UP Board Class 11 Chemistry Syllabus 2025-26, Download PDF

UP Board Class 11 Chemistry Syllabus is a vital resource for students. It outlines all topics covered for the academic year 2025-26. Understanding this syllabus helps students plan their studies effectively.

It provides a clear roadmap for exam preparation. Knowledge of the syllabus ensures complete coverage of necessary concepts. This prepares students not only for current exams but also for future competitive tests. It forms a strong foundation for advanced chemistry studies.

UP Board Class 11 Chemistry 2026 

The Uttar Pradesh Madhyamik Shiksha Parishad (UPMSP) sets the curriculum for Class 11 Chemistry. This syllabus guides students through essential chemical principles.

It includes topics from atomic structure to hydrocarbons. Chemistry for Class 11 builds a strong base for future science studies. Knowing the UP Board class 11 syllabus 2025-26 is crucial for strategic exam preparation. It helps students identify important areas and allocate study time.

Class 11 Chemistry Syllabus 2025-26 UP Board Overview

This section presents the full UP Board Class 11 Chemistry Syllabus structure. It lists the main units along with their assigned marks. The theoretical paper carries 70 marks, with an additional 30 marks for practical examinations.

UP Board Class 11 Chemistry Syllabus 2026 PDF Download

Accessing the UP Board syllabus PDF is beneficial. The PDF allows students to review the complete syllabus offline. It helps them mark important topics, track progress, and create a study schedule. This ensures students stay updated with the official curriculum. It is a valuable tool for comprehensive and organized exam preparation.  Here is the direct link to download UP Board Syllabus Chemistry 2026 Class 11 PDF Download:

UP Board Class 11 Chemistry Syllabus PDF Download

Subject-Wise UP Board Class 11 Chemistry Syllabus

This section provides detailed information for each unit of the UP Board Class 11 Chemistry Syllabus. It covers main topics and sub-topics, presented clearly for easy understanding.

Unit 1: Some Basic Concepts of Chemistry (07 Marks)

• General Introduction: Importance and scope of Chemistry.

• Nature of Matter: Particle nature of matter and historical approach.

• Laws of Chemical Combination: Dalton's atomic theory.

• Concepts: Elements, atoms, and molecules.

• Mass: Atomic and molecular mass, Mole concept, and molar mass.

• Formulae: Percentage composition, empirical and molecular formulae.

• Chemical Reactions: Stoichiometry and calculations based on it.

Unit 2: Structure of Atom (08 Marks)

• Discovery: Electrons, protons, and neutrons.

• Basics: Atomic number, isotopes, and isobars.

• Models: Thomson's model (limitations), Rutherford's model (limitations), and Bohr's model (limitations).

• Shells & Subshells: Concept of shells and subshells.

• Modern Physics: Dual nature of matter and light, de Broglie's relationship, Heisenberg Uncertainty Principle.

• Orbitals: Concept of orbitals, quantum numbers, shapes of s, p, and d orbitals.

• Electronic Filling: Rules for filling electrons in orbitals—Aufbau principle, Pauli exclusion principle, and Hund's rule.

• Configuration: Electronic configuration of atoms, stability of half-filled and completely filled orbitals.

Unit 3: Classification of Elements and Periodicity in Properties (07 Marks)

• Significance: Need for classification, brief history of the development of the periodic table.

• Modern Table: Modern periodic law and the present form of the periodic table.

• Periodic Trends: Atomic radii, ionic radii, inert gas radii.

• Properties: Ionization enthalpy, electron gain enthalpy, electronegativity, and valence.

• Nomenclature: Naming of elements with atomic numbers greater than 100.

Unit 4: Chemical Bonding and Molecular Structure (07 Marks)

• Bonding: Valence electrons, ionic bond, covalent bond.

• Parameters: Bond parameters, Lewis structures, polar character of covalent bonds, covalent character of ionic bonds.

• Theories: Valence Bond Theory (VBT), Resonance.

• Geometry: VSEPR theory and the geometry of covalent molecules.

• Hybridization: Concept of hybridization, shapes of s, p, and d orbitals and common molecules.

• Molecular Orbital Theory: Bonding in homonuclear diatomic molecules (qualitative introduction only).

• Hydrogen Bonding.

Unit 5: Thermodynamics (06 Marks)

• Concepts: System (types), surroundings, work, heat, energy, extensive and intensive properties, state functions.

• First Law: Internal energy and Enthalpy (H), heat capacity, specific heat, measurement of Delta U and Delta H.

• Hess's Law: Hess’s law of constant heat summation.

• Enthalpies: Bond dissociation, formation, combustion, atomization, sublimation, phase transition, ionization, solution, and dilution.

• Second & Third Laws: Introduction of entropy as a state function, free energy change for spontaneous and non-spontaneous processes, criteria for equilibrium. Brief introduction to Second and Third laws of Thermodynamics.

Unit 6: Equilibrium (08 Marks)

• Nature: Equilibrium in physical and chemical processes, dynamic nature of equilibrium.

• Law of Mass Action: Equilibrium constant (K_c and K_p).

• Factors: Factors affecting equilibrium, Le Chatelier's principle.

• Ionic Equilibrium: Ionization of acids and bases, strong and weak electrolytes, degree of ionization.

• Acids & Bases: Ionization of polybasic acids, acid strength, concept of pH, Henderson equation.

• Hydrolysis: Hydrolysis of salts (elementary idea), buffer solutions, solubility product, common ion effect (with examples).

Unit 7: Redox Reactions (07 Marks)

• Concept: Concept of oxidation and reduction.

• Redox Reactions: Types of redox reactions.

• Oxidation Number: Calculating oxidation numbers.

• Balancing: Balancing redox equations (based on electron transfer and oxidation number methods).

• Applications: Applications of redox reactions.

Unit 8: Organic Chemistry – Some Basic Principles and Techniques (10 Marks)

• Introduction: Purification of organic compounds, methods of qualitative and quantitative analysis.

• Nomenclature: Classification and IUPAC nomenclature of organic compounds.

• Electronic Displacements: Inductive effect, electromeric effect, resonance, and hyperconjugation.

• Bond Fission: Homolytic and heterolytic fission: free radicals, carbocations (carbonium ions), carbanions, electrophiles, and nucleophiles.

• Mechanisms: General mechanisms of organic reactions.

Unit 9: Hydrocarbons (10 Marks)

• Classification: Classification of hydrocarbons.

• Alkanes: Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions (including free radical mechanism of halogenation), combustion, and pyrolysis.

• Alkenes: Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation.

• Reactions: Addition of hydrogen, halogen, water, and hydrogen halides (Markovnikov's rule and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition.

• Alkynes: Nomenclature, structure of triple bond (ethyne), physical properties, methods of preparation.

• Reactions: Acidic nature of alkynes, addition reactions with hydrogen, halogens, hydrogen halides, and water.

• Aromatic Hydrocarbons: Introduction, IUPAC nomenclature, Benzene (resonance, aromaticity, chemical properties, electrophilic substitution mechanism).

• Named Reactions: Nitration, sulphonation, halogenation, Friedel-Crafts alkylation and acylation.

• Directing Influence: Directive influence of functional groups in mono-substituted benzene, carcinogenicity, and toxicity.
  

UP Board Class 11 Chemistry Practical Syllabus

The practical exam for Class 11 Chemistry carries 30 marks. It includes various experiments and projects designed to enhance practical skills. 

1. Laboratory Techniques

• Cutting a glass tube or glass rod.

• Bending a glass tube.

• Drawing out a glass jet from a glass tube.

• Boring a hole in a cork.

2. Purification and Characterization of Chemical Substances

• Determination of the Melting Point of organic substances.

• Determination of the Boiling Point of organic substances.

• Preparation of pure crystals from an impure sample through Crystallization (e.g., Alum, Copper Sulphate, Benzoic Acid).

3. Experiments Related to pH Change

• Determination of pH of fruit juices, acids, bases, and salt solutions using pH paper or Universal Indicator.

• Comparison of pH values of strong and weak acids of the same concentration.

• Study of pH change in the titration of a strong acid with a strong base using a universal indicator.

• Study of pH change by the Common Ion Effect for weak acids and weak bases.

4. Chemical Equilibrium

• Study of equilibrium shift by changing the concentration of solutions containing Ferric Fe(3+) and Thiocyanate  SCN(−) ions.

• Study of equilibrium shift by changing the concentration of solutions containing Chloride ions and Hydrated Cobalt ions.

5. Quantitative Estimation (Titration)

• Learning the use of a Chemical Balance.

• Preparation of a standard solution of Oxalic Acid.

• Determination of the strength of an unknown Sodium Hydroxide (NaOH) solution by titration against a standard solution of Oxalic Acid.

• Preparation of a standard solution of Sodium Carbonate.

• Determination of the strength of an unknown Hydrochloric Acid (HCl) solution by titration against a standard solution of Sodium Carbonate.

6. Qualitative Analysis

Identification of one Cation and one Anion in a given salt.

• Cations: Pb(2+), Cu(2+), As(3+), Al(3+), Fe(3+), Mn(2+), Ni(2+), Zn(2+), Co(2+), Ca(2+), Sr(2+), Ba(2+), Mg(2+), NH4(+)

• Anions: CO3(2−), S(2−), SO4(2−), NO2(−), NO3(−), Cl(−), Br(−), I(−), PO4(3−), C2O4(2−), CH3COO(−)

Detection of elements (Nitrogen, Sulphur, Chlorine) in organic compounds (Lassaigne's Test).

7. Projects

• Detection of bacteria by testing for Sulphide ions in contaminated water.

• Study of various methods for Water Purification.

• Testing for Water Hardness, and the presence of Chloride, Fluoride, and Iron ions.

• Study of the foaming capacity of different laundry soaps.

• Study of the acidity in various samples of Tea Leaves.

• Determination of the evaporation rate of different liquids.

• Study of the effect of acids and bases on the tensile strength of fibers.

• Analysis of fruit and vegetable juices to determine their acidity.

How to Prepare UP Board Class 11 Chemistry Syllabus?

Preparing for the UP Board Class 11 Chemistry Syllabus requires a focused and systematic approach. These tips can help students perform well.

• Understand Concepts: Focus on understanding basic chemical principles. Avoid rote memorization.

• Regular Practice: Solve numerical problems and practice chemical equations daily.

• Make Notes: Create short notes for formulas, reactions, and key definitions.

• Revise Frequently: Review important topics regularly to strengthen retention.

• Practical Skills: Pay attention in lab sessions. Practical knowledge helps theoretical understanding.

• Previous Papers: Go through past year question papers. This familiarizes you with the exam pattern.