identify the chemical properties of different elements. Learning how to read and use the periodic table is an important step in learning chemistry.

What is an element?

Before delving into the periodic table, it is important to understand what an element is. An element is a substance that cannot be broken down into simpler substances by chemical means. Each element is made up entirely of one type of atom. For example, gold is an element, and a gold atom is the smallest unit of gold.

Structure of the periodic table

The periodic table is arranged in rows and columns. Each row is called a period, and each column is called a group or family. The elements are ordered in the table according to their atomic number, which is the number of protons in the nucleus of an atom.

Period

Horizontal rows of the periodic table. There are 7 periods in the periodic table. As you move from left to right in a period, the atomic number of the elements increases. This means that each element has one more proton than the element before it.

Group

Groups are vertical columns of the table. Elements in the same group tend to have similar chemical properties. This is because they have the same number of electrons in their outer shell, which is important for the way they react. For example, all of the elements in group 1 are known as the alkali metals and they are very reactive.

Metals, nonmetals, and metalloids

Elements can also be classified into three main categories: metals, nonmetals, and metalloids.

  • Metals: Located on the left side of the periodic table. They are generally shiny, good conductors of electricity, and malleable.
  • Nonmetals: Found on the right side of the periodic table. They have opposite properties to metals, such as being poor conductors of electricity.
  • Metalloids: These elements have properties of both metals and nonmetals and can be found along the zig-zag line in the periodic table.

Understanding element information

Each element in the periodic table is represented by a symbol, usually one or two letters. You'll also find other information for each element, such as its atomic number, atomic mass, and sometimes its electron configuration.

Examples: Hydrogen

Let's take a closer look at the element hydrogen:

H
Atomic Number: 1 Atomic Mass: 1.008

Hydrogen is the first element in the periodic table. Its atomic number is 1 and atomic mass is about 1.008. Its symbol is "H".

Interactive example with SVG

Hydrogen Symbol: H Atomic Number: 1 Atomic mass: 1.008

Importance of periodic table

The periodic table is an important tool for scientists because it organizes all the known elements in an informative way. It helps chemists understand why different elements react in a certain way and helps predict how they will interact with other elements.

Chemical reactions

The most important use of the periodic table is to understand chemical reactions. Elements react with each other to form new compounds, and the way different elements react depends on their position in the periodic table. For example, elements in group 1 (such as sodium) react vigorously with water.

Example: Sodium and water reaction

When sodium (Na), a Group 1 element, comes in contact with water, it reacts to form sodium hydroxide (NaOH) and hydrogen gas (H 2).

2 Na + 2 H 2 O → 2 NaOH + H 2

Conclusion

Although this is just a simple introduction to the periodic table, the concepts covered here lay the groundwork for more advanced studies in chemistry. By understanding the structure of each element and the information it contains, students can begin to predict chemical properties and reactions, developing a deeper understanding and appreciation of the world around them.


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Periodic table

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