Maharashtra State BoardHSC Science (General) 11th
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Chemistry 11th HSC Science (General) Maharashtra State Board Topics and Syllabus

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Maharashtra State Board Syllabus For 11th Chemistry: Knowing the Syllabus is very important for the students of 11th. Shaalaa has also provided a list of topics that every student needs to understand.

The Maharashtra State Board 11th Chemistry syllabus for the academic year 2021-2022 is based on the Board's guidelines. Students should read the 11th Chemistry Syllabus to learn about the subject's subjects and subtopics.

Students will discover the unit names, chapters under each unit, and subtopics under each chapter in the Maharashtra State Board 11th Chemistry Syllabus pdf 2021-2022. They will also receive a complete practical syllabus for 11th Chemistry in addition to this.

Academic year:

Maharashtra State Board 11th Chemistry Revised Syllabus

Maharashtra State Board 11th Chemistry and their Unit wise marks distribution

Maharashtra State Board 11th Chemistry Course Structure 2021-2022 With Marking Scheme

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1 Some Basic Concepts of Chemistry
2 Introduction to Analytical Chemistry
3 Basic Analytical Techniques
4 Structure of Atom
  • Subatomic Particles 
    • Discovery of electron
    • Discovery of proton
    • Discovery of neutron
  • Atomic Number and Atomic Mass Number 
  • Isotopes, Isobars and Isotones 
  • Drawbacks of Rutherford Atomic Model 
  • Bohr’s Atomic Model 
    • Developments leading to the Bohr’s atomic model
    • Wave-particle duality of electromagnetic radiation
      a) Characteristics of electromagnetic wave
      i) Wavelength (λ)
      ii) Frequency (ν)
      iii) Wavenumber (ν)
      iv) Amplitude (A)
      b) Particle nature of electromagnetic radiation
    • Line emission spectrum of hydrogen
  • Bohr’S Model for Hydrogen Atom 
    • Postulates of Bohr atomic theory
    • Results of Bohr’s theory
    • Explanation of the line spectrum of hydrogen using Bohr theory
    • Limitations of Bohr model
    • Reasons for failure of the Bohr model
  • Quantum Mechanical Model of Atom 
    • Schrodinger equation
    • Atomic orbitals and quantum numbers
    • Shapes of atomic orbitals
    • Energies of orbitals
    • Aufbau principle
      i) The increasing order of energies of orbitals
      ii) Pauli exclusion principle
      iii) Hund’s rule of maximum multiplicity 
    • Electronic configuration of atoms and its representation 
    • Condensed orbital notation of electronic configuration
    • Electronic configurations of Cu and Cr - Chromium, Copper, Isoelectronic species
5 Chemical Bonding
  • Introduction of Chemical Bonding 
    • Kossel – Lewis approach to chemical bonding
  • Kossel-lewis Approach to Chemical Bonding - Octet Rule 
  • Concept of Kossel-lewis Approach to Chemical Bonding 
    • Ionic bond
      I. Formation of sodium chloride (NaCl)
      II. Formation of calcium chloride (CaCl2)
    • Ionic solids and Lattice Enthalpy
    • Covalent bond 
      I. Formation of H2 molecule
      II. Formation of Cl2
      III. Formation of Multiple bonds
    • Lewis structures (Lewis representations of simple molecules)
    • Steps to write Lewis dot structures
  • Kossel-lewis Approach to Chemical Bonding - Formal Charge 
  • Kossel-lewis Approach to Chemical Bonding - Limitations of the Octet Rule 
    • Molecules with an incomplete octet
    • Molecules with an expanded octet
    • Odd electron molecules
  • The Valence Shell Electron Pair Repulsion (Vsepr) Theory 
    • Rules of VSEPR
      1. Ammonia NH3 
      2. Water molecule H2O
    • Advanced theories of Bonding
  • Valence Bond Theory 
    • Postulates of Valence Bond Theory
    • Interacting forces during covalent bond formation
    • Overlap of atomic orbitals -
      1. sigma bond (σ)
      a. s-s overlap
      b. p-p overlap
      c. s-p σ bond
      2. pi bond (π)
    • Hybridization
    • Steps considered in Hybridization
      i) Formation of the excited state
      ii) Mixing and Recasting of orbitals
    • Types of Hybridization and Geometry of Molecules 
      i) sp3 Hybridization - Formation of methane (CH4) molecule
      ii) sp2 Hybridization - Formation of C2H4 molecule
      iii) sp hybridization - Formation of acetylene molecule
    • Importance and limitation of valence bond theory
    • Limitations of valence bond theory
    • Salient features of VB Theory
  • Molecular Orbital Theory 
    • Formation of molecular orbitals
    • Conditions for the combination of Atomic Orbitals
    • Types of molecular orbitals
    • Energy levels and electronic configuration
    • Key ideas of MO theory
    • MO description of simple diatomic Molecules
      1. Hydrogen molecule - H2
      2. Lithium molecule (Li2)
      3. N2 molecule 
      4. O2 molecule
      5. F2 molecule
    • The salient features of Molecular orbital Theory (MOT)
    • Bonding in some Homonuclear di-atomic molecules
    • Bonding in some Heteronucleardi-atomic molecules
    • Metallic bonding
  • Parameters of Covalent Bond 
    • Bond angle 
    • Bond Enthalpy
    • Bond length
    • Bond Order 
    • Polarity of a Covalent Bond
  • Dipole Moment 
    • Dipole moments of polyatomic molecules
    • Lone pairs and dipole moment
    • CH4
    • Covalent character of an ionic bond
  • Resonance 
    • Resonance Energy
6 Redox Reactions
7 Modern Periodic Table
8 Elements of Group 1 and 2
  • Hydrogen 
    • Occurrence
    • Position of hydrogen in the periodic 
    • Isotopes of Hydrogen
    • Preparation of dihydrogen
      A. Laboratory methods
      B. Industrial methods
    • Properties of dihydrogen
      A. Physical properties
      B. Chemical properties
    • Uses of dihydrogen
    • Ortho and Para−Hydrogen
  • Alkali Metals and Elements of Group 2 
    • Introduction 
    • Electronic configuration of elements of group 1 and group 2
    • Trends in atomic and physical properties of elements of group 1 and group 2
    • Chemical properties of elements of group 1 and group 2
      i) Reaction with oxygen/air
      ii) Reaction with water
      iii) Reaction with Hydrogen
      iv) Reaction with Halogens
      v) Reducing nature
      vi) Solution in liquid ammonia
    • Diagonal Relationship
    • Uses of elements of group 1 and group 2
    • Biological importance of elements of group 1 and group 2
  • Some Important Compounds of Elements of S-block 
    • Sodium Carbonate (washing soda) Na2CO3. 10H2O
    • Sodium hydroxide (caustic soda) NaOH
    • Calcium Carbonate (CaCO3)
    • Hydrogen peroxide (H2O2)
    • Lithium aluminium hydride (LiAlH4)
9 Elements of Group 13, 14 and 15
10 States of Matter

11 Adsorption and Colloids

12 Chemical Equilibrium
13 Nuclear Chemistry and Radioactivity
  • Introduction: Nuclear Chemistry is a Branch of Physical Chemistry 
    • Similarity between the solar system and the structure of the atom
  • Classification of Nuclides 
    • On the basis of the number of neutrons and protons constituting the nucleus, the nuclides (which refer to the atomic nucleus without relation to the outer sphere)
      i) Isotopes
      ii) Isobars
      iii) Mirror nuclei
      iv) Isotones
      v) Nuclear isomers 
    • Classification on the basis of nuclear stability
      i) Stable nuclides
      ii) Unstable or radioactive nuclides
  • Nuclear Stability 
    • Even-odd nature of the number of protons and neutrons
    • Neutron to Proton ratio (N/Z)
    • Magic numbers
    • Nuclear Potential
    • Nuclear binding energy and mass defect
  • Radioactivity 
    • Alpha decay
    • Beta decay
    • Gamma decay
    • Law of radioactive decay
    • Half-life
    • Carbon dating
    • Discovery of Neutrons
  • Radioactive Decays 
    • Rate of decay
    • Rate law
    • Expression for decay constant
    • Half-life of radioelement (t1/2)
    • Graphical representation of decay
    • Units of radioactivity
  • Modes of Decay 
    • Alpha decay
    • β- decay
    • γ - decay
  • Nuclear Reactions 
    • Transmutation
    • Induced or artificial radioactivity
    • Nuclear fission
    • Nuclear fusion
  • Applications of Radio Isotopes 
    • Radiocarbon dating
    • Electrical energy from Nuclear fission
    • Applications in medicine
    • Other applications of radioisotopes
14 Basic Principles of Organic Chemistry
  • Introduction of Basic Principles of Organic Chemistry 
  • Structural Representation of Organic Molecules 
    • Condensed formula
    • Bond line formula or zig-zag formula
    • Drawing the molecules in three dimensions
      I. Wedge formula
      II. Fischer projection formula or cross formula
      III. Newman projection formula
      IV. Sawhorse or andiron or perspective formula
  • Classification of Organic Compounds 
    • Classification based on the carbon skeleton - Acyclic or open-chain compounds, Cyclic compounds, Alicyclic compounds, Aromatic compounds.
    • Classification based on the functional group - Homologous series
  • Nomenclature of Organic Compounds 
    • Common/trivial names
    • IUPAC Nomenclature 
    • IUPAC names of straight-chain alkanes
    • IUPAC names of branched saturated hydrocarbons 
    • IUPAC nomenclature of unsaturated hydrocarbons (Alkenes and Alkynes)
    • IUPAC Names of simple monocyclic hydrocarbons
    • IUPAC nomenclature of compounds containing one or more functional groups
    • Naming monofunctional compounds
    • Polyfunctional compounds
    • IUPAC Rules for naming mono or polyfunctional compounds
    •  IUPAC nomenclature of substitued benzene
    • Monosubstituted benzene 
    • Disubstituted benzene derivatives
    • Trisubstituted benzene derivatives
  • Isomerism 
    • Structural isomerism
      a) Chain isomerism 
      b) Position isomerism
      c) Functional group isomerism
      d) Metamerism
      e) Tautomerism
  • Theoretical Basis of Organic Reactions 
    • Types of cleavage of covalent bond
      (i) Homolytic cleavage
      (ii) Heterolytic cleavage
    • Types of reagent
    • Electronic effects in organic reaction
    • Inductive effect
    • Resonance structures
    • Resonance Effect
    • Electromeric effect
    • Hyperconjugation
15 Hydrocarbons
  • Alkanes 
    • Isomerism in alkanes
    • Conformation in alkanes
    • Industrial preparation of alkanes
    • Physical properties of alkanes
    • Chemical properties of alkanes 
    • Uses of alkanes
  • Alkenes 
    • Isomerism in alkenes
    • Preparation of alkenes
    • Physical properties of alkenes
    • Chemical properties of alkenes
    • Uses of alkenes
  • Alkynes 
    • Isomerism in alkynes
    • Preparation of alkynes
    • Physical properties of alkynes
    • Chemical properties of alkynes
    • Uses of acetylene
  • Aromatic Hydrocarbons 
    • Benzene
    • Structure of benzene
    • Aromatic character (Huckel Rule)
    • Preparation of aromatic compounds
    • Physical properties of benzene
    • Chemical properties of benzene
    • Directive influence of a functional group in monosubstituted benzene
      - Meta directing and deactivating groups
      - Metadirective influence of -NO2 group can be explained by resonance theory
    • Carcinogenicity and Toxicity
    • Sources of aromatic compound
16 Chemistry in Everyday Life
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