Syllabus
Surface chemistry: Elementary concepts of adsorption (excluding adsorption isotherms); Colloids: types, methods of preparation and general properties; Elementary ideas of emulsions, surfactants and micelles (only definitions and examples).
Elementary concepts of adsorption
The term adsorption implies the presence of excess concentration of any particular component in one of the three phases of matter (known as adsorbate) at the surface of liquid or solid phase (known as adsorbent) as compared to that present in the bulk of the material.
On the basis of the forces of attraction between adsorbent and adsorbate, two types of adsorption, namely, physisorption (i.e. physical adsorption) and chemisorption, may be identified.
The characteristics of physisorption are;
1. the forces of attraction are of van der waals type (weak forces).
2. Predominates at low temperature.
3. All gases show this adsorption at low temperatures.
4. Heat of adsorption is low, about 40 kJ/mol.
5. Reversible in nature.
6. Low activation energy (appx. 5 kJ)
7. Adsorption is multilayer.
The characteristics of chemisorption are:
1. the forces of attraction are of a chemical nature (strong forces)
2. Predominates at high temperature.
3. This is highly specific in nature.
4. Heat of adsorption is large 9appx. 80 to 420 kJ/mol)
5. Usually irreversible.
6. Large activation energy
7. Adsorption is monolayer.
The extent of adsorption of gases increases with increase in the pressure of the gases and it decreases with increase in temperature of the gas.
Colloids
Colloids or sols are the substances whose sizes lie in between the solutes present in a true solution (e.g., salt, sugar) and the solutes present in suspension (e.g., sand). It can also be explained that colloids are intermediate between solutions and precipitates. The particles in colloids are larger than the molecules or ions that make up solutions. The diameters of colloidal particles may range from 1 to 100 nm. The particles in colloidal state do not settle down on standing, are not visible and they can pass through a filter paper. However, they do not pass through a perchment paper or animal membrane.
In the case colloids, we use the terms dispersed particles and dispersing medium. Dispersed particles are the colloidal particles. Milk is an example of a colloid; butterfat constitutes the dispersed particles and water is the dispersing medium.
Types of colloids
Colloids may consists of dispersed particles of various phases and dispersing mediums of various phases. These different types of colloids have different names.
Type Examples
Solid sol Coloured gems and glasses, some alloys, minerals
Sol Starch or proteins in water, paints, gold sol
Solid aerosol Smoke, dust, storm
Gel Jellies, cheese, butter, boot polish
Emulsion Emulsified oils, milk, cod liver oil, medicines
Liquid aerosol Mist, fog, cloud, insecticide sprays
Solid foam Styrene foam, rubber, occluded gases
Foam or froth Whipped cream, lemonade, froth, soap suds
Solid sol is a solid dispersed in a solid.
Sol is a solid dispersed in a liquid.
Solid aerosol is a solid dispersed in a gas.
Gel is a liquid dispersed in a solid
Emulsion is a liquid dispersed in a liquid.
Liquid aerosol is a liquid dispersed in a gas.
Solid foam is a gas dispersed in a solid.
A foam is a gas dispersed in a liquid.
The colloid (dispersing particles + medium) is a two phase system.
Properties of Colloids
Besides particle size, colloids have other identifying properties. Properties peculiar to colloids are (1) optical effects, (2) motion effect, and (3) electrical charge effect.
Optical effect
When a relatively narrow beam of light is passed through a colloid, such dust particles in the air, the light is scattered by the dust particles and they appear in the beam a bright, tiny specks of light. Many of us have seen this phenomenon.
The scattering of light in a colloid is due to the reflection of the light by the large colloidal particles producing a visible beam of light. This optical effect is named the Tyndall effect after John Tyndall, who investigated it in 1860.
Motion effect
If a colloid is viewed with a special microscope, dispersed colloidal particles appear to move in a zigzag, random motion. This erratic random motion is due to bombardment of the dispersed colloidal particles by the medium and this constant bombardment keeps the dispersed colloidal particles suspended indefinitely. They will not settle down. This movement of colloidal particles is called Brownian movement, and this could be observed because of the Tyndall effect.
Electrical charge effect
Very often a colloid will have ions from the dispersing medium adsorbed on its surface. This along with the Brownian motion of the colloid, prevents colloids from coagulating and precipitating.
To facilitate precipitation, an electrolyte of some type is added to the solution, which will neutralize the charge. For instance, in the case of qualitative analysis, if charge on colloids is interfering with the precipitation, an electrolyte of some type is added. This property is used in removing suspended particles from the effluent gases in industrial smokestacks., In the gas coming of out various industrial equipment is given an electrical charge. Before this exhaust gas goes into atmosphere, it is passed through charged plates. These charged plates attract the charged colloidal particles, which then are held on the plates till the current giving the plates their charge is shut off. Then the particles fall to the ground and can be collected. The response of colloid particles to electrical charge is electrical phoresis.
Emulsions
Emulsions are sols of liquid in liquid. Two types of emulsions may be distinguished, namely, oil-in-water and water-in-oil. To make emulsions stable, emulsifying agents such as soaps and detergents are added.
Surfactants
Any substance which can decrease the surface tension of water to a large extent is known as surfactant. Examples of soap and detergents. Such substances have larger concentrations at the surface of water as compared to the bulk of the solution.
Micelle
From http://www.chemicool.com/definition/micelle.html
Definition of micelle
Surfactants in solution are often association colloids, that is, they tend to form aggregates of colloidal dimensions, which exist in equilibrium with the molecules or ions from which they are formed. Such aggregates are termed micelles. (IUPAC MANUAL APPENDIX II (1972)).
What is colloidal micelle?
The heart of this new chemistry is the technology used to develop a "colloidal micelle." Sub-microscopic particles are created in a microscopic field similar to a magnetic field. It differs from traditional chemistry in that the molecular attraction is not the usual attraction between positive and negative poles. Rather, it is between like poles.
An analogy would be that negative attracts negative and positive attracts positive. The micelle has a hydrophilic (water seeking) pole and a hydrophobic (water repelling) pole. The hydrophobic poles attract each other, thus forming the interior of the micelle. The hydrophilic poles form a tough outer surface.
When a micelle comes in contact with a hydrocarbon molecule, the center of the micelle bonds to a similar hydrophobic hydrocarbon. It disrupts the attraction to other hydrocarbon molecules and/or to the surface. Detergent particles in water form particles with hydrophobic poles and hydrophilic poles. In the case of clothes, the hydrophobic pole of a detergent particle attracts the grease and dirt particles on the clothes and pull them apart. As such micelles come together, an outlayer or hydrophilic poles forms. These associative colloid particles are then washed away by water and leaving clothes clean.
The action of a single micelle is multiplied by billions of other micelles. The molecular level emulsification process penetrates highly viscous and sticky materials, lifting them from the surface to which they adhere.
Considering the damage inflicted on life and the planet by harsh cleaners and solvents, colloidal chemistry is an exceptionally advance towards environmental preservation.
Level I lecgtures are meant to explain the basic concepts of the topic. More advanced treatment of the topic will be attempted in level II and level III lectures.
Wednesday, May 30, 2007
Tuesday, May 29, 2007
IIT JEE Chemistry Lecture Atomic Structure
Syllabus
Atomic structure and chemical bonding: Bohr model, spectrum of hydrogen atom, quantum numbers; Wave-particle duality, de Broglie hypothesis; Uncertainty principle; Quantum mechanical picture of hydrogen atom (qualitative treatment), shapes of s, p and d orbitals; Electronic configurations of elements (up to atomic number 36); Aufbau principle; Pauli's exclusion principle and Hund's rule; Orbital overlap and covalent bond; Hybridisation involving s, p and d orbitals only; Orbital energy diagrams for homonuclear diatomic species; Hydrogen bond; Polarity in molecules, dipole moment (qualitative aspects only); VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, trigonal bipyramidal, tetrahedral and octahedral).
The lecture is based on chapter 4 : the Structure of Atom in Fundamentals of Chemistry by Fred H. Redmore, Prentice Hall 1979.
In 1913, Niels Bohr proposed a model of the atom. He proposed that the electrons in an atom could only be in certain orbits, or energy levels, around the nucleus. Refinement of Bohr theory led to the modern theory of atomic structure based on quantum mechanics. The energy levels proposed by Bohr were calculated and it was further modeled that each energy level or orbit has sublevels and each sublevels has one or more orbitals.
Orbit - sublevel – Orbital
Electrons are moving around the nucleus and orbitals represent a space where a pair of electrons is most likely to be found. This means that electrons may sometimes go out of the orbital but most of the time they are found in the orbital.
The quantum mechanics calculations gave out the result that there is a limit to the number of electrons that can occupy a given orbit or energy level.
Orbits
The orbits are called as shells. The energy level of orbits or shells increases as they increase in distance from the nucleus of the atom. The orbits or shells are represented by numbers as 1,2,3,4,5,6 or 7. They are represented by letters as K,L,M,N,O,P,Q.
It is found that the maximum number of electrons in each energy level is equal to 2n2 where n is the number of energy level.
Therefore energy level 1 will have 2 electrons.
Energy level 2 will have 2*4 = 8 electrons
Energy level 3 will have 2*9 = 18 electrons.
Sublevel of an Orbit
The energy levels, or orbits or shells are further divided into sublevels, or subshells. These subshells are designated by letters: s for the first possible sublevel, p for the second possible sublevel, d for the third, f for the fourth, g for the fifth, and from here on they simply go in alphabets.
The number of sublevels of each energy level is equal to the number of the energy levels. This means energy level 1, the K shell will have only one sub levels – s sublevel. The energy level 2, the L shell will have 2 sub levels – s and p.
Orbitals
Sublevels have further divisions called orbitals. Electrons are found in these orbitals. Each orbital contains two electrons.
“s” sublevel has only one orbital. “p” sublevel has 3 orbitals. “d” sublevel has 5 orbitals. “f” sublevel has 7 orbitals.
As each orbital can hold two electrons, orbitals of s can hold two electrons. The orbitals are of p sublevel are named as px and py and pz. The orbitals of p contain 6 electrons. The orbitals of d are 5. The orbitals of d are named as dxy, dxz,dyz,dx2-y2 and dz2. The d sublevel orbitals contain 10 electrons.
The two electons in each orbital spin in different directions.
Shape of Orbitals
Each type of orbital( s, px and py and pz, dxy, dxz,dyz,dx2-y2 and dz2 ) has a unique shape.
1. Spherical shape for s.
2. Dumbbell shape for orbitals of p.
3. Four-lobed shape for orbitals of d.
4. Complex shape for all orbitals of higher sublevels.
Electron Structure or Configuration
In the orbital-sub level-orbit structure, energy level of orbit 1 is less than that of 2 and so on. In each orbit, the sublevel s if of lower energy than the p sublevel, and p is of lower energy than the d sublevel and so on. Orbital of a sublevel are all of equal energy.
Electrons occupy the lowest energy sublevels that are available. This is known as ‘aufbau’ order or principles. In the case of an atom having atomic number of 1, the lone electron occupied the s orbital of sublevel s of orbit 1(represented as 1s1). In case of an atom having atomic number 3 the electrons first occupy the sublevel of orbit 1(this can hold only two electrons) and then occupy p sublevels of orbit 2 (represented as 1s2,2s1).
Hund’s rule says that, for any set of orbitals of equal energy say p orbitals of orbit 2, there is one electron is each orbital before the second electron enters or occupies an orbital.
The energy level of some sublevels at higher orbits is less than the some sublevels at lower orbitals. This fact is to be kept in mind when electron configuration is determined for any atom. The increasing order of energy levels of sublevels is:
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f*, 5d, 6p, 7s, 5f*, 6d, 7p, 8s
* In this case one electron one electron goes into 5d and then 4f fills completely and then rest of 5d. Similar thing happens in 5f and 4d.
Atomic structure and chemical bonding: Bohr model, spectrum of hydrogen atom, quantum numbers; Wave-particle duality, de Broglie hypothesis; Uncertainty principle; Quantum mechanical picture of hydrogen atom (qualitative treatment), shapes of s, p and d orbitals; Electronic configurations of elements (up to atomic number 36); Aufbau principle; Pauli's exclusion principle and Hund's rule; Orbital overlap and covalent bond; Hybridisation involving s, p and d orbitals only; Orbital energy diagrams for homonuclear diatomic species; Hydrogen bond; Polarity in molecules, dipole moment (qualitative aspects only); VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, trigonal bipyramidal, tetrahedral and octahedral).
The lecture is based on chapter 4 : the Structure of Atom in Fundamentals of Chemistry by Fred H. Redmore, Prentice Hall 1979.
In 1913, Niels Bohr proposed a model of the atom. He proposed that the electrons in an atom could only be in certain orbits, or energy levels, around the nucleus. Refinement of Bohr theory led to the modern theory of atomic structure based on quantum mechanics. The energy levels proposed by Bohr were calculated and it was further modeled that each energy level or orbit has sublevels and each sublevels has one or more orbitals.
Orbit - sublevel – Orbital
Electrons are moving around the nucleus and orbitals represent a space where a pair of electrons is most likely to be found. This means that electrons may sometimes go out of the orbital but most of the time they are found in the orbital.
The quantum mechanics calculations gave out the result that there is a limit to the number of electrons that can occupy a given orbit or energy level.
Orbits
The orbits are called as shells. The energy level of orbits or shells increases as they increase in distance from the nucleus of the atom. The orbits or shells are represented by numbers as 1,2,3,4,5,6 or 7. They are represented by letters as K,L,M,N,O,P,Q.
It is found that the maximum number of electrons in each energy level is equal to 2n2 where n is the number of energy level.
Therefore energy level 1 will have 2 electrons.
Energy level 2 will have 2*4 = 8 electrons
Energy level 3 will have 2*9 = 18 electrons.
Sublevel of an Orbit
The energy levels, or orbits or shells are further divided into sublevels, or subshells. These subshells are designated by letters: s for the first possible sublevel, p for the second possible sublevel, d for the third, f for the fourth, g for the fifth, and from here on they simply go in alphabets.
The number of sublevels of each energy level is equal to the number of the energy levels. This means energy level 1, the K shell will have only one sub levels – s sublevel. The energy level 2, the L shell will have 2 sub levels – s and p.
Orbitals
Sublevels have further divisions called orbitals. Electrons are found in these orbitals. Each orbital contains two electrons.
“s” sublevel has only one orbital. “p” sublevel has 3 orbitals. “d” sublevel has 5 orbitals. “f” sublevel has 7 orbitals.
As each orbital can hold two electrons, orbitals of s can hold two electrons. The orbitals are of p sublevel are named as px and py and pz. The orbitals of p contain 6 electrons. The orbitals of d are 5. The orbitals of d are named as dxy, dxz,dyz,dx2-y2 and dz2. The d sublevel orbitals contain 10 electrons.
The two electons in each orbital spin in different directions.
Shape of Orbitals
Each type of orbital( s, px and py and pz, dxy, dxz,dyz,dx2-y2 and dz2 ) has a unique shape.
1. Spherical shape for s.
2. Dumbbell shape for orbitals of p.
3. Four-lobed shape for orbitals of d.
4. Complex shape for all orbitals of higher sublevels.
Electron Structure or Configuration
In the orbital-sub level-orbit structure, energy level of orbit 1 is less than that of 2 and so on. In each orbit, the sublevel s if of lower energy than the p sublevel, and p is of lower energy than the d sublevel and so on. Orbital of a sublevel are all of equal energy.
Electrons occupy the lowest energy sublevels that are available. This is known as ‘aufbau’ order or principles. In the case of an atom having atomic number of 1, the lone electron occupied the s orbital of sublevel s of orbit 1(represented as 1s1). In case of an atom having atomic number 3 the electrons first occupy the sublevel of orbit 1(this can hold only two electrons) and then occupy p sublevels of orbit 2 (represented as 1s2,2s1).
Hund’s rule says that, for any set of orbitals of equal energy say p orbitals of orbit 2, there is one electron is each orbital before the second electron enters or occupies an orbital.
The energy level of some sublevels at higher orbits is less than the some sublevels at lower orbitals. This fact is to be kept in mind when electron configuration is determined for any atom. The increasing order of energy levels of sublevels is:
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f*, 5d, 6p, 7s, 5f*, 6d, 7p, 8s
* In this case one electron one electron goes into 5d and then 4f fills completely and then rest of 5d. Similar thing happens in 5f and 4d.
Sunday, May 27, 2007
Organic Chemistry chapter names TMH IIT JEE Chemistry
19. Hybridization, Isomerism
20. Inductive and Resonance Effects
21. Alkanes
22. Alkenes
23. Alkynes
24. Benzene
25. Alcohols
26. Alkyl and Aryl Halides
27. Aldehydes and Ketones
28. Carboxylic Acids
29. Phenols
30. Amines
31. Carbohydrates
32. Aminoacids and Peptides
33. Polymers
34. Exercises in Organic Chemistry
Syllabus
Organic Chemistry
Concepts: Hybridisation of carbon; Sigma and pi-bonds; Shapes of molecules; Structural and geometrical isomerism; Optical isomerism of compounds containing up to two asymmetric centers, (R,S and E,Z nomenclature excluded); IUPAC nomenclature of simple organic compounds (only hydrocarbons, mono-functional and bi-functional compounds); Conformations of ethane and butane (Newman projections); Resonance and hyperconjugation; Keto-enol tautomerism; Determination of empirical and molecular formula of simple compounds (only combustion method); Hydrogen bonds: definition and their effects on physical properties of alcohols and carboxylic acids; Inductive and resonance effects on acidity and basicity of organic acids and bases; Polarity and inductive effects in alkyl halides; Reactive intermediates produced during homolytic and heterolytic bond cleavage; Formation, structure and stability of carbocations, carbanions and free radicals.
Preparation, properties and reactions of alkanes: Homologous series, physical properties of alkanes (melting points, boiling points and density); Combustion and halogenation of alkanes; Preparation of alkanes by Wurtz reaction and decarboxylation reactions.
Preparation, properties and reactions of alkenes and alkynes: Physical properties of alkenes and alkynes (boiling points, density and dipole moments); Acidity of alkynes; Acid catalysed hydration of alkenes and alkynes (excluding the stereochemistry of addition and elimination); Reactions of alkenes with KMnO4 and ozone; Reduction of alkenes and alkynes; Preparation of alkenes and alkynes by elimination reactions; Electrophilic addition reactions of alkenes with X2, HX, HOX and H2O (X=halogen); Addition reactions of alkynes; Metal acetylides.
Reactions of benzene: Structure and aromaticity; Electrophilic substitution reactions: halogenation, nitration, sulphonation, Friedel-Crafts alkylation and acylation; Effect of o-, m- and p-directing groups in monosubstituted benzenes.
Phenols: Acidity, electrophilic substitution reactions (halogenation, nitration and sulphonation); Reimer-Tieman reaction, Kolbe reaction.
Characteristic reactions of the following (including those mentioned above):
Alkyl halides: rearrangement reactions of alkyl carbocation, Grignard reactions, nucleophilic substitution reactions;
Alcohols: esterification, dehydration and oxidation, reaction with sodium, phosphorus halides, ZnCl2/conc.-HCl, conversion of alcohols into aldehydes and ketones;
Aldehydes and Ketones: oxidation, reduction, oxime and hydrazone formation; aldol condensation, Perkin reaction; Cannizzaro reaction; haloform reaction and nucleophilic addition reactions (Grignard addition);
Carboxylic acids: formation of esters, acid chlorides and amides, ester hydrolysis;
Amines: basicity of substituted anilines and aliphatic amines, preparation from nitro compounds, reaction with nitrous acid, azo coupling reaction of diazonium salts of aromatic amines, Sandmeyer and related reactions of diazonium salts; carbylamine reaction; Haloarenes: nucleophilic aromatic substitution in haloarenes and substituted haloarenes - (excluding Benzyne mechanism and Cine substitution).
Carbohydrates: Classification; mono and di-saccharides (glucose and sucrose); Oxidation, reduction, glycoside formation and hydrolysis of sucrose.
Amino acids and peptides: General structure (only primary structure for peptides) and physical properties.
Properties and uses of some important polymers: Natural rubber, cellulose, nylon, teflon and PVC.
Practical organic chemistry: Detection of elements (N, S, halogens); Detection and identification of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl, amino and nitro; Chemical methods of separation of mono-functional organic compounds from binary mixtures.
We can see from a comparison of chapters and syllabus that every major head of the syllabus is covered in the above chapters
20. Inductive and Resonance Effects
21. Alkanes
22. Alkenes
23. Alkynes
24. Benzene
25. Alcohols
26. Alkyl and Aryl Halides
27. Aldehydes and Ketones
28. Carboxylic Acids
29. Phenols
30. Amines
31. Carbohydrates
32. Aminoacids and Peptides
33. Polymers
34. Exercises in Organic Chemistry
Syllabus
Organic Chemistry
Concepts: Hybridisation of carbon; Sigma and pi-bonds; Shapes of molecules; Structural and geometrical isomerism; Optical isomerism of compounds containing up to two asymmetric centers, (R,S and E,Z nomenclature excluded); IUPAC nomenclature of simple organic compounds (only hydrocarbons, mono-functional and bi-functional compounds); Conformations of ethane and butane (Newman projections); Resonance and hyperconjugation; Keto-enol tautomerism; Determination of empirical and molecular formula of simple compounds (only combustion method); Hydrogen bonds: definition and their effects on physical properties of alcohols and carboxylic acids; Inductive and resonance effects on acidity and basicity of organic acids and bases; Polarity and inductive effects in alkyl halides; Reactive intermediates produced during homolytic and heterolytic bond cleavage; Formation, structure and stability of carbocations, carbanions and free radicals.
Preparation, properties and reactions of alkanes: Homologous series, physical properties of alkanes (melting points, boiling points and density); Combustion and halogenation of alkanes; Preparation of alkanes by Wurtz reaction and decarboxylation reactions.
Preparation, properties and reactions of alkenes and alkynes: Physical properties of alkenes and alkynes (boiling points, density and dipole moments); Acidity of alkynes; Acid catalysed hydration of alkenes and alkynes (excluding the stereochemistry of addition and elimination); Reactions of alkenes with KMnO4 and ozone; Reduction of alkenes and alkynes; Preparation of alkenes and alkynes by elimination reactions; Electrophilic addition reactions of alkenes with X2, HX, HOX and H2O (X=halogen); Addition reactions of alkynes; Metal acetylides.
Reactions of benzene: Structure and aromaticity; Electrophilic substitution reactions: halogenation, nitration, sulphonation, Friedel-Crafts alkylation and acylation; Effect of o-, m- and p-directing groups in monosubstituted benzenes.
Phenols: Acidity, electrophilic substitution reactions (halogenation, nitration and sulphonation); Reimer-Tieman reaction, Kolbe reaction.
Characteristic reactions of the following (including those mentioned above):
Alkyl halides: rearrangement reactions of alkyl carbocation, Grignard reactions, nucleophilic substitution reactions;
Alcohols: esterification, dehydration and oxidation, reaction with sodium, phosphorus halides, ZnCl2/conc.-HCl, conversion of alcohols into aldehydes and ketones;
Aldehydes and Ketones: oxidation, reduction, oxime and hydrazone formation; aldol condensation, Perkin reaction; Cannizzaro reaction; haloform reaction and nucleophilic addition reactions (Grignard addition);
Carboxylic acids: formation of esters, acid chlorides and amides, ester hydrolysis;
Amines: basicity of substituted anilines and aliphatic amines, preparation from nitro compounds, reaction with nitrous acid, azo coupling reaction of diazonium salts of aromatic amines, Sandmeyer and related reactions of diazonium salts; carbylamine reaction; Haloarenes: nucleophilic aromatic substitution in haloarenes and substituted haloarenes - (excluding Benzyne mechanism and Cine substitution).
Carbohydrates: Classification; mono and di-saccharides (glucose and sucrose); Oxidation, reduction, glycoside formation and hydrolysis of sucrose.
Amino acids and peptides: General structure (only primary structure for peptides) and physical properties.
Properties and uses of some important polymers: Natural rubber, cellulose, nylon, teflon and PVC.
Practical organic chemistry: Detection of elements (N, S, halogens); Detection and identification of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl, amino and nitro; Chemical methods of separation of mono-functional organic compounds from binary mixtures.
We can see from a comparison of chapters and syllabus that every major head of the syllabus is covered in the above chapters
Study of Organic Chemistry Chapters
Today, I completed a preliminary reading of all chapters of Organic Chemistry given in TMH IIT JEE chemistry book. With this I completed a full reading of the lessons given in book. I need to a study a detailed book on organic chemistry. The material given in TMH book is too brief. I have a book from my library. Many in their blogs recommended Morrison and Boyd. I shall have to look at the book that I have now and then go to book stall and have a look at Morrison and Boyd and if required purchase it.
My Physics Blog
I am maintaining my record of study of Physics in my blog www.iit-jee-physics.blogspot.com
Saturday, May 26, 2007
Study 26th May 2007 Inorganic Chemistry
On the 26th May 2007, I studied the five chapters given in TMH IIT JEE Chemistry book. I answered the questions of the first part in the lesson on non metals. I am posting the main contents of the chapters below.
Chapter 13 Non-Metals
Boron
Silicon
Nitrogen
Phosphorus
Oxygen
Sulphur
Halogens
Allotropes of Carbon
Ozone
Syllabus
Isolation/preparation and properties of the following non-metals: Boron, silicon, nitrogen, phosphorus, oxygen, sulphur and halogens; Properties of allotropes of carbon (only diamond and graphite), phosphorus and sulphur.
Chapter 14 Compounds of Metals
Sodium and Potassium
Oxides, Peroxides, Hydroxides, Carbonates and Bicarbonates, Sulphates
Potassium permanganate, Potassium dichromate
Aluminium
Tin and Lead
Iron
Zinc
Silver
Preparation and properties of the following compounds: Oxides, peroxides, hydroxides, carbonates, bicarbonates, chlorides and sulphates of sodium, potassium, magnesium and calcium;
Aluminium: alumina, aluminium chloride and alums;
Preparation and properties of the following compounds: Oxides and chlorides of tin and lead; Oxides, chlorides and sulphates of Fe2+, Cu2+ and Zn2+; Potassium permanganate, potassium dichromate, silver oxide, silver nitrate, silver thiosulphate.
Syllabus
Chapter 15 Compound of Nonmetals
Hydrogen
Boron
Carbon
Silicon
Nitrogen
Phosphorus
Sulphur
Halogens
Xenon
Syllabus
Preparation and properties of the following compounds:
Boron: diborane, boric acid and borax;
Carbon: oxides and oxyacid (carbonic acid);
Silicon: silicones, silicates and silicon carbide;
Nitrogen: oxides, oxyacids and ammonia;
Phosphorus: oxides, oxyacids (phosphorus acid, phosphoric acid) and phosphine; Oxygen: ozone and hydrogen peroxide;
Sulphur: hydrogen sulphide, oxides, sulphurous acid, sulphuric acid and sodium thiosulphate;
Halogens: hydrohalic acids, oxides and oxyacids of chlorine, bleaching powder;
Xenon fluorides; Fertilizers: commercially available (common) NPK type.
Chapter 16 Transition Elements
1. Variable Oxidation State
2. Formation of Complexes
3. Size of Atoms
4. Density
5. Melting and Boiling Points
6. Ionization Energies
7. Colour
8. Magnetic Properties
9. Catalytic Activity
Syllabus
Transition elements (3d series): Definition, general characteristics, oxidation states and their stabilities, colour (excluding the details of electronic transitions) and calculation of spin-only magnetic moment; Coordination compounds: nomenclature of mononuclear coordination compounds, cis-trans and ionisation isomerisms, hybridization and geometries of mononuclear coordination compounds (linear, tetrahedral, square planar and octahedral).
Chapter 17 Ores/Minerals and Extractive Metallurgy
1. Iron and tin
2. Copper and Lead
3. Magnesium and Aluminium
4. Silver
Syllabus
Ores and minerals: Commonly occurring ores and minerals of iron, copper, tin, lead, magnesium, aluminium, zinc and silver.
Extractive metallurgy: Chemical principles and reactions only (industrial details excluded); Carbon reduction method (iron and tin); Self reduction method (copper and lead); Electrolytic reduction method (magnesium and aluminium); Cyanide process (silver and gold).
Syllabus
Principles of qualitative analysis: Groups I to V (only Ag+, Hg2+, Cu2+, Pb2+, Bi3+, Fe3+, Cr3+, Al3+, Ca2+, Ba2+, Zn2+, Mn2+ and Mg2+); Nitrate, halides (excluding fluoride), sulphate, sulphide and sulphite.
As I am aware of the various concepts discussed in these lessons, I can study more detailed materials about them in various books. Atomic structure seems to very important topic to understand thoroughly as the concepts of that topic are used subsequently in various lessons. Remembering x class inorganic chemistry portion is very important, as you will feel very comfortable learning only the incremental material on these topics if you remember the old material already.
Chapter 13 Non-Metals
Boron
Silicon
Nitrogen
Phosphorus
Oxygen
Sulphur
Halogens
Allotropes of Carbon
Ozone
Syllabus
Isolation/preparation and properties of the following non-metals: Boron, silicon, nitrogen, phosphorus, oxygen, sulphur and halogens; Properties of allotropes of carbon (only diamond and graphite), phosphorus and sulphur.
Chapter 14 Compounds of Metals
Sodium and Potassium
Oxides, Peroxides, Hydroxides, Carbonates and Bicarbonates, Sulphates
Potassium permanganate, Potassium dichromate
Aluminium
Tin and Lead
Iron
Zinc
Silver
Preparation and properties of the following compounds: Oxides, peroxides, hydroxides, carbonates, bicarbonates, chlorides and sulphates of sodium, potassium, magnesium and calcium;
Aluminium: alumina, aluminium chloride and alums;
Preparation and properties of the following compounds: Oxides and chlorides of tin and lead; Oxides, chlorides and sulphates of Fe2+, Cu2+ and Zn2+; Potassium permanganate, potassium dichromate, silver oxide, silver nitrate, silver thiosulphate.
Syllabus
Chapter 15 Compound of Nonmetals
Hydrogen
Boron
Carbon
Silicon
Nitrogen
Phosphorus
Sulphur
Halogens
Xenon
Syllabus
Preparation and properties of the following compounds:
Boron: diborane, boric acid and borax;
Carbon: oxides and oxyacid (carbonic acid);
Silicon: silicones, silicates and silicon carbide;
Nitrogen: oxides, oxyacids and ammonia;
Phosphorus: oxides, oxyacids (phosphorus acid, phosphoric acid) and phosphine; Oxygen: ozone and hydrogen peroxide;
Sulphur: hydrogen sulphide, oxides, sulphurous acid, sulphuric acid and sodium thiosulphate;
Halogens: hydrohalic acids, oxides and oxyacids of chlorine, bleaching powder;
Xenon fluorides; Fertilizers: commercially available (common) NPK type.
Chapter 16 Transition Elements
1. Variable Oxidation State
2. Formation of Complexes
3. Size of Atoms
4. Density
5. Melting and Boiling Points
6. Ionization Energies
7. Colour
8. Magnetic Properties
9. Catalytic Activity
Syllabus
Transition elements (3d series): Definition, general characteristics, oxidation states and their stabilities, colour (excluding the details of electronic transitions) and calculation of spin-only magnetic moment; Coordination compounds: nomenclature of mononuclear coordination compounds, cis-trans and ionisation isomerisms, hybridization and geometries of mononuclear coordination compounds (linear, tetrahedral, square planar and octahedral).
Chapter 17 Ores/Minerals and Extractive Metallurgy
1. Iron and tin
2. Copper and Lead
3. Magnesium and Aluminium
4. Silver
Syllabus
Ores and minerals: Commonly occurring ores and minerals of iron, copper, tin, lead, magnesium, aluminium, zinc and silver.
Extractive metallurgy: Chemical principles and reactions only (industrial details excluded); Carbon reduction method (iron and tin); Self reduction method (copper and lead); Electrolytic reduction method (magnesium and aluminium); Cyanide process (silver and gold).
Syllabus
Principles of qualitative analysis: Groups I to V (only Ag+, Hg2+, Cu2+, Pb2+, Bi3+, Fe3+, Cr3+, Al3+, Ca2+, Ba2+, Zn2+, Mn2+ and Mg2+); Nitrate, halides (excluding fluoride), sulphate, sulphide and sulphite.
As I am aware of the various concepts discussed in these lessons, I can study more detailed materials about them in various books. Atomic structure seems to very important topic to understand thoroughly as the concepts of that topic are used subsequently in various lessons. Remembering x class inorganic chemistry portion is very important, as you will feel very comfortable learning only the incremental material on these topics if you remember the old material already.
Friday, May 25, 2007
Reactivity Series of Metals
A mnemonic to aid in learning the reactivity series of metals:
Popular Potassium K
Scientists Sodium Na
Can Calcium Ca
Make Magnesium Mg
A Aluminium Al
Zoo Zinc Zn
In Iron Fe
The Tin Sn
Low Lead Pb
Humid Hydrogen [H]
Country Copper Cu
More Mercury Hg
Satisfactory Silver Ag
Source: http://www.ankurb.info/search/label/Education: See this site for a lot of information on various competitive examinations
Popular Potassium K
Scientists Sodium Na
Can Calcium Ca
Make Magnesium Mg
A Aluminium Al
Zoo Zinc Zn
In Iron Fe
The Tin Sn
Low Lead Pb
Humid Hydrogen [H]
Country Copper Cu
More Mercury Hg
Satisfactory Silver Ag
Source: http://www.ankurb.info/search/label/Education: See this site for a lot of information on various competitive examinations
Study 25-5-2007
I studied the topics 5 to 12 (the entire portion of Physical Chemistry remaining to be read by me) in the IIT JEE guide of TMH. Of course only main topics were coveed in the explanatory notes. But it gives me a good background to read the detailed topics from various books. I was able to study all topics at a go because I remember the x class material very well. I recommend to all to keep their x material fresh till they study XI and XII material related to them
Choice of IITs
A quick start - Top JEE ranker's joining IIT in 2006. Source PanIIT.
IIT Bombay 46
IIT Delhi 28
IIT Guwahati 0
IIT Kanpur 20
IIT Kharagpur 0
IIT Madras 6
IIT Roorkee 0
Source for me for this information
http://highheaven.blogspot.com/2007_01_01_archive.html
IIT Bombay 46
IIT Delhi 28
IIT Guwahati 0
IIT Kanpur 20
IIT Kharagpur 0
IIT Madras 6
IIT Roorkee 0
Source for me for this information
http://highheaven.blogspot.com/2007_01_01_archive.html
MIT courseware on Organic Chemistry
You can download MIT courseware on Organic Chemistry from
http://ocw.mit.edu/OcwWeb/Chemistry/5-12Organic-Chemistry-ISpring2003/DownloadthisCourse/index.htm
It is a zip file.
http://ocw.mit.edu/OcwWeb/Chemistry/5-12Organic-Chemistry-ISpring2003/DownloadthisCourse/index.htm
It is a zip file.
Thursday, May 24, 2007
IIT JEE Chemistry syllabus
JEE Chemistry Syllabus
Physical chemistry
General topics: The concept of atoms and molecules; Dalton's atomic theory; Mole concept; Chemical formulae; Balanced chemical equations; Calculations (based on mole concept) involving common oxidation-reduction, neutralisation, and displacement reactions; Concentration in terms of mole fraction, molarity, molality and normality.
Gaseous and liquid states: Absolute scale of temperature, ideal gas equation; Deviation from ideality, van der Waals equation; Kinetic theory of gases, average, root mean square and most probable velocities and their relation with temperature; Law of partial pressures; Vapour pressure; Diffusion of gases.
Atomic structure and chemical bonding: Bohr model, spectrum of hydrogen atom, quantum numbers; Wave-particle duality, de Broglie hypothesis; Uncertainty principle; Quantum mechanical picture of hydrogen atom (qualitative treatment), shapes of s, p and d orbitals; Electronic configurations of elements (up to atomic number 36); Aufbau principle; Pauli's exclusion principle and Hund's rule; Orbital overlap and covalent bond; Hybridisation involving s, p and d orbitals only; Orbital energy diagrams for homonuclear diatomic species; Hydrogen bond; Polarity in molecules, dipole moment (qualitative aspects only); VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, trigonal bipyramidal, tetrahedral and octahedral).
Energetics: First law of thermodynamics; Internal energy, work and heat, pressure-volume work; Enthalpy, Hess's law; Heat of reaction, fusion and vapourization; Second law of thermodynamics; Entropy; Free energy; Criterion of spontaneity.
Chemical equilibrium: Law of mass action; Equilibrium constant, Le Chatelier's principle (effect of concentration, temperature and pressure); Significance of DG and DGo in chemical equilibrium; Solubility product, common ion effect, pH and buffer solutions; Acids and bases (Bronsted and Lewis concepts); Hydrolysis of salts.
Electrochemistry: Electrochemical cells and cell reactions; Electrode potentials; Nernst equation and its relation to DG; Electrochemical series, emf of galvanic cells; Faraday's laws of electrolysis; Electrolytic conductance, specific, equivalent and molar conductance, Kohlrausch's law; Concentration cells.
Chemical kinetics: Rates of chemical reactions; Order of reactions; Rate constant; First order reactions; Temperature dependence of rate constant (Arrhenius equation).
Solid state: Classification of solids, crystalline state, seven crystal systems (cell parameters a, b, c, a, b, g), close packed structure of solids (cubic), packing in fcc, bcc and hcp lattices; Nearest neighbours, ionic radii, simple ionic compounds, point defects.
Solutions: Raoult's law; Molecular weight determination from lowering of vapor pressure, elevation of boiling point and depression of freezing point.
Surface chemistry: Elementary concepts of adsorption (excluding adsorption isotherms); Colloids: types, methods of preparation and general properties; Elementary ideas of emulsions, surfactants and micelles (only definitions and examples).
Nuclear chemistry: Radioactivity: isotopes and isobars; Properties of a, b and g rays; Kinetics of radioactive decay (decay series excluded), carbon dating; Stability of nuclei with respect to proton-neutron ratio; Brief discussion on fission and fusion reactions.
Inorganic Chemistry
Isolation/preparation and properties of the following non-metals: Boron, silicon, nitrogen, phosphorus, oxygen, sulphur and halogens; Properties of allotropes of carbon (only diamond and graphite), phosphorus and sulphur.
Preparation and properties of the following compounds: Oxides, peroxides, hydroxides, carbonates, bicarbonates, chlorides and sulphates of sodium, potassium, magnesium and calcium; Boron: diborane, boric acid and borax; Aluminium: alumina, aluminium chloride and alums; Carbon: oxides and oxyacid (carbonic acid); Silicon: silicones, silicates and silicon carbide; Nitrogen: oxides, oxyacids and ammonia; Phosphorus: oxides, oxyacids (phosphorus acid, phosphoric acid) and phosphine; Oxygen: ozone and hydrogen peroxide; Sulphur: hydrogen sulphide, oxides, sulphurous acid, sulphuric acid and sodium thiosulphate; Halogens: hydrohalic acids, oxides and oxyacids of chlorine, bleaching powder; Xenon fluorides; Fertilizers: commercially available (common) NPK type.
Transition elements (3d series): Definition, general characteristics, oxidation states and their stabilities, colour (excluding the details of electronic transitions) and calculation of spin-only magnetic moment; Coordination compounds: nomenclature of mononuclear coordination compounds, cis-trans and ionisation isomerisms, hybridization and geometries of mononuclear coordination compounds (linear, tetrahedral, square planar and octahedral).
Preparation and properties of the following compounds: Oxides and chlorides of tin and lead; Oxides, chlorides and sulphates of Fe2+, Cu2+ and Zn2+; Potassium permanganate, potassium dichromate, silver oxide, silver nitrate, silver thiosulphate.
Ores and minerals: Commonly occurring ores and minerals of iron, copper, tin, lead, magnesium, aluminium, zinc and silver.
Extractive metallurgy: Chemical principles and reactions only (industrial details excluded); Carbon reduction method (iron and tin); Self reduction method (copper and lead); Electrolytic reduction method (magnesium and aluminium); Cyanide process (silver and gold).
Principles of qualitative analysis: Groups I to V (only Ag+, Hg2+, Cu2+, Pb2+, Bi3+, Fe3+, Cr3+, Al3+, Ca2+, Ba2+, Zn2+, Mn2+ and Mg2+); Nitrate, halides (excluding fluoride), sulphate, sulphide and sulphite.
Organic Chemistry
Concepts: Hybridisation of carbon; Sigma and pi-bonds; Shapes of molecules; Structural and geometrical isomerism; Optical isomerism of compounds containing up to two asymmetric centers, (R,S and E,Z nomenclature excluded); IUPAC nomenclature of simple organic compounds (only hydrocarbons, mono-functional and bi-functional compounds); Conformations of ethane and butane (Newman projections); Resonance and hyperconjugation; Keto-enol tautomerism; Determination of empirical and molecular formula of simple compounds (only combustion method); Hydrogen bonds: definition and their effects on physical properties of alcohols and carboxylic acids; Inductive and resonance effects on acidity and basicity of organic acids and bases; Polarity and inductive effects in alkyl halides; Reactive intermediates produced during homolytic and heterolytic bond cleavage; Formation, structure and stability of carbocations, carbanions and free radicals.
Preparation, properties and reactions of alkanes: Homologous series, physical properties of alkanes (melting points, boiling points and density); Combustion and halogenation of alkanes; Preparation of alkanes by Wurtz reaction and decarboxylation reactions.
Preparation, properties and reactions of alkenes and alkynes: Physical properties of alkenes and alkynes (boiling points, density and dipole moments); Acidity of alkynes; Acid catalysed hydration of alkenes and alkynes (excluding the stereochemistry of addition and elimination); Reactions of alkenes with KMnO4 and ozone; Reduction of alkenes and alkynes; Preparation of alkenes and alkynes by elimination reactions; Electrophilic addition reactions of alkenes with X2, HX, HOX and H2O (X=halogen); Addition reactions of alkynes; Metal acetylides.
Reactions of benzene: Structure and aromaticity; Electrophilic substitution reactions: halogenation, nitration, sulphonation, Friedel-Crafts alkylation and acylation; Effect of o-, m- and p-directing groups in monosubstituted benzenes.
Phenols: Acidity, electrophilic substitution reactions (halogenation, nitration and sulphonation); Reimer-Tieman reaction, Kolbe reaction.
Characteristic reactions of the following (including those mentioned above): Alkyl halides: rearrangement reactions of alkyl carbocation, Grignard reactions, nucleophilic substitution reactions;
Alcohols: esterification, dehydration and oxidation, reaction with sodium, phosphorus halides, ZnCl2/conc.-HCl, conversion of alcohols into aldehydes and ketones;
Aldehydes and Ketones: oxidation, reduction, oxime and hydrazone formation; aldol condensation, Perkin reaction; Cannizzaro reaction; haloform reaction and nucleophilic addition reactions (Grignard addition);
Carboxylic acids: formation of esters, acid chlorides and amides, ester hydrolysis;
Amines: basicity of substituted anilines and aliphatic amines, preparation from nitro compounds, reaction with nitrous acid, azo coupling reaction of diazonium salts of aromatic amines, Sandmeyer and related reactions of diazonium salts; carbylamine reaction;
Haloarenes: nucleophilic aromatic substitution in haloarenes and substituted haloarenes - (excluding Benzyne mechanism and Cine substitution).
Carbohydrates: Classification; mono and di-saccharides (glucose and sucrose); Oxidation, reduction, glycoside formation and hydrolysis of sucrose.
Amino acids and peptides: General structure (only primary structure for peptides) and physical properties.
Properties and uses of some important polymers: Natural rubber, cellulose, nylon, teflon and PVC.
Practical organic chemistry: Detection of elements (N, S, halogens); Detection and identification of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl, amino and nitro; Chemical methods of separation of mono-functional organic compounds from binary mixtures.
Source: http://www.iitjee.org/iit-jee-syllabus.html
Physical chemistry
General topics: The concept of atoms and molecules; Dalton's atomic theory; Mole concept; Chemical formulae; Balanced chemical equations; Calculations (based on mole concept) involving common oxidation-reduction, neutralisation, and displacement reactions; Concentration in terms of mole fraction, molarity, molality and normality.
Gaseous and liquid states: Absolute scale of temperature, ideal gas equation; Deviation from ideality, van der Waals equation; Kinetic theory of gases, average, root mean square and most probable velocities and their relation with temperature; Law of partial pressures; Vapour pressure; Diffusion of gases.
Atomic structure and chemical bonding: Bohr model, spectrum of hydrogen atom, quantum numbers; Wave-particle duality, de Broglie hypothesis; Uncertainty principle; Quantum mechanical picture of hydrogen atom (qualitative treatment), shapes of s, p and d orbitals; Electronic configurations of elements (up to atomic number 36); Aufbau principle; Pauli's exclusion principle and Hund's rule; Orbital overlap and covalent bond; Hybridisation involving s, p and d orbitals only; Orbital energy diagrams for homonuclear diatomic species; Hydrogen bond; Polarity in molecules, dipole moment (qualitative aspects only); VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, trigonal bipyramidal, tetrahedral and octahedral).
Energetics: First law of thermodynamics; Internal energy, work and heat, pressure-volume work; Enthalpy, Hess's law; Heat of reaction, fusion and vapourization; Second law of thermodynamics; Entropy; Free energy; Criterion of spontaneity.
Chemical equilibrium: Law of mass action; Equilibrium constant, Le Chatelier's principle (effect of concentration, temperature and pressure); Significance of DG and DGo in chemical equilibrium; Solubility product, common ion effect, pH and buffer solutions; Acids and bases (Bronsted and Lewis concepts); Hydrolysis of salts.
Electrochemistry: Electrochemical cells and cell reactions; Electrode potentials; Nernst equation and its relation to DG; Electrochemical series, emf of galvanic cells; Faraday's laws of electrolysis; Electrolytic conductance, specific, equivalent and molar conductance, Kohlrausch's law; Concentration cells.
Chemical kinetics: Rates of chemical reactions; Order of reactions; Rate constant; First order reactions; Temperature dependence of rate constant (Arrhenius equation).
Solid state: Classification of solids, crystalline state, seven crystal systems (cell parameters a, b, c, a, b, g), close packed structure of solids (cubic), packing in fcc, bcc and hcp lattices; Nearest neighbours, ionic radii, simple ionic compounds, point defects.
Solutions: Raoult's law; Molecular weight determination from lowering of vapor pressure, elevation of boiling point and depression of freezing point.
Surface chemistry: Elementary concepts of adsorption (excluding adsorption isotherms); Colloids: types, methods of preparation and general properties; Elementary ideas of emulsions, surfactants and micelles (only definitions and examples).
Nuclear chemistry: Radioactivity: isotopes and isobars; Properties of a, b and g rays; Kinetics of radioactive decay (decay series excluded), carbon dating; Stability of nuclei with respect to proton-neutron ratio; Brief discussion on fission and fusion reactions.
Inorganic Chemistry
Isolation/preparation and properties of the following non-metals: Boron, silicon, nitrogen, phosphorus, oxygen, sulphur and halogens; Properties of allotropes of carbon (only diamond and graphite), phosphorus and sulphur.
Preparation and properties of the following compounds: Oxides, peroxides, hydroxides, carbonates, bicarbonates, chlorides and sulphates of sodium, potassium, magnesium and calcium; Boron: diborane, boric acid and borax; Aluminium: alumina, aluminium chloride and alums; Carbon: oxides and oxyacid (carbonic acid); Silicon: silicones, silicates and silicon carbide; Nitrogen: oxides, oxyacids and ammonia; Phosphorus: oxides, oxyacids (phosphorus acid, phosphoric acid) and phosphine; Oxygen: ozone and hydrogen peroxide; Sulphur: hydrogen sulphide, oxides, sulphurous acid, sulphuric acid and sodium thiosulphate; Halogens: hydrohalic acids, oxides and oxyacids of chlorine, bleaching powder; Xenon fluorides; Fertilizers: commercially available (common) NPK type.
Transition elements (3d series): Definition, general characteristics, oxidation states and their stabilities, colour (excluding the details of electronic transitions) and calculation of spin-only magnetic moment; Coordination compounds: nomenclature of mononuclear coordination compounds, cis-trans and ionisation isomerisms, hybridization and geometries of mononuclear coordination compounds (linear, tetrahedral, square planar and octahedral).
Preparation and properties of the following compounds: Oxides and chlorides of tin and lead; Oxides, chlorides and sulphates of Fe2+, Cu2+ and Zn2+; Potassium permanganate, potassium dichromate, silver oxide, silver nitrate, silver thiosulphate.
Ores and minerals: Commonly occurring ores and minerals of iron, copper, tin, lead, magnesium, aluminium, zinc and silver.
Extractive metallurgy: Chemical principles and reactions only (industrial details excluded); Carbon reduction method (iron and tin); Self reduction method (copper and lead); Electrolytic reduction method (magnesium and aluminium); Cyanide process (silver and gold).
Principles of qualitative analysis: Groups I to V (only Ag+, Hg2+, Cu2+, Pb2+, Bi3+, Fe3+, Cr3+, Al3+, Ca2+, Ba2+, Zn2+, Mn2+ and Mg2+); Nitrate, halides (excluding fluoride), sulphate, sulphide and sulphite.
Organic Chemistry
Concepts: Hybridisation of carbon; Sigma and pi-bonds; Shapes of molecules; Structural and geometrical isomerism; Optical isomerism of compounds containing up to two asymmetric centers, (R,S and E,Z nomenclature excluded); IUPAC nomenclature of simple organic compounds (only hydrocarbons, mono-functional and bi-functional compounds); Conformations of ethane and butane (Newman projections); Resonance and hyperconjugation; Keto-enol tautomerism; Determination of empirical and molecular formula of simple compounds (only combustion method); Hydrogen bonds: definition and their effects on physical properties of alcohols and carboxylic acids; Inductive and resonance effects on acidity and basicity of organic acids and bases; Polarity and inductive effects in alkyl halides; Reactive intermediates produced during homolytic and heterolytic bond cleavage; Formation, structure and stability of carbocations, carbanions and free radicals.
Preparation, properties and reactions of alkanes: Homologous series, physical properties of alkanes (melting points, boiling points and density); Combustion and halogenation of alkanes; Preparation of alkanes by Wurtz reaction and decarboxylation reactions.
Preparation, properties and reactions of alkenes and alkynes: Physical properties of alkenes and alkynes (boiling points, density and dipole moments); Acidity of alkynes; Acid catalysed hydration of alkenes and alkynes (excluding the stereochemistry of addition and elimination); Reactions of alkenes with KMnO4 and ozone; Reduction of alkenes and alkynes; Preparation of alkenes and alkynes by elimination reactions; Electrophilic addition reactions of alkenes with X2, HX, HOX and H2O (X=halogen); Addition reactions of alkynes; Metal acetylides.
Reactions of benzene: Structure and aromaticity; Electrophilic substitution reactions: halogenation, nitration, sulphonation, Friedel-Crafts alkylation and acylation; Effect of o-, m- and p-directing groups in monosubstituted benzenes.
Phenols: Acidity, electrophilic substitution reactions (halogenation, nitration and sulphonation); Reimer-Tieman reaction, Kolbe reaction.
Characteristic reactions of the following (including those mentioned above): Alkyl halides: rearrangement reactions of alkyl carbocation, Grignard reactions, nucleophilic substitution reactions;
Alcohols: esterification, dehydration and oxidation, reaction with sodium, phosphorus halides, ZnCl2/conc.-HCl, conversion of alcohols into aldehydes and ketones;
Aldehydes and Ketones: oxidation, reduction, oxime and hydrazone formation; aldol condensation, Perkin reaction; Cannizzaro reaction; haloform reaction and nucleophilic addition reactions (Grignard addition);
Carboxylic acids: formation of esters, acid chlorides and amides, ester hydrolysis;
Amines: basicity of substituted anilines and aliphatic amines, preparation from nitro compounds, reaction with nitrous acid, azo coupling reaction of diazonium salts of aromatic amines, Sandmeyer and related reactions of diazonium salts; carbylamine reaction;
Haloarenes: nucleophilic aromatic substitution in haloarenes and substituted haloarenes - (excluding Benzyne mechanism and Cine substitution).
Carbohydrates: Classification; mono and di-saccharides (glucose and sucrose); Oxidation, reduction, glycoside formation and hydrolysis of sucrose.
Amino acids and peptides: General structure (only primary structure for peptides) and physical properties.
Properties and uses of some important polymers: Natural rubber, cellulose, nylon, teflon and PVC.
Practical organic chemistry: Detection of elements (N, S, halogens); Detection and identification of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl, amino and nitro; Chemical methods of separation of mono-functional organic compounds from binary mixtures.
Source: http://www.iitjee.org/iit-jee-syllabus.html
Wednesday, May 23, 2007
Glossary 2 Chemistry Solutions Chapter
Solute: the substance dissolved; the substance present in a solution in the lesser amount.
Solvent: the dissolving medium; the substance in a solution in the greater amount.
Solution: a homogeneous mixture of two or more substances.
volume percent
Vol% = 100*volume of solute/(volume of solute + volume of solvent)
mass percent
mass % = 100*(mass of solute)/(mass of solute + mass of solvent)
parts per million
ppm = 10^6*(mass of solute)/(mass of solute + mass of solvent)
molality
m = number of moles of solute/kilograms of solvent
molar concentration or moles per liter or Molarity
M = number of moles of solute/liters solution
Mole fraction
Xy (y is subscript) = number of moles of y in mixture/totals moles in mixture
Solvent: the dissolving medium; the substance in a solution in the greater amount.
Solution: a homogeneous mixture of two or more substances.
volume percent
Vol% = 100*volume of solute/(volume of solute + volume of solvent)
mass percent
mass % = 100*(mass of solute)/(mass of solute + mass of solvent)
parts per million
ppm = 10^6*(mass of solute)/(mass of solute + mass of solvent)
molality
m = number of moles of solute/kilograms of solvent
molar concentration or moles per liter or Molarity
M = number of moles of solute/liters solution
Mole fraction
Xy (y is subscript) = number of moles of y in mixture/totals moles in mixture
Chemistry Online Resources
A good web page for online resources on Chemistry.
http://www.towson.edu/csme/mctp/Technology/Chemistry.html
http://www.towson.edu/csme/mctp/Technology/Chemistry.html
Tuesday, May 22, 2007
Chemistry Glossary 1
Princiapl quantum number, n: an integer that represents, and can be used to calculate, the total energy of an electron in an atom. Its values are n = 1,2,3,...
Spin quantum number,s: a quantum number that repreents a property of an electron which is likened to spin.
electron configuration: an arrangement of electrons in a sequence of atomic orbitals starting with the lowest energy orbital.
Aufbau principle: a rule that states that electrons in unexcited atoms are distributed within the levels using the lowest energy orbital first, the next lowest second, and so on.
Hund's rule: when placing electrons into a set of equivalent orbitals, each orbital receives one electron before any orbital is given two.
Pauli exclusion principle: no two electrons in an atom can have all four of their quantum numbers exactly the same.
Spin quantum number,s: a quantum number that repreents a property of an electron which is likened to spin.
electron configuration: an arrangement of electrons in a sequence of atomic orbitals starting with the lowest energy orbital.
Aufbau principle: a rule that states that electrons in unexcited atoms are distributed within the levels using the lowest energy orbital first, the next lowest second, and so on.
Hund's rule: when placing electrons into a set of equivalent orbitals, each orbital receives one electron before any orbital is given two.
Pauli exclusion principle: no two electrons in an atom can have all four of their quantum numbers exactly the same.
Study 23 May 2007
Today I studied Chapter 2, 3 & 4 of TMH IIT JEE study guide.
In the second chapter, liquids section there is discussion of surface tension and viscocity.
In the solids section, there is discussion on crystalline structure of solids.
In the third chapter on Atomic Structure, the four quantum numbers are given. One of the principles says that no two electrons in an atom will have all the four quantum numbers same.
In the fourth chapter, on periodicity, it is mostly the material that was covered in the x class. Revising x portion is very important for a quick understanding of XI and XII material.
In the second chapter, liquids section there is discussion of surface tension and viscocity.
In the solids section, there is discussion on crystalline structure of solids.
In the third chapter on Atomic Structure, the four quantum numbers are given. One of the principles says that no two electrons in an atom will have all the four quantum numbers same.
In the fourth chapter, on periodicity, it is mostly the material that was covered in the x class. Revising x portion is very important for a quick understanding of XI and XII material.
IIT JEE Chemistry Suggested Books
The suggestions from blogs are very scarce.
From http://chem-iitjee-preparations.blogspot.com/2006/10/books.html
Organic
Morrison Boyd: Its fantastic. It makes your concepts so clear that you dont require to remember reactions at all. Just go through it thoroughly and understand it properly. Effect of protic and aprotic solvents on reactions, impact of structure on reaction rates and correspondence of reaction mechanism with structure and solvents are very beautifully described in the book. Morrison boyd is exactly what JEE syllabus is.
RK Gupta: Its a great book to practice. Collection of questions is good.
Physical Chemistry: For Physical Chemistry I studied only OP Agrawal and FIITJEE RSM (and ofcourse the board syllabus books). I choosed OP Agrawal only because I was not doing tutions and it had very large number of solved problems. I also solved some problems of ionic equilibrium from Rosenburg. But I dont say I loved that a lot. FIITJEE RSM is great for physical chemistry.
Inorganic: As I said CBSE syllabus is sufficient for all its part except for Salt analysis. I did salt analysis from RK Gupta and liked it. FIITJEE RSM is also good
T.Dubey,a IIT student on http://www.mouthshut.com/review/Successful_Preparation_for_IIT_JEE-41404-1.html recommends
Maths M.L.Khanna
Physics Resnick - Halliday, H.C.Verma
Chemistry O.P Agarwal, Morrison - Boyd, Finar, J.D Lee
From http://chem-iitjee-preparations.blogspot.com/2006/10/books.html
Organic
Morrison Boyd: Its fantastic. It makes your concepts so clear that you dont require to remember reactions at all. Just go through it thoroughly and understand it properly. Effect of protic and aprotic solvents on reactions, impact of structure on reaction rates and correspondence of reaction mechanism with structure and solvents are very beautifully described in the book. Morrison boyd is exactly what JEE syllabus is.
RK Gupta: Its a great book to practice. Collection of questions is good.
Physical Chemistry: For Physical Chemistry I studied only OP Agrawal and FIITJEE RSM (and ofcourse the board syllabus books). I choosed OP Agrawal only because I was not doing tutions and it had very large number of solved problems. I also solved some problems of ionic equilibrium from Rosenburg. But I dont say I loved that a lot. FIITJEE RSM is great for physical chemistry.
Inorganic: As I said CBSE syllabus is sufficient for all its part except for Salt analysis. I did salt analysis from RK Gupta and liked it. FIITJEE RSM is also good
T.Dubey,a IIT student on http://www.mouthshut.com/review/Successful_Preparation_for_IIT_JEE-41404-1.html recommends
Maths M.L.Khanna
Physics Resnick - Halliday, H.C.Verma
Chemistry O.P Agarwal, Morrison - Boyd, Finar, J.D Lee
Monday, May 21, 2007
Started studying chemistry
I started studying chemistry also along with Physics. I bought Tata McGrawhill JEE 2007 book sometime back. I read the first lesson and material relating to Gases in the second lesson. The authors should have recommended good books on the subject in their guide. The lessons given in the guide are too brief and one cannot understand anything by just reading that material. The guide may be useful to give practice in answering large number of questions. But it is absolutely inadequate for learning the subject or to attempt answering the questions given. I shall write to McGraw-Hill people about it.
I have fundamentals of Chemistry, by Fred Redmore, a book given to me by a colleague to refer now.
I have fundamentals of Chemistry, by Fred Redmore, a book given to me by a colleague to refer now.
Wednesday, May 16, 2007
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