Atoms, Molecules and Chemical Arithmetic :
Dalton’s atomic theory; Gay Lussac’s law of gaseous volume; Avogadro’s
Hypothesis and its applications.
Atomic mass; Molecular mass; Equivalent weight; Valency; Gram atomic
weight; Gram molecular weight; Gram equivalent weight and mole concept;
Chemical formulae; Balanced chemical equations; Calculations (based on mole
concept) involving common oxidation-reduction, neutralization, and
displacement reactions; Concentration in terms of mole fraction, molarity,
molality and normality.
Percentage composition, empirical formula and molecular formula;
Numerical problems.
Atomic Structure:
Concept of Nuclear Atom – electron, proton and neutron (charge and
mass), atomic number; Rutherford’s model and its limitations; Extra nuclear
structure; Line spectra of hydrogen atom.
Quantization of energy (Planck’s equation E = hv); Bohr’s model of
hydrogen atom and its limitations, Sommerfelds modifications (elementary
idea); The four quantum numbers, ground state electronic configurations of
many electron atoms and mono-atomic ions; The Aufbau Principle; Pauli’s
Exclusion Principle and Hund’s Rule.
Uncertainty principle; The concept of atomic orbitals, shapes of s, p
and d orbitals (pictorial approach)
Radioactivity and Nuclear Chemistry:
Radioactivity – α-, β-, γ-rays and their properties; Artificial
transmutation; Rate of radioactive decay, decay
constant, half-life and average life period of radio-elements; Units of
radioactivity; Numerical problems.
Stability of the atomic nucleus – effect of neutron–proton (n/p) ratio on the
modes of decay, group displacement law, radioisotopes and their uses (C, P, Co
and I as examples) isobars and isotones (definition and examples), elementary
idea of nuclear fission and fusion reactions.
The Periodic Table and Chemical Families:
Modern periodic law (based on atomic number); Modern periodic table based on
electronic configurations, groups (Gr. 1–18) and periods. Types of
elements-representative (s-block and p-block), transition (d-block) elements and
inner transition (f-block / lanthanides and actinides) and their general
characteristics. Periodic trends in physical and chemical properties–atomic
radii, valency, ionization energy, electron affinity, electronegativity,
metallic character, acidic and basic characters of oxides and hydrides of the
representative elements (up to Z = 36). Position of hydrogen and the noble gases
in the periodic table; Diagonal relationships.
Chemical Bonding and Molecular Structure:
Valence electrons, the Octet rule, electrovalent, covalent and coordinate
covalent bonds with examples; Properties of electrovalent and covalent
compounds. Limitations of Octet rule (examples); Fajan’s Rule.
Directionality of covalent bonds, shapes of poly-atomic molecules (examples);
Concept of hybridization of atomic orbitals (qualitative pictorial approach) :
sp, sp2, sp3 and dsp2.
Molecular orbital energy diagrams for homonuclear diatomic species – bond
order and magnetic properties.
Valence Shell Electron Pair Repulsion (VSEPR) concept (elementary idea) –
shapes of molecules. Concept of resonance (elementary idea), resonance
structures (examples). Elementary idea about electronegativity, bond polarity
and dipole moment, inter- and intra- molecular hydrogen bonding and its effects
on physical properties (mp, bp and solubility); Hydrogen bridge bonds in
diborane.
Double salts and complex salts, co-ordination compounds (examples only),
co-ordination number (examples of co-ordination number 4 and 6 only).
Gaseous state:
Measurable properties of gases. Boyle’s Law and Charles Law, absolute scale
of temperature, kinetic theory of gases, ideal gas equation – average, root mean
square and most probable velocities and their relationship with temperature.
Dalton’s Law of partial pressure, Graham’s Law of gaseous diffusion.
Deviations from ideal behavior.
Liquefaction of gases, real gases, van der Waal’s equation; Numerical
problems.
Chemical Energetics and Chemical Dynamics
Chemical Energetics – conservation of energy principle, energy changes in
physical and chemical transformations. First law of thermodynamics; Internal
energy, work and heat, pressure-volume work; Enthalpy. Internal energy change (ΔE)
and Enthalpy change (ΔH) in a chemical reaction. Hess’s Law and its applications
(Numerical problems). Heat of reaction, fusion and vapourization; Second law of
thermodynamics; Entropy; Free energy; Criterion of spontaneity.
Chemical Equilibria – The Law of mass action, dynamic nature of
chemical equilibria. Equilibrium constants, Le Chatelier’s Principle.
Equilibrium constants of gaseous reactions (Kp and Kc) and
relation between them (examples). Significance of ΔG and ΔG°.
Chemical Dynamics – Factors affecting the rate of chemical reactions
(concentration, pressure, temperature, catalyst). Arrhenius equation and concept
of activation energy.
Order and molecularity (determination excluded); First order reactions, rate
constant, half-life (numerical problems), examples of first order and second
order reactions.
Physical Chemistry of Solutions:
Colloidal Solutions – differences from true solutions; Hydrophobic and
hydrophilic colloids (examples and uses); Coagulation and peptization of
colloids; Dialysis and its applications; Brownian motion; Tyndall effect and its
applications; Elementary idea of emulsion, surfactant and micelle.
Electrolytic Solutions – Specific conductance, equivalent conductance, ionic
conductance, Kohlrausch’s law, Faraday’s laws of electrolysis, applications.
Numerical problems.
Non-electrolytic Solutions – Types of solution, vapour pressure of solutions.
Raoult’s Law; Colligative properties – lowering of vapour pressure, elevation of
boiling point, depression of freezing point, osmotic pressure and their
relationships with molecular mass (without derivations); Numerical problems.
Ionic and Redox Equilibria
Ionic equilibria – ionization of weak electrolytes, Ostwald’s dilution law.
Ionization constants of weak acids and bases, ionic product of water, the pH –
scale, pH of aqueous solutions of acids and bases; Buffer solutions, buffer
action and Henderson equation.
Acid-base titrations, acid-base indicators (structures not required).
Solubility and Solubility Products.
Common ion effect (no numerical problems).
Redox Equilibria – Oxidation-Reduction reactions as electron transfer
processes, oxidation numbers, balancing of redox reactions by oxidation number
and ion-electron methods. Standard electrode potentials (E°), Electrochemical
series, feasibility of a redox reaction. Significance of Gibb’s equation :
ΔG° = – nFΔE° (without derivation), no numerical problems. Redox titrations with
(examples); Nernst equations (Numerical problems).
Chemistry of Non-metallic Elements and their Compounds:
Carbon – occurrence, isotopes, allotropes (graphite, diamond, fullerene); CO
and CO2 production, properties and uses.
Nitrogen and Phosphorus – occurrence, isotopes, allotopes, isolation from
natural sources and purification, reactivity of the free elements. Preparation,
properties, reactions of NH3, PH3 , NO, NO2 ,
HNO2, HNO3, P4O10, H3PO3
and H3PO4.
Oxygen and Sulfur – Occurrence, isotopes, allotropic forms, isolation from
natural sources and purification, properties and reactions of the free elements.
Water, unusual properties of water, heavy water (production and uses). Hydrogen
peroxide and ozone (production, purification, properties and uses).
Halogen
Halogens – comparative study, occurrence, physical states and chemical
reactivities of the free elements, peculiarities of fluorine and iodine;
Hydracids of halogens (preparation, properties, reactions and uses),
inter-halogen compounds (examples); Oxyacids of chlorine.
Chemistry of metals :
General principles of metallurgy – occurrence, concentration of ores,
production and purification of metals, mineral wealth of India.
Typical metals (Na, Ca, Al, Fe, Cu and Zn) – occurrence, extraction,
purification (where applicable), properties and reactions with air, water, acids
and non-metals.
Manufacture of steels and alloy steel (Bessemer, Open-Hearth and L.D.
process).
Principles of chemistry involved in electroplating, anodizing and
galvanizing.
Chemistry in Industry:
Large scale production (including physicochemical principles where
applicable omitting technical details and uses of individual items).
Heavy chemicals : Sulfuric acid (contact process), Ammonia (Haber’s
process), Nitric acid (Ostwald’s process), sodium bi-carbonate and sodium
carbonate (Solvey process).
Polymers, Polythene, Nylon-66, rubber from natural source, vulcanization.
Electrochemicals – sodium hydroxide, chlorine, bleaching powder as by-products.
Fuel Gases – LPG, CNG.
Silicon carbide and silicones.
Environmental Chemistry:
Common modes of pollution of air, water and soil. Ozone layer, ozone hole –
important chemical reactions. Green House effect; Smog; Pollution of water by
domestic and industrial effluents; Pollutants– esticides, fertilizers and
plastics.
Chemistry of carbon compounds:
Hybridization of carbon – σ- and π-bonds.
Isomerism – constitutional and stereoisomerism; Geometrical and optical
isomerism of compounds containing upto two asymmetric carbon atoms. IUPAC
nomenclature of simple organic compounds– hydrocarbons, mono and bifunctional
molecules only (alicyclic and heterocyclic compounds excluded). Conformations of
ethane and n-butane (Newman projection only).
Electronic effects – inductive, resonance and hyperconjugation. Stability
of carbocation, carbanion and free radicals; Rearrangement of carbocation;
Electrophiles and nucleophiles, tautomerism in β- dicarbonyl compounds, acidity
and basicity of simple organic compounds.
Aliphatic Compounds:
Alkanes – Preparation from alkyl halides and carboxylic acids; Reactions –
halogenation and combustion.
Alkenes and Alkynes – Preparation by elimination of alcohols, alkyl halides
and quaternary ammonium hydroxides, Saytzeff and Hofmann rules; Reactions –
electrophilic addition of X2, HX, HOX, H2O (X = halogen),
ozonolysis, epoxidation and oxidation with KMnO4, OsO4
(stereochemistry of addition excluded).
Markownikoff’s and anti-Markownikoff’s additions; Hydroboration;
Oxymercuration – demercuration, reduction of alkenes and alkynes (H2/Lindler
catalyst and Na in liquid NH3), metal acetylides.
Alkyl halides – Preparation from alcohols; Formation of Grignard reagents and
their synthetic applications for the preparation of alkanes, alcohols, aldehydes,
ketones and acids; SN1 and SN2
reactions (preliminary concept).
Alcohols – Preparation from carbonyl compounds and esters. Reaction –
dehydration, oxidation, esterification, reaction with sodium, ZnCl2 /
HCl, phosphorous halides.
Ethers – Preparation by Williamson’s synthesis; Cleavage with HCl and HI.
Aldehydes and Ketones – Preparation from esters, acid chlorides, gem-dihalides,
Ca-salt of carboxylic acids. Reaction – Nucleophilic addition with HCN,
hydrazine, hydroxyl amines, semi carbazides, alcohols; Aldol condensation,
Clemmensen and Wolff-Kishner reduction, haloform, Cannizzaro and Wittig
reactions.
Carboxylic Acids – Hydrolysis of esters (mechanism excluded) and cyanides;
Hunsdicker and HVZ reactions.
Aliphatic Amines – Preparation from nitro, cyano and amido compounds.
Distinction of 1º, 2º and 3º amines (Hinsberg method); Reaction with HNO2;
Carbyl amine reaction.
Aromatic Compounds:
Benzene – Kekule structure, aromaticity and Hückel rule. Electrophilic
substitution – halogenation, sulfonation, nitration, Friedel Crafts reaction,
ozonolysis. Directive influence of substituents in monosubstituted benzenes.
Amines – Preparation from reduction of nitro compounds; Formation of
diazonium salts and their stability; Replacement of diazonium group with H, OH,
X (halogen), CN and NO2, diazocoupling and reduction.
Haloarenes – Nucleophilic substitution, cine substitution (excluding
mechanism). Phenols – halogenation, sulfonation, nitration, Reimer-Tiemann and
Kolbe reactions.
Aromatic Aldehydes – Preparation by Gattermann, Gattermann – Koch,
Rosenmund and Stephen’s method. Reactions – Perkin, Benzoin and Cannizzaro.
Application Oriented chemistry:
Main ingredients, their chemical natures (structures excluded) and their
side effects, if any, of common antiseptics, analgesics, antacids, vitamin-C.
Introduction to Bio-molecules:
Carbohydrates – Pentoses and hexoses. Distinctive chemical reactions of
glucose.
Aminoacids – glycine, alanine, aspartic acid, cysteine (structures). Zwitterion
structures of amino acids, peptide bond.
ADP and ATP – structures and role in bioenergetics; Nucleic acids – DNA and
RNA skeleton structures. Names of essential elements in biological system.
Principles of qualitative analysis:
Detection of water soluble noninterfaring Acid and Basic Radicals by dry
and wet tests from among :
(a) Acid Radicals : Cl-, S2-, SO42-,
NO-3, CO32-
(b) Basic Radicals: Cu2+, Al3+, Fe3+, Fe2+,
Zn2+, Ca2+, Mg2+, Na+, NH4+
Detection of special elements (N, Cl, Br, I and S) in organic
compounds by chemical tests. Identification of functional groups in :
phenols, aromatic amines, aldehydes, ketones and carboxylic acids.
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Atoms, Molecules and Chemical Arithmetic :
Dalton’s atomic theory; Gay Lussac’s law of gaseous volume; Avogadro’s
Hypothesis and its applications.
Atomic mass; Molecular mass; Equivalent weight; Valency; Gram atomic
weight; Gram molecular weight; Gram equivalent weight and mole concept;
Chemical formulae; Balanced chemical equations; Calculations (based on mole
concept) involving common oxidation-reduction, neutralization, and
displacement reactions; Concentration in terms of mole fraction, molarity,
molality and normality.
Percentage composition, empirical formula and molecular formula;
Numerical problems.
Atomic Structure:
Concept of Nuclear Atom – electron, proton and neutron (charge and
mass), atomic number; Rutherford’s model and its limitations; Extra nuclear
structure; Line spectra of hydrogen atom.
Quantization of energy (Planck’s equation E = hv); Bohr’s model of
hydrogen atom and its limitations, Sommerfelds modifications (elementary
idea); The four quantum numbers, ground state electronic configurations of
many electron atoms and mono-atomic ions; The Aufbau Principle; Pauli’s
Exclusion Principle and Hund’s Rule.
Uncertainty principle; The concept of atomic orbitals, shapes of s, p
and d orbitals (pictorial approach)
Radioactivity and Nuclear Chemistry:
Radioactivity – α-, β-, γ-rays and their properties; Artificial
transmutation; Rate of radioactive decay, decay
constant, half-life and average life period of radio-elements; Units of
radioactivity; Numerical problems.
Stability of the atomic nucleus – effect of neutron–proton (n/p) ratio on the
modes of decay, group displacement law, radioisotopes and their uses (C, P, Co
and I as examples) isobars and isotones (definition and examples), elementary
idea of nuclear fission and fusion reactions.
The Periodic Table and Chemical Families:
Modern periodic law (based on atomic number); Modern periodic table based on
electronic configurations, groups (Gr. 1–18) and periods. Types of
elements-representative (s-block and p-block), transition (d-block) elements and
inner transition (f-block / lanthanides and actinides) and their general
characteristics. Periodic trends in physical and chemical properties–atomic
radii, valency, ionization energy, electron affinity, electronegativity,
metallic character, acidic and basic characters of oxides and hydrides of the
representative elements (up to Z = 36). Position of hydrogen and the noble gases
in the periodic table; Diagonal relationships.
Chemical Bonding and Molecular Structure:
Valence electrons, the Octet rule, electrovalent, covalent and coordinate
covalent bonds with examples; Properties of electrovalent and covalent
compounds. Limitations of Octet rule (examples); Fajan’s Rule.
Directionality of covalent bonds, shapes of poly-atomic molecules (examples);
Concept of hybridization of atomic orbitals (qualitative pictorial approach) :
sp, sp2, sp3 and dsp2.
Molecular orbital energy diagrams for homonuclear diatomic species – bond
order and magnetic properties.
Valence Shell Electron Pair Repulsion (VSEPR) concept (elementary idea) –
shapes of molecules. Concept of resonance (elementary idea), resonance
structures (examples). Elementary idea about electronegativity, bond polarity
and dipole moment, inter- and intra- molecular hydrogen bonding and its effects
on physical properties (mp, bp and solubility); Hydrogen bridge bonds in
diborane.
Double salts and complex salts, co-ordination compounds (examples only),
co-ordination number (examples of co-ordination number 4 and 6 only).
Gaseous state:
Measurable properties of gases. Boyle’s Law and Charles Law, absolute scale
of temperature, kinetic theory of gases, ideal gas equation – average, root mean
square and most probable velocities and their relationship with temperature.
Dalton’s Law of partial pressure, Graham’s Law of gaseous diffusion.
Deviations from ideal behavior.
Liquefaction of gases, real gases, van der Waal’s equation; Numerical
problems.
Chemical Energetics and Chemical Dynamics
Chemical Energetics – conservation of energy principle, energy changes in
physical and chemical transformations. First law of thermodynamics; Internal
energy, work and heat, pressure-volume work; Enthalpy. Internal energy change (ΔE)
and Enthalpy change (ΔH) in a chemical reaction. Hess’s Law and its applications
(Numerical problems). Heat of reaction, fusion and vapourization; Second law of
thermodynamics; Entropy; Free energy; Criterion of spontaneity.
Chemical Equilibria – The Law of mass action, dynamic nature of
chemical equilibria. Equilibrium constants, Le Chatelier’s Principle.
Equilibrium constants of gaseous reactions (Kp and Kc) and
relation between them (examples). Significance of ΔG and ΔG°.
Chemical Dynamics – Factors affecting the rate of chemical reactions
(concentration, pressure, temperature, catalyst). Arrhenius equation and concept
of activation energy.
Order and molecularity (determination excluded); First order reactions, rate
constant, half-life (numerical problems), examples of first order and second
order reactions.
Physical Chemistry of Solutions:
Colloidal Solutions – differences from true solutions; Hydrophobic and
hydrophilic colloids (examples and uses); Coagulation and peptization of
colloids; Dialysis and its applications; Brownian motion; Tyndall effect and its
applications; Elementary idea of emulsion, surfactant and micelle.
Electrolytic Solutions – Specific conductance, equivalent conductance, ionic
conductance, Kohlrausch’s law, Faraday’s laws of electrolysis, applications.
Numerical problems.
Non-electrolytic Solutions – Types of solution, vapour pressure of solutions.
Raoult’s Law; Colligative properties – lowering of vapour pressure, elevation of
boiling point, depression of freezing point, osmotic pressure and their
relationships with molecular mass (without derivations); Numerical problems.
Ionic and Redox Equilibria
Ionic equilibria – ionization of weak electrolytes, Ostwald’s dilution law.
Ionization constants of weak acids and bases, ionic product of water, the pH –
scale, pH of aqueous solutions of acids and bases; Buffer solutions, buffer
action and Henderson equation.
Acid-base titrations, acid-base indicators (structures not required).
Solubility and Solubility Products.
Common ion effect (no numerical problems).
Redox Equilibria – Oxidation-Reduction reactions as electron transfer
processes, oxidation numbers, balancing of redox reactions by oxidation number
and ion-electron methods. Standard electrode potentials (E°), Electrochemical
series, feasibility of a redox reaction. Significance of Gibb’s equation :
ΔG° = – nFΔE° (without derivation), no numerical problems. Redox titrations with
(examples); Nernst equations (Numerical problems).
Chemistry of Non-metallic Elements and their Compounds:
Carbon – occurrence, isotopes, allotropes (graphite, diamond, fullerene); CO
and CO2 production, properties and uses.
Nitrogen and Phosphorus – occurrence, isotopes, allotopes, isolation from
natural sources and purification, reactivity of the free elements. Preparation,
properties, reactions of NH3, PH3 , NO, NO2 ,
HNO2, HNO3, P4O10, H3PO3
and H3PO4.
Oxygen and Sulfur – Occurrence, isotopes, allotropic forms, isolation from
natural sources and purification, properties and reactions of the free elements.
Water, unusual properties of water, heavy water (production and uses). Hydrogen
peroxide and ozone (production, purification, properties and uses).
Halogen
Halogens – comparative study, occurrence, physical states and chemical
reactivities of the free elements, peculiarities of fluorine and iodine;
Hydracids of halogens (preparation, properties, reactions and uses),
inter-halogen compounds (examples); Oxyacids of chlorine.
Chemistry of metals :
General principles of metallurgy – occurrence, concentration of ores,
production and purification of metals, mineral wealth of India.
Typical metals (Na, Ca, Al, Fe, Cu and Zn) – occurrence, extraction,
purification (where applicable), properties and reactions with air, water, acids
and non-metals.
Manufacture of steels and alloy steel (Bessemer, Open-Hearth and L.D.
process).
Principles of chemistry involved in electroplating, anodizing and
galvanizing.
Chemistry in Industry:
Large scale production (including physicochemical principles where
applicable omitting technical details and uses of individual items).
Heavy chemicals : Sulfuric acid (contact process), Ammonia (Haber’s
process), Nitric acid (Ostwald’s process), sodium bi-carbonate and sodium
carbonate (Solvey process).
Polymers, Polythene, Nylon-66, rubber from natural source, vulcanization.
Electrochemicals – sodium hydroxide, chlorine, bleaching powder as by-products.
Fuel Gases – LPG, CNG.
Silicon carbide and silicones.
Environmental Chemistry:
Common modes of pollution of air, water and soil. Ozone layer, ozone hole –
important chemical reactions. Green House effect; Smog; Pollution of water by
domestic and industrial effluents; Pollutants– esticides, fertilizers and
plastics.
Chemistry of carbon compounds:
Hybridization of carbon – σ- and π-bonds.
Isomerism – constitutional and stereoisomerism; Geometrical and optical
isomerism of compounds containing upto two asymmetric carbon atoms. IUPAC
nomenclature of simple organic compounds– hydrocarbons, mono and bifunctional
molecules only (alicyclic and heterocyclic compounds excluded). Conformations of
ethane and n-butane (Newman projection only).
Electronic effects – inductive, resonance and hyperconjugation. Stability
of carbocation, carbanion and free radicals; Rearrangement of carbocation;
Electrophiles and nucleophiles, tautomerism in β- dicarbonyl compounds, acidity
and basicity of simple organic compounds.
Aliphatic Compounds:
Alkanes – Preparation from alkyl halides and carboxylic acids; Reactions –
halogenation and combustion.
Alkenes and Alkynes – Preparation by elimination of alcohols, alkyl halides
and quaternary ammonium hydroxides, Saytzeff and Hofmann rules; Reactions –
electrophilic addition of X2, HX, HOX, H2O (X = halogen),
ozonolysis, epoxidation and oxidation with KMnO4, OsO4
(stereochemistry of addition excluded).
Markownikoff’s and anti-Markownikoff’s additions; Hydroboration;
Oxymercuration – demercuration, reduction of alkenes and alkynes (H2/Lindler
catalyst and Na in liquid NH3), metal acetylides.
Alkyl halides – Preparation from alcohols; Formation of Grignard reagents and
their synthetic applications for the preparation of alkanes, alcohols, aldehydes,
ketones and acids; SN1 and SN2
reactions (preliminary concept).
Alcohols – Preparation from carbonyl compounds and esters. Reaction –
dehydration, oxidation, esterification, reaction with sodium, ZnCl2 /
HCl, phosphorous halides.
Ethers – Preparation by Williamson’s synthesis; Cleavage with HCl and HI.
Aldehydes and Ketones – Preparation from esters, acid chlorides, gem-dihalides,
Ca-salt of carboxylic acids. Reaction – Nucleophilic addition with HCN,
hydrazine, hydroxyl amines, semi carbazides, alcohols; Aldol condensation,
Clemmensen and Wolff-Kishner reduction, haloform, Cannizzaro and Wittig
reactions.
Carboxylic Acids – Hydrolysis of esters (mechanism excluded) and cyanides;
Hunsdicker and HVZ reactions.
Aliphatic Amines – Preparation from nitro, cyano and amido compounds.
Distinction of 1º, 2º and 3º amines (Hinsberg method); Reaction with HNO2;
Carbyl amine reaction.
Aromatic Compounds:
Benzene – Kekule structure, aromaticity and Hückel rule. Electrophilic
substitution – halogenation, sulfonation, nitration, Friedel Crafts reaction,
ozonolysis. Directive influence of substituents in monosubstituted benzenes.
Amines – Preparation from reduction of nitro compounds; Formation of
diazonium salts and their stability; Replacement of diazonium group with H, OH,
X (halogen), CN and NO2, diazocoupling and reduction.
Haloarenes – Nucleophilic substitution, cine substitution (excluding
mechanism). Phenols – halogenation, sulfonation, nitration, Reimer-Tiemann and
Kolbe reactions.
Aromatic Aldehydes – Preparation by Gattermann, Gattermann – Koch,
Rosenmund and Stephen’s method. Reactions – Perkin, Benzoin and Cannizzaro.
Application Oriented chemistry:
Main ingredients, their chemical natures (structures excluded) and their
side effects, if any, of common antiseptics, analgesics, antacids, vitamin-C.
Introduction to Bio-molecules:
Carbohydrates – Pentoses and hexoses. Distinctive chemical reactions of
glucose.
Aminoacids – glycine, alanine, aspartic acid, cysteine (structures). Zwitterion
structures of amino acids, peptide bond.
ADP and ATP – structures and role in bioenergetics; Nucleic acids – DNA and
RNA skeleton structures. Names of essential elements in biological system.
Principles of qualitative analysis:
Detection of water soluble noninterfaring Acid and Basic Radicals by dry
and wet tests from among :
(a) Acid Radicals : Cl-, S2-, SO42-,
NO-3, CO32-
(b) Basic Radicals: Cu2+, Al3+, Fe3+, Fe2+,
Zn2+, Ca2+, Mg2+, Na+, NH4+
Detection of special elements (N, Cl, Br, I and S) in organic
compounds by chemical tests. Identification of functional groups in :
phenols, aromatic amines, aldehydes, ketones and carboxylic acids.
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