Telangana Class 11 Syllabus 2024 Chemistry

TELANGANA STATE BOARD OF INTERMEDIATE EDUCATION: HYDERABAD

ANNUAL ACADEMIC PLAN 2023-24
CHEMISTRY I YEAR
Month & Chapter and Topics to be covered /Assignments /Unit No. of
No. of Tests /Examinations / EAMCET classes to be periods
working conducted allotted for
days/No.of each topic
periods
June Syllabus dictation and discussion of IPE question paper – 01
24 weightage of marks to each chapter
1. ATOMIC STRUCTURE
1.1 Sub- atomic particles
1.2 Atomic models- Rutherford’s nuclear model
of atom
1.3 Developments to the Bohr’s model of atom
1.4 Bohr’s model for hydrogen atom.
1.5 Towards quantum mechanical model of the 15
atom.
1.6 Quantum mechanical model of an atom.
Important features of quantum mechanical
model of atom-orbitals and quantum
numbers-shapes of atomic
orbitals-energies of orbitals-filling of orbitals
in atoms. Aufbau principle,
Pauli’s exclusion principle and Hund’s rule
of maximum multiplicity-
Electronic configurations of atoms-Stability
of half filled and completely
filled orbitals.
2. CLASSIFICATION OF ELEMENTS AND
PERIODICITY IN PROPERTIES
2.1 Need to classify elements 06
2.2 Genesis of periodic classification
2.3 Modern periodic law and present form of the
periodic table
ASSIGNMENT-I 01
EAMCET 01

July 2.4 Nomenclature of elements with atomic
23 number greater than100 04
2.5 Electronic configuration of elements and the
periodic table
2.6 Electronic configuration and types of
elements s,p,d and f
2.7 Trends in physical properties-periodic 06
trends in chemical properties-Periodic
trends and chemical reactivity

3. CHEMICAL BONDING AND MOLECULAR
STRUCTURE
3.1 Kossel – Lewis approach to chemical
bonding 10
3.2 Ionic or electrovalent bond
3.3 Bond Parameters
3.4 The Valence Shell Electron Pair Repulsion
(VSEPR) theory.
3.5 Valence bond theory
ASSIGNMENT-II 01
UNIT TEST-I 01
EAMCET 01
August 3.6 Hybridisation 08
25 3.7 Coordinate bond
3.8 Molecular orbital theory –bonding in some
homonuclear diatomic molecules
3.9 Hydrogen bonding

PRACTICALS: I. Acquinttance with Laboratory
Equipment:
1.Bunsen burner, Spirit Lamp Basic Laboratory equipment
(Burette, pipette, conical flask, volumetric flask, measuring,
cylinder, wash bottle etc.,)
4. STATES OF MATTER: GASES AND LIQUIDS
4.1 Intermolecular forces 14
4.2 Thermal energy
4.3 Intermolecular forces Vs Thermal interactions.
4.4 The gaseous state
4.5 The gas laws
4.6 Ideal gas equation
4.7 Graham’s law of diffusion – Dalton’s law of
partial pressures
4.8 Kinetic molecular theory of gases

4.9 Kinetic gas equation of an ideal gas (no
derivation)- Deduction of gas laws from
kinetic gas equation
4.10 Distribution of molecular speeds – rms,
average and most probable speeds-kinetic
energy of gas molecules
4.11 Behaviour of real gases – deviation from
ideal gas behaviour – compressibility factor
Vs pressure diagrams of real gases
4.12 Liquefaction of gases
4.13 Liquid state – properties of liquids in terms
of inter molecular interactions – vapour
pressure, viscosity and surface tension
(Qualitative idea only, no mathematical
derivation)
ASSIGNMENT-III 01
UNIT TEST-II 01
EAMCET 01
September 5. STOICHIOMETRY 05
22 5.1 Some basic concepts
5.2 Laws of chemical combinations, Gay
Lussac’s law of Gaseous volumes, Dalton’s
atomic theory, Avogadro law
5.3 Atomic and molecular masses- mole concept
and molar mass concept of equivalent
weight
5.4 Percentage composition of compounds and
calculations of empirical and molecular
formulae of compounds
5.5 Stoichiometry and stoichiometric
calculations
5.6 Methods of expressing concentrations of
solutions
PRACTICALS : II. Basic Laboratory Techniques

5.7 Redox reactions 05
5.8 Oxidation number concept
5.9 Types of redox reactions
5.10 Balancing of redox reactions – oxidation
number method-half reaction (ion-
electron) method
5.11 Redox reactions in titrimetry

6. THERMODYNAMICS 09
6.1 Thermodynamic terms
6.2 Applications-work-enthalpy-extensive and
intensive properties-heat capacity
6.3 Measurement of “U and H”: Calorimetry
ASSIGNMENT-IV 01
UNIT TEST-III 01
EAMCET 01
October 6.4 Enthalpy change, ‘rH’ of reactions 05
18 6.5 Enthalpies for different types of reactions
6.6 Spontaneity
6.7 Gibbs Energy change and equilibrium
6.8 Absolute entropy and the third law of
thermodynamics
Practicals: III. Purification of Chemical substances

MID TERM HOLIDAYS
FROM 19-10-2023 TO 25-10-2023

7. CHEMICAL EQUILIBRIUM AND ACIDS- ACIDS-
BASES 07
7.1 Equilibrium in physical process
7.2 Equilibrium in chemical process – dynamic
equilibrium
7.3 Law of chemical equilibrium - law of mass
action and equilibrium constant
7.4 Homogeneous equilibria, equilibrium
constant in gaseous systems, relationship
between Kp and Kc
7.5 Heterogeneous equilibri
7.6 Applications of equilibrium constant
7.7 Relationship between equilibrium constant
‘K’, reaction Quotient ‘Q’ and Gibbs energy
‘G’
7.8 Factors affecting equilibria,-Le-chatelier’s
principle application to industrial synthesis
of ammonia and sulphur trioxide
7.9 Ionic equilibrium in solutions. 04
7.10 Acids, bases and salts- Arrhenius,
Bronsted-Lowry and Lewis concepts of acids
and bases
7.11 Ionisation of acids and bases
7.12 Buffer solutions

7.13 Solubility equilibria of sparingly soluble
salts
Solubility product constant-common ion
effect on solubility of Ionic salts
ASSIGNMENT-V 01
EAMCET 01
November 8. HYDROGEN AND ITS COMPOUNDS 06
24 8.1 Position of hydrogen in the periodic table
8.2 Dihydrogen-occurance and isotopes
8.3 Preparation of dihydrogen
8.4 Properties of dihydrogen
8.5 Hydrides: Ionic, covalent, and non-
stiochiometric hydrides
8.6 Water: Physical properties; structure of
water, ice chemical properties of water;
hard and soft water
temporary and permanent hardness of water
8.7 Hydrogen peroxide: Preparation; physical
properties; structure and chemical
properties; storage and uses.
8.8 Heavy water
8.9 Hydrogen as a fuel
Practicals:
IV. Experiments related to pH change
V. Chemical equilibrium
VI. Quantitative estimation (Volumetric analysis)

9. s – BLOCK ELEMENTS (ALKALI AND 03
ALKALINE EARTH METALS)
METALS
Group 1 Elements:
9.1 Alkali metals; Electronic configurations;
atomic and ionic radii; ionization enthalpy;
hydration enthalpy; physical properties;
chemical properties; uses
9.2 General characteristics of the compounds of
the alkali metals: oxides; halides; salts of
oxy acids
9.3 Anomalous properties of lithium:
9.4 Some important compounds of sodium:
Sodium carbonate; sodium chloride; sodium
hydroxide; sodium hydrogen carbonate.
9.5 Biological importance of sodium and
potassium.

Group 2 Elements:
9.6 Alkaline earth elements; Electronic
configuration; ionization enthalpy; hydration
enthalpy; physical properties; chemical
properties; uses
9.7 General characteristics of compounds of the 03
Alkaline earth metals. oxides, hydroxides,
halides, salts of oxyacids (carbonates,
sulphates and nitrates)
9.8 Anomalous behaviour of beryllium; its
diagonal relationship with aluminum
9.9 Some important compounds of calcium
9.10 Biological importance of calcium and
magnesium

10. p-BLOCK ELEMENTS GROUP 13 (BORON 05
FAMILY)
10.1 General introduction – Electronic
configuration, atomic radii, ionization
enthalpy, electro negativity;
physical & chemical properties
10.2 Important trends and anomalous properties
of boron
10.3 Some important compounds of boron –
borax, ortho boric acid, diborane
10.4 Uses of boron, aluminium and their
compounds
HALF YEARLY EXAMINATIONS 06
FROM 20-11-2023 TO 25-11-2023
EAMCET 01
December 11. p-BLOCK
BLOCK ELEMENTS - GROUP 14
23 (CARBON FAMILY)
11.1 General introduction - Electronic
05
configuration, atomic radii, ionization
enthalpy, electro negativity; physical &
chemical properties
11.2 Important trends and anomalous properties
of carbon
11.3 Allotropes of carbon
11.4 Uses of carbon
11.5 Some important compounds of carbon and
silicon – carbonmonoxide, carbon dioxide,
silica, silicones, silicates and zeolites

12. ENVIRONMENTAL CHEMISTRY
12.1 Definition of terms: Air, Water and Soil 04
Pollutions
12.2 Environmental pollution
12.3 Atmospheric pollution
12.4 Acid rain: Particulate pollutants
12.5 Stratospheric pollution
Practicals: VII. Qualitative Analysis
1.Reactions of the following anions with atleast one
confirmatory test for each anion. Carbonate(CO3 2-)
Sulphide(S2-),Sulphite(SO3 2- ) , Sulphate(SO4 2),
- -
Nitrite(NO2 ),Nitrate(NO3 ) Chloride(Cl-)
Bromide(Br ), Iodide(I ), Phosphate (PO4 3-),
- -

Acetate (CH3COO-)
02
12.6 Water pollution
12.7 Soil Pollution: Pesticides, industrial wastes.
12.8 Strategies to control environmental pollution
12.9 Green chemistry

13. ORGANIC CHEMISTRY-
CHEMISTRY-SOME BASIC
PRINCIPLES AND TECHNIQUESTECHNIQUES AND
HYDROCARBONS
13.1 General introduction 09
13.2 Tetravalency of Carbon: shapes of organic
compounds
13.3 Structural representations of organic
compounds
13.4 Classification of organic compounds
13.5 Nomenclature of organic compounds
13.6 Isomerism
13.7 Fundamental concepts in organic reaction
mechanisms
13.8 Methods of purification of organic
compounds
13.9 Qualitative elemental analysis of organic
compounds
13.10 Quantitative elemental analysis of organic
compounds
HYDROCARBONS
13.11 Classification of hydrocarbons
01
ASSIGNMENT
ASSIGNMENT- NT-VI
01
EAMCET
01
UNIT TEST-
TEST-IV

January 13.12 Alkanes – Nomenclature, isomerism 14
2024 (structural and conformations of ethane
23
only) preparation of alkanes -properties of
alkanes
13.13 Alkenes- Nomenclature, structure of ethane,
isomerism (structural and geometrical)-
methods of
preparation of alkenes-properties of alkenes
13.14 Alkynes – Nomenclature and isomerism,
structure of acetylene methods of
preparation of acetylene-physical
properties and chemical reactions of alkynes
13.15 Aromatic Hydrocarbons: Nomenclature and
isomerism structure of benzene, resonance
and aromaticity-preparation of benzene
physical and chemical properties of
benzene-directive influence of functional
groups in mono substituted benzene.
Carcinogenicity and toxicity
Practicals: VII. 2. Reactions of the following cations with
atleast one confirmatory test for each cation
Lead(Pb2+), Copper (Cu2+), Aluminium(Al3+),
Ferric(Fe3+),Manganese (Mn2+), Nickle (Ni2+),
Zinc(Zn2+),Cobalt(Co2+),Calcium(Ca2+),Strontium(Sr2+),
Barium(Ba2+), Magnesium(Mg2+) and Ammonium (NH4+ )
SANKRANTHI HOLIDAYS
FROM 13-01-2024 TO 16-01-2024
PRE-FINAL EXAMINATIONS
FROM 22-01-2024 TO 29-01-2024
February REVISION
23
March I.P.E. THEORY EXAMINATIONS
22 First Week of March 2024
LAST WORKING DAY: 31.03.2024

SUMMER VACATION
FROM 01-04-2024 TO 31-05-2024
ADVANCED SUPPLIMENTARY EXAMINATIONS
(IPASE)
Last week of May 2024
Re-Opening of Colleges : 01-06-2024
Prepared by: Smt. G. SRILATHA JL. In Chemistry
GOVT. Jr. College, KANDUKUR.