Grade 8
  1. Introduction to Chemistry  1.1. Nature and scope of chemistry  1.2. Importance of chemistry in daily life  1.3. Chemistry and its relation with other sciences  1.4. The role of chemistry in industry, medicine and the environment  1.5. Scientific investigation and experimental methods in chemistry
  2. Matter and its properties  2.1. Definition and classification of matter  2.2. Physical and chemical properties of matter  2.3. Law of conservation of matter  2.4. Extensive and Intensive Properties of Matter  2.5. Kinetic molecular theory of matter  2.6. States of matter: solids, liquids, gases, plasmas, and Bose-Einstein condensates  2.7. Changes in state and energy are involved  2.8. Diffusion and Brownian motion
  3. Elements, Compounds, and Mixtures  3.1. Definition and differences between elements, compounds, and mixtures  3.2. Atomic Structure and Atomic Number  3.3. Chemical symbols and formulas  3.4. Trends in the Periodic Table (Groups and Periods)  3.5. Classification of Elements: Metals, Nonmetals and Metalloids  3.6. Rare Earth Elements and Transition Metals  3.7. Types of mixtures: homogeneous and heterogeneous  3.8. Separation of Mixtures Using Physical and Chemical Methods
  4. Separation Techniques  4.1. Filtration, Sedimentation and Decantation  4.2. Evaporation and crystallization  4.3. Distillation and Fractional Distillation  4.4. Chromatography and its applications  4.5. Sublimation in the purification of compounds  4.6. The role of centrifugation in biochemical processes
  5. Atomic Structure  5.1. Dalton's atomic theory  5.2. Structure of the atom: protons, neutrons and electrons  5.3. Bohr's atomic model  5.4. Introduction to Quantum Mechanical Model  5.5. Electron Configuration and Energy Levels  5.6. Excitation and emission spectra  5.7. Isotopes and their applications
  6. Periodic Table and Chemical Trends  6.1. History and Development of the Periodic Table  6.2. Modern periodic law  6.3. Periodicity and trends in atomic and ionic sizes  6.4. Ionization Energy, Electron Affinity and Electronegativity  6.5. Introduction to Lanthanides and Actinides  6.6. Application of periodic trends in chemistry
  7. Chemical Bonding and Molecular Structure  7.1. Types of chemical bonds: ionic, covalent and metallic bonds  7.3. Polar and Nonpolar Molecules  7.4. Hydrogen bonding and its applications  7.5. Intermolecular forces: dipole-dipole, London dispersion force
  8. Chemical Reactions and Stoichiometry  8.1. Chemical Equations and Balance  8.2. Types of Chemical Reactions: Combination, Decomposition, Displacement and Redox  8.3. Introduction to stoichiometry and the mole concept  8.4. Limiting reactant in chemical equations  8.5. Reaction rate, catalyst, and factors affecting reaction rate
  9. Acids, Bases and Salts  9.1. Definition and Properties of Acids and Bases  9.2. Strong vs. Weak Acids and Bases  9.3. pH Scale and pH Calculation  9.4. Neutralization reactions  9.5. Buffer solutions and their importance  9.6. Applications of Acids, Bases and Salts in Daily Life
  10. Solutions and Solubility  10.1. Definition of Solution, Solute, and Solvent  10.2. Factors Affecting Solubility  10.3. Concentration units: molarity and molality  10.4. Saturated, unsaturated and supersaturated solutions  10.5. Concept of osmosis and reverse osmosis  10.6. Concentrative properties of solutions
  11. Gases and Gas Laws  11.1. Properties of gases  11.2. Introduction to Ideal and Real Gases  11.3. Boyle's Law, Charles' Law and Avogadro's Law  11.4. Ideal Gas Equation and Its Applications  11.5. Application of Gas Laws in Real Life
  12. Thermochemistry and energy transformation  12.1. Energy in Chemical Reactions  12.2. Exothermic vs. Endothermic Reactions  12.3. Heat and Enthalpy Changes  12.4. Calorimetry and heat transfer in reactions
  13. Metals and Nonmetals  13.1. Physical and Chemical Properties of Metals and Nonmetals  13.2. Reactivity Series of Metals  13.3. Corrosion and its prevention  13.4. Extraction of metals from ores  13.5. Uses of metals and non-metals in daily life
  14. Introduction to Organic Chemistry  14.1. Characteristics of carbon and organic compounds  14.2. Functional groups and their importance  14.3. Simple Hydrocarbons: Alkenes, Alkenes and Alkynes  14.4. Isomerism in organic compounds  14.5. Introduction to polymers and their uses
  15. Environmental Chemistry and Sustainability  15.1. Green Chemistry Principles  15.2. Effects of Chemical Pollution on Ecosystems  15.3. Acid rain and its effects  15.4. Ozone layer depletion and global warming  15.5. Waste Management and Recycling in Chemistry

Grade 8 → Introduction to Chemistry ↓


Nature and scope of chemistry


Chemistry is often called the "central science" because it connects the physical sciences to the life sciences and applied sciences. It is important in everyday life and serves as the backbone for many scientific fields, including biology, medicine, engineering, and environmental science. Understanding basic chemistry concepts is important for developing scientific literacy and solving problems related to the environment, energy, and health.

What is chemistry?

Chemistry is the scientific study of matter, its properties, and its behavior with other substances. Matter is everything that has mass and occupies space. Chemistry involves investigating how atoms and molecules interact through chemical reactions, creating new substances with different properties.

Branches of chemistry

Chemistry is divided into several branches, each of which focuses on specific areas. Let's take a closer look at these branches:

Organic chemistry

This branch deals with the study of carbon-containing compounds. Organic chemistry is essential for understanding biological processes and is fundamental in fields such as pharmaceuticals and petrochemicals.

Methane: CH 4

Example of a simple organic molecule: methane (CH4)

Inorganic chemistry

Unlike organic chemistry, inorganic chemistry focuses on compounds that do not typically contain carbon. This includes minerals, metals, and other non-carbon-based materials.

Sodium Chloride: NaCl

Example of an inorganic compound: Sodium chloride (NaCl), commonly known as table salt.

Physical chemistry

This branch combines the principles of physics and chemistry. It studies how matter behaves at the molecular and atomic level, and how chemical reactions occur. Physical chemistry involves the study of reaction rates, energy changes, and properties of substances.

Analytical chemistry

Analytical chemistry involves analysing substances to determine their composition. It includes techniques for detecting, identifying and quantifying substances, which helps in quality control and assurance in industries.

Biochemistry

This branch studies the chemical processes within and related to living organisms. Biochemistry is important in understanding cellular and molecular biology, and it is the basis for advances in medical research.

Nature of chemical science

To fully understand the nature of chemistry, it is important to understand some basic concepts:

Atoms and molecules

Atoms are the basic units of matter. They are composed of a nucleus surrounded by electrons. Different elements are composed of different types of atoms. When atoms join together, they form molecules.

Atom

Periodic table

The periodic table organizes all known elements according to their properties. Each element has a unique atomic number, which is the number of protons in its nucleus.

Chemical bond

Chemical bonds are the forces that hold atoms together in a molecule. There are many types of bonds, the most common being ionic, covalent, and metallic bonds.

  • Ionic bond: It is formed when electrons transfer from one atom to another, creating positive and negative ions.
  • Covalent bonds: formed when atoms share electrons.
  • Metallic bonding: It involves the sharing of free electrons between lattices of metal atoms.

Chemical reactions

Chemical reactions occur when substances interact, resulting in the formation of new substances. Reactions can be classified into several categories such as synthesis, decomposition, single-replacement, and double-replacement reactions.

2H 2 + O 2 → 2H 2 O

Example of a chemical reaction: Formation of water by combining hydrogen and oxygen.

Scope of chemistry in everyday life

Chemistry is ubiquitous in everyday life. From the food we eat and the cleaning products we use to the medicines that keep us healthy, chemistry plays a vital role.

Food chemistry

This field explores the chemical nature of food and the changes it undergoes during processing and consumption. Understanding this helps enhance the taste and preserve food.

C 6 H 12 O 6 (Glucose) + 6O 2 → 6CO 2 + 6H 2 O + energy

Food chemistry example: Breakdown of glucose in cellular respiration.

Medicinal chemistry

This field involves the design and synthesis of medicines. Chemistry helps to understand diseases and develop medicines to fight them.

Environmental chemistry

Environmental chemistry focuses on the chemical processes that occur in the environment. It is important for studying pollution, finding sustainable solutions, and conserving resources.

Industrial chemistry

Chemistry is vital in manufacturing processes. From producing plastics to refining metals, industrial chemistry provides us with the materials we need for a variety of technologies.

Visual example via model

Let's look at some of these basic concepts with simple models:

Molecule model

The above model shows a diatomic molecule where two atoms are bonded together.

Water molecule

This model shows a water molecule (H2O) with one oxygen atom and two hydrogen atoms.

Conclusion

The nature and scope of chemistry provides a fascinating insight into the workings of the universe. By studying chemistry, we can understand the structure of substances, the forces that bind them, and the energy transformations involved. This allows us to innovate, protect our environment, improve health, and make positive contributions to society.


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Nature and scope of chemistry

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