Topics
Some Basic Concepts of Chemistry
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
- Chromatography Method > Adsorption Chromatography
- Chromatography Method > Partition Chromatography
Structure of Atom
Chemical Bonding
- Concept of Chemical Bonding
- Kossel-lewis Approach to Chemical Bonding - Octet Rule
- Kossel and Lewis Approach to Chemical Bonding
- Formal Charge
- Limitations of the Octet Rule
- Valence Shell Electron Pair Repulsion (VSEPR) Theory
- Valence Bond Theory (VBT)
- Molecular Orbital Theory
- Parameters of Covalent Bond
- Dipole Moment
- Resonance
Redox Reactions
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
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
- Carbon: A Versatile Element
- Allotropes of Carbon > Diamond
- 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
Adsorption and 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
- Organic Chemistry
- Structural Representation of Organic Molecules
- Classification of Organic Compounds
- Nomenclature
- Isomerism
- Theoretical Basis of Organic Reactions
Hydrocarbons
Chemistry in Everyday Life
Estimated time: 10 minutes
Maharashtra State Board: Class 12
Key Points: Properties of Matter and Their Measurement
Types of Properties
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Physical Properties — can be observed or measured without altering the chemical nature of the substance. Examples: colour, odour, melting point, boiling point, density.
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Chemical Properties — involve a chemical change in the substance; the original substance is converted into something new. Example: burning coal produces CO₂.
SI Fundamental Units
The International System of Units (SI) defines seven base units that serve as building blocks for all scientific measurement:
| Physical Quantity | SI Unit | Symbol |
|---|---|---|
| Mass | Kilogram | kg |
| Temperature | Kelvin | K |
| Length | Metre | m |
| Time | Second | s |
| Electric Current | Ampere | A |
| Amount of Substance | Mole | mol |
| Luminous Intensity | Candela | cd |
Key Notes to Remember:
- Mass measures the quantity of matter and is independent of location. Weight depends on gravity — the same object has different weight on Earth vs. the Moon, but identical mass.
- Temperature and heat are not the same. Heat is energy being transferred; temperature tells us the direction of that transfer.
- 0°C = 32°F; 100°C = 212°F. A rise of 1°C corresponds to a rise of 9/5°F on the Fahrenheit scale.
- Units can be written in two equivalent ways: g/cm³ or g cm⁻³ — both are acceptable.
