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 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: 6 minutes
Maharashtra State Board: Class 12
Key Points: Subatomic Particles
Atoms are made up of three fundamental subatomic particles — electron, proton, and neutron. Their discovery was a milestone in understanding atomic structure.
Discovery Timeline:
| Particle | Year | Scientist | Experiment |
|---|---|---|---|
| Electron | 1897 | J.J. Thomson | Cathode ray tube experiment — cathode rays are streams of tiny, negatively charged particles |
| Proton | 1911 | Ernest Rutherford | Alpha-particle scattering on gold foil — hydrogen nucleus identified and renamed proton |
| Neutron | 1932 | James Chadwick | Nuclear reaction: bombardment of beryllium with alpha-particles produced neutral, massive particles |
Properties of Subatomic Particles
| Particle | Symbol | Absolute Charge (C) | Relative Charge | Mass (kg) | Mass (u) | Approx. Mass (u) |
|---|---|---|---|---|---|---|
| Electron | e⁻ | −1.6022 × 10⁻¹⁹ | −1 | 9.10938 × 10⁻³¹ | 0.00054 | 0 |
| Proton | p+ | +1.6022 × 10⁻¹⁹ | +1 | 1.6726 × 10⁻²⁷ | 1.00727 | 1 u |
| Neutron | no | 0 | 0 | 1.67493 × 10⁻²⁷ | 1.00867 | 1 u |
Video Tutorials
Shaalaa.com | History of atom
to track your progress
Related QuestionsVIEW ALL [7]
Match the following:
| Element | No. of Neutron |
| a. \[\ce{^40_18AR}\] | i. 7 |
| b. \[\ce{^14_6C}\] | ii. 21 |
| c. \[\ce{^40_19K}\] | iii. 8 |
| d. \[\ce{^14_7N}\] | iv. 22 |
Make the pairs:
| ‘A’ | ‘B’ |
| a. Neutrons | i. six electrons |
| b. p-orbital | ii. -1.6×10-19 C |
| c. charge on electron | iii. Ultraviolet region |
| d. Lyman series | iv. Chadwick |
