Class 11 Chemistry - Detailed Notes
CLASS 11 CHEMISTRY - DETAILED NOTES
CHAPTER 1: SOME BASIC CONCEPTS OF CHEMISTRY
- **Matter**: Anything that has mass and occupies space.
- **Laws of Chemical Combination**:
- Law of Conservation of Mass: Mass is neither created nor destroyed in a chemical reaction.
- Law of Definite Proportions: A given compound always contains the same elements in the same proportion by mass.
- Law of Multiple Proportions: When two elements form more than one compound, the ratio of masses of one element
that combine with a fixed mass of the other is in small whole numbers.
- **Mole Concept**:
- 1 mole = 6.022 x 10^23 particles (Avogadro's number).
- Molar Mass: Mass of 1 mole of a substance in grams.
- **Empirical and Molecular Formulas**:
- Empirical formula: Simplest whole-number ratio of atoms in a compound.
- Molecular formula: Actual number of atoms in a molecule.
CHAPTER 2: STRUCTURE OF ATOM
- **Subatomic Particles**: Proton (+1 charge), Electron (-1 charge), Neutron (neutral).
- **Bohr's Model**:
- Electrons revolve around the nucleus in fixed orbits.
- Energy of an electron in nth orbit: E = -13.6 Z²/n² eV.
- **Quantum Mechanical Model**:
- Principal Quantum Number (n): Energy level.
- Azimuthal Quantum Number (l): Subshell (s, p, d, f).
- Magnetic Quantum Number (m): Orientation of orbital.
- Spin Quantum Number (s): Electron spin (+1/2, -1/2).
- **Electronic Configuration**:
- Aufbau Principle: Electrons fill lower energy orbitals first.
- Hund's Rule: Every orbital in a subshell gets one electron before pairing.
- Pauli Exclusion Principle: No two electrons can have the same set of quantum numbers.
CHAPTER 3: CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
CLASS 11 CHEMISTRY - DETAILED NOTES
CHAPTER 1: SOME BASIC CONCEPTS OF CHEMISTRY
- **Matter**: Anything that has mass and occupies space.
- **Laws of Chemical Combination**:
- Law of Conservation of Mass: Mass is neither created nor destroyed in a chemical reaction.
- Law of Definite Proportions: A given compound always contains the same elements in the same proportion by mass.
- Law of Multiple Proportions: When two elements form more than one compound, the ratio of masses of one element
that combine with a fixed mass of the other is in small whole numbers.
- **Mole Concept**:
- 1 mole = 6.022 x 10^23 particles (Avogadro's number).
- Molar Mass: Mass of 1 mole of a substance in grams.
- **Empirical and Molecular Formulas**:
- Empirical formula: Simplest whole-number ratio of atoms in a compound.
- Molecular formula: Actual number of atoms in a molecule.
CHAPTER 2: STRUCTURE OF ATOM
- **Subatomic Particles**: Proton (+1 charge), Electron (-1 charge), Neutron (neutral).
- **Bohr's Model**:
- Electrons revolve around the nucleus in fixed orbits.
- Energy of an electron in nth orbit: E = -13.6 Z²/n² eV.
- **Quantum Mechanical Model**:
- Principal Quantum Number (n): Energy level.
- Azimuthal Quantum Number (l): Subshell (s, p, d, f).
- Magnetic Quantum Number (m): Orientation of orbital.
- Spin Quantum Number (s): Electron spin (+1/2, -1/2).
- **Electronic Configuration**:
- Aufbau Principle: Electrons fill lower energy orbitals first.
- Hund's Rule: Every orbital in a subshell gets one electron before pairing.
- Pauli Exclusion Principle: No two electrons can have the same set of quantum numbers.
CHAPTER 3: CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
