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Textbook And Solution from NCERT
OFFICIAL SYLLABUS
Chemistry(Theory)
Unit I: Some Basic Concepts of Chemistry
General Introduction: Importance and scope of chemistry. Historical approach to particulate 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
Discovery of electron, proton and neutron; atomic number, isotopes and isobars. Thomson’s model and its limitations, Rutherford’s model and its limitations. 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 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
Significance of classification, brief history of the development of periodic table, modern periodic law and the present form of periodic table, periodic trends in properties of elements -atomic radii, ionic radii. Ionization enthalpy, electron gain enthalpy, electro negativity, valence
Unit IV: Chemical Bonding and Molecular Structure
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 homo nuclear diatomic molecules (qualitative idea only), hydrogen bond. Three states of matter. Intermolecular interactions, type 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. Derivation from ideal behaviour, liquefaction of gases, critical temperature. Liquid State - Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations).
Unit V: States of Matter
Gases and Liquids Three states of matter. Intermolecular interactions, type 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. Derivation from ideal behaviour, liquefaction of gases, critical temperature. Liquid State - Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations).
Unit VI: Thermodynamics
Concepts Of System, 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 ?U and ?H, Hess’s law of constant heat summation, enthalpy of: bond dissociation, combustion, formation, atomization, sublimation. Phase transformation, ionization, and solution. Introduction of entropy as a state function, free energy change for spontaneous and nonspontaneous processes, criteria for equilibrium.
Unit VII: Equilibrium
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, concept of pH. Hydrolysis of salts (elementary idea). Buffer solutions, solubility product, common ion effect (with illustrative examples).
Unit VIII: Redox Reactions
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, applications of redox reactions.
Unit IX : Hydrogen
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, properties and structure; hydrogen as a fuel.
Unit X: s- Block Elements (Alkali and Alkaline earth metals)
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 hydrogen carbonate, biological importance of sodium and potassium. CaO, CaCO3 and industrial use of lime and limestone, biological importance of Mg and Ca
Unit XI: Some p-Block Elements
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 acids, boron hydrides. Aluminium: uses, reactions with acids and alkalies.
Group 14 elements: General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, anomalous behaviour of first element, 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.
Unit XII: Organic Chemistry - Some Basic Principles and Techniques
General introduction, methods of qualitative and quantitative analysis, classification and IUPAC nomenclature of organic compounds Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions; electrophiles and nucleophiles, types of organic reactions
<...OFFICIAL SYLLABUS
Chemistry(Theory)
Unit I: Some Basic Concepts of Chemistry
General Introduction: Importance and scope of chemistry. Historical approach to particulate 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
Discovery of electron, proton and neutron; atomic number, isotopes and isobars. Thomson’s model and its limitations, Rutherford’s model and its limitations. 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 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
Significance of classification, brief history of the development of periodic table, modern periodic law and the present form of periodic table, periodic trends in properties of elements -atomic radii, ionic radii. Ionization enthalpy, electron gain enthalpy, electro negativity, valence
Unit IV: Chemical Bonding and Molecular Structure
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 homo nuclear diatomic molecules (qualitative idea only), hydrogen bond. Three states of matter. Intermolecular interactions, type 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. Derivation from ideal behaviour, liquefaction of gases, critical temperature. Liquid State - Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations).
Unit V: States of Matter
Gases and Liquids Three states of matter. Intermolecular interactions, type 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. Derivation from ideal behaviour, liquefaction of gases, critical temperature. Liquid State - Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations).
Unit VI: Thermodynamics
Concepts Of System, 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 ?U and ?H, Hess’s law of constant heat summation, enthalpy of: bond dissociation, combustion, formation, atomization, sublimation. Phase transformation, ionization, and solution. Introduction of entropy as a state function, free energy change for spontaneous and nonspontaneous processes, criteria for equilibrium.
Unit VII: Equilibrium
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, concept of pH. Hydrolysis of salts (elementary idea). Buffer solutions, solubility product, common ion effect (with illustrative examples).
Unit VIII: Redox Reactions
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, applications of redox reactions.
Unit IX : Hydrogen
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, properties and structure; hydrogen as a fuel.
Unit X: s- Block Elements (Alkali and Alkaline earth metals)
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 hydrogen carbonate, biological importance of sodium and potassium. CaO, CaCO3 and industrial use of lime and limestone, biological importance of Mg and Ca
Unit XI: Some p-Block Elements
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 acids, boron hydrides. Aluminium: uses, reactions with acids and alkalies.
Group 14 elements: General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, anomalous behaviour of first element, 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.
Unit XII: Organic Chemistry - Some Basic Principles and Techniques
General introduction, methods of qualitative and quantitative analysis, classification and IUPAC nomenclature of organic compounds Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions; electrophiles and nucleophiles, types of organic reactions
Unit XIII: Hydrocarbons
Classification of hydrocarbons
Alkanes - Nomenclature, isomerism, conformations (ethane only), physical properties, chemical reactions including free radical mechanism of halogenation, combustion and pyrolysis. AlkenesNomenclature, structure of double bond (ethene) geometrical isomerism, physical properties, methods of preparation; chemical reactions: addition of hydrogen, halogen,water, hydrogen halides (Markovnikov’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, IUPACnomenclature; benzene: resonance aromaticity; chemical properties: mechanism of electrophilic substitution. – nitration sulphonation, halogenation, Friedel Craft’s alkylation and acylation: directive influence of functional group in mono-substituted benzene; carcinogenicity and toxicity.
Unit XIV: Environmental Chemistry
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, strategy for control of environmental pollution.
Practicals
Evaluation Scheme for Examination |
Volumetric Analysis Salt Analysis Content Based Experiment Class Record and Viva Investigatory project |
PRACTICALS SYLLABUS
A. 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
B. 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 anyone of the following: Alum, copper sulphate, Benzoic acid.
C. Experiments related to pH change
(a) Anyone of the following experiments:
• Determination of pH of some solutions obtained from fruit juices, varied concentrations of acids. ,bases and salts using pH paper or universal indicator.
• Comparing the pH of solutions of strong and weak acid of same concentration.
• Study the pH change in the titration of a strong base using universal indicator.
(b) Study of pH change by common-ion effect in case of weak acids and weak bases.
D. Chemical equilibrium
One of the following experiments:
(a) Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/ decreasing the concentration of either ions.
(b) Study the shift in equilibrium between [Co(H2O)6] 2+ and chloride ions by changing the concentration of either of the ions.
E. Quantitative estimation
• Using a chemical balance.
• Preparation of standard solution of oxalic acid.
• Determination of strength of a given solution of sodium hydroxide by titrating it against standard solution of oxalic acid.
• Preparation of standard solution of sodium carbonate.
• Determination of strength of a given solution of hydrochloric acid by titrating it against standard sodium carbonate solution.
F. Qualitative analysis
Determination of one anion and one cation in a given salt
Cation : Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Zn2+, Cu2+, Ni2+, Ca2+, Sr2+, Ba2+, Ng2+, NH4+
Anions: (CO3)2-, S2-, (SO3)2-, (NO2)-, (SO4)2-, Cl-, Br-, I-, PO4-, C2O2-4, CH3COO-
(Note: Insoluble salts excluded)
G. Detection of nitrogen, sulphur, Chlorine
bromine and iodine in an organic compound.
PROJECT
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 the study of causes of presences 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 them.
• Study of the acidity of different samples of the tea leaves.
• Determination of the rate of evaporation of different liquids.
• Study of the effect of acids and bases on the tensile strength of fibers.
• Analysis of fruit and vegetable juices for their acidity.
Note: Any other investigatory project, which involves about 10 period of work, can be chosen with the approval of the teacher.
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Paper Format
Paper Type - Theory + Practical
Paper Marks - Theory (70 Marks) + Practical (30 Marks)
Maximum Total marks - 70 + 30 = 100 Marks
Time duration - 3 hours (Only For Theory Exam)
Unit & their Weightage
S.No. | Unit | Total Weightage |
1. | Some Basic Concepts of Chemistry | 03 marks |
2. | Structure of Atom | 06 marks |
3. | Classification of Elements and Periodicity in Properties | 04 marks |
4. | Chemical Bonding and Molecular Structure | 05 marks |
5. | States of Matter: Gases and Liquids | 04 marks |
6. | Thermodynamics | 06 marks |
7. | Equilibrium | 06 marks |
8. | Redox Reactions | 03 marks |
9. | Hydrogen | 03 marks |
10. | s -Block Elements | 05 marks |
11. | Some p -Block Elements | 07 marks |
12. | Organic Chemistry: Some Basic Principles and Techniques | 07 marks |
13. | Hydrocarbons | 08 marks |
14. | Environment Chemistry | 03 marks |
Total | 70 marks |
Paper II: Practical
Evaluation Scheme for Examination | Marks |
Volumetric Analysis | 10 |
Salt Analysis | 06 |
Content-Based Experiment | 04 |
Project Work | 05 |
Class record and viva | 05 |
Total | 30 |
For More Information:- Click Here
Conditions of eligibility for admission to class XI.
1. Candidates who have been studying in a School recognised by or affiliated to this Board or any other recognised Board of Secondary Education in India.
2. Candidates can not take admission directly in class XI.
3. Candidates had completed a regular course of study for class X and passed class X examination from a school affilicated to this Board.
4. The candidates percentage for attendance should be 75% so that the Board to make him/her eligible for the Examinations.
5. Candidate can be admitted to a school only on the transfer of the parents(s) or shifting of their families from one place to another, after procuring from the student the marksheet and the Transfer Certificate duly countersigned by the Educational Authorities of the Board concerned.
6. There is no age limit for candidates taking the Examination
7. Candidate should have doucments in support of his having passed the qualifying or equivalent qualifying examination.
TIME TABLE 2023
Date & Day | Subject | Time Duration |
Tuesday 28 March 2023 | Chemistry | 10:00 AM to 01:00 PM (3 Hrs.) |
Date & Day | Subject | Time Duration |
Thursday 16 March 2023 | Hindi, Agriculture Hindi (Only for Agriculture Part II) | 10:00 AM to 01:00 PM (3 Hrs.) |
Saturday 18 March 2023 | Geography, Geology | 10:00 AM to 01:00 PM (3 Hrs.) |
Monday 20 March 2023 | Urdu, Punjabi, Physics, Accountancy Agronomy Paper I (Only for Agriculture Part I) agronomy Paper VI (Only for Agriculture Part II) | 10:00 AM to 01:00 PM (3 Hrs.) |
Tuesday 21 March 2023 | Sociology | 10:00 AM to 01:00 PM (3 Hrs.) |
Thursday 23 March 2023 | Political Science Agricultural Botony Paper II (Only for Agriculture Part I) Agricultural Economics Paper VII (Only for Agriculture Part II) | 10:00 AM to 01:00 PM (3 Hrs.) |
Friday 24 March 2023 | Drawing & Painting | 10:00 AM to 01:00 PM (3 Hrs.) |
Saturday 25 March 2023 | Mathematics | 10:00 AM to 01:00 PM (3 Hrs.) |
Monday 27 March 2023 | Sanskrit, Agricultural Physics and Climatology Paper III (Only for Agricultural Part I) Agricultural Zoology Paper VIII (Only for Agriculture Part II) | 10:00 AM to 01:00 PM (3 Hrs.) |
Tuesday 28 March 2023 | Psychology, Education, Chemistry | 10:00 AM to 01:00 PM (3 Hrs.) |
Wednesday 29 March 2023 | Military Science, Computer Science | 10:00 AM to 01:00 PM (3 Hrs.) |
Friday 31 March 2023 | Economics | 10:00 AM to 01:00 PM (3 Hrs.) |
Saturday 01 April 2023 | Biology, Indian Music (Vocal), Indian Music (Mailodic Instrument), Indian Music (Purssion Instrument), Agricultural Engineering Paper IV (Only for Agriculture Part I) Agricultural Animal Husbandry and Veterinary Science Paper IX (Only for Agriculture Part II) | 10:00 AM to 01:00 PM (3 Hrs.) |
Monday 03 April 2023 | English | 10:00 AM to 01:00 PM (3 Hrs.) |
Wednesday 05 April 2023 | History Agricultural Mathematics and Preliminary Statistics Paper V (Only for Agriculture Part I) Agricultural Chemistry Paper X (Only for Agricultural Part II) | 10:00 AM to 01:00 PM (3 Hrs.) |
Thursday 06 April 2023 | Home Science, Business Study | 10:00 AM to 01:00 PM (3 Hrs.) |
For More Information:- Click Here
Paper Analysis
1. There are in all 30 questions in this question paper.
2. Question no. 1 to 8 carry 1 marks each.
3. Question no. 9 to 18 carry 2 marks each.
4. Question no. 19 to 27 carry 3 marks each.
5. Question no. 28 to 30 carry 5 marks each.
And
There is no overall choice. However an internal choice has been provided in two question of two marks, three questions of three marks and all questions of 5 marks each. You have to attempt only one of the choices in such questions.
Comment
1. The Difficulty level of the Chemistry paper 2020: Easy.
2. The pattern of the Chemistry paper was similar to the latest Chemistry Sample Paper 2020.
3. All the questions in the paper were asked from the latest syllabus and based on NCERT textbooks
4. The average range of expected marks was 60+ (out of 70).
1. There are total 30 questions in this question paper.
2. Question numbers 1 to 8 carry 1 mark each.
3. Question numbers 9 to 18 carry 2 marks each.
4. Question numbers 19 to 27 carry 3 marks each.
5. Question numbers 28 to 30 carry 5 marks each.
6. Question numbers 1 to 4 are multiple choice questions. In each of these questions, 4 options are given for the answer.
7. There is no overall option. However, internal choice has been provided in two questions of two marks, three questions of three marks and all questions of 5 marks each.
8. You have to attempt only one option out of such questions.
9. Log tables can be used if necessary.
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