Chemistry HSC Science (General) 11th Standard Maharashtra State Board Syllabus 2025-26

• Pure substances versus mixtures

1. Metals
2.  Non-metals
3. Metalloids

• States of matter

• Properties and Measurement of Matter
• SI Units and Base Quantities

• Introduction
• Experiment

• Atomic Mass
• Average Atomic Mass
• Molecular Mass
• Formula Mass

• Concept of Mole
• Quantities Related on Mole Concept and Their Formula
• Experiment

• Importance of analytical chemistry

• Chemical methods of qualitative analysis 
• Chemical methods of quantitative analysis

• Scientific notation (exponential notation) 
• Precision and accuracy of measurement
• Significant Figures
• Rules for deciding significant figures
• Calculations with significant figures

• Percent composition and empirical formula

• Stoichiometric problems

• Reactions in solutions

1. Mass percentage
2. Mole fraction
3. Molarity
4. Molality
5. Volume percentage

• Discovery of electron
• Discovery of proton
• Discovery of neutron

• Wave particle duality of electromagnetic radiation
• Line emission spectrum of hydrogen
• Radii of the Orbits
• Energy of the Electrons
• Limitations of Bohr’s Model
• De Broglie’s Explanation

• Explanation of the line spectrum of hydrogen using Bohr theory
• Bohr's theory and atomic spectrum of hydrogen
• Ionization energy

• Schrodinger wave equation
• Physical significance of Ψ and Ψ²
• Radial probability distribution curves
• Difference between orbit and orbital
• Atomic orbitals and quantum numbers
• Shapes of atomic orbitals
• Energies of orbitals
• Aufbau principle
• Electronic configuration of atoms and its representation 
• Electronic configurations of Cu and Cr

1. Chromium
2. Copper
3. Isoelectronic species

• Chemical bond
• Causes of chemical combination
  i) Tendency to acquire stability
  ii) Tendency to acquire noble gas configuration

• Kossel and Lewis theory
• Lewis symbols
• Significance of Lewis symbols
• Lewis symbols and valence of elements

• Formal charge (F.C.)
• Assigning formal charge

• Limitations of the octet rule

1. The incomplete octet of the central atom
2. The expanded octet
3. Odd-electron molecules
4. Shape and geometry of a molecule
5. Other drawbacks of the octet theory

• VSEPR theory
• Main postulates of VSEPR theory
• Geometry of some molecules
• Geometry of some molecules
• Steps to predict the molecular geometry using VSEPR theory

• Postulates of Valence Bond Theory
• Interacting forces during covalent bond formation
  i) Force of repulsion
  ii) Force of attraction
• Formation of hydrogen molecule on the basis of valence bond theory (VBT)
• Overlap of atomic orbitals
• Limitation of VBT

• 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

• Bond angle
• Bond Enthalpy
• Bond length
• Bond Order
• Polarity of a Covalent Bond

• Classical ideas of redox reactions
• Redox reaction in terms of electron transfer

• Rules to assign oxidation number
• Stock notation
• Redox reaction in terms of oxidation number

• Oxidation number method
• Ion electron method (Half reaction method)

Standard electrode potential

• Electronic Configurations in Periods
• Electronic configuration in groups
• Electronic configuration in the four blocks - s-Block, p-Block, d-Block, f-Block

• Characteristics of s-block elements
• Characteristics of p-block elements
• Characteristics of d-block elements
• Characteristics of f-block elements

• Effective nuclear charge and screening effect
• Periodic trends in physical properties
  a) Atomic radius
  b) Ionic radius
  c) Ionization enthalpy
  d) Electron gain enthalpy
  e) Electronegativity
• Periodic trends in chemical properties
  a) Periodic trends in valency
  b) Periodic trends in metallic - nonmetallic character
  c) Periodic trends in chemical reactivity

• Occurrence
• Position of hydrogen in the periodic table
• Isotopes of Hydrogen
• Preparation of dihydrogen
• Properties of dihydrogen
• Uses of dihydrogen

• 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
• Diagonal Relationship
• Uses of elements of group 1 and group 2
• Biological importance of elements of group 1 and group 2

• Sodium Carbonate (washing soda) Na₂CO₃.10H₂O
• Sodium hydroxide (caustic soda) NaOH
• Calcium Carbonate (CaCO₃)
• Hydrogen peroxide (H₂O₂)
• Lithium aluminium hydride (LiAlH₄)

• Oxidation state
• Bonding in compounds of group 13, 14, and 15 elements
• Reactivity towards air/oxygen
  a) Group 13 elements
  b) Group 14 elements 
  c) Group 15 elements
• Reaction with water
• Reaction with halogens

• Allotropy
• Allotropes of Carbon

• Boron trichloride (BCl₃)
• Aluminium Chloride (AlCl₃)
• Orthoboric acid / boric acid (H₃BO₃)
• Diborane (B₂H₆)
• Silicon dioxide (SiO₂)
• Nitric acid (HNO₃) 
• Orthophosphoric acid/phosphoric acid (H₃PO₄)

• Borax (Na₂, B₄O₇)
• Silicones
• Ammonia (NH₃)

• Types of Intermolecular Forces

1. Dipole-dipole interactions
2. Ion-dipole interactions
3. Dipole-Induced dipole interaction
4. London Dispersion Force
5. Hydrogen Bonding

• Intermolecular Forces and Thermal energy

• The Gas Laws
• Standard variables for gas laws

1. The volume (V)
2. The pressure (P)
3. The temperature (T)

• Ideal behaviour of gases
• Gases law: Boyle's law, Charles' law, Gay Lussac's law, Avogadro's law
• Universal gas constant
• Ideal gas equation
• Ideal gas
• Nature of universal gas constant 'R'
• Values of universal gas constant 'R' in different units
• Combined gas equation
• Relation between density (d), molar mass (M), and pressure (P) of a gas
• Expression for Molar mass

• Kinetic molecular theory of gases
• Postulates of kinetic molecular theory
• Kinetic gas equation
• Calculation of kinetic energy (K.E.)
• Molecular speeds
• Types of speed
  a) Most probable speed (u_mp)
  b) Average speed (u_av)
  c) Root mean square speed (u_r.m.s.)
• Relation between molecular speeds, temperature, and molecular mass

1. Ideal Gas
2. Real Gas

1. Vapour Pressure
2. Surface Tension
3. Viscosity

• Unbalanced forces
• Why does adsorption occur?
• Desorption
• Sorption

• Types of adsorption

1. Physical adsorption (Physisorption or van der Waals' adsorption)
2. Chemical adsorption (Chemisorption or activated adsorption)

• Difference between physisorption and chemisorption

• Factors affecting adsorption of gases on solids

1. Nature of the gas (adsorbate)
2. Nature of adsorbent
3. Surface area of the adsorbent
4. Temperature of the surface
5. Pressure of gas

• Adsorption isotherm
• Freundlich adsorption isotherm
• Langmuir adsorption isotherm

• Catalyst
• Catalysis and Theories of Catalysis
• Homogeneous Catalysis
• Heterogeneous Catalysis
• Inhibitors

• Important features of solid catalysts

1. Catalytic activity
2. Catalytic selectivity
3. Shape selective catalysis by zeolites

• Examples of colloids
• Classification of colloids
• Preparation of Colloids
• Purification of colloidal solution
• Properties of colloidal dispersions
• Methods to effect coagulation
• Emulsions
• Applications of colloids
• Dispersed phase and dispersion medium
• True solutions, colloids, and suspensions
• Types of colloidal systems

• Chemical equilibrium
• Two types of chemical equilibrium
  1) Homogeneous equilibrium
  2) Heterogeneous equilibrium
• Characteristics of equilibria involving chemical processes
• Graphical representation of chemical equilibrium

1. Liquid - Vapour equilibrium 
2. Solid - liquid equilibrium
3. Solid - vapour equilibrium

• Rate of chemical reaction
• Law of mass action
• Equilibrium constant 
• Equilibrium constant with respect to partial pressure (K_P) 
• Relationship between partial pressure and concentration
• Relationship between K_P and K_C

• Homogeneous reactions and Heterogeneous reactions
• Equilibrium constant for heterogeneous equilibria
• Units of equilibrium constant

• Prediction of the direction of the reaction
• To know the extent of reaction
• To calculate equilibrium concentrations
• Link between chemical equilibrium and chemical kinetics

• Le Chatelier's Principle
• Influencing factors of Le Chatelier's Principle
  a) Change of concentration
  b) Effect of Pressure
  c) Effect of Temperature
  d) Effect of Catalyst

• The Haber process
  a) Effect of temperature
  b) Effect of pressure

• Similarity between the solar system and the structure of the atom

• 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

• 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

• Alpha Decay
• Beta Decay
• Gamma Decay
• Rate of decay
• Rate law
• Expression for decay constant
• Half life of radioelement (t_1/2)
• Graphical representation of decay
• Units of radioactivity

• Alpha decay
• β- decay
• γ - decay

• Transmutation
• Induced or artificial radioactivity
• Nuclear fission
• Nuclear fusion
• Theoretical (qualitative) prediction of exothermic (with the release of energy) nuclear reaction, in fusing together two light nuclei to form a heavier nucleus and in splitting heavy nucleus to form middle order (lower mass number) nuclei, is evident from the shape of BE per nucleon versus mass number graph. Also, calculate the disintegration energy Q for a heavy nucleus (A = 240) with BE/A ∼ 7.6 MeV per nucleon split into two equal halves with A = 120 each and BE/A ∼ 8.5 MeV/nucleon; Q ∼ 200 MeV.

• Radiocarbon dating
• Electrical energy from Nuclear fission
• Applications in medicine
• Other applications of radioisotopes

• Condensed formula
• Bond line formula or zig-zag formula
• Drawing the molecules in three dimensions

1. Wedge formula
2. Fischer projection formula or cross formula
3. Newman projection formula
4. Sawhorse or andiron or perspective formula

• Classification based on carbon skeleton
• Classification based on functional group
• Homologous Series

• Common Naming System
• IUPAC Nomenclature

• Structural isomerism

1. Chain isomerism
2. Position isomerism
3. Functional group isomerism
4. Metamerism
5. Tautomerism

• Stereoisomerism
• Geometrical isomerism/Cis-trans isomerism
• Optical isomerism: enantiomers, dextrorotatory, laevorotatory, diastereomers, racemic mixture/ racemate, resolution.

• Types of cleavage of covalent bond

1. Homolytic cleavage
2. Heterolytic cleavage

•  Types of reagent

1. Electrophiles
2. Nucleophiles

• Electronic effects in organic reaction
• Inductive effect
• Resonance structures
• Resonance Effect
• Electromeric effect
• Hyperconjugation

• Isomerism in alkanes
• Conformations in alkanes
• Industrial preparation of alkanes
• Physical properties of alkanes
• Chemical properties of alkanes
• Uses of alkanes

• Isomerism in alkenes
• Preparation of alkenes
• Physical properties of alkenes
• Chemical properties of alkenes
• Uses of alkenes

• Isomerism in alkynes
• Preparation of alkynes
• Physical properties of alkynes
• Chemical properties of alkynes
• Uses of acetylene

• 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
• Carcinogenicity and Toxicity

• Food quality chemistry
  (i) Browning of cut fruit/vegetables
  (ii) Rancidity of oils and fats
  (iii) Saturated, unsaturated and trans fats
  (iv) Omega-3
  (v) Antioxidants as food additives

• Analgesics and antipyretics
• Antimicrobials 
  a) Antiseptics and disinfectants
  b) Antibiotics
• Traditional knowledge in medicine

• Types of cleansing agents
  a) Soaps
  b) Synthetic detergents
• Mechanism of cleansing action
• Differences between soaps and detergents