Cbse Class 12 Marking Scheme Chemistry 2018-2019.pdf

Class: XII Chemistry Marking Scheme 2018-19 Time allowed: 3 Hours

Maximum Marks: 70

Q No

SECTION A

Marks

On heating ZnO , it loses oxygen and there is excess of Zn2+ions in the crystal.

1

OR When silicon is doped with phosphorous (group 15 element), the increase in conductivity is due to the delocalised negatively charged electrons.

1

2.

Associated colloids

1

3.

t 23g eg3

1

1.

OR The orbital splitting energies, Δ t are not sufficiently large for forcing pairing of electrons in the tetrahedral coordination entity formation.

1

4.

B

1

5.

Poly   hydroxybutyrate  co    hydroxy valerate

1

SECTION B 6.

+

HBr → H + Br i 1    n n 2 i 1   T f  iK f m

–

T f  (1   )1.86 x T f  3.53

½ ½ 8.1 1000 x 81 100

½

T f0  00 C

½ ½ ½

T f  T f0  T f' T f'  3.5340 C

Mole fraction of water ,  H 2O

OR  0.88

Mole fraction of ethanol ,  C2 H5OH  1 0.88 = 0.12 n  C2 H 5OH  2 n1  n2 ……………(1) 1

½

n2= number of moles of ethanol. n1 = number of moles of water.Molality of ethanol means the number of moles of ethanol present in 1000 g of water. 1000 n1   55.5 moles 18

½

Substituting the value of n1 in equation (1) ½

n2  0.12 55.5  n2

½

n2  7.57 moles Molality of ethanol ( C2H5OH) = 7.57 m Alternatively, ½ Mole fraction of water = 0.88 Mole fraction of ethanol = 1-0.88 = 0.12 Therefore 0.12 moles of ethanol are present in 0.88 moles of water. Mass of water = 0.88 x 18 =15.84 g of water. Molality = number of moles of solute (ethanol) present in 1000 g of solvent (water) = 12 x 1000 / 15.84 = 7.57 m Molality of ethanol ( C2H5OH) = 7.57 m 7.(a) (b)

Reaction : Hell-Volhard-Zelinsky reaction. IUPAC : 2-Bromopropanoic acid. Reaction : Rosenmund reduction reaction. IUPAC : Benzaldehyde.

½

½ ½ ½ ½

OR ½ i)

2-Methylbut-2-enal

CH3

½

CH3-CH=CH-CHO ii)

½

Pent-2-enal

½

CH3-CH2-CH=CH-CHO

8.(a) (b)

Tert-butyl peroxide acts as a free radical generating initiator(catalyst) CH2 = CH- CH = CH2 C6H5 – CH= CH2

2

1 ½ ½

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9.

Step 1 : Formation of protonated alcohol.

Step 2 : Formation of carbocation.

½

1

Step 3: Formation of ethane by elimination of a proton. ½

10.

(i) Zero order reaction (ii) Slope represents –k ; Intercept represents [R]o (iii) mol L1 s 1

½ ½+½ ½

11.(a) 1

(b) 1

12.(i)

Since Ti4+/Ti3+ has lower reduction potential than Fe3+/Fe2+, it cannot be reduced in 1 comparison with Fe3+/Fe2+ ions. Hence Ti4+ cannot oxidise Fe2+ to Fe3+. ½

(ii)

As the value of reduction potential increases the stability of +2 oxidation increases. 1 Therefore correct order of stability is Cr3+/Cr2+ < Fe3+/Fe2+ < Mn3+/Mn2+ ½

3

SECTION C 13.

r

½

3 a 4

3 a 4 a = 330.4 pm zM  3 a NA 143.1 



½ ½

2 x 93 (330.4 x10 ) x 6.023 x 1023

½

10 3

  8.58 g / cm3 14.(a) (b)

(c)

½+½

Molecules of benzoic acid dimerise in benzene, the number of particles are reduced.

1

The intermolecular interactions between ethanol and acetone are weaker/ the 1 escaping tendency of ethanol and acetone molecules increases on mixing / the vapour pressure increases. 1 Due to osmosis, a bacterium on fruit loses water, shrivels and dies.

15. CH3 A:

1

CH3-CH-CH2-OH

CH3 B : CH3-CH-COOH

½

CH3 ½

C : CH3-CH = CH2

CH3

½ D : CH3- CH- CH3 OH

½ A and D are position isomers.

4

16.

C6H5 CH2Cl will undergo SN1reaction faster. The carbocation formed by C6 H5 CH2Cl gets stabilized through resonance. Greater the stability of carbocation, greater will be its ease of formation from the respective halide.

½ ½ 1

1

OR

Cl

½

CH3-CH-CH2Cl

½ ½

CH2Cl-CH2-CH2Cl CH3-CH2-CHCl2

½

Cl ½

CH3-C-CH3

½

Cl The following isomer will exhibit enantiomerism:

Cl CH3-CH-CH2Cl IUPAC name: 1,2-Dichloropropane. 17.(a)

(b)

N-OH

1

HOOC - CH2 - CH2 - CH2 - CH2 – COOH

5

1

O (c)

C

1

NH C O 18.(i) (ii)

(iii) 19.(a) (b) (c)

It is unstable at cooking temperature. 1 Excessive hydrogencarbonate can make the stomach alkaline and trigger the production of even more acid. Metal hydroxides being insoluble do not increase the 1 pH above neutrality. Aspirin has anti blood clotting action. 1 Amylopectin. C- 2 Two peptide linkages.

(1) (2) (3) (4)

20.

1 1 1

OR Glucose does not give 2,4- DNP test. Glucose does not give Schiff’s test. The pentaacetate of glucose does not react with hydroxylamine. Glucose does not form the hydrogensulphite addition product with NaHSO3. (Any three points )

2 N 2O5 ( g )  2 N 2O4 ( g )  O2 ( g ) At t = 0 0.5 atm 0 atm 0 atm x atm 0.5  2 x atm 2 x atm At time t pt  pN2O5  pN2O4  pO2 =  (0.5  2 x)  2 x  x =  0.5  x x  pt  0.5 pN 2O5  0.5  2 x

1 1 1

½

 0.5  2( pt  0.5) = 1.5 – 2pt At t = 100 s ; pt = 0.512 atm pN2O5  1.5  2  0.512  0.476 atm

½

p 2.303 log i t pA 2.303 0.5 atm k log 100s 0.476 atm 2.303 k  0.0216  4.98 104 s 1 100s OR

½

k

½

1 1

The Arrhenius equation: k  Ae  Ea / RT Taking log on both sides: log k  log A 

6

Ea 2.303RT

Ea (1) 2.303RT Ea (2) For reaction (ii) log k2  log A  2.303RT Subtracting (i) from (ii) E (1)  Ea (2) k log 1  a k2 2.303RT k 24.9 1000 = log 1   4.342 k2 2.303  8.3  300 k1  anti log( 4.342) = 2.198×104 k2

For reaction (i) log k1  log A 

21. (a)

Negative charge is developed on the sol. Sol is represented as AgI / I 

1

1

½ ½

(b)

Adsorption of reactants on the solid surface of the catalysts increases the rate of 1 reaction.

(c)

Na3PO4 Hardy-Schulze rule

22. (a)

(b)

½ ½

Leached gold complex is treated with Zinc and gold is recovered by displacement method ½  2 2 Au[(CN ) 2 ] (aq)  Zn(s)  2 Au (s)  [Zn(CN ) 4 ] (aq) ½ Zirconium iodide is decomposed on a tungsten filament; electrically heated to 1800 ½ K. Pure Zr metal is deposited on the filament. ½ ZrI4  Zr  I 2 Silica is added to the ore and heated. It helps to slag off iron oxide as iron silicate

(c)

½ ½

FeO  SiO2  FeSiO 3 (slag )

(a)

OR NaCN is used as depressants to separate two sulphide ores ( ZnS and PbS) in Froth Floatation Method.

(1)

(b)

Carbon monoxide forms a volatile complex of nickel, nickel tetracarbonyl.

(1)

(c)

Coke is used as a reducing agent to reduce zinc oxide to zinc.

(1)

23. (a)

Co2+ : [Ar]3d7 Sc3+ : [Ar]3d0 Cr3+ : [Ar]3d3 Co2+ and Cr3+ have unpaired electrons. Thus, they are coloured in aqueous 1 solution.Sc3+ has no unpaired electron. Thus it is colourless.

(b)

Metal copper has high enthalpy of atomisation and enthalpy of ionisation. Therefore 1 the high energy required to convert Cu(s) to Cu2+(aq) is not balanced by its hydration enthalpy. 7

(c)

24. (a) (b) (c)

Due to lanthanoid contraction the size of lanthanoid ion decreases regularly with increase in atomic size. Thus covalent character between lanthanoid ion and OH- 1 increases from La3+ to Lu3+. Thus the basic character of hydroxides decreases from La(OH)3 to Lu(OH)3

Isomer A: [Cr(NH3)4 BrCl ]Cl Isomer B: [Cr (NH3)4 Cl2]Br Hybridisation of Cr in isomer A and B is d2sp3. Number of unpaired electrons in Cr3+(3d3) is 3 Magnetic moment = n(n  2)

½ ½ 1

1

= 3(3  2) = 3.87 BM (deduct half mark for wrong unit/unit not written) 25.(a)

A = AgNO2

½

CH2 - NH2

½

B= O CH2 - C - NH2

½

C=

½

D = CHCl3 + KOH , Heat. (b) (i)

(ii)

Experiment Azo dye test: Dissolve the amine in HCl, cool it and then add cold aqueous solution of NaNO2 and then solution of  - naphthol

Aniline

Benzylamine

A brilliant orange red dye is observed.

No dye is formed.

Experiment Methylamine Carbylamine test: To the organic A foul smelling compound add substance chloroform and (isocyanide) ethanolic potassium hydroxide and heat (or any other suitable test) 8

1

Dimethylamine No reaction.

1

(c)

A = CH3CH2CH2NH2

½

B = CH3CH2CH2OH

½ OR

(a)(i)

In strongly acidic medium, aniline is protonated to form the anilium ion which is meta directing.

1

(ii)

Aryl halides do not undergo nucleophilc substitution with the anion formed by phthalimide.

1

NH3,  CH3-CO-NH2

CH3- COOH

NaOH + Br2

CH3NH2

1

(b)(i) NHCOCH3

NH2

(ii)

NHCOCH3 -

NH2 +

OH or H

(CH3CO)2O

Br2

pyridine

CH3COOH Br

1 Br

(c)

p- Nitroaniline < Aniline < p- Toludine.

1

26.(a) (b)

Ecell decreases. Anode: Cl2 ↑ Cathode : H2 ↑ Cu 2 (aq.)  Ni(s)  Ni 2 (aq.)  Cu(s)

1 ½ ½ ½

(c)

0 0 E 0 cell  Ecathode  Eanode

E 0 cell  0.34  (0.25) E 0 cell  0.59V

½

2.303RT [ Ni 2 ] Ecell  E  log nF [Cu 2 ] 0.059 [0.01 ] Ecell  0.59  log 2 [0.1 ] Ecell  0.6195V

½

0 cell

½ ½ +½ OR 1



 2

(a)



(b)

Conductivity of NaCl decreases on dilution as the number of ions per unit volume decreases.

0 m ( CaCl2 )

0 Ca2

0 Cl 

9

1

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(c)

27. (a)

(b)

(a)

(b)

(c)

Whereas molar conductivity of NaCl increases on dilution as on dilution the interionic interactions are overcome and ions are free to move.

1

G*   R 1.29   0.0129 S cm 1 100 1000  m  C 1000 x 0.0129 m  0.1  m 129 S cm 2 mol 1

½

(i)S atom in SF4 is not sterically protected as it is surrounded by only four F atoms, so attack of water molecules can take place easily. In contrast, S atom in SF6 is protected by six F aoms. Thus attack by water molecules cannot take place easily.

1

(ii) Chlorine water produces nascent oxygen (causes oxidation) which is responsible for bleaching action. Cl2  H 2O  2HCl  [O]

1

(iii) Due to inert pair effect Bi(V) can accept a pair of electrons to form more stable Bi (III). (+3 oxidation state of Bi is more stable than its +5 oxidation state).

1

½ ½

½

(i)Phosphorus undergoes disproportionation reaction to form phosphine gas. P4  3NaOH  3H 2O  PH 3  3NaH 2 PO2

1

(ii)On partial hydrolysis, XeF6 gives oxyfluoride XeOF4 and HF. XeF6  H 2O  XeOF4  2HF

1

OR N.Bartlett first prepared a red compound O2+PtF6-. He then realised that the first 1 ionisation enthalpy of molecular oxygen was almost identical with Xenon. So he carried out reaction between Xe and PtF6. 1 (i) I2 < F2 < Br2 < Cl2 1 (ii) NH3 > PH3 > AsH3 > SbH3 > BiH3 1

(i)

2 NaOH  Cl2  NaCl  NaOCl  H 2O 1

(ii)

2Fe 3  SO2  2H 2 O  2Fe 2  SO42  4H 

********** 10

Class 12 Chemistry NCERT Solutions

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CBSE Notes

Chapter 1 The Solid State

Solid State

The Solid State

Chapter 2 Solutions

Solutions

Solutions

Chapter 3 Electro chemistry

Electrochemistry

Electro chemistry

Chapter 4 Chemical Kinetics

Chemical Kinetics

Chemical Kinetics

Chapter 5 Surface Chemistry

Surface Chemistry

Surface Chemistry

Chapter 6 General Principles and Processes of Isolation of Elements

General Principles and Processes of Isolation of Elements

General Principles and Processes of Isolation of Elements

Chapter 7 The p Block Elements

The p-Block Elements

The p Block Elements

Chapter 8 The d and f Block Elements The d- and f-Block Elements

The d and f Block Elements

Chapter 9 Coordination Compounds

Coordination Compounds

Coordination Compounds

Chapter 10 Haloalkanes and Haloarenes

Haloalkanes and Haloarenes

Haloalkanes and Haloarenes

Chapter 11 Alcohols Phenols and Ethers

Alcohols, Phenols and Ethers

Alcohols Phenols and Ethers

Chapter 12 Aldehydes Ketones and Carboxylic Acids

Aldehydes, Ketones and Carboxylic Acids

Aldehydes Ketones and Carboxylic Acids

Chapter 13 Amines

Amines

Amines

Chapter 14 Biomolecules

Biomolecules

Biomolecules

Chapter 15 Polymers

Polymers

Polymers

Chapter 16 Chemistry in Everyday Life

Chemistry in Everyday Life

Chemistry in Everyday Life

JEE Main Chemistry Chapter wise Previous Year Questions Basic Concepts and Stoichometry

Haloalkenes and Haloarenes

States of Matter: Gases,Liquids and Solids

Alcohols,Ethers,Carobonyls and Carboxylic Acids

Atomic Structure and Electronic Configuration

Nitro,Amine and Azo Compounds

Periodic Classification and Properties

Solutions and Colligative Properties

Chemical Bonding and Molecular Structure

Kinetics,Catalysis and Surface Chemistry

Elements of S-Block : Hydrogen,Group 1 and 2

Chemical and Lonic Equilibrium

Elements of p-Block: Groups 13,14,15,16,17 and 18 Redox Reactions and Electrochemistry Elements of d-Block,f-Block and Complexes

Thermodynamics and Chemical Energitics

Metallurgy and Environmental Chemistry

Biomolecules and Polymers

General Organic Chemistry

Chemistry in Everyday Life and Miscellaneous

Alkanes ,Alkenes ,Alkynes and Arenes

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Class 12 Chemistry Lab Manual 1. Introduction to Basic Laboratory Equipment 1. Viva Questions with Answers. 2. Surface Chemistry 1. Exp-2.1 : To prepare colloidal solution (sol) of starch. 2. Exp-2.2 : To prepare a colloidal solution of gum. 3. Exp-2.3 : To prepare colloidal solution (or sol) of egg albumin. 4. Exp-2.4 : To prepare ferric hydroxide, [Fe(OH)3] sol. 5. Exp-2.5 : To prepare aluminium hydroxide, [Al(OH)3] sol. 6. Exp-2.6 : To prepare colloidal solution of arsenious sulphide, [As2 S3]. 7. Exp-2.7 :To study the dialysis of starch sol containing sodium chloride through a cellophane or parchment paper. 8. Exp-2.8 : Compare the precipitation values of sodium chloride, barium chloride and aluminium chloride for arsenious sulphide sol. 9. Exp-2.9 : To study the effectiveness of different common oils (castor oil, cotton seed oil, coconut oil, kerosene oil, mustard oil) in forming emulsions. 10. Exp-2.10 : To compare the effectiveness of a number of emulsifying agents in forming emulsions. 11. Surface Chemistry Viva Questions with Answers. 3. Chemical Kinetics 1. Exp-3.1 : To study the effect of concentration on the rate of reaction between sodium thiosulphate and hydrochloric acid. 2. Exp-3.2 : To study the effect of change in temperature on the rate of reaction between sodium thiosulphate and hydrochloric acid. 3. Exp-3.3 : To study the reaction rate of reaction of iodide ions with hydrogen peroxide at different concentrations of iodide ions. 4. Exp-3.4 : To study the reaction rate of the reaction between potassium iodate (KIO3) and sodium sulphite (Na2S03) using starch solution as indicator. 5. Chemical Kinetics Viva Questions with Answers. 4. Thermochemistry 1. Exp-4.1 : Determine the calorimeter constant (W) of calorimeter (polythene bottle). 2. Exp-4.2 : Determine the enthalpy of dissolution of given solid copper sulphate (CuS04.5H20) in water at room temperature. 3. Exp-4.3 : Determine the enthalpy of neutralisation of hydrochloric acid with sodium hydroxide solution. 4. Exp-4.4 : Determine the enthalpy change during the interaction (hydrogen bond formation) between acetone and chloroform. 5. Thermochemistry Viva Questions with Answers. 5. Electrochemistry 1. Exp-5.1 : To set up simple Daniell cell and determine its emf . 2. Exp-5.2 : To set up simple Daniell cell using salt bridge and determine its emf . 3. Exp-5.3 : To study the variation of cell potential in Zn | Zn2+ || Cu2+ | Cu cell with change in concentration of electrolytes (CuS04 and ZnS04) at room temperature. 4. Electrochemistry Viva Questions with Answers. 6. Chromatography 1. Exp-6.1 : Separate the coloured components present in the mixture of red and blue inks by ascending paper chromatography and find their Rf values . 2. Exp-6.2 : Separate the coloured components present in the given grass/flower by ascending paper chromatography and determine their Rf values . 3. Exp-6.3 : Separate Co2+ and Ni2+ ions present in the given mixture by using ascending paper chromatography and determine their Rf values . 4. Chromatography Viva Questions with Answers. 7. Preparation of Inorganic Compounds 1. Exp-7.1 : To prepare a pure sample of ferrous ammonium sulphate (Mohr’s salt), [FeSO4 . (NH4)2 SO4.6HO20] . 2. Exp-7.2 : To prepare a pure sample of potash alum (Fitkari), [K2SO4.Al2 (SO4)3. 24H20] . CBSE Sample Papers

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8.

9.

10.

11.

3. Exp-7.3 : To prepare a pure sample of the complex potassium trioxalatoferrate(III), Kg[Fe(C2O4)3l . 3H20 . 4. Preparation of Inorganic Compounds Viva Questions with Answers. Preparation of Organic Compounds 1. Exp-8.1 : To prepare a sample of acetanilide from aniline. 2. Exp-8.2 : To prepare a sample of dibenzalacetone. 3. Exp-8.3 : To prepare a sample of p-nitroacetanilide from acetanilide . 4. Exp-8.4 : To prepare 2-naphthol aniline or phenyl-azo-β-naphtholdye . 5. Preparation of Organic Compounds Viva Questions with Answers. Tests for the Functional Groups Present in Organic Compounds 1. Exp-9.1 : Identify the functional group present in the given organic compound. 2. Tests for the Functional Groups Present in Organic Compounds Viva Questions with Answers. Tests of Carbohydrates, Fats and Proteins in Pure Samples and Detection of Their Presence in Given Food Stuffs 1. Exp-10.1 : To study some simple tests of carbohydrates . 2. Exp-10.2 : To study some simple tests of oils and fats . 3. Exp-10.3 : To study some simple tests of proteins . 4. Exp-10.4 : To detect the presence of carbohydrates, fats and proteins in the following food stuffs : Grapes, potatoes, rice, butter, biscuits, milk, groundnut, boiled egg . 5. Tests of Carbohydrates, Fats and Proteins in Pure Samples and Detection of Their Presence in Given Food Stuffs Viva Questions with Answers. Volumetric Analysis 1. Exp-11.1 : Prepare 250 ml of M/10 solution of oxalic acid from crystalline oxalic acid . 2. Exp-11.2 : Prepare 250 ml of a N/10 solution of oxalic acid from crystalline oxalic acid . 3. Exp-11.3 : Preparation of 250 ml of M/20 solution of Mohr’s salt . 4. Exp-11.4 : Preparation of 250 ml of N/20 solution of Mohr’s salt . 5. Exp-11.5 : Prepare M/20 solution of ferrous ammonium sulphate (Mohr’s salt). Using this solution find out the molarity and strength of the given KMn04 solution. 6. Exp-11.6 : Prepare a solution of ferrous ammonium sulphate (Mohr’s salt) containing exactly 17.0 g of the salt in one litre. With the help of this solution, determine the molarity and the concentration of KMnO4 in the given solution. 7. Exp-11.7 : Prepare M/20 ferrous ammonium sulphate (Mohr’s salt) solution. Find out the percentage purity of impure KMnO4 sample 2.0 g of which have been dissolved per litre . 8. Exp-11.8 : Determine the equivalent mass and number of molecules of water of crystallisation in a sample of Mohr’s salt, FeSO4(NH4)2 SO4 . nH20. Provided KMnO4. 9. Exp-11.9 : Prepare M/50 solution of oxalic acid. With its help, determine 50 the molarity and strength of the given solution of potassium permanganate (KMnO4). 10. Exp-11.10 : Find out the percentage purity of impure sample of oxalic acid. You are supplied M/100 KMnO4 solution. 11. Exp-11.11 : The given solution has been prepared by dissolving 1.6 g of an alkali metal permanganate per litre of solution. Determine volumetrically the atomic mass of the alkali metal. Prepare M/20 Mohr’s salt solution for titration. 12. Exp-11.12 : Determine the percentage composition of a mixture of sodium

oxalate and oxalic acid . Provided M/100 KMnO4 solution. 13. Exp-11.13 : You are provided with a partially oxidised sample of ferrous sulphate (FeSO4.7H20) crystals. Prepare a solution by dissolving 14.0 g of these crystals per litre and determine the percentage oxidation of the given sample. Given M/100 KMnO4 solution. 14. Exp-11.14 : Calculate the percentage of Fe2+ ions in a sample of ferrous sulphate. Prepare a solution of the given sample having strength exactly equal to 14.0 g/litre. Provided M/100 KMnO4 . 15. Exp-11.15 : Prepare N/20 Mohr’s salt solution. Using this solution, determine the normality and strength of the given potassium permanganate solution. CBSE Sample Papers

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16. Exp-11.16 : Prepare N/20 solution of oxalic acid. Using this solution, find out strength and normality of the given potassium permanganate solution . 17. Exp-11.17 : Determine the percentage purity of the given sample of oxalic acid. Ask for your requirement . 18. Exp-11.18 : Determine the percentage composition of a mixture of sodium

oxalate and oxalic acid . Provided N/20 KMnO4 . 19. Exp-11.19 : Determine the equivalent mass and number of molecules of water of crystallisation in a sample of Mohr’s salt FeSO4 (NH4)2 SO4.nH20. Provided N/20 KMnO4. 20. Volumetric Analysis Viva Questions with Answers. 12. Chemistry Qualitative Analysis 1. Exp-12.1 : To analyse the given salt for acidic and basic radicals . 2. Exp-12.2 : To analyse the given salt for acidic and basic radicals CO, Zn. 3. Qualitative Analysis Viva Questions with Answers.

NEET Chemistry Chapter wise Important Questions Some Basic Concepts of Chemistry

Chemical Kinetics

Atomic Structure

Concept of Chemical Kinetics

Classification and Periodicity of Elements

Order of Reaction

Chemical Bonding and Molecular Structure

Effect of Temperature on Rate of Reactions

States of Matter ( Gaseous and Liquid State)

Surface Chemistry

Unit Test 1(General Chemistry)

Concept of Surface Chemistry

Chemical Thermodynamics

Factors Affecting Adsorption of Gases on Solids

Thermodynamics

Promoters and Inhibitors

First Law of Thermodynamics

Preparation of Lyophobic Solution

Hess’s Law of Constant Heat Summation

Unit Test 5(Physical Chemistry II)

Second Law of Thermodynamics

General Principles and Processes of Isolation of Metals

Equilibrium

Earth Crust

Equilibrium State

Extraction of Crude Metal from Concentrated Ore

Le-Chatelier's Principle

Thermodynamics of Metallurgy

Acids and Bases

p-Block Elements

Salt Hydrolysis

Group-15 Elements: Nitrogen Family

Redox Reactions

Dinitrogen

Concepts of Oxidation and Reduction

Phosphorus

Oxidation Number

Group-16 Elements: Oxygen Family

Redox Reactions

Allotropic forms of Sulphur

Unit Test 2(Physical Chemistry I)

Group-17 Elements: Halogens

Hydrogen

Group-18 Elements: Noble Gases

Occurrence of Hydrogen

The d- and f- Block Elements

Compounds of Hydrogen

d-Block Elements

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Hard and Soft Water

General Properties of the Transition Elements

s-Block Elements

Some Important Compounds of Transition Elements

General Introduction of S-Block Elements

Coordination Compounds

Anomalous Properties of Lithium

Complex or Coordination Compounds

Biological Importance of Sodium and Potassium

Effective Atomic Number Rule

p-Block Elements (Inorganic Chemistry)

Bonding in Coordination Compounds

Concept of p-Block Elements

Crystal Field Theory (CFT)

Group 13 Elements: Boron Family

Unit Test 6(Inorganic Chemistry II)

Some Important Compounds of Group 13 Elements

Haloalkanes and Haloarenes

Group 14 Elements: Carbon Family

Alkyl and Aryl Halides

Unit Test 3(Inorganic Chemistry I)

Preparation of Aryl Halides

Some Basic Principles and Techniques

Stereochemical Aspects of Nucleophilic Substitution Reactions

Concept of Organic Chemistry

Polyhalogen Compounds

Representation of Different Formula

Alcohols, Phenols and Ethers

Isomerism

Alcohols and Phenols

Free Radicals

Chemical Properties of Alcohols

Types of Organic Reactions

Phenols

Chromatography

Ethers

Hydrocarbons

Aldehydes, Ketones and Carboxylic Acids

Concept of Hydrocarbons

Aldehydes and Ketones

Chemical Properties of Alkanes

Preparation of Aldehydes

Alkenes

Preparation of Ketones

Alkynes

Properties

Aromatic Hydrocarbons

Uses of Aldehydes and Ketones

Environmental Chemistry

Organic Compounds Containing Nitrogen

Environmental Pollution

Amines

Air Pollution

Properties of Amines

Tropospheric Pollution

Hofmann Mustard Oil Reaction

Water Pollution

Cyanides

Unit Test 4(Oreganic and Environmental Chemistry I)

Biomolecules

Solid State

Concept of Biomolecules

Concept of Solids

Structure of Fructose

Packing Efficiency

Proteins

Defects or Imperfections in Solids

Nucleic Acids

Magnetic Properties of Solids

Polymers

Solutions

Concept of Polymers

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Solutions in Chemistry

Polymerisation

Vapour Pressure

Vulcanisation of Rubber

Ideal Solutions

Polyesters

Electrochemistry

Chemistry in Everyday life

Concept of Electrochemistry

Chemicals in Medicines

Electrochemical Cell

Antimicrobials

Representation of a Cell

Soaps

Nernst Equation

Unit Test 7(Organic Chemistry II) Mock Test 1 Mock Test 2 Mock Test 3

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