Topics
Some Basic Concepts of Chemistry
- Introduction of Some Basic Concepts of Chemistry
- Nature of Chemistry
- Properties of Matter and Their Measurement
- Laws of Chemical Combination
- Dalton's Atomic Theory
- Atomic and Molecular Masses
- Mole Concept
- Moles and Gases
Introduction to Analytical Chemistry
- Introduction of Analytical Chemistry
- Analysis
- Mathematical Operation and Error Analysis
- Determination of Molecular Formula
- Chemical Reactions and Stoichiometric Calculations
- Limiting Reagent
- Concentration of a Solution
- Use of Graph in Analysis
Basic Analytical Techniques
- Introduction of Some Analytical Techniques
- Purification of Solids
- Crystallisation Method
- Fractional Crystallization
- Simple Distillation Method
- Solvent Extraction
- Chromatography Method
- Adsorption Chromatography
- Partition Chromatography
Structure of Atom
- Subatomic Particles
- Atomic Number and Atomic Mass Number
- Isotopes, Isobars and Isotones
- Drawbacks of Rutherford Atomic Model
- Bohr’s Atomic Model
- Bohr’s Model for Hydrogen Atom
- Quantum Mechanical Model of Atom
Chemical Bonding
- Introduction of Chemical Bonding
- Kossel-lewis Approach to Chemical Bonding - Octet Rule
- Kossel and Lewis Approach to Chemical Bonding
- Kossel-lewis Approach to Chemical Bonding - Formal Charge
- Kossel-lewis Approach to Chemical Bonding - Limitations of the Octet Rule
- Valence Shell Electron Pair Repulsion Theory (VSEPR)
- Valence Bond Theory
- Molecular Orbital Theory
- Parameters of Covalent Bond
- Dipole Moment
- Resonance
Redox Reactions
- Introduction of Redox Reactions
- Oxidation Number
- Balancing Redox Reactions in Terms of Loss and Gain of Electrons
- Redox Reaction and Electrode Potential
Modern Periodic Table
- Introduction of Periodic Table
- Structure of the Modern Periodic Table
- Periodic Table and Electronic Configuration
- Blockwise Characteristics of Elements
- Periodic Trends in Elemental Properties
Elements of Group 1 and 2
- Hydrogen
- Alkali Metals and Alkaline Earth Metals
- Some Important Compounds of Elements of S-block
Elements of Group 13, 14 and 15
- Electronic Configuration of Elements of Groups 13, 14 and 15
- Trends in Atomic and Physical Properties of Elements of Groups 13, 14 and 15
- Chemical Properties of the Elements of the Groups 13,14 and 15
- Catenation
- Allotropy and Allotropes of Carbon
- Molecular Structures of Some Important Compounds of the Group 13, 14 and 15 Elements
- Chemistry of Notable Compounds of Elements of Groups 13, 14 and 15
States of Matter
- Introduction of States of Matter: Gaseous and Liquid States
- Intermolecular Forces
- Characteristic Properties of Gases
- The Gas Laws
- Ideal Gas Equation
- Kinetic Molecular Theory of Gases
- Deviation from Ideal Behaviour
- Liquefaction of Gases and Critical Constant
- Liquid State
Adsorption and Colloids
- Introduction of Adsorption
- Adsorption
- Types of Adsorption
- Factors Affecting Adsorption of Gases on Solids
- Adsorption Isotherms (Freundlich and Langmuir Adsorption Isotherm)
- Applications of Adsorption
- Catalysis
- Adsorption Theory of Heterogeneous Catalysis
- Colloids
Chemical Equilibrium
- Introduction of Chemical Equilibrium
- Equilibrium in Physical Processes
- Equilibrium in Chemical Processes - Dynamic Equilibrium
- Law of Mass Action and Equilibrium Constant
- Homogeneous and Heterogenous Equilibria
- Characteristics of Equilibrium Constant
- Applications of Equilibrium Constants
- Le Chaterlier's Principle and Factors Altering the Composition of Equilibrium
- Industrial Application
Nuclear Chemistry and Radioactivity
- Introduction: Nuclear Chemistry is a Branch of Physical Chemistry
- Classification of Nuclides
- Nuclear Stability
- Radioactivity
- Radioactive Decays
- Modes of Decay
- Nuclear Reactions
- Applications of Radio Isotopes
Basic Principles of Organic Chemistry
- Introduction of Basic Principles of Organic Chemistry
- Structural Representation of Organic Molecules
- Classification of Organic Compounds
- Nomenclature of Organic Compounds
- Isomerism
- Theoretical Basis of Organic Reactions
Hydrocarbons
- Alkanes
- Alkenes
- Alkynes
- Aromatic Hydrocarbons
Chemistry in Everyday Life
- Chemistry in Everyday Life
- Basics of Food Chemistry
- Compounds with Medicinal Properties
- Cleansing Agents
- Properties and Measurement of Matter
- SI Units and Base Quantities
Properties and Measurement of Matter
Matter exhibits distinct properties that are classified into two main categories:
1. Physical Properties
These can be observed or measured without changing the chemical composition of a substance.
Examples: colour, odour, melting point, boiling point, density.
2. Chemical Properties
These involve a change in chemical composition due to a chemical reaction.
Examples: burning of coal to form carbon dioxide and combustion of magnesium to form magnesium oxide.
Measurement of Properties:
- Many properties of matter are quantitative (measurable).
- Measurement is a comparison with a standard unit, which is fixed, reproducible, and universally accepted.
- A quantitative measurement has two components: a number and its unit.
Example: 10 m (10 = number, m = metre, the unit for length).
Common systems of units:
- CGS: centimetre-gram-second
- FPS: foot-pound-second
- MKS: metre-kilogram-second
SI Units and Base Quantities
- In 1960, the General Conference on Weights and Measures adopted the International System of Units (SI units) based on the metric (decimal) system.
- SI units provide a universal standard for scientific measurements.
Seven SI Base Units:
| Base Quantity | Symbol | SI Unit | Unit Symbol |
|---|---|---|---|
| Length | l | metre | m |
| Mass | m | kilogram | kg |
| Time | t | second | s |
| Electric Current | I | ampere | A |
| Thermodynamic Temperature | T | kelvin | K |
| Amount of Substance | n | mole | mol |
| Luminous Intensity | Iᵥ | candela | cd |
All derived units (e.g., speed, area, volume, density) are formed from these seven base quantities.
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