NCERT Chemistry Syllabus for Class 11
ncert chemistry class 11, chemistry class 11, class 11 chemistry syllabus
CLASS-XI (THEORY) (2018-19)
COURSE STRUCTURE
Total Periods (Theory 160+ Practical 60)
Time: 3 Hours Total Marks 70
Unit
|
Chapter
|
1
|
|
2
|
|
3
|
|
4
|
|
5
|
|
6
|
|
7
|
|
8
|
|
9
|
|
10
|
|
11
|
|
12
|
|
13
|
|
14
|
|
Stay tuned to chemistryfriend.com for latest NCERT study materials and syllabus.
Exam Structure of NCERT Chemistry Syllabus Class 11
Unit
|
Title
|
Marks
|
I
|
Basic Concepts of Chemistry
|
11
|
II
|
Structure of Atom
|
|
III
|
Classification of Elements &
Periodicity in Properties
|
04
|
IV
|
Chemical Bonding and Molecular
Structure
|
21
|
V
|
States of Matter: Gases and
Liquids
|
|
VI
|
Thermodynamics
|
|
VII
|
Equilibrium
|
|
VIII
|
Redox Reactions
|
16
|
IX
|
Hydrogen
|
|
X
|
s-Block Elements
|
|
XI
|
Some p-Block Elements
|
|
XII
|
Organic Chemistry: Basic
Principles & Techniques
|
18
|
XIII
|
Hydrocarbons
|
|
XIV
|
Environmental Chemistry
|
|
Total
|
70
|
Unit
I: Some Basic Concepts of Chemistry
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
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'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
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, 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
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 and Liquids
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)
Unit VI: Chemical Thermodynamics
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 ΔU and ΔH, 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
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 Reaction
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
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)
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: 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 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.
Unit XII: Organic Chemistry - Some Basic Principles and Technique
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 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 HydrocarbonsAliphatic 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
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.
#100%Unique
PRACTICALS
Micro-chemical methods are available for several of the practical experiments.
Wherever possible such techniques should be used:
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 any one of the following: Alum, Copper Sulphate, Benzoic Acid.
C. Experiments based on pH
(a) 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.
(b) Study the pH change by common-ion 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 of the 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
i) Using a chemical balance.
ii) Preparation of standard solution of Oxalic acid.
iii) Determination of strength of a given solution of Sodium Hydroxide by titrating it against standard solution of Oxalic acid.
iv) Preparation of standard solution of Sodium Carbonate.
v) Determination of strength of a given solution of Hydrochloric acid by titrating it against standard
Sodium Carbonate solution.
F. Qualitative Analysis
(a) 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]+
Anions – [CO3]2-, S2-, [SO3]2-, [SO4]2-, [NO3]-, Cl- ,Br-, I-, [PO4]3-, [C2O4]2-, CH3COO-
(Note: Insoluble salts excluded)
(b) Detection of -Nitrogen, Sulphur, Chlorine in organic compounds.
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 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.
A. 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
B. List of Experiments
A. Characterization and Purification of Chemical Substances
1. Crystallization of an impure sample of any one of the following: copper sulphate, benzoic acid
B. 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.
C. 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.
D. 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.
E. 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.
Note: The above practicals may be carried out in an experiential manner rather than recording observations. Prescribed Books:
1. Chemistry Part -I, Class-XI, Published by NCERT.
2. Chemistry Part -II, Class-XI, Published by NCERT
CHEMISTRY (Code No. 043)
QUESTION PAPER DESIGN
CLASS - XI (2018-19)
Time 3 Hours Max. Marks: 70
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
Ncert-chemistry-class-11-
chemistry-class-11-
class-11-chemistry –syllabus
ncert
chemistry class 11 |chemistry class 11 |class 11 chemistry syllabus
No comments:
Post a Comment