UK Board Class 11 Chemistry Syllabus

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UK Board Class 11 Chemistry Syllabus in PDF format for free download. Chemistry syllabus for Class 11 UK Board is now available in myCBSEguide app. The curriculum for Uttarakhand Board exams is designed by UBSE, Uttarakhand as per NCERT text books for the session.

UK Board Class 11 Chemistry Syllabus Download as PDF

UK Board Class 11 Chemistry Syllabus

UK Board Syllabus Class 11

UK Board Class 11 Chemistry Chapter list in (Hindi)

रसायन (भाग 1 तथा भाग 2)

  1. रसायन विज्ञान की कुछ मूल अवधारणाएँ
  2. परमाणु की संरचना
  3. तत्वों का वर्गीकरण एवं गुणधर्मों में आवर्तिता
  4. रासायनिक आबंधन तथा आण्विक संरचना
  5. द्रव्य के अवस्थाएँ
  6. उष्मागतिकी
  7. साम्यावस्था
  8. अपचयोपचय अभिक्रियाएँ
  9. हाइड्रोजन
  10. s – बलॉक तत्व
  11. p – बलॉक तत्व
  12. कार्बनिक रसायन: कुछ आधारभूत सिद्धांत तथा तकनीकें
  13. हाइड्रोकार्बन
  14. पर्यावरणीय रसायन

Uttarakhand Board Class 11 Chemistry Chapter list in (English)

  1. Some Basic Concepts of Chemistry
  2. Structure of Atom
  3. Classification of Elements and Periodicity in Properties
  4. Chemical Bonding and Molecular Structure
  5. States of Matter
  6. Thermodynamics
  7. Equilibrium
  8. Redox Reactions
  9. Hydrogen
  10. The s – Block Elements
  11. The p – Block Elements
  12. Organic Chemistry – Some Basic Principles and Techniques
  13. Hydrocarbons
  14. Environmental Chemistry

UK Board Class 11 Chemistry Syllabus

Higher Secondary is the most crucial stage of school education because at this juncture specialized discipline-based, content-oriented courses are introduced. Students reach this stage after 10 years of general education and opt for Chemistry with a purpose of pursuing their career in basic sciences or professional courses like medicine, engineering, technology, and other applied areas. Therefore, there is a need to provide learners with sufficient conceptual background of Chemistry, which will make them competent to meet the challenges of academic and professional courses after the senior secondary stage.

The new and updated curriculum is based on disciplinary approach with rigour and depth taking care that the syllabus is not heavy and at the same time it is comparable to the international level. The knowledge related to the subject of Chemistry has undergone tremendous changes during the past one decade. Many new areas like synthetic materials,  io -molecules, natural resources, industrial chemistry are coming in a big way and deserve to be an integral part of chemistry syllabus at senior secondary stage. At international level, new formulations and nomenclature of elements and compounds, symbols and units of physical quantities floated by scientific bodies like IUPAC and CGPM are of immense importance and need to be incorporated in the updated syllabus.

The revised syllabus takes care of all these aspects. Greater emphasis has been laid on use of new nomenclature, symbols and formulations, teaching of fundamental concepts, application of concepts in chemistry to industry/ technology, logical sequencing of units, removal of obsolete content and repetition, etc.

Objectives For UK Board Class 11 Chemistry Syllabus

The curriculum of Chemistry at Senior Secondary Stage aims to:

  • promote understanding of basic facts and concepts in chemistry while retaining the excitement of chemistry.
  • make students capable of studying chemistry in academic and professional courses (such as medicine, engineering, technology) at tertiary level.
  • expose the students to various emerging new areas of chemistry and apprise them with their relevance in future studies and their application in various spheres of chemical sciences and technology.
  • equip students to face various challenges related to health, nutrition, environment, population, weather, industries and agriculture.
  • develop problem solving skills in students.
  • expose the students to different processes used in industries and their technological applications.
  • apprise students with interface of chemistry with other disciplines of science such as physics, biology, geology, engineering etc.
  • acquaint students with different aspects of chemistry used in daily life.
  • develop an interest in students to study chemistry as a discipline.
  • integrate life skills and values in the context of chemistry.

COURSE STRUCTURE

Total Periods (Theory 160+ Practical 60)
Time: 3 Hours Total Marks 70

Unit No.TitleNo. of PeriodsMarks
Unit ISome Basic Concepts of ChemistryO808
Unit IIStructure of Atom10
Unit IIIClassification of Elements and Periodicity in Properties0604
Unit IVChemical Bonding and Molecular Structure1420
Unit VStates of Matter: Gases, Liquids and solids18
Unit VIChemical Thermodynamics16
Unit VIIEquilibrium14
Unit VIIIRedox Reactions0620
Unit IXHydrogen08
Unit Xs -Block Elements10
Unit XIp -Block Elements18
Unit XIIOrganic Chemistry: Some basic Principles and Techniques1418
Unit XIIIHydrocarbons12
Unit XIVEnvironmental Chemistry06
Total16070

Unit I: Some Basic Concepts of Chemistry 8 Periods

General Introduction: Importance and scope of chemistry.
Nature of matter, laws of chemical combination, Dalton’s atomic theory: concept of elements, atoms and molecules.
Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry and calculations based on stoichiometry.

Unit II: Structure of Atom 10 Periods

Bohr’s model and its limitations, concept of shells and subshells, dual nature of matter and light, de Broglie’s relationship, Heisenberg uncertainty principle, concept of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals – Aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of atoms, stability of half-filled and completely filled orbitals.

Unit III: Classification of Elements and Periodicity in Properties 06 Periods

Modern periodic law and the present form of periodic table, periodic trends in properties of elements -atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomic number greater than 100

Unit IV: Chemical Bonding and Molecular structure 14 Periods

Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules, VSEPR theory, concept of hybridization, involving s, p and d orbitals and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules(qualitative idea only), hydrogen bond.

Unit V: States of Matter: Gases, Liquids and Solids 18 Periods

Three states of matter, intermolecular interactions, types of bonding, melting and boiling points, role of gas laws in elucidating the concept of the molecule, Boyle’s law, Charles law, Gay Lussac’s law, Avogadro’s law, ideal behaviour, empirical derivation of gas equation, Avogadro’s number, ideal gas equation. Deviation from ideal behaviour, liquefaction of gases, critical temperature, kinetic energy and molecular speeds (elementary idea) Liquid State: vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations) Solid state: Classification of solids based on different binding forces: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea). Unit cell in two dimensional and three dimensional lattices, calculation of density of unit cell, packing in solids, packing efficiency, voids, number of atoms per unit cell in a cubic unit cell, point defects, electrical and magnetic properties.

Unit VI: Chemical Thermodynamics 16 Periods

Concepts of System and types of systems, surroundings, work, heat, energy, extensive and intensive properties, state functions. First law of thermodynamics -internal energy and enthalpy, heat capacity and specific heat, measurement of AU and AH, Hess’s law of constant heat summation, enthalpy of bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionization, solution and dilution. Second law of Thermodynamics (brief introduction). Introduction of entropy as a state function, Gibb’s energy change for spontaneous and non- spontaneous processes, criteria for equilibrium. Third law of thermodynamics (brief introduction).

Unit VII: Equilibrium 14 Periods

Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, equilibrium constant,factors affecting equilibrium- Le Chatelier’s principle, ionic equilibrium- ionization of acids and bases, strong and weak electrolytes, degree of ionization, ionization of poly basic acids, acid strength, concept of pH, Henderson Equation, hydrolysis of salts (elementary idea), buffer solution, solubility product, common ion effect (with illustrative examples).

Unit VIII: Redox Reactions 06 Periods

Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, in terms of loss and gain of electrons and change in oxidation number, applications of redox reactions.

Unit IX: Hydrogen 08 Periods

Position of hydrogen in periodic table, occurrence, isotopes, preparation, properties and uses of hydrogen, hydrides-ionic covalent and interstitial; physical and chemical properties of water, heavy water, hydrogen peroxide -preparation, reactions and structure and use; hydrogen as a fuel.

Unit X: s-Block Elements (Alkali and Alkaline Earth Metals) 10 Periods

Group 1 and Group 2 Elements General introduction, electronic configuration, occurrence,
anomalous properties of the first element of each group, diagonal relationship, trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii), trends in chemical reactivity with oxygen, water, hydrogen, and halogens, uses. Preparation and Properties of Some Important Compounds: Sodium Carbonate, Sodium Chloride, Sodium Hydroxide and Sodium Hydrogencarbonate, Biological importance of Sodium and Potassium. Calcium Oxide and Calcium Carbonate and their industrial uses, biological importance of Magnesium and Calcium

Unit XI: p -Block Elements 18 Periods

General Introduction to p -Block Elements

Group 13 Elements: General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, anomalous properties of first element of the group, Boron – physical and chemical properties, some important compounds, Borax, Boric acid, Boron Hydrides, Aluminium: Reactions with acids and alkalies, uses.

Group 14 Elements: General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, anomalous behaviour of first elements. Carbon-catenation, allotropic forms, physical and chemical properties; uses of some important compounds: oxides. Important compounds of Silicon and a few uses: Silicon Tetrachloride, Silicones, Silicates and Zeolites, their uses.

Group -15 Elements: General introduction, electronic configuration, occurrence, oxidation states, trends in physical and chemical properties; Nitrogen preparation properties and uses; compounds of Nitrogen, preparation and properties of Ammonia and Nitric Acid, Oxides of Nitrogen(Structure only) ; Phosphorus – allotropic forms, compounds of Phosphorus: Preparation and Properties of Phosphine, Halides and Oxoacids (elementary idea only).

Unit XII: Organic Chemistry – Some Basic Principles and Techniques 14 Periods

General introduction, methods of purification, qualitative and quantitative analysis, classification and IUPAC nomenclature of organic compounds. Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance, and hyperconjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.

Unit XIII: Hydrocarbons 12 Periods

Classification of Hydrocarbons

Aliphatic 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, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markownikov’s addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition.

Alkynes – Nomenclature, structure of triple bond (ethyne), physical properties, methods of preparation, chemical reactions: acidic character of alkynes, addition reaction of – hydrogen, halogens, hydrogen halides and water.

Aromatic Hydrocarbons: Introduction, IUPAC nomenclature, benzene: resonance, aromaticity, chemical properties: mechanism of electrophilic substitution. Nitration, sulphonation, halogenation, Friedel Craft’s alkylation, and acylation, directive influence of functional group in monosubstituted benzene. Carcinogenicity and toxicity.

Unit XIV: Environmental Chemistry 6 Periods

Environmental pollution – air, water and soil pollution, chemical reactions in atmosphere, smog, major atmospheric pollutants, acid rain, ozone and its reactions, effects of depletion of ozone layer, greenhouse effect and global warming- pollution due to industrial wastes, green chemistry as an alternative tool for reducing pollution, strategies for control of environmental pollution.

PRACTICALS For UK Board Class 11 Chemistry Syllabus

Evaluation Scheme for ExaminationMarks
Volumetric Analysis08
Salt Analysis08
Content-Based Experiment06
Project Work04
Class record and viva04
Total30

PRACTICAL For UK Board Class 11 Chemistry Syllabus

Micro-chemical methods are available for several of the practical experiments. Wherever possible such techniques should be used:

  1. Basic Laboratory Techniques

    1. Cutting glass tube and glass rod
    2. Bending a glass tube
    3. Drawing out a glass jet
    4. Boring a cork
  2. Characterization and Purification of Chemical Substances
    1. Determination of melting point of an organic compound.
    2. Determination of boiling point of an organic compound.
    3. Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.
  3. Experiments based on pH

    1. Any one of the following experiments:
      • Determination of pH of some solutions obtained from fruit juices, solution of known and varied concentrations of acids, bases and salts using pH paper or universal indicator.
      • Comparing the pH of solutions of strong and weak acids of same concentration.
      • Study the pH change in the titration of a strong base using universal indicator.
    2. Study the pH change by common-ion in case of weak acids and weak bases.
  4. Chemical Equilibrium

    One of the following experiments:

    1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions.
    2. Study the shift in equilibrium between [Co(H2O)6]2+ and chloride ions by changing the concentration of either of the ions.
  5. Quantitative Estimation

    1. Using a chemical balance.
    2. Preparation of standard solution of Oxalic acid.
    3. Determination of strength of a given solution of Sodium Hydroxide by titrating it against standard solution of Oxalic acid.
    4. Preparation of standard solution of Sodium Carbonate.
    5. Determination of strength of a given solution of Hydrochloric acid by titrating it against standard Sodium Carbonate solution.
  6. Qualitative Analysis

    1. Determination of one anion and one cation in a given salt
      Cations- Pb2+, Cu2+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+,Ba2+, Mg2+, [NH4]+
    2. Detection of -Nitrogen, Sulphur, Chlorine inorganic compounds.

PROJECT FOR UK Board Class 11 Chemistry Syllabus

Scientific investigations involving laboratory testing and collecting information from other sources.

A few suggested Projects

  • Checking the bacterial contamination in drinking water by testing sulphide ion.
  • Study of the methods of purification of water.
  • Testing the hardness, presence of Iron, Fluoride, Chloride, etc., depending upon the regional variation in drinking water and study of causes of presence of these ions above permissible limit (if any).
  • Investigation of the foaming capacity of different washing soaps and the effect of addition of Sodium Carbonate on it.
  • Study the acidity of different samples of tea leaves.
  • Determination of the rate of evaporation of different liquids.
  • Study the effect of acids and bases on the tensile strength of fibers.
  • Study of acidity of fruit and vegetable juices.

Note: Any other investigatory project, which involves about 10 periods of work, can be chosen with the approval of the teacher.

Practical Examination for Visually Impaired Students Class XI

Note: Same Evaluation scheme and general guidelines for visually impaired students as given for Class XII may be followed.

  1. List of apparatus for identification for assessment in practicals (All experiments)

    Beaker, Tripod stand, Wire gauze, glass rod, funnel, filter paper, Bunsen burner, test tube, test tube stand, dropper, test tube holder, ignition tube, china dish, tongs, funnel, tripod stand, wire gauze, Bunsen burner, standard flask, pipette, burette, conical flask, funnel, clamp stand, dropper, wash bottle, filter paper

    • Odour detection in qualitative analysis
    • Procedure/Setup of the apparatus
  2. List of Experiments

    1. Characterization and Purification of Chemical Substances
      1. Crystallization of an impure sample of any one of the following: copper sulphate, benzoic acid
    2. Experiments based on pH
      1. Determination of pH of some solutions obtained from fruit juices, solutions of known and varied concentrations of acids, bases and salts using pH paper
      2. Comparing the pH of solutions of strong and weak acids of same concentration.
    3. Chemical Equilibrium

      1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either ions.
      2. Study the shift in equilibrium between [Co(H2O)6]2+ and chloride ions by changing the concentration of either of the ions.
    4. Quantitative estimation

      1. Preparation of standard solution of oxalic acid.
      2. Determination of molarity of a given solution of sodium hydroxide by titrating it against standard solution of oxalic acid.
    5. Qualitative Analysis

      1. Determination of one anion and one cation in a given salt
      2. Cations- NH4+
        Anions – [CO3]2- , S2-, [SO3]2-, Cl, CH3COO
        (Note: insoluble salts excluded)
      3. Detection of Nitrogen in the given organic compound.
      4. Detection of Halogen in the given organic compound.
  3. Chemistry Part -I, Class-XI, Published by NCERT.
  4. Chemistry Part -II, Class-XI, Published by NCERT.
Type of QuestionMark per QuestionTotal No. of QuestionsTotal Marks
VSA1505
SA-I2714
SA-II31236
LA5315
Total2770

QUESTION WISE BREAK UP

  1. Internal Choice: There is no overall choice in the paper. However, there is an internal choice in one question of 2 marks weightage, one question of 3 marks weightage and all the three questions of 5 marks weightage.
  2. The above template is only a sample. Suitable internal variations may be made for generating similar templates keeping the overall weightage to different form of questions and typology of questions same.

For study material on UK Board Class 11 Chemistry Syllabus download myCBSEguide app.UK Board Class 11 Chemistry Syllabus is also available in myCBSEguide website. UK Board Class 11 Chemistry Syllabus for the session 2018-19 is available here in PDF format. For latest UK Board Class 11 Chemistry Syllabus, please visit UBSE official website.



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