CISCE Syllabus For Class 12 Chemistry (Theory): Knowing the Syllabus is very important for the students of Class 12. Shaalaa has also provided a list of topics that every student needs to understand.
The CISCE Class 12 Chemistry (Theory) syllabus for the academic year 2023-2024 is based on the Board's guidelines. Students should read the Class 12 Chemistry (Theory) Syllabus to learn about the subject's subjects and subtopics.
Students will discover the unit names, chapters under each unit, and subtopics under each chapter in the CISCE Class 12 Chemistry (Theory) Syllabus pdf 2023-2024. They will also receive a complete practical syllabus for Class 12 Chemistry (Theory) in addition to this.
CISCE Class 12 Chemistry (Theory) Revised Syllabus
CISCE Class 12 Chemistry (Theory) and their Unit wise marks distribution
CISCE Class 12 Chemistry (Theory) Course Structure 2023-2024 With Marking Scheme
Syllabus
CISCE Class 12 Chemistry (Theory) Syllabus for Relative Molecular Mass and Mole
- Vapour Pressure of Liquid
- Vapour Pressure of Liquid- Liquid Solutions
- Raoult's Law
- Vapour Pressure of Liquid- Liquid Solutions
- Raoult'S Law and Colligative Properties
- Intensive property
definition and examples
- Extensive Property
definition and examples
- Solubility of Gases in Liquids
Numericals
- Intensive property
- Ideal and Non-ideal Solutions
- Ideal Solutions
- Non-ideal Solutions
- Non-ideal solutions - positive deviation from Rauolt's Law
- Non-ideal solutions - negative deviation from Rauolt's Law
- Factors responsible for deviation from Raoult’s law
- Solute-solvent interactions
- Dissociation of solute
- Association of solute
- Temperature
- Pressure
- Concentration
- Solubility
- Solubility of a Gas in a Liquid
- Factors affecting the solubility of gases in liquids
1) Nature of gas (solute) and liquid (solvent)
2) Effect of temperature
3) Effect of pressure - Limitations of Henry's law
- Applications of Henry's law
1) In the production of carbonated beverages
2) In scuba diving (deep-sea diving)
3) At high altitudes
- Factors affecting the solubility of gases in liquids
- Solubility of a Gas in a Liquid
Raoult's law and colligative properties.
Intensive property – definition and examples.
Extensive property – definition and examples.
Colligative properties – definition and examples.
Raoult’s Law – I (for volatile solutes),
– II (for non-volatile solutes).
Ideal solution, non-ideal solution. Azeotropic mixtures – definition, types and examples. Solubility of gases in liquids – Henry’s Law, simple numericals.
- Dissociation- Electrolytic Solute
- Meaning of Electrolytic Solute
if strong electrolyte
- Meaning of Electrolytic Solute
if weak electrolyte
- Numericals
Dissociation- Electrolytic solute
- Meaning of Electrolytic Solute
Dissociation- Electrolytic solute.
Meaning of electrolytic solute – (if strong electrolyte) – the number of particles of the solute in solution is an exact multiple of the number of ions present in one molecule of the solute. Meaning of electrolytic solute – (if weak electrolyte) – the number of particles of the solute in solution is not an exact multiple of the number of ions present in one molecule of the solute but a part of it depending on the degree of dissociation. (This part may be taught after teaching ionic equilibria). Numericals included.
- Relative Molecular Mass of Non-volatile Substances
- Depression in Freezing Point
- Freezing point depression as a consequence of vapour pressure lowering
- Freezing point depression and concentration of solute
- Molar mass of solute from freezing point depression
- Freezing Point Depression
molal depression constant (cryoscopic constant)
- Freezing Point Depression
Numericals
- Elevation in Boiling Point Method
Relative molecular mass
- Boiling Point Elevation
molal elevation constant or ebullioscopic constant
- Boiling point elevation as a consequence of vapour pressure lowering
- Boiling point elevation and concentration of solute
- Molar mass of solute from boiling point elevation
- Boiling Point Elevation
Numericals
- Van’t Hoff- Charles’ Law
statement, mathematical form, simple calculations
- Van’t Hoff
Numericals
- Depression in Freezing Point
Relative molecular mass of non-volatile substances:
(a) By relative lowering of vapour pressure.
Determination of relative molecular mass by measurement of lowering of vapour pressure. Problems based on the above. Experimental details not required.
(b) Depression in freezing point.
Freezing point depression - molal depression constant (cryoscopic constant) – definition and mathematical expression (derivation included). Problems based on the above. Experimental details not required.
(c) Elevation in boiling point method.
Boiling point elevation – molal elevation constant or ebullioscopic constant– definition and mathematical expression (derivation included). Problems based on the above. Experimental details not required.
(d) Osmotic pressure and its application in the determination of relative molecular mass
Osmotic pressure – definition and explanation, natural and chemical semipermeable membranes, reverse osmosis.
van’t Hoff- Boyle’s Law, van’t Hoff – Charles’ Law, van’t Hoff - Avogadro’s law.
Problems based on the above. Experimental details not required.
(e) van’t Hoff factor.
van’t Hoff factor for the electrolytes which dissociate and the molecules which associate in solution. Modification of the formula of colligative properties based on van’t Hoff factor. Simple problems. Calculation of degree of dissociation and association. Experimental details not required.
(f) van’t Hoff equation and its interpretation.
Self-explanatory.
(g) Simple numerical problems on different methods mentioned above for the determination of molecular masses. Abnormal molecular masses in case of electrolytes and in case of solutes which associate.
Self-explanatory.
- Association
- Numericals
Association
- Numericals
Association.
The meaning of association with respect to dimer formation. Numericals included.
- Normality, Molality
- Normality, Molality, Molarity, Mole Fraction, as Measures of Concentration
defination with examples
- Simple Problems Relating Mass, Molar Mass and Mole
Normality, molality
- Normality, Molality, Molarity, Mole Fraction, as Measures of Concentration
Normality, molality, molarity, mole fraction, as measures of concentration.
Definition of the above terms with examples. Simple problems relating mass, molar mass and mole
Nonvolatile, non electrolytic solute.
Explanation of non-volatile solute and non-electrolytic solute with examples
CISCE Class 12 Chemistry (Theory) Syllabus for States of Matters: Structure and Properties Solid State
- Crystal Lattices and Unit Cells
- Unit cell
- Crystal lattice or space lattice
- Two-dimensional lattice and unit cell
- Three-dimensional lattice and unit cell
- States of Matters: Structure and Properties Solid State
- Types of Unit Cell
Types of unit cell (scc, fcc, bcc)
- Calculation of Density of Unit Cell
Calculation of density of unit cell, formula of the compound – numericals based on it
- Packing in 3 – D
packing in 3 – D, packing fraction in scc, fcc, bcc with derivation
- Voids – Types, Location, Formation
voids – types, location, formation (derivation of radius of voids).
- Characteristics of Crystalline Solids;
ionic (NaCl), metallic (Cu), atomic (diamond and graphite)
- Point Defects – F Centers
Point defects: Stoichiometric, non- stoichiometric and impurity defects (F- centres).
- Types of Unit Cell
- Calculations Involving Unit Cell Dimensions
- Calculation of density of unit cell
- Amorphous and Crystalline Solids
- Classification of solids
- Crystalline solids
- Amorphous solids
- The distinction between Crystalline and Amorphous Solids
- Isomorphous solids and polymorphous solids
- Electrical Properties
Electrical properties: Conductors, semiconductors (n & p types) and insulators (Band Theory), piezoelectricity and pyroelectricity.
- Magnetic Properties
- Magnetic properties:
- Magnetising field
- Magnetic permeability
- Intensity of magnetisation
- Magnetic induction or total magnetic field
- Magnetic susceptibility
- Substances can be classified into five categories:
- Paramagnetic
- Diamagnetic
- Ferromagnetic
- Antiferromagnetic
- Ferrimagnetic
2017
Crystalline and amorphous substances; lattice; unit cell; 3–D packing of atoms in a crystal lattice; relation between radius, edge length and nearest neighbour distance of atoms in a unit cell; density of a unit cell; interstitial void; imperfections in solids, ionic, metallic and atomic solids, electrical and magnetic properties.
Definition of crystal lattice, unit cell; types of unit cell (scc, fcc, bcc); calculation of the number of atoms per unit cell; packing in 3 – D; concept of radius, edge length and nearest neighbour distance; calculation of density of unit cell, radius, edge length, formula of the compound – numericals based on it; voids – types, location, formation; point defects – F centers; electrical and magnetic properties – piezoelectricity, pyroelectricity, ferromagnetic, ferrimagnetic, antiferromagnetic; crystalline and amorphous substances; characteristics of crystalline solids; ionic (NaCl), metallic (Cu), atomic (diamond and graphite).
2019
Solids: their classification based on different binding forces such as: ionic, covalent molecular; amorphous and crystalline solids
(difference), metals. Type of unit cell in two dimensional and three dimensional lattices, number of atoms per unit cell (all types).
Calculation of density of unit cell, packing in solids, packing efficiency, voids, point defects, electrical and magnetic properties.
Band theory of metals. Conductors, semiconductors (n and p type) and insulators.
(i) Crystalline and amorphous solids.
(ii) Definition of crystal lattice, unit cell; types of unit cell (scc, fcc, bcc); calculation of the number of atoms per unit cell; relationship
between radius, edge length and nearest neighbour distance. Calculation of density of unit cell, formula of the compound –
numericals based on it; packing in 3 – D, packing fraction in scc, fcc, bcc with derivation; voids – types, location, formation (derivation of radius of voids).
(iii) Characteristics of crystalline solids; ionic (NaCl), metallic (Cu), atomic (diamond and graphite).
(iv) Point defects: Stoichiometric, non- stoichiometric and impurity defects (F- centres).
(v) Electrical properties: Conductors, semiconductors (n & p types) and insulators (Band Theory), piezoelectricity and pyroelectricity.
(vi) Magnetic properties: diamagnetic, paramagnetic, ferromagnetic, ferrimagnetic and antiferromagnetic.
CISCE Class 12 Chemistry (Theory) Syllabus for Chemical Kinetics
Qualitative meaning of chemical kinetics, comparison with chemical dynamics; slow and fast reactions; rate of reactions; factors affecting the rate of reaction such as: concentration, temperature, nature of reactants and products, surface area of reactants, presence of catalyst and radiation; Rate constant; Rate law; Law of Mass Action; concept of energy barrier; threshold energy, activation energy; formation of activated complex; exothermic and endothermic reactions; collision theory for a chemical change; order of a reaction; rate equation of zero and first order reaction; half life period; molecularity of a reaction; mechanism of elementary and overall reaction; variation of rate constant with temperature; Arrhenius equation – K=Ae-Ea/RT; related graphs; catalyst
- Meaning.
- Relation between order and stoichiometric coefficients in balanced equations.
- Order as an experimental quantity.
- Rate equation for zero order reaction and its unit.
- Mathematical derivation of rate equation for first order reaction.
- Characteristics of first order reaction – rate constant is independent of the initial concentration, units to be derived.
- Definition of half-life period.
- Derivation of expression of half-life period from first order rate equation.
- Problems based on first order rate equation and half life period.
- Collision Theory of Chemical Reactions
- Collision between reactant molecules
- Energy requirement - Activation energy
- Orientation of reactant molecules
- Collision Theory
- Condition for a Chemical change
Close contact, particles should collide, heat, light, electricity, pressure, catalysts with examples
- Collisions to Be Effective
optimum energy and proper orientation during collision
- Difference in Energy of the Reactant and the Product
exoergic and endoergic reactions with proper graphs and labelling
- Condition for a Chemical change
- Condition for a Chemical change – Close contact, particles should collide.
- Collisions to be effective – optimum energy and proper orientation during collision.
- Energy barrier built-up when the collision is about to take place.
- Activated complex formation.
- Difference in energy of the reactant and the product – exoergic and endoergic reactions with proper graphs and labelling
- Meaning of elementary reaction.
- Meaning of complex and overall reaction.
- Explanation of the mechanism of the reaction.
- Bottleneck principle and slow step.
- Relationship between the rate expression, order of reactants and products at the rate- determining step.
- Units of rate constant – explanation with suitable examples.
- Chemical Kinetics
- Collision Theory of Chemical Reactions
- Collision between reactant molecules
- Energy requirement - Activation energy
- Orientation of reactant molecules
- Effect of Temperature on the Rate Constant of a Reaction
- Arrhenius equation – K=Ae-Ea/RT .
- Meaning of the symbols of Arrhenius equation.
- Related graph, evaluation of Ea and A from the graph.
- Meaning of slope of the graph.
- Conversion from exponential to log form of the equation.
- Relationship between the increase in temperature and the number of collisions.
- Numerical based on Arrhenius equation.
- Chemical Kinetics
- The Concept of Energy
- Temperature Dependence of the Rate of a Reaction
- Activation energy
- Arrhenius equation
- Most probable kinetic energy
- Effect of Catalyst
- Exothermic and endothermic reactions.
- Concept of energy barrier.
- Threshold and activation energy.
- Formation of activated complex.
- Effect of catalyst on activation energy and reaction rate.
- Catalyst
- Types of Catalyst
positive and negative
- Homogeneous and Heterogeneous Catalyst
based on the state of the reactant and the catalyst
- Characteristics of a Catalyst
promoter, poison, specificity
- Types of Catalyst
- Effect of Catalyst on the Rate of Reaction
- Definition.
- Types of catalyst – positive and negative.
- Homogeneous and heterogeneous catalyst based on the state of the reactant and the catalyst.
- Elementary treatment of intermediate compound formation theory with examples; Adsorption Theory.
- Effect of catalyst on the rate of reaction – the change in the energy of activation in the activation energy curve.
- Characteristics of a catalyst – promoter, poison, specificity, surface area of a catalyst.
- Meaning of Chemical Kinetics
- Slow and Fast Reactions
explanation in terms of bonds
- Slow and Fast Reactions
- Scope and importance of Kinetics of the reaction.
- Slow and fast reactions – explanation in terms of bonds.
- Rate of a Chemical Reaction
- Average rate of a reaction
- Units of rate of a reaction
- Instantaneous rate
- Stoichiometry and rate of a reaction
- Rate law and rate constant
- Differences between rate and rate constant of a reaction
- Rate of a Reaction
- Factors Affecting Rate of Reaction
- Definition
- Representation of rate of reaction in terms of reactants and products.
- Determination of rate of reactions graphically.
- Instantaneous and average rate of reaction
- Law of Mass Action
- Explanation with an Example – General Reactions
Law of Mass Action
- Explanation with an Example – General Reactions
- Chemical Kinetics
- Statement and meaning of active mass.
- Explanation with an example – general reactions
- Chemical Kinetics
- Dependence of Rate on Reactant Concentrations: Rate Law and Rate Constant
- Qualitative Treatment
Based on the law of Mass Action
- General rate equation
Rate = k(Concentration of the reactant) n
- Qualitative Treatment
- Qualitative treatment Based on the law of Mass Action.
- Statement of rate law.
- General rate equation – Rate = k(Concentration of the reactant) n
where k is rate constant and n is the order of the reaction.
Relation between the rate of the reaction with rate constant with respect to various reactants.
- Meaning – physical picture.
- Relation between order, molecularity and the rate of a reaction.
- Differences between order and molecularity of a reaction.
CISCE Class 12 Chemistry (Theory) Syllabus for Chemical Equilibria
- Chemical Equilibria
- Reversible Reactions and Dynamic Equilibrium
- The Dynamic Nature
Law of mass action
- Relationship Between Kp and Kc
Derivation required
- The Dynamic Nature
Reversible reactions and dynamic equilibrium. The concept of equilibrium constant in terms of concentration or partial pressure to indicate the composition of the equilibrium mixture. The following are the examples: the dissociation of dinitrogen tetroxide, hydrolysis of simple esters, the Contact Process for the manufacture of sulphuric acid, the synthesis of ammonia by Haber’s process.
- Irreversible and reversible reactions.
- Chemical equilibrium:
- Characteristics of chemical equilibrium.
- The dynamic nature. - Law of mass action.
- Equilibrium constant in terms of concentration Kc.
- Gaseous reactions. Equilibrium constant in terms of partial pressures Kp.
- Relationship between Kp and Kc (Derivation required).
- Characteristics of equilibrium constant.
- Units for equilibrium constant.
- Simple calculations of equilibrium constant and concentration
The following examples should be considered to show maximum yield of products:
- Synthesis of ammonia by Haber’s process.
- The dissociation of dinitrogen tetra oxide.
- Hydrolysis of simple esters.
- The Contact Process for the manufacture of sulphuric acid.
- Factors affecting equilibrium: Le Chatelier’s principle
- Le Chatelier’s Principle
Statement and explanation
- Change of Concentration
- Effect of change in concentration
- Change of Temperature
- Effect of change in temperature
- Change of Pressure
- Effect of change in pressure
- Addition of Inert Gas
- Effect of addition of inert gas
- Addition of an inert gas at constant volume
- Addition of an inert gas at constant pressure
- Le Chatelier’s Principle
Le Chatelier’s Principle. Statement and explanation.
Factors affecting chemical and physical equilibria should be discussed in the light of Le Chatelier’s Principle.
- Change of concentration.
- Change of temperature.
- Change of pressure.
- Effect of catalyst.
- Addition of inert gas.
CISCE Class 12 Chemistry (Theory) Syllabus for Ionic Equilibria
- Acids
- Arrhenius, Bronsted-lowry and Lewis Concept of Acids and Bases
- Arrhenius Concept of Acids and Bases
- The Brönsted-Lowry Acids and Bases
- Lewis Acids and Bases
- Arrhenius, Bronsted-lowry and Lewis Concept of Acids and Bases
Arrhenius, Brönsted-Lowry and Lewis concept of acids and bases, Multistage ionization of acids and bases with examples.
Self explanatory
- Ionic Equilibria
- Multistage Ionization of Acids and Bases with Examples
Ionic Equilibria
- Multistage Ionization of Acids and Bases with Examples
Ionic product of water, pH of solutions and pH indicators.
Ionic product of water – definition, pH, pOH, pKw of solutions; Numericals on the above concepts. pH indicators and their choice in titrimetry.
- Ionic Equilibria
- Salt Hydrolysis
- Salts of strong acid and a strong base
- Hydrolysis of Salt of strong base and weak acid (Anionic Hydrolysis)
- Hydrolysis of salt of strong acid and weak base (Cationic Hydrolysis)
- Hydrolysis of Salt of weak acid and weak base (Anionic & Cationic Hydrolysis)
- Salt Hydrolysis
Salt hydrolysis – salts of strong acids and weak bases, weak acids and strong bases, weak acids and weak bases and the derivation of pH of the solutions of these salts in water with suitable examples (in detail). Numericals
- Buffer Solutions
- Types of buffer solutions
- Buffer action
- Buffer capacity and buffer index
- Henderson - Hasselbalch equation
- Properties of buffer solution
- Applications of buffer solution
- In biochemical system
- Agriculture
- Industry
- Medicine
- Analytical chemistry
- Ionic Equilibria
- Buffer Interpretations
based on Le Chatelier’s principle
- Buffer
Numericals
- Buffer Interpretations
Buffer solutions: definition, examples, action; its interpretations based on Le Chatelier’s principle. Henderson’s equation. Numericals.
- Solubility Product
- Solubility product
definition and application in qualitative salt analysis (Group II, III and IV cations).
- Solubility product
- Solubility equilibria
- Relationship between solubility and solubility product
- Condition of precipitation
- Determination of solubility product from molar solubility
- Solubility product
Solubility product: definition and application in qualitative salt analysis (Group II, III and IV cations). Numericals on solubility product.
Ostwald’s dilution law and its derivation.
Strength of acids and bases based on their dissociation constant.
Ostwald’s dilution law - statement and derivation. Strengths of acids and bases based on their dissociation constant; problems based on the Ostwald’s dilution law.
- Ionization of Acids and Bases
- Ionic Equilibria
- Common Ion Effect Example
acetic acid and Sodium acetate; ammonium hydroxide and ammonium chloride
- Common Ion Effect Example
Common ion effect – definition, examples (acetic acid and Sodium acetate; ammonium hydroxide and ammonium chloride), applications in salt analysis.
CISCE Class 12 Chemistry (Theory) Syllabus for Electrochemistry
- Applications of Electrolysis
- Faraday’s 1st Law of Electrolysis
Statement, mathematical form
- Faraday’s 1st Law of Electrolysis
Numericals
- Faraday’s 2nd Law of Electrolysis
Simple problems
- Faraday’s 2nd Law of Electrolysis
Statement, mathematical form
- Faraday’s 1st Law of Electrolysis
Faraday’s laws of Electrolysis, Coulometer. Faraday’s Ist law of electrolysis. Statement, mathematical form. Simple problems.
Faraday’s IInd law of electrolysis: Statement, mathematical form. Simple problems.
- Batteries
- Primary Batteries
- Dry cell
- Mercury cell
- Primary Batteries
- Galvanic Cells, Mechanism of Current Production in a Galvanic Cell;
- principle – oxidation reduction
Galvanic cells
- Measurement of potential
Galbanic Cell
- Single Electrode Potentials
Galvaniv cell
- Standard Hydrogen Electrode
definition, preparation, application and limitations
- principle – oxidation reduction
- Nernst Equation - Introduction
- Derivation of Nernst equation
- Applications of Nernst equation
Galvanic cells, mechanism of current production in a galvanic cell; and electrode potential, standard hydrogen electrode, electrochemical series, Nernst equation.
Galvanic cells - introduction; representation, principle – oxidation reduction. Mechanism of production of electric current in a galvanic cell. Measurement of potential. Single electrode potentials. Electrical double layer. Standard hydrogen electrode - definition, preparation, application and limitations.
(a) Standard electrode potential, measurement of standard electrode potential.
Measurement of standard electrode potential of Zn ++ / Zn0 half cell (using standard hydrogen electrode).
(b) Idea of heterogeneous equilibria on the surface of the electrode. Cell notation.
(c) Factors affecting electrode potential. Factors affecting electrode potential with explanation - main emphasis on the temperature and concentration and nature of the electrode.
(d) Electrochemical series and its explanation on the basis of standard electrode potential. Electrochemical series. Its explanation on the basis of standard reduction potential. Prediction of the feasibility of a reaction.
(e) Numericals based on calculation of emf of a cell from the values of standard electrode potential.
(f) Nernst equation (correlation with the free energy of the reaction).
- Nernst equation with suitable examples.
- Prediction of spontaneity of a reaction based on the cell emf.
- Numericals on cell emf and standard electrode potential of half-cells.
Relation between Faraday, Avogadro’s number and charge on an electron. F = NAe should be given (no details of Millikan’s experiment are required).
Self-explanatory
- Electrochemistry
- Kohlrausch's law
Numericals
- Kohlrausch's law
- Electrolytic Conductance
- General Relationship Between
specific conductance, molar conductance and equivalent conductance
- Units, numericals, graph
Electrolytic conductance
- General Relationship Between
- Conductance of Electrolytic Solutions
- Variation of Conductivity and Molar Conductivity with Concentration
- Variation of conductivity with concentration
- Molar conductivity
- Limiting molar conductivity
- Variation of molar conductivity for strong electrolytes
- Kohlrausch's law of independent migration of ions
- Variation of molar conductivity for weak electrolytes
- Applications of Kohlrausch's law
- Variation of Conductivity and Molar Conductivity with Concentration
Electrolytic conductance: specific conductance. Measuring of molar and equivalent conductance; Kohlrausch's law.
Comparison of metallic conductance and electrolytic conductance. Relationship between conductance and resistance. Specific resistance and specific conductance.
Cell constant: Calculation of cell constant. Meaning of equivalent conductance. Meaning of molar conductance. General relationship between specific conductance, molar conductance and equivalent conductance.
Units, numericals, graph.
Molar conductance of a weak electrolyte at a given concentration and at infinite dilution. Kohlrausch’s Law – definition and numericals.
- Electrochemistry
- Batteries
- Lead storage battery
structure, reactions and uses
- fuel cell
structure, reactions and uses
- Lead storage battery
Primary and Secondary Cells: Lead storage battery and fuel cell – structure, reactions and uses.
- Concept of Corrosion
- Corrosion
- Corrosion of iron (Rusting)
- Mechanism of Electrochemical Reaction
Corrosion
- Corrosion Prevention
- Prevention of corrosion
- Coating metal surface by paint or chemicals
- Galvanization (coating with Zn)
- Cathodic Protection
Concept, mechanism of electrochemical reaction, factors affecting it and its prevention
CISCE Class 12 Chemistry (Theory) Syllabus for Coordination Compounds
- Coordination Compounds
- calculation for a complex coordination sphere
coordination number
- calculation for a complex coordination sphere
- Definitions of Some Important Terms Pertaining to Coordination Compounds
Coordination entity, Central atom/ion, Ligands, Colour, Shapes, Coordination number, Coordination sphere, Coordination polyhedron, Oxidation number of central atom, Homoleptic and heteroleptic complexes, charge number
- Nomenclature of Coordination Compounds - Naming of Mononuclear Coordination Compounds
- Isomerism in Coordination Compounds
- Stereoisomerism
Geometric Isomerism, Optical Isomerism
- Stereoisomerism
- Importance and Applications of Coordination Compounds
- Bonding in Coordination Compounds
- Valence Bond Theory (VBT)
- Valence bond theory (VBT)
- Salient features of valence bond theory
- Coordination number and types of hybridisation
- Steps used to understand metal-ligand bonding in coordination complex using valence bond theory
- Structures of some complex compounds based on valence bond theory
- Magnetic properties of coordination compounds based on Valence Bond Theory
- Limitations of valence bond theory
- Crystal Field Theory (CFT)
- Crystal field theory
- Crystal field splitting in octahedral and tetrahedral coordination entities
- Application of crystal field theory to octahedral complexes and tetrahedral complexes
- Limitations of Crystal Field Theory
- Valence Bond Theory (VBT)
- Stability of Coordination Compounds
- Stability of coordination compounds
- Factors which govern stability of the complex
- Charge to size ratio of the metal ion
- Nature of the ligand
- Stability of chelates
Concept of complexes; definition of ligands; classification of ligands, coordination number, coordination sphere; IUPAC nomenclature of coordination compounds; isomerism; magnetic characteristics of coordination compounds on the basis of valence bond theory and crystal field theory. Stability constant; uses of coordination compounds in different fields.
- Definition of coordination compounds / complex compounds.
- Differences with a double salt.
- Study of ligands – mono-, bi-, tri-, tetra-, penta-, hexa- and polydentate, chelating ligands.
- Definition of coordination number, its calculation for a complex coordination sphere.
- Study of oxidation state of an element in a complex, its calculation. IUPAC rules of nomenclature of coordination compounds.
- Isomerism – types and examples.
- Valence bond theory of coordination compounds – examples of formation of inner orbital [Fe(CN)6] 3-, [Co(NH3)6] 3+ and outer orbital [CoF6] 3-, [Fe(H2O)6] 2+ complexes, prediction of magnetic character. Crystal field theory – crystal field splitting in tetra and octahedral systems. Explanation of colour and magnetic character.
- Stability of coordination compounds (explain stability on the basis of magnitude of K).
- Importance and uses.
CISCE Class 12 Chemistry (Theory) Syllabus for Chemistry of p-Block Elements: Group 16, 17, 18
- Concept of Group 16 Elements
Occurrence, Electronic Configuration, Atomic and Ionic Radii, Ionisation Enthalpy, Electron Gain Enthalpy, Electronegativity, Physical Properties and Chemical Properties (Oxidation states and trends in chemical reactivity and Anomalous behaviour of oxygen)
- P - Block Group 16 Elements
- Ozone
- Preparation, Properties, Uses
- Sulphur - Allotropic Forms
- Rhombic sulphur (α-sulphur)
- Monoclinic sulphur (β-sulphur)
- Sulphur Dioxide
- Preparation, Properties, Uses
- Reaction of Sulphur Dioxide
with NaOH, Cl2 and KMnO4
- Sulphuric Acid
- Manufacture, Properties, uses
- Ozone
- Concept of Group 17 Elements
Occurrence, Electronic Configuration, Atomic and Ionic Radii, Ionisation Enthalpy, Electron Gain Enthalpy, Electronegativity, Physical Properties and Chemical Properties (Oxidation states and trends in chemical reactivity and Anomalous behaviour of fluorine)
- P - Block Group 17 Elements
- Reaction of Fluorine
with hydrogen, water, hydrogen sulphide, dilute and conc. Alkalies
- Chlorine
preparation from MnO2 and HCl, from NaCl, MnO2 and conc. H2SO4 (only equations)
- Reaction of Fluorine
- P - Block Group 18 Elements
- Concept of Group 18 Elements
Occurrence, Electronic Configuration, Ionisation Enthalpy, Atomic Radii, Electron Gain Enthalpy, Physical Properties and Chemical Properties (Xenon-fluorine compounds and Xenon-oxygen compounds)
- State, Low Reactivity
Group 18 Elements
- Concept of Group 18 Elements
- Hybridization, Shape and Structure of Compounds
Group 16, 17, 18 - The following should be included:
(a) Occurrence, (b) Physical State, (c) Electronic configuration, (d) Atomic and ionic radii, (e) Common oxidation states, (f) Electronegative character, (g) Ionisation enthalpy, (h) Oxidising nature, (i) Nature of oxides, hydroxides, hydrides, carbonates, nitrates, chlorides, sulphates, wherever applicable.
Group 16: O, S, Se, Te
General Characteristics in terms of physical and chemical properties. Oxygen – lab method of preparation, formation of oxides with metals and non-metals and their common nature.
Sulphur – extraction by Frasch process, allotropes of sulphur rhombic, monoclinic), structure of sulphur.
Group 17: F, Cl, Br, I
General characteristics in terms of physical and chemical properties.
Fluorine – electrolysis of potassium hydrogen fluoride; reaction of fluorine with hydrogen, water, hydrogen sulphide, dilute and conc. Alkalies.
Chlorine – preparation from MnO2 and HCl, from NaCl, MnO2 and conc. H2SO4 (only equations), reactions of chlorine with H2S, NH3, cold, dilute NaOH and hot, concentrated NaOH.
Interhalogen compounds – structure, hybridization and shapes. XX′, XX′3, XX′5, XX′7.
Group 18: Noble gases – He, Ne, Ar, Kr, Xe
General Characteristics – state, low reactivity, formation of Xenon compounds with fluorine and oxygen – equation, hybridization, shape and structure of compounds; uses of noble gases.
CISCE Class 12 Chemistry (Theory) Syllabus for Preparation/ Manufacture, Properties and Uses of Compounds of Groups 16, 17, – Ozone, Sulphur Dioxide, Sulphuric Acid, Hydrochloric Acid
- P - Block Group 16 Elements
- Ozone
- Preparation, Properties, Uses
- Sulphuric Acid
- Manufacture, Properties, uses
- Ozone
- Ozone Layer Depletion
- Oxidising Nature
ozone
- Ozone Depletion in the Stratosphere
- Ozone Layer Depletion
- causes and prevention (to be covered theoretically, no reactions are required)
- Formation of ozone:- relevant equations
- Function in the atmosphere.
- Destruction of the ozone layer:- chemicals responsible for this to be named but reactions not required.
- Hydrogen Peroxide
- Physical properties
- Chemical properties
- Uses of hydrogen peroxide
- Structure of hydrogen peroxide
- Oxidising Nature
- Hydrogen Peroxide
- Preparation from Peroxide
Hydrogen peroxide
- Oxidising Properties
Hydrogen peroxide
- Reaction with Ki, Pbs, Acidified Feso4,
Hydrogen peroxide
- Reducing Properties
reaction with acidified KMnO4 and chlorine
- Preparation from Peroxide
- Structure of Hydrogen Peroxide
- Hydrochloric Acid
- Hydrochloric Acid
- Importance of Hydrochloric Acid
- Lab preparation, its acidic nature, reaction with ammonia, carbonates and sulphites, formation of aqua regia and its uses
Hydrochloric Acid
Group 16:
Ozone:
Manufacture by Siemen’s Ozoniser, thermal decomposition of ozone, its oxidising nature – reaction with lead sulphide, potassium iodide and mercury, ozonolysis of ethene, ozone layer depletion :causes and prevention (to be covered theoretically, no reactions are required), resonance in ozone structure and its uses.
Hydrogen peroxide:
Preparation from peroxide, structure, oxidising properties: reaction with KI, PbS, acidified FeSO4,; reducing properties – reaction with acidified KMnO4 and chlorine.
Sulphur Dioxide:
Laboratory and industrial preparation from sulphites and sulphide ores, reaction of sulphur dioxide with NaOH, Cl2 and KMnO4.
Sulphuric Acid:
Manufacture by Contact Process (equations, conditions and diagram), properties - acidic nature, mode of dilution, oxidising action and dehydrating nature, uses of sulphuric acid in industry.
Group 17:
Hydrochloric acid: Lab preparation, its acidic nature, reaction with ammonia, carbonates and sulphites, formation of aqua regia and its uses.
CISCE Class 12 Chemistry (Theory) Syllabus for Chemistry of Transition and Inner-Transition Elements: d-Block: 3d, 4d and 5d series f-Block: 4f and 5f series
- Chemistry of Transition and Inner-transition Elements: D-block: 3d, 4d and 5d Series
- Chemistry of Transition and Inner-transition Elements: F-block: 4f and 5f Series
- General Properties of the Transition Elements (D-block)
- Properties of the first-row transition metals – metallic character
- Atomic and ionic radii
- Metallic character
- Melting and boiling points
- Colour
- Physical Properties
- Variation in Atomic and Ionic Sizes of Transition Metals
- Ionisation Enthalpies
- Oxidation States
- Standard electrode potentials
- Trends in the M2+/M Standard Electrode Potentials
- Trends inthe M3+/M2+ Standard Electrode Potentials
- Trends in Stability of Higher Oxidation States
- Chemical Reactivity and Eθ Values
- Magnetic Properties
- Formation of Coloured Ions
- Formation of Complex Compounds
- Catalytic Properties
- Complex formation
- Formation of Interstitial Compounds
- Alloy Formation
- Oxides and oxoanions of transition metals
- F-block Elements
- The Lanthanoids
Electronic Configurations, Atomic and Ionic Sizes, Oxidation States, General Characteristics, Chemical Reactivity and Lanthanoid Contraction and Its Consequences
- Radioactive Nature
Lanthanoids
- The Actinoids
Electronic Configurations, Ionic Sizes, Oxidation States, General Characteristics and Comparison with Lanthanoids between lanthanoids and actinoids
- Compounds Agno3, Kmno4
Actinoids
- The Lanthanoids
- Shielding Effect
- Electrochemical Principles of Metallurgy
- Aluminium - Hall-Heroult process
- Copper from Low Grade Ores and Scraps
- Electrolytic Refining and Uses
- Silver Nitrate: Equation of Preparation
- Use in Laboratory and in Photography
Silver nitrate
- Potassium Permanganate
- Structure and Shape
Potassium permanganate
- Equation of Extraction from Pyrolusite Ore
Potassium permanganate
- Oxidising Nature in Acidic, Basic and Neutral Medium
Potassium permanganate
- Use in Redox Titration
Potassium permanganate
- Potassium Dichromate
- Equation of Extraction from Chromite Ore
Potassium dichromate
- Structure and Shape of Molecule and Its Use in Titration
Potassium dichromate
- Occurrence of Metals
- Occurrence of metals
- Minerals and ores
d-Block: 3d, 4d and 5d series
f-Block: 4f and 5f series
Study in terms of metallic character, atomic and ionic radii, ionisation enthalpy, oxidisation states, variable valency, formation of coloured compounds, formation of complexes, alloy formation.
Lanthanoids: Lanthanoid contraction, shielding effect, radioactive nature.
Actinoids – general electronic configuration, oxidation state, comparison with lanthanoids and uses.
Metallurgy of Al, Zn, Fe, Cu and Ag in terms of equations, thermodynamics and electrochemical principles involved in the extraction of metals; electrolytic refining and uses.
Compounds –
1. Silver nitrate: equation of preparation, use in laboratory and in photography.
2. Potassium permanganate: structure, shape, equation of extraction from pyrolusite ore, its oxidising nature in acidic, basic and neutral medium, use in redox titration.
Oxidising nature in acidic [FeSO4, (COOH)2.2H2O, KI], basic (KI) and neutral (H2S) mediums to be done.
3. Potassium dichromate: equation of extraction from chromite ore, structure and shape of molecule and its use in titration.
Self-explanatory.
CISCE Class 12 Chemistry (Theory) Syllabus for Alkyl and Aryl Halides
- Organometallic Compounds
- Preparation and Uses
organometallic-compounds
- Preparation and Uses
Organometallic compounds including Grignard’s reagent, preparation and their uses. Wilkinson’s and Ziegler-Natta catalyst.
Naming the halogen derivatives of alkanes by using common system and IUPAC system for mono, di and tri-halo derivatives.
- Haloalkanes
- Preparation of Haloalkanes from - Alcohol
PCl3, PCl5 and SOCl2
- General properties of Haloalkanes
Combustibility, Nucleophilic substitution reactions
- Preparation of Haloalkanes from - Alcohol
Preparation from:
- Alkane and halogen.
- Alkene and hydrohalide.
- Alcohols with PCl3, PCl5 and SOCl2.
General properties:
- Combustibility.
- Nucleophilic substitution reactions.
Reaction with:
- sodium nitrite.
- silver nitrite.
- aq. sodium hydroxide.
- alcoholic potassium hydroxide.
Uses:
Uses of halogen derivatives of alkanes in day to day life and in industry may be discussed
- Chlorobenzene
- Chlorobenzene
- Preparation from Aniline
Chlorobenzene
- Physical Properties and Chemical Properties
Chlorobenzene
- Nucleophilic Substitution
Chlorobenzene
- Reduction to Benzene
Chlorobenzene
- Addition Reaction with Magnesium
formation of Grignard reagent
- Preparation from Aniline
- Phenols
- Polyhalogen Compounds
- Dichloromethane (Methylene chloride)
- Trichloromethane (Chloroform)
- Triiodomethane (Iodoform)
- Tetrachloromethane (Carbon tetrachloride)
- Freons
- p,p’-Dichlorodiphenyltrichloroethane (DDT)
- Environmental effects of polyhalogen compounds
Chlorobenzene.
Preparation from aniline.
Physical properties
Chemical properties:
- Electrophilic substitution (chlorination nitration and sulphonation).
- Nucleophilic substitution
- replacement of chlorine with -OH, -NH2.
- Reduction to benzene.
- Wurtz-Fittig reaction.
- Fittig reaction.
- Addition reaction with magnesium (formation of Grignard reagent).
- Formula of DDT
- Preparation, Properties, and Uses of the Following: Ethyl Bromide, Chloroform, Iodoform, Haloform Reaction
- Haloform Reaction for the Preparation of Chloroform and Iodoform from Alcohol Should Be Discussed
Preparation, properties, and uses of the following: ethyl bromide, chloroform, iodoform, haloform reaction.
Preparation.Properties and uses of ethyl bromide, chloroform, iodoform.
Haloform reaction for the preparation of chloroform and iodoform from alcohol should be discussed.
CISCE Class 12 Chemistry (Theory) Syllabus for Alcohols and Phenols
- Alcohol
- Methods of Preparation
Alcohols
- Uses of Alcohols
- Uses of methyl alcohol
- Uses of ethyl alcohol
- Methods of Preparation
- Methods of Preparation and Manufacture of Alcohol
- Reaction with Hydrogen Halides
property of alcohol
- Reaction with Hydrogen Halides
Methods of preparation:
- Hydration of Alkenes
– direct hydration, hydroboration oxidation.
- From Grignard’s reagent.
- Hydrolysis of alkyl halides.
- Reduction of carboxylic acids.
Manufacture of methanol by Bosch process and ethanol by fermentation of carbohydrates, chemical equations required (only outline of the method of manufacture, detail not required).
Properties:
- Acidity of alcohols: reaction with sodium.
- Esterification with mechanism.
- Reaction with hydrogen halides.
- Reaction with PCl5, PCl3 and SOCl2.
- Reaction with acid chlorides and acid anhydrides
- Oxidation.
- Dehydration with mechanism.
Uses of alcohols
- Preparation, Properties and Uses of Ethane-1, 2 Diol
- Physical Properties, Chemical Properties
Ethane-1, 2-diol
- Physical Properties, Chemical Properties
- Preparation, Properties and Uses of Propane-1, 2, 3 Triol
- Preparation from Soap: Saponification
Propane – 1, 2, 3-triol
- Physical Properties
Propane – 1, 2, 3-triol
- Oxidation with Kmno4 and Reaction with Oxalic Acid
Propane – 1, 2, 3-triol
- Preparation from Soap: Saponification
- Chemical Properties
- Laboratory test of haloalkanes
- Nucleophilic substitution reactions of haloalkanes
- Mechanism of SN reaction
- Factors influencing SN1 and SN2 mechanism
- Elimination reaction : Dehydrohalogenation
Ethane-1, 2-diol:
- Preparation from ethene.
- Physical properties.
- Chemical properties: Oxidation to oxalic acid and reaction with HCl.
Propane – 1, 2, 3-triol:
- Preparation from soap: saponification.
- Physical properties.
- Chemical properties: Oxidation with KMnO4 and reaction with oxalic acid.
- Alcohol
- Phenols
- Physical and Chemical Properties
Phenols
- Phenol Reaction with Zinc
Reaction with zinc
- Reimer
Phenol
- Physical and Chemical Properties
- Chemical Properties of Phenol
- Chemical Properties of Phenol
- Reactions involving cleavage of O-H bond: Reaction with metals, Esterification, Acetylation
- Electrophilic aromatic substitution reactions of phenol
(i) Nitration
(ii) Halogenation (bromination) - Kolbe's reaction
- Reimer-Tiemann reaction
- Reaction of phenol with zinc dust
- Catalytic hydrogenation
- Oxidation reaction
- Distinguishing test between alcohols and phenols
- Differentiation between alcohols and phenols
v) Distinction between primary, secondary and tertiary alcohols. Distinction through oxidation, dehydration and Lucas’ Test.
- Phenol
Preparation of phenol from diazonium salt, chlorobenzene (Dow’s process) and from benzene sulphonic acid.
Manufacture from Cumene.
Physical properties.
Chemical properties:
- Acidic character of phenol.
- Reaction with sodium hydroxide.
- Reaction with sodium.
- Reaction with zinc.
- Reaction with acetyl chloride and acetic anhydride.
- Reaction with phosphorus penta chloride.
- Bromination, nitration and sulphonation (Electrophilic substitution reactions).
- Kolbe’s reaction (formation of salicylic acid).
- Reimer
– Tiemann reaction Test for phenol
– FeCl3 test, azo dye test.
Classification into monohydric, dihydric and polyhydric alcohols, general formulae, structure and nomenclature of alcohols. Difference between primary, secondary and tertiary alcohols in terms of structure, physical properties and chemical properties.
Conversion of one alcohol into another. Self-explanatory.
CISCE Class 12 Chemistry (Theory) Syllabus for Ethers, Carbonyl Compounds
- Introduction of Aldehydes, Ketones and Carboxylic Acids
- Preparation of Aldehydes and Ketones
- Methods for the preparation of aldehydes and ketones
- By oxidation of alcohols
- By dehydrogenation of alcohols
- From hydrocarbons
(i) By ozonolysis of alkenes
(ii) By hydration of alkynes
- Aldehydes and Ketones
- Preparation of Aldehydes and Ketones From acid chlorides
Rosenmund’s reduction, reaction with dialkyl cadmium
- Chemical Reactions of Aldehydes and Ketones - Nucleophilic Addition Reactions
- Mechanism of nucleophilic addition reactions
- Reactivity
- Some important examples of nucleophilic addition and nucleophilic addition-elimination reactions
(a) Addition of hydrogen cyanide (HCN)
(b) Addition of sodium hydrogensulphite
(c) Addition of Grignard reagents
(d) Addition of alcohols
(e) Addition of ammonia and its derivatives
- Reactions with Ammonia, Hydroxylamine, Hydrazine and Phenyl Hydrazine
aldehydes and ketones
- Oxidation Reactions
aldehydes and ketones
- Reduction to Alcohol and Alkanes
Clemmensen’s reduction and Wolff-Kishner reduction, Red phosphorus and HI.
- Base Catalysed Reactions
Aldol, cross Aldol condensation, Cannizzaro’s reaction
- Nucleophilic Addition Reaction
hydrogen cyanide and sodium bisulphite
- Benzaldehyde Reactions with Ammonia and Its Derivatives
hydroxyl amine, hydrazine and phenyl hydrazine
- Preparation of Aldehydes and Ketones From acid chlorides
- Uses of Aldehydes and Ketones
- Phenols
- Physical Properties – State and Boiling Point
methods of preparation, properties and uses of aldehydes and ketones.
Preparation:
- From alcohol.
- From alkenes (ozonolysis).
- From alkynes (hydration).
- From acid chlorides (Rosenmund’s reduction, reaction with dialkyl cadmium).
- From calcium salt of carboxylic acids.
Physical properties.
Chemical properties:
- Nucleophilic addition reactions.
- Reactions with ammonia, hydroxylamine, hydrazine and phenyl hydrazine.
- Oxidation reactions.
- Reduction: reduction to alcohol and alkanes (Clemmensen’s reduction and Wolff-Kishner reduction).
- Base catalysed reactions: Aldol, cross Aldol condensation, Cannizzaro’s reaction.
- Iodoform reaction.
Uses.
Tests: difference between formaldehyde and acetaldehyde; aldehydes and ketones.
- Benzaldehyde
Lab preparation from Toluene, oxidation by chromyl chloride.
Physical properties.
Chemical properties:
- Oxidation and reduction.
- Nucleophilic addition reaction (hydrogen cyanide and sodium bisulphite).
- Reactions with ammonia and its derivatives (hydroxyl amine, hydrazine and phenyl hydrazine).
- Reaction with phosphorus pentachloride.
- Cannizzaro reaction.
- Benzoin condensation.
- Electrophilic substitution
- halogenation, nitration and sulphonation.
Test: distinction between aromatic and aliphatic aldehydes.
Uses of benzaldehyde
- General Formula and Structure
Ether
- Alcohols, Phenols and Ethers
- Ethers
- Preparation of Ethers
- From alcohols by dehydration (continuous etherification process)
- From alkyl halides (Williamson synthesis)
- Preparation of Ethers
general formula and structure. Nomenclature; preparation, properties and uses of ether (outline, no detail), with reference to diethyl ether.
Ethers: structure of ethereal group.
Preparation from alcohol (Williamson’s synthesis).
Physical properties.
Chemical properties:
- Reaction with chlorine.
- Oxidation (peroxide formation).
- Reaction with HI.
- Reaction with PCl5.
Uses of ether.
CISCE Class 12 Chemistry (Theory) Syllabus for Carboxylic acids and Acid Derivatives
- Introduction of Carboxylic Acids
- Classification of mono and di carboxylic acids with examples.
- Acids
- Methods of Preparation of Carboxylic Acids
- Oxidation of primary alcohols and aldehydes
- Oxidation of alkyl benzene
- From nitriles and amides (hydrolysis)
- From aryl amines and alkyl halides
- Carboxylation of Grignard reagent
- Hydrolysis of acyl chloride and acid anhydride
- Hydrolysis of esters
- Decarboxylation
chemical and Kolbe’s electrolytic reaction
- Decarboxylation
chemical and Kolbe’s electrolytic reaction
- Methods of Preparation of Carboxylic Acids
- Physical Properties of Carboxylic Acids
- Classification of Mono and Di Carboxylic Acids with Examples
- Preparation of Carboxylic Acids from Alcohols, Aldehydes
- Acid Derivatives
- Oxalic Acid
- Esterification Reaction
Oxalic acid
- Esterification Reaction
- Benzoic Acid
- Esterification reaction
Benzoic acid
classification, general formulae, structure and nomenclature: monocarboxylic acids, general methods of preparation, properties and uses of acids.
Carboxylic acids: Classification of mono and di carboxylic acids with examples.
Preparation:
- From alcohols, aldehydes.
- From nitriles.
- From Grignard’s reagent.
Physical properties.
Chemical properties:
- Acidic character: reaction with active metals, alkalies, carbonates and bicarbonates,
- Formation of acid derivatives.
- Decarboxylation (chemical and Kolbe’s electrolytic reaction).
- HVZ reactions. Tests for acids: formic acid and acetic acid.
Uses of formic acid and acetic acid.
- Oxalic acid: Preparation from glycol and sodium formate.
Physical properties.
Chemical properties:
- Reaction with alkali.
- Esterification reaction.
- Reaction with PCl5 .
- Action of heat on oxalic acid.
- Oxidation by potassium permanganate.
Test for oxalic acid.
Uses of oxalic acid.
- Benzoic acid Preparation from benzaldehyde and Toluene.
Physical properties
Chemical properties:
- With sodium hydroxide, sodium carbonate.
- Esterification reaction.
- With phosphorus pentachloride.
- Decarboxylation.
- Substitution of benzene ring (meta directive effect of carboxylic acid group) nitration and sulphonation.
Test for Benzoic acid.
Uses of Benzoic acid.
- Acid Derivatives
- Properties and Uses of
Acetyl Chloride, acetic anhydride, acetamide, ethylacetate
- Laboratory Preparation and Uses of
Acetyl chloride, acetic anhydride, ethyl acetate, acetamide, urea (Wohler’s synthesis)
- Properties and Uses of
- Salt Formation with Nitric Acid
- Aldehydes and Ketones
- Preparation of Aldehydes
- Preparation of Aldehydes:
- From acyl chloride (acid chloride)
- From nitriles and esters
- From hydrocarbons
(i) By oxidation of methylbenzene
(a) Use of chromyl chloride (CrO2Cl2)
(b) Use of chromic oxide (CrO3)
(ii) By side chain chlorination followed by hydrolysis
(iii) By Gatterman – Koch reaction
- Preparation of Aldehydes
laboratory preparation, properties and uses of acetyl chloride, acetic anhydride, acetamide, ethylacetate; urea preparation (by Wohler's synthesis), properties and uses of urea, manufacture of urea from ammonia and by cyanamide process.
Acid derivatives:general and structural formula, IUPAC nomenclature, trivial names, laboratory preparation and uses of the following compounds:
Acetyl chloride, acetic anhydride, ethyl acetate, acetamide, urea (Wohler’s synthesis).
Manufacture of Urea from ammonia and by cyanamide process.
Physical properties.
Chemical properties:
(a) Acetyl chloride:
- Hydrolysis.
- Acetylation of alcohol, ammonia and amines.
- Rosenmund’s reduction .
- Formation of acetic anhydride.
- Reaction with Grignard reagent.
(b) Acetic anhydride
- Hydrolysis.
- Acetylation of ethanol and aniline.
- Reaction with PCl5 .
(c) Acetamide
- Acid hydrolysis.
- Reaction with alkalies.
- Hoffmann’s degradation.
- Reaction with nitrous acid.
- Dehydration.
- Reduction
- Amphoteric nature (Reaction with HCl and reaction with HgO).
(d) Ethyl acetate
- Acid hydrolysis.
- Saponification.
- Reaction with ammonia.
- Reaction with phosphorus penta chloride.
- Reduction.
(e) Urea
- Hydrolysis.
- Salt formation with nitric acid.
- Biuret reaction (Test).
- Reaction with hot sodium hydroxide (formation of ammonia and carbon dioxide).
CISCE Class 12 Chemistry (Theory) Syllabus for Cyanides, Isocyanides, Nitro compounds, Amines and Diazonium Salt
- Cyanides, Isocyanides and Nitro Compounds
- Cyanides
- Isocyanides
- Nitro Compounds
- Cyanides and Isocyanides
- Nitrobenzene Method of Preparation
by nitration of benzene with a mixture of concentrated nitric and sulphuric acids
- Nitrobenzene
- Introduction of Amines
- Amines
- Preparation of Amines
- From alkyl halides (by ammonolysis/Hoffmann's ammonolysis method)
- Gabriel phthalimide synthesis
- From alkyl cyanides, amides, and nitro compounds
- From amides (By Hoffmann bromamide degradation)
- Additional methods for the preparation of amines
- Method of Preparation Amines from amides
Hofmann degradation
- Chemical Reactions of Amines - Basic Character of Amines
- Structure-basicity relationship of amines
(a) Alkanamines versus ammonia
(b) Arylamines versus ammonia
- Structure-basicity relationship of amines
- Chemical Reactions of Amines - Alkylation and Acylation
- Alkylation of amines (Hoffmann's exhaustive alkylation)
- Hoffmann elimination
- Benzoylation
- Distinction Between Primary, Secondary and Tertiary Amines
Hinsberg’s Test
- Chemical Reactions of Amines - Electrophilic Substitution
- Bromination
- Nitration
- Sulphonation
- Preparation of Amines
- Classification of Amines
- Classification of amines
- Aliphatic amines
- Aromatic amines
- Physical Properties of Amines
- Aniline
- Aniline Method of Preparation
by the reduction of nitrobenzene
- Acetylation, Alkylation
aniline
- Diazotisation
aniline
- Aniline Method of Preparation
- Anline Reaction with HCl and H2so4
- Benzoylation
- Introduction of Diazonium Salts
- Introduction
- Resonance structure
- Method of preparation of Diazonium salts
- Physical properties
- Chemical reactions
- Replacement reactions involving loss of nitrogen
- Reactions involving retention of diazo group
- Diazonium Salts
- Method of Preparation of Diazonium Salts
- Preparation of diazonium salts by reaction of Aniline and nitrous acid
- Method of Preparation of Diazonium Salts
- Properties of Diazonium Salts
- Sandmeyer’s reaction, Gattermann reaction and replacement of diazo group by – H, -OH, -NO2, coupling reaction with phenol and aniline.
heir nomenclature, general methods of preparation, correlation of physical properties with their structure, chemical properties, their uses
- Cyanides, isocyanides and nitro compounds.
Methods of preparation:
Cyanides:
- From alkyl halide.
- From amide.
Isocyanides:
- From alkyl halide.
- From primary amines.
Nitro compounds:
- From alkyl halide.
- From primary amines.
Physical properties.
Chemical properties:
Cyanides and isocyanides:
- Hydrolysis.
- Reduction.
Nitro compounds:
- Reduction in acidic and neutral medium.
Uses.
- Nitrobenzene Method of preparation (by nitration of benzene with a mixture of concentrated nitric and sulphuric acids).
Physical Properties.
Chemical properties:
- Electrophilic substitution (Chlorination and nitration)
– meta substitution.
- Reduction to aniline. Uses of nitrobenzene.
- Amines Nomenclature, classification with examples, general formula, methods of preparation. Preparation:
- From alcohol.
- From alkyl halide.
- From cyanide.
- From amide (Hofmann degradation).
- From nitro compounds.
Physical properties.
Chemical properties:
- Basic character of amines.
- Alkylation and acylation.
- Reaction with nitrous acid.
- Carbylamine reaction.
Distinction between primary,
secondary and tertiary amines (Hinsberg’s Test).
- Aniline Method of preparation (by the reduction of nitrobenzene).
Physical properties.
Chemical properties.
- Reaction with HCl and H2 SO4 .
- Acetylation, alkylation.
- Benzoylation.
- Carbylamine reaction.
- Diazotisation.
- Electrophilic substitution (bromination, nitration and sulphonation).
Test for aniline
Uses of aniline.
- Diazonium Salts: Preparation from aniline, importance in synthesis of other organic compounds. - Sandmeyer’s reaction, Gattermann reaction and Balz
– Scheimann reaction.
CISCE Class 12 Chemistry (Theory) Syllabus for Polymers
- Polymers
- The Principle of Addition and Condensation Polymerisation
illustrated by reference to natural and synthetic polymers e.g. proteins, polyolefins and synthetic fibres
- PVC
Polymers
- PTFE
Polymers
- The Principle of Addition and Condensation Polymerisation
- Types of Polymerisation Reactions - Rubber
- Natural rubber (Vulcanisation of rubber),
- Synthetic rubbers
- Buna-S rubber
- Buna-N rubber or nitrile rubber
- Neoprene rubber
- Types of Polymerisation Reactions - Condensation Polymerisation Or Step Growth Polymerisation
- Condensation Polymerisation or Step Growth Polymerisation
- Some Important Condensation Polymers
(a) Polyamides: Nylons
(i) Nylon 6, 6
(ii) Nylon 6
(b) Polyesters
(c) Phenol - formaldehyde polymer (Bakelite and related polymers)
(d) Melamine - formaldehyde polymer
Polymerisation: the principle of addition and condensation polymerisation illustrated by reference to natural and synthetic polymers e.g. proteins, polyolefins and synthetic fibres; thermoplastics, thermosetting plastics, chemotrophs; reference should also be made to the effect of chain-length and cross-linking on physical properties of polymers.
Classification: Polythene, polypropene, PVC, PTFE, polystyrene, natural rubber, polyester, Nylon 66, Nylon 6, bakelite (to be learnt in terms of monomers). Uses
CISCE Class 12 Chemistry (Theory) Syllabus for Biomolecules – carbohydrates, proteins, enzymes, vitamins and nucleic acids
- Introduction of Carbohydrates
- Carbohydrates classification
mono (aldose, ketose), oligo (di, tri, tetra saccharides) and poly saccharides – examples: reducing sugars and non reducing sugars – examples and uses
- D-L configuration
- Heating with HI, reaction with hydroxylamine, bromine water, acetic anhydride, nitric acid. Test for glucose and fructose (bromine water test with equation).
- Carbohydrates
- Structures of Glucose
- Structures of glucose
- Open chain structure of glucose
- Cyclic structure of glucose
- Haworth projection formulae
- Structures of Glucose
- Introduction of Proteins
- Amino Acids
- Proteins
- Biomolecules in the Cell
- Enzymes
- Enzymes
- Properties of Enzymes
- Enzymes
- Introduction of Vitamins
- Classification and functions of vitamins
- Vitamins
- Introduction of Nucleic Acids
- Structure of DNA
- Structure of RNA
- Differences between DNA and RNA
- Nucleic Acids
Carbohydrates: definition, classification - mono (aldose, ketose), oligo (di, tri, tetra saccharides) and poly saccharides – examples: reducing sugars and non reducing sugars – examples and uses.
Structures for glucose and fructose (Open and cyclic).
Test for glucose and fructose (bromine water test with equation).
Proteins: Amino acids – general structure, classification and zwitter ion formation. Isoelectric point. Classification of proteins on the basis of molecular shape; primary and secondary structures of proteins – denaturation. (Definitions only. Details and diagrams are not required).
Enzymes: definition, mechanism of enzymatic action.
Vitamins A, B, C, D, E and K: classification (fat soluble and water soluble), deficiency diseases. (Chemical names and structures are not required).
Nucleic acids: basic unit – purine and pyrimidine, DNA – structure (double helical), RNA (No chemical structure required).
CISCE Class 12 Chemistry (Theory) Syllabus for Chemistry in Everyday Life
- Chemicals in Medicines
Chemicals in medicines - analgesics, tranquilizers antiseptics, disinfectants, antimicrobials, antifertility drugs, antibiotics, antacids, antihistamines.
In medicine: antipyretics, analgesics, tranquillisers, antiseptics, disinfectants, anti-microbials, anti-fertility drugs, antihistamines, antibiotics, antacids.
Definition, common examples, uses.
Differences between antiseptics and disinfectants.
- Chemicals in Food
Chemicals in food - preservatives, artificial sweetening agents, elementary idea of antioxidants.
Preservatives: role, example (Sodium benzoate).
Artificial sweetening agents: role, examples (aspartame, saccharine, sucralose and alitame). Soaps and detergents - Classification and their
cleansing action - Soaps and Detergents
Soaps and detergents - classification, structure and some important examples.
Advantage of detergents over soaps; classification of detergents into
anionic/biodegradable, cationic/non- biodegradable and non-ionic - Therapeutic Action of Different Classes of Drugs - Antimicrobials
- Antibiotics
- Antiseptics and disinfectants
Chemicals in medicines - analgesics, tranquilizers antiseptics, disinfectants, antimicrobials, antifertility drugs, antibiotics, antacids, antihistamines.
In medicine: antipyretics, analgesics, tranquillisers, antiseptics, disinfectants, anti-microbials, anti-fertility drugs, antihistamines, antibiotics, antacids.
Definition, common examples, uses.
Differences between antiseptics and disinfectants. Structure not required.
Chemicals in food - preservatives, artificial sweetening agents, elementary idea of antioxidants.
Preservatives: role, example (Sodium benzoate).
Artificial sweetening agents: role, examples (aspartame, saccharine, sucralose and alitame). Soaps and detergents - Classification and their
cleansing action.
Soaps and detergents - classification, structure and some important examples.
Advantage of detergents over soaps; classification of detergents into
anionic/biodegradable, cationic/non- biodegradable and non-ionic
CISCE Class 12 Chemistry (Theory) Syllabus for Surface Chemistry
- Difference Between Absorption and Adsorption
- Definition of physisorption and chemisorption and their differences.
- Factors affecting adsorption of gases on solids.
- Factors Affecting Adsorption of Gases on Solids
- Factors affecting adsorption of gases on solids
- Nature of the gas (adsorbate)
- Nature of adsorbent
- Surface area of the adsorbent
- Temperature of the surface
- Pressure of gas
- Colloidal State
- Thomas Graham classified the substances as crystalloid and colloid
- Classification of substances on the basis of the particle size i.e. true solution, sol and suspension
- Colloidal system is heterogeneous. lyophilic and lyophobic colloid
- Classification of colloidal solutions as micro, macro and associated colloids
- Properties of Colloidal Solutions
- Colligative properties
- Tyndall effect
- Colour
- Brownian movement
- Charge on colloidal particles
- Electrophoresis
- Coagulation of lyophilic sols
- Coagulation or precipitation
- Methods to effect coagulation
- Methods to prevent coagulation of colloids (Protection of colloids)
- Various Application of Colloids