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 Organic Chemistry


Welcome to the fascinating world of organic chemistry! You may be wondering what organic chemistry is and why it is important. This subject focuses on the study of carbon-based compounds, which make up all living things and many substances we use every day. Let's find out what organic chemistry is.

What is organic chemistry?

Organic chemistry is the branch of chemistry that deals with the study of compounds containing carbon. Carbon is a very special element because it can form stable bonds with many elements, including itself. This allows carbon to form many more compounds than any other element. Compounds in organic chemistry contain primarily carbon and hydrogen, but they may also contain other elements such as oxygen, nitrogen, sulfur, and halogens.

Why is carbon important?

Carbon is the backbone of organic chemistry for a few reasons. First, carbon atoms can form up to four covalent bonds with other atoms. This property allows carbon to form many complex structures, including chains and rings. Secondly, carbon-carbon bonds are strong and stable, making them ideal for building complex molecules.

Here's the simplified structure of methane, one of the simplest organic molecules:

    CH₄

Methane has one carbon atom bonded to four hydrogen atoms.

C H H H H

Key concepts in organic chemistry

Hydrocarbons

Hydrocarbons are the simplest organic compounds and contain only carbon and hydrogen. They are divided into several types depending on their structure:

  • Alkanes: These hydrocarbons have only single bonds between carbon atoms. These are also known as saturated hydrocarbons. Example: C₂H₆ (ethane)
  • Alkenes: These hydrocarbons have at least one double bond between carbon atoms. Example: C₂H₄ (ethylene)
  • Alkynes: These hydrocarbons have at least one triple bond between carbon atoms. Example: C₂H₂ (acetylene)

Functional group

Functional groups are specific groups of atoms within molecules that are responsible for specific chemical reactions of those molecules. Here are some common functional groups:

  • Alcohol: Contains -OH group. Example: CH₃OH (methanol)
  • Carboxylic acid: It contains -COOH group. Example: CH₃COOH (acetic acid)
  • Aldehyde: Contains -CHO group. Example: CH₃CHO (acetaldehyde)
  • Ketone: It contains C=O group. Example: CH₃COCH₃ (acetone)

Representation of organic molecules

Organic molecules can be represented in a variety of ways, including:

  • Molecular formula: Shows the number and type of atoms. Example: C₂H₆
  • Structural formula: This shows how the atoms are arranged and connected to each other. Example of ethane:
    HH
     ,
      C - C
     ,
    HH
  • Line-angle (skeletal) formula: Simplified representation, where each vertex represents a carbon atom.

Isomers

Isomers are compounds that have the same molecular formula but different structures. This difference in structure can lead to different properties. There are two main types of isomers:

  • Structural isomers: differ in the order in which atoms are joined. Example: C₄H₁₀ can be butane or isobutane.
  • Stereoisomers: atoms are connected in the same order but differ in spatial arrangement.

Reactions in organic chemistry

Organic chemistry involves many types of reactions. Some common reactions are as follows:

  • Substitution reactions: One atom or group of atoms in a molecule is replaced by another.
  • Addition reactions: atoms add to double or triple bonds in a molecule.
  • Elimination reactions: Removal of atoms from a molecule, often leading to the formation of a double bond.

Applications of organic chemistry

The study of organic chemistry is important to many industries and applications:

  • Pharmaceuticals: Organic chemistry is essential in the manufacture of drugs and medicines.
  • Plastics: Many plastics and polymers are made from organic compounds.
  • Fuel: Hydrocarbons are the main components of fuels such as gasoline and natural gas.

Conclusion

Organic chemistry is a vast and exciting field that touches many aspects of everyday life. From the food we eat to the medicines we take, organic chemistry is everywhere. Understanding the basics of organic chemistry provides a foundation for exploring more complex topics and discovering the remarkable chemistry of life.

Thank you for this journey into the world of organic chemistry!


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Introduction to Organic Chemistry

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