Therithal - Important questions with answers: 12 th Std Class Chemisty

Wednesday 30 March 2016

12 th Std Class Chemisty - Importance questions with Answer Key

12 th Std Class Chemisty - Importance questions with Answer Key

Inorganic Chemistry

UNIT 1 : Atomic Structure - II

Molecular Orbital Theory: Energy level diagram for molecular orbitals -- - Download - Key Answer
Electronic configuration of a molecule and its correlation with molecular behaviour -- - Download - Key Answer
Molecular orbital energy level diagrams -Hydrogen, Hypothetical, Nitrogen, Oxygen -- - Download - Key Answer
Hybridization : Salient Features, Type, Example -- - Download - Key Answer
Importance, Strength, Types of Hydrogen bonds - Intermolecular Forces -- - Download - Key Answer

UNIT 2 : Periodic Classification - II

UNIT 3 : p - Block Elements

General characteristics of p-block elements -- - Download - Key Answer
Electronic configuration of the Boron family elements -- - Download - Key Answer

UNIT 4 : d - Block Elements

UNIT 5 : f - Block Elements

General Characteristics of f-block elements and extraction -- - Download - Key Answer
General properties of Lanthanides -- - Download - Key Answer
General Properties of Actinide Series -- - Download - Key Answer
Comparison of Lanthanides and Actinides -- - Download - Key Answer
Uses of Lanthanides and actinides -- - Download - Key Answer
Simple salt and Molecular (or) addition compounds -- - Download - Key Answer

UNIT 6 : Coordination Compounds and Bio-Coordination Compounds

Terminology Used In Coordination Chemistry -- - Download - Key Answer
IUPAC Nomenclature Of Mononuclear Coordination Compounds -- - Download - Key Answer
Types of Isomerism: Structural and Stereo isomerism -- - Download - Key Answer
Theories Of Coordination Compounds: Werner's theory, Valence bond theory -- - Download - Key Answer
Uses of coordination compounds -- - Download - Key Answer
Bio Coordination Compounds ‘ aemoglobin, Chlorophyll -- - Download - Key Answer

UNIT 7 : Nuclear Chemistry

Nuclear Chemistry - Indroduction -- - Download - Key Answer
Difference between chemical reactions and nuclear reactions -- - Download - Key Answer
Type Of Nuclear Reaction -- - Download - Key Answer
Radiocarbon Dating and Uses -- - Download - Key Answer
Uses Of Radioactive Isotopes -- - Download - Key Answer

Physical Chemistry

UNIT 8 : Solid State - II

Types of Cubic System -- - Download - Key Answer
Bragg's Equation and spectrometer method -- - Download - Key Answer

Types Of Crystals -- - Download - Key Answer
Imperfections In Solids -- - Download - Key Answer
Super conductors property of Crystalline solids -- - Download - Key Answer
Glasses - Amorphous solids -- - Download - Key Answer

UNIT 9 : Thermodynamics - II

UNIT 10 : Chemical Equilibrium – II

Attainment Of Equilibrium In Chemical Reactions -- - Download - Key Answer

Le Chatelier's Principle: Haber's and Contact Process -- - Download - Key Answer

UNIT : 11 Chemical Kinetics II

Rate And Order Of A Reaction -- - Download - Key Answer
Rate equation for first order reactions -- - Download - Key Answer
Pseudo-First Order Reactions -- - Download - Key Answer
Determination of rate constant of acid catalysed hydrolysis of an ester -- - Download - Key Answer
Temperature Dependance Of Rate Constant -- - Download - Key Answer
Simple And Complex Reactions : Difference and Types -- - Download - Key Answer

UNIT : 12 Surface Chemistry

UNIT : 13 Electro Chemistry I

UNIT : 14 Electro Chemistry II

Electrochemistry ‘ Cells and Daniel cell -- - Download - Key Answer
Electro Chemistry - Cell Terminology -- - Download - Key Answer
Single Electrode Potential -- - Download - Key Answer

Organic Chemistry

UNIT : 15 Isomerism in Organic Chemistry

UNIT : 16 Hydroxy Derivatives

UNIT : 17 Ethers

UNIT : 18 Carbonyl Compounds

UNIT : 19 Carboxylic Acids

UNIT : 20 Organic Nitrogen Compounds

UNIT : 21 Biomolecules

UNIT : 22 Chemistry in Action

Inorganic Chemistry

UNIT 1 : Atomic Structure - II

B. Answer in one or two sentences

What do you understand by the dual character of matter?

State Heisenberg's uncertainty principle.

What is the significance of negative electronic energy?

Define an orbital.

What are molecular orbitals?

Why He2 is not formed?

What is bond order?

Define hybridisation.

Answer not exceeding 60 words

Discuss the Davisson and Germer experiment.

Derive de-Broglie's equation. What is its significance?

Discuss the shapes of s, p and d orbitals.

Briefly explain Molecular Orbital Theory.

Explain the formation of O2 molecule by molecular orbital theory.

UNIT 2 : Periodic Classification - II

Answer the following questions

1. Which element has the most positive value of electron affinity?

2. Which element has low electronegativity?

3. Mention the disadvantage of Pauling and Mulliken scale.

4. Why EA of fluorine is less than that of chlorine?

Answer not exceeding 60 words

1. How is atomic radii calculated from covalent bond length? 26. Explain Pauling method to determine ionic radii.

2. Explain the variation of IE along the group and period. 28. Explain the various factors that affect electron affinity.

3. How electronegativity values help to find out the nature of bonding between atoms?

UNIT 3 : p - Block Elements

Answer in one or two sentences

Write a note on plumbo solvency.

H3PO3 is diprotic. Why?

Draw the structure of a) PCl 5 b) H3PO3

Prove that P2O5 a powerful dehydrating agent.

Why H2O is a liquid while H2S is a gas?

Why the compounds of fluorine with oxygen are called fluorides of oxygen and not oxides of fluorine?

Fluorine atom is more electronegative than iodine atom yet, HF has lower acid strength than HI. Explain?

What are interhalogen compounds? How are they formed?

Discuss the oxidising power of fluorine.

How is XeF6 prepared?

Why do noble gases form compounds with fluorine and oxygen only?

Write the uses of Neon?

C. Answer not exceeding 60 words

1. What are silicones? How are they prepared? Mention its uses?

2. Give an account of manufacture of lead. Describe its important properties and uses.

3. 30. How are the following compounds prepared from phosphorus?

4. a) P2O3 b) P2O5 c) PCl3 d) PCl5 e) PH3

5. 31. How fluorine is isolated from their fluorides? Describe its important properties and uses.

6. 32. Give a detailed account of the interhalogen compounds with special reference to the compounds involving iodine. Draw their structures.

7. 33. Describe in detail how noble gases are isolated from air?

8. 34. Give an account of various types of compounds which are formed by xenon?

UNIT 4 : d - Block Elements

Answer in one or two sentences

What are "d"-block elements?

How d-block elements are classified?

Explain why d-block elements exhibit variable oxidation states?

Why transistion elements form complexes?

Why does Mn(II) show maximum paramagnetic character among the bivalent

ions of the first transistion series?

Why Zn2+ salts are white while Ni2+ salts are coloured?

[Ti (H2O)6]3+ is coloured while [Sc (H2O)6]3+ is colourless. Explain.

A substance is found to have a magnetic moment of 3.9 BM. How many unpaired electrons does it contain?

Explain why the melting and boiling points of Zn,Cd,Hg are low?

Explain why Mn2+ is more stable than Mn3+?

Write two alloys of copper and their uses.

Write short notes on alumino thermic process?

Name the first and last element in the second transition series.

Name the lightest and the heaviest elements (in terms of density) among the transition elements.

Which of the following ions would form colourless complexes?

Cu2+, Zn2+, Ti3+, Ti4+, Cd2+

What happens when KI solution is added to an aqueous solution of copper sulphate?

What is the action of heat on copper sulphate crystals?

Answer not exceeding 60 words

Explain briefly the extraction of copper from its chief ore.

Name the ores of gold. Explain how it is extracted from its alluvial gavel.

List the ores of silver. How silver is extracted from Argentite? 47. Briefly explain the extraction of zinc from zinc blende.

Explain how dichromate is extracted from its chromite are. Write the balanced chemical equation for the reaction between an acidified solution of K2Cr2O7 and KI.

UNIT 5 : f - Block Elements

Answer in one or two sentences

What are inner transition ( f-block) elements? Give two examples.

What is the difference in the electronic configuration of transition and inner- transition elements?

What are lanthanides? Give the various oxidation states of lanthanides.

What are mish metals? Give their uses.

Write the uses of Lanthanides and Actinides.

Answer not exceeding 60 words

What is lanthanide contraction? Discuss its causes and consequences. 21. Account for the following.

i) +3 oxidation state of lanthanides is the most stable.

ii) A few 4f elements show +2 or +4 oxidation states in addition to the

characteristic oxidation state of +3.

iii) Lanthanides are grouped together.

Comparing La(OH)3 and Lu(OH)3, which is more basic and explain why?

Discuss the position of lanthanides in the periodic table.

Describe the extraction of Lanthanides from monozite sand.

UNIT 6 : Coordination Compounds and Bio-Coordination Compounds

Answer in one or two sentences

What are simple salts? Give one example.

What are double salts? Give one example.

In what way complex salt differs from double salt?

What are ligands and coordination number?

Give one example for a monodentate ligand, a bidentate ligand and a chelating ligand.

Calculate the charge on the central metal ion present in the following complexes.

a) [Fe(NH3)4Cl2] NO3 b) Na[B(NO3)4]

Name the following complexes

a) [Co(NH3)5(H2O)]Cl3 b) Na[B(NO3)4]

Write the formula structure of the following

a) tris(ethylenediamine)cobalt(III) ion

b) pentaamminesulphatocobalt(III) chloride

Draw the structure of cis and trans-[Pt(NH3)2Cl2]

What are chelates? Give one example.

Answer not exceeding 60 words

Explain coordination and ionisation isomerism with suitable examples.

Mention the type of hybridisation and magnetic property of the following complexes using VB theory

a) [FeF6]4- b) [Fe(CN)6]4-

For the complexes K4[Fe(CN)6], [Cu(NH3)4] SO4 mention

a) Name b) Central metal ion c) Ligands d) Coordination number

How is the paramagnetic moment related to the number of unpaired electrons in?

a) K4[Fe(CN)6] b) K3[Fe(CN)6]

In what way [FeF6]4- differs from [Fe(CN)6]4-.

[Ni(CN)4]2- diamagnetic, whereas [NiCl4]2- is paramagnetic. Explain.

[Cu(NH3)4]2+ is square planar, where as [NiCl4]2- is tetrahedral. Explain.

Explain the limitations of VB theory.

Taking [FeF6]4- as an example, discuss geometry, nature of d-orbital splitting and magnetic property using VB theory.

Mention the function of haemoglobin in natural process.

Howchlorophyllisimportantinenvironmentalchemistry?Mentionitsfunction.

UNIT 7 : Nuclear Chemistry

Answer not exceeding 60 words

What is radioactivity? How was the phenomenon discovered?

What is nuclear fission? What are controlled and uncontrolled fission reactions? How can the energy released in such reactions be used for practical purposes?

What is nuclear fusion? How do nuclear fusion reactions differ from fission reactions?

Differentiate chemical reactions from nuclear reactions.

Explain the use of radioactive isotopes with specified examples.

Physical Chemistry

UNIT 8 : Solid State - II

Answer in one or two sentences

Define the terms; space lattice and unit cell. 18. State Bragg's law.

What are superconductors?

Sketch the (a) simple cubic (b) face-centred cubic and (c) body centred cubic lattices.

How crystals are classified?

Give example for molecular and ionic crystals.

What is a vitreous state?

Give two example for AB and AB2 type ionic crystals.

What is imperfection in solids?

What is coordination number?

Write a note on the assignment of atoms per unit cell in fcc. 28. Write a short note on metallic crystals.

How are glasses formed?

Answer not exceeding 60 words

What is Bragg's equation? Give its significance.

Write the properties of ionic crystals. Explain Schottky and Frenkel defects.

What is super conductivity? Give its uses.

Explain AB and AB2 type ionic crystals with one example for each.

How Bragg's equation is used for determining crystal structure.

Explain Bragg's spectrometer method. Explain the nature of glass.

UNIT 9 : Thermodynamics - II

Answer in one or two sentences

What is entropy? What are the units of entropy?

Predict the feasibility of a reaction when

i) bothDH andDS increase

ii) bothDH andDS decrease

iii)DH decreases butDS increases

What is Gibb's free energy?

Give Kelvin statement of second law of thermodynamics.

. HowDG is related toDH andDS? What is the meaning ofDG = 0? 15. Mention the essential condition for spontaneity in a chemical reaction.

Answer not exceeding 60 words

State the various statements of second law of thermodynamics.

What are spontaneous reactions? What are the conditions for the spontaneity of a process?

UNIT 10 : Chemical Equilibrium – II

Answer in one or two sentences

Dissociation of PCl5 decreases in presence of increase in Cl2 why?

Write the equilibrium constant for the following

i) H2O2(g) --- > H2O(g) + ½O2(g)

ii) CO(g) + H2O(g) --- > CO2(g) + H2(g)

iii) N2O4(g) --- > 2 NO2(g)

State Le Chatelier's principle.

What is equilibrium constant?

Why do equilibrium reactions referred to as dynamic equilibrium?

What happens whenDng = 0,Dng = -ve,Dng = +ve in a gaseous reaction.

CalculateDng, for the following reactions

i) H2(g) + I2(g) 2HI(g)

ii) 2H2O(g) + 2Cl2(g) 4HCl(g) + O(g)

Answer not exceeding 60 words

Derive the relation Kp = Kc (RT)Dng for a general chemical equilibrium reaction.

State Le Chatelier's principle. Discuss the effect of pressure, concentration and temperature on the following reaction

N2g) + O2(g) 2NO(g)

Derive the expressions for Kc and Kp for decomposition of PCl5.

UNIT : 11 Chemical Kinetics II

Answer in one or two sentences :

Define order of a reaction.

Derive the relationship between half-life period and rate constant for a first order reaction.

What is activation energy ?

What is meant by zero order reaction ? What is the rate constant of such a reaction ?

Write the Arrhenius equation and explain the terms.

Define half life period.

Give examples for first order reaction.

What are simple and complex reactions ?

Give examples for opposing reactions.

Answer not exceeding sixty words :

Explain the experimental determination of rate constant of acid hydrolysis of methyl acetate.

Write an account of the Arrhenius equation for rates of chemical reactions.

Write notes on (i) consecutive reactions, (ii) parallel reactions and (iii) opposing reactions.

State the characteristics of order of reaction.

Explain the experimental determination of rate constant for decomposition of H₂O₂ is aqueous solution.

UNIT : 12 Surface Chemistry

Answer in one or two sentences :

1. Define adsorption.

2. Define colloidal solution.

3. What is electrophoresis?

4. What is catalysis ?

5. What are the two types of catalysis?

6. What are active centers ?

7. Why colloidal system in gas in gas does not exist ?

8. Why colloids are purified ?

9. What are emulsions ?

What is Tyndall effect ?

Answer not exceeding sixty words :

Distinguish between physical adsorption and chemical adsorption.

Discuss the factors affecting adsorption.

Write notes on catalytic reactions

Write notes on

Positive catalyst

Negative catalyst

Auto catalyst

Induced catalyst

Write briefly about the theories of catalysis.

Write the applications of catalysis.

Write briefly about the preparation of colloids by dispersion methods.

Write briefly about the preparation of colloids by condensation methods.

Write notes on

Dialysis

Electrodialysis

Ultrafiltration

Write notes on

Brownian movement

Tyndall effect

Helmholtz double layer

What is electro osmosis ? Explain.

Write the applications of colloids.

UNIT : 13 Electro Chemistry I

Answer in one or two sentences :

Differentiate between electrolytic conductor and metallic conductor.

Define Faraday.

Define electrochemical equivalent.

What are insulators. Give examples.

State Ostwald’s dilution law.

What is common ion effect. Give examples.

What is a buffer action ?

What are indicators ?

Define specific and equivalent conductance. How are they related ?

What is Henderson equation ?

Answer not exceeding sixty words :

1. Write an account of the Arrhenius theory of electrolytic dissociation.

2. Explain Faraday’s laws of electrolysis.

3. Explain Ostwald’s dilution law.

4. Explain buffer action with example.

5. Derive Henderson equation.

6. write notes on (i) Ostwald’s theory of indicators, (ii) Quinonoid theory of indicators.

7. Define molar, equivalent and specific conductance and describe the effect of dilution.

8. State and explain Kohlrausch’s law.

9. State and explain Debye-Huckel-Onsager equation.

UNIT : 14 Electro Chemistry II

Answer in one or two sentences :

What are the types of changes in the cathode and anode in electrolytic and electrochemical cells.

11. What are two types of cells ?

12. What is single electrode potential ?

13. Define standard emf of a cell.

14. How to predict the feasibility of a cell reaction ?

15. Write the Nernst equation.

Answer not exceeding sixty words :

1. Write the differences between electrolytic and electrochemical cells.

2. How emf of a cell is determined ?

Organic Chemistry

UNIT : 15 Isomerism in Organic Chemistry

Short answer questions.

1. Explain the following with examples.

(a) cis-trans isomerism (b) optical isomerism.

2. Distinguish enantiomers and diasteromers ?

3. What is a racemic mixture ? Explain with suitable example.

4. Mesotartaric acid is an optically inactive compound with chiral carbon atoms. Justify.

5. Distinguish racemic form from Mesoform.

6. Describe the D, L-system of designation of configurations.

UNIT : 16 Hydroxy Derivatives

) Answer not exceeding sixty words :

What are alcohols ? How do they differ from inorganic hydroxides ?

Account for the following :

lower members of alcohols are soluble in water but higher members are not

Alcohols cannot be used as solvent for grignard reagent.

Give reason.

Methanol is miscible with water while iodo methane is not.

Give chemical test to distinguish between ethanol and methanol.

Compare the acid strength in 1^o, 2^o and 3^o alcohol giving reason.

Write the mechanism briefly when alcohols are treated with anhydrous zinc chloride and HCl.

Why is that tertiary alcohols show greater reactivity towards hydrogen halides than secondary and primary alcohols ?

How do primary, secondary and tertiary alcohols differ in terms of their oxidation ?

How will you convert C₂H₅OH to C₂H₅OC₂H₅ ?

Explain the mechanism of acid catalysed dehydration of ethanol at high temperature.

How do primary, secondary and tertiary alcohols differ in terms of their dehydrogenation ?

Give chemical tests to distinguish between propan-2-ol and 2-methyl-propan-2-ol.

Explain ‘esterification’ reaction with an example.

Why is glycol more viscous than ethanol ?

What happens when ethylene reacts with alkaline KMnO₄ solution ?

Explain oxidation reactions of ethylene glycol.

How is terylene prepared from glycol ?

Write the conversion of ethylene glycol to 1,4-dioxan ?

How is glycerol obtained commercially ? State its two uses.

How does glycerol react with (i) PCl₅ (ii) KHSO₄.

Give a brief account of the following reaction. (i) esterification, (ii) Riemer Tiemann reaction.

Explain Kolbe’s reaction.

Account for the following :

Phenol has a smaller dipole moment than methanol.

Phenols do not give protonation reaction readily.

Explain why phenol does not undergo substitution of the –OH group like alcohol.

Give chemical test to distinguish between methanol and phenol.

Give a brief account of coupling reaction.

What happens when phenol is treated with diazonium chloride in presence of NaOH ?

Explain Dow’s process.

What are monohydric alcohols ? How are they classified ? Give any three methods of preparing ethyl alcohol.

How will you distinguish the primary, secondary and tertiary alcohols by Victor Meyer’s method ?

Write equation for the following conversions.

Ethyl alcohol to ethylene

Ethyl alcohol to diethyl ether

Ethyl alcohol to ethyl amine

Explain the mechanism of esterification.

Give short notes on the following :

Kolbe’s reaction

Riemer Tiemann reaction

Coupling reaction

Explain the action of glycerol with

oxalic acid at 383 K

oxalic acid at 530 K

concentrated HNO₃ and H₂SO₄.

What are the oxidation products of glycerol ?

How is ethylene glycol prepared ? Give three methods.

Starting from phenol how would you obtain the following compounds ?

p-quinone, (b) picric acid and (c) Anisole.

How would you distinguish between

methyl alcohol and ethyl alcohol

benzyl alcohol and phenol

ethyl alcohol and benzyl alcohol

Give any four methods of preparing benzyl alcohol.

Write a note on the ‘Acidic nature of phenol’.

UNIT : 17 Ethers

Answer in one or two sentences :

1. Write the IUPAC names of

C₂H₅OCH₃ (b) C₆H₅OC₂H₅

2.Ethers should not be heated to dryness. Why ?

3. Ethers are the best solvents of Grignard reagents- Account for this statement.

Write a note on williamson synthesis.

1. Why are ethers not soluble in water ?

2. Mention the uses of diethyl ether.

3. What happens when anisole is treated with Lewis acid ?

4. What happens when anisole is nitrated ?

5. Write equation for the conversion of phenol to anisole

Answer not exceeding sixty words :

1. Write all possible isomers with the molecular formula C₄H₁₀O and name them.

2. Give any three methods of preparing diethyl ether.

3. Mention the methods of preparation of anisole.

4. How does diethyl ether react with the following reagents ?

(a) O₂ / long contact (b) HI in excess

5. Give any two chemical differences between anisole and an aliphatic ether.

6. Illustrate electrophilic substitution reactions of anisole.

7. Explain the formation of CH₃ I and phenol when anisole is heated with HI.

Diethyl ether forms peroxide easily while anisole does not form peroxide easily - Explain.

UNIT : 18 Carbonyl Compounds

Answer in one or two sentences :

1. Give the structural formulae of

(a) mesitylene (b) phorone and (c) mesityl oxide

2. What is Rosenmund’s reduction ? What is the purpose of adding BaSO ₄ in it ?

3. Name one reagent used to distinguish acetaldehyde and acetone.

Give four examples of carbonyl compounds ?

1. Does formaldehyde undergo aldol condensation ? Justify your answer.

2. What type of aldehydes undergo Cannizzaro reaction ?

3. What is urotropine ? Give its use.

4. What happens when calcium acetate is dry distilled ?

5. What is formalin - write its use.

6. Ethanal is more reactive towards nucleophilic addition reaction than propanone. Why ?

7. How is acetophenone prepared by Friedel-Crafts method ?

8. Write a note on haloform reaction.

9. How will you convert acetophenone to phenacyl bromide ?

10. Though benzophenone gives all reactions of carbonyl compounds, it does not form addition product with NaHSO₃ - give reasons.

11. Arrange the following in increasing order of reactivity towards nucleophilic addition. HCHO ; CH₃CHO and CH₃COCH₃

12. Predict the formulae of the products in the following reactions.

CH₃COCH₃ + HCN

C₆H₅COCH₃ + NH₂OH

13. Formaldehyde and benzaldehyde give Cannizzaro reaction but acetaldehyde does not - Account for this

14. Give two tests for aldehydes.

15. Mention the industrial uses of formaldehyde.

16. How will you distinguish between formaldehyde and acetaldehyde.

Answer not exceeding sixty words :

17. Write any three methods of preparing formaldehyde from alcohol.

18. How does formaldehyde react with (i) NH₃, (ii) CH₃MgI followed by hydrolysis and (iii) NaOH.

Illustrate the reducing property of acetaldehyde with examples.

1. How is acetone converted to

mesitylene (b) mesityl oxide, (iii) phorone and (iv) isopropyl alcohol.

2. Write giving chemical equations, a brief account of the following :

Rosenmund Reduction, (ii) Cannizzaro reaction

Clemmenson reduction, and (iv) Aldol condensation

3. Give nucleophilic addition reaction of acetaldehyde with (a) NaHSO₃, and (b) LiAlH₄.

4. Discuss aldol condensation.

5. How are the following conversions carried out ?

benzaldehyde from Toluene, (ii) acetophenone from benzene, and

benzoin from benzaldehyde.

6. Distinguish acetaldehyde from acetone.

7. Write a note on (i) Perkins reaction, and (ii) Knoevenagal reaction.

8. How will you distinguish between formaldehyde and acetaldehyde.

How will you synthesise acetaldehyde from formaldehyde ?

UNIT : 19 Carboxylic Acids

Answer in one or two sentences :

1. What are carboxylic acids ?

2. Give the source and trivial names of

C₃H₇COOH and (ii) HCOOH.

3. How is the conversion of acetonitrile to acetic acid effected ?

4. Boling point of carboxylic acids are higher than those of alcohols of same molecular mass - reason out.

5. Formic acid reduces Tollen's reagent, but acetic acid does not-Give reasons.

6. Write two tests of carboxylic acid.

7. Give the resonance structure of carboxylate anion.

8. Mention the inductive effect in monochloro acetic acid.

9. Write a note on esterification reaction with an example.

10. What happens when calcium salt of acetic acid is distilled.

11. Mention the uses of oxalic acid.

12. What is the action of dilute sulphuric acid with lactic acid ?

13. Give the structure of lactyl chloride and lactide.

Answer not exceeding sixty words :

1. How is oxalic acid manufactured from sodium formate ?

2. Explain the isomerism exhibited by carboxylic acids.

3. Write a note on the acidic nature of acetic acid.

4. Give the mechanism involved in the esterification of a carboxylic acid with alcohol.

5. Explain why carboxylic acids behave as acids. Discuss briefly the effect of electron withdrawing and donating substituents on acid strength of carboxylic acids.

6. Account for reducing nature of Formic acid.

7. Explain the following :

Choloro acetic acid is stronger acid than acetic acid.

Fluoro acetic acid is stronger acid than chloro acetic acid.

Formic acid is stronger acid than acetic acid.

8. How do you distinguish formic acid from acetic acid ?

1. What happens when lactic acid is

treated with dilute H₂SO₄

heated alone

oxidised with alkaline KMnO₄

2. Give the uses of (a) oxalic acid and (b) salicylic acid.

3. Outline the mechanism of (a) formation of ethylacetate from acetic acid and ethyl alcohol. (b) Hydrolysis of ethyl cyanide to propionic acid.

4. Explain the order of strength of the following acids.

CCl₃COOH > CHCl₂COOH > CH₂ClCOOH > CH₃COOH

p-nitrophenol > m-nitro phenol > phenol > cresol.

UNIT : 20 Organic Nitrogen Compounds

Answer in one or two sentences :

1. How are nitro alkanes prepared ?

2. Write about the functional isomerism of nitro methane ?

3. Give the reduction of nitromethane in (a) acid medium, (b) neutral medium.

4. Mention the uses of nitromethane.

5. How will you convert benzene to m-dinitro benzene ?

6. Explain the electrolytic reduction of nitro benzene ?

7. What are amines ? How are they classified ?

8. Give the structural formula of (i) 2-amino-2-methyl propane. (ii) 2-(N, N-dimethyl) amino butane

9. What happens when acetonitrile is hydrolysed ?

10. Write the name and structure of four isomeric amines having the molecular formula C₃H₉N.

11. How will you distinguish between ethylamine and diethylamine ?

12. Write a note on the basicity of amines ?

13. Explain why ethylamine is stronger than ammonia ?

14. What is Gabriel phthalimide synthesis ?

15. How is nitrobenzene converted to aniline ?

16. What happens when aniline is treated with bromine ?

17. What happens when aniline is treated with phosgene ?

18. How will you distinguish between aniline and ethylamine ?

19. Explain why aniline is less basic than methylamine ?

20. How is benzene diazonium chloride prepared ?

21. Write a note on Sandmeyer reaction.

How will you synthesise, benzylamine from aniline ?

What are the reagents that would convert the following into Ethyl amines ?

CH₃CONH₂ (b) CH₃CN (c) CH₃CH₂NO₂ (d) CH₃CH = NOH

2. Account for the following :

(CH₃)₂NH is a stronger base than NH₃

CH₃CH₂NH₂ is more basic than CH₃CONH₂

Aniline is less basic than Ethyl amine

On sulphonation of aniline, p-amino benzene sulphonic acid is formed.

3. What is the action of NaNO₂/HCl (aq) at ice cold temperature on

C₂H₅NH₂ (b) C₆H₅NH₂ (c) (CH₃)₂NH (d) (CH₃)₃N

4. What happens when ethylamine is treated with

CHCl₃/NaOH (b) CS₂ (c) COCl₂ (d) C₆H₅CHO

5. Justify :

Diazo coupling reaction is an example of aromatic electrophilic substitution reaction

Formation of acetanilide from aniline and acetic anhydride is a nucleophilic attack by aniline

Formation of methylamine by ammonolysis of methyl iodide is an example of S_N² reaction

Addition of bromine water to aniline, gives a white precipitate.

This is an example of aromatic electrophilic substitution.

6. What is the action of

Diethyl oxalate on Ethylamine

Diethyl oxalate on Diethyl amine

Nitrous acid on Diethyl amine

Nitrous acid on Triethyl amine

UNIT : 21 Biomolecules

Answer in one or two sentences :

1. What are carbohydrates ? Give two examples

2. Give the structure of sucrose.

3. What is starch ? What are the ultimate hydrolysis products ?

4. What is the action of con. HI on glucose ?

5. What is Saponification ?

Answer not exceeding sixty words :

6. Outline the classification of carbohydrates giving example for each.

7. How can a reducing sugar differ from non-reducing sugar.

8. Distinguish glucose from fructose.

9. Show the formation of a peptide bond with an equation.

10. Mention the biological importance of lipids.

11. Write about the preparation and properties of glucose.

12. How is the structure of fructose determined ?

Write short notes on the manufacture of Soap and Wax ?

UNIT : 22 Chemistry in Action

Answer in one or two sentences :

1. Define chemotherapy.

2. What are anaesthetics ? Give one example.

3. In what way antipyretics are important.

4. Why Iodoform and phenolic solutions are called antiseptic ?

5. Give two examples of antimalarials.

6. What are antibiotics ?

7. In what way antacids are important ?

8. What are antipasmodics ?

9. Give any two characteristics of Dye.

10. What are chromophores ? Give two examples.

11. What are artificial sweetening agents ? Give two examples.

12. What is Buna-S ?

Answer not exceeding sixty words :

13. Write briefly on antibiotics ? In what way antipasmodics are helpful ?

Explain briefly on characteristics of rocket propellants.

CHEMISTRY

HIGHER SECONDARY - SECOND YEAR

Syllabus : Higher Secondary - Second Year Chemistry Volume - I

INORGANIC CHEMISTRY

Unit 1 - Atomic Structure -II

Dual properties of electrons - de-Broglie relation - Heisenberg's uncertainty principle - Wave nature of an electron - Schrodinger wave equation (only equation, no derivation) - Eigen values and Eigen function- significance only - molecular orbital method. Application to Homo diatomic and Hetero diatomicmolecules-MetallicBond Hybridization of atomic orbitals Hybridization involving s, p and d Orbitals - Types of forces between molecules.

Unit 2 - Periodic classification-II

Review of periodic properties - Calculation of atomic radii - Calculation of ionic radii - Method of determination of Ionisation potential - Factors affecting ionisation potential - Method to determine the electron affinity - Factors affecting EA - Various scales on electro negativity values.

Unit 3 - p - Block Elements - II

Group -13 General trends - Potash alum- Preparation, Properties and uses - Group 14 General trends - Silicates - Types and structure - Silicones - Structure and uses - Extraction of lead - Group - 15. General trends - Phosphorous - Allotropes and extraction - Compounds of phosphorous - Group - 16. General trends - H2SO4 - Manufacture and properties. - Group - 17 General characteristics. Physical and Chemical properties - Isolation of fluorine and its properties - Interhalogen compounds Group-18 Inert gases - Isolation, properties and uses.

Unit 4 d - BLOCK ELEMENTS

General characteristics of d-block elements - First transition series - Occurrence and principles of extraction - chromium, copper and zinc - Alloys - Second transition series - Occurrence and principles of extraction of silver - Third transition series - Compounds - K2Cr2O7, CuSO45H2O, AgNO3, Hg2Cl2,

ZnCO3, Purple of cassius.

Unit 5 - f-block elements

General characteristics of f - block elements and extraction - Comparison of Lanthanides and Actinides - Uses of lanthanides and actinides.

Unit 6 - Coordination Compounds and Bio-coordination Compounds

An introduction - Terminology in coordination chemistry - IUPAC nomenclature of mononuclear coordination compounds - Isomerism in coordination compounds - Structural isomerism - Geometrical isomerism in 4 - coordinate, 6 - coordinate complexes - Theories on coordination compounds - Werner's theory (brief) - Valence Bond theory - Crystal field theory - Uses of coordination compounds - Biocoordination compounds. Haemoglobin and chlorophyll.

Unit 7 - Nuclear chemistry

Nuclear energy nuclear fission and fusion - Radio carbon dating - Nuclear reaction in sun - Uses of radioactive isotopes.

PHYSICAL CHEMISTRY

Unit 8 - Solid state II

Types of packing in crystals - X-Ray crystal structure - Types of ionic crystals - Imperfections in solids - Properties of crystalline solids - Amorphous solid.

Unit 9 - Thermodynamics - II

Review of I law - Need for the II law of thermodynamics - Spontaneous and non spontaneous processes - Entropy - Gibb's free energy - Free energy change and chemical equilibrium - Third law of thermodynamics.

Unit 10 - Chemical equilibrium II

Applications of law of mass action - Le Chatlier's principle.

Unit 11 - Chemical Kinetics -II

First order reaction and pseudo first order reaction - Experimental determination of first order reaction - method of determining order of reaction - temperature dependence of rate constant - Simple and complex reactions.

Unit 12 - Surface Chemistry

Adsorption - Catalysis - Theory of catalysis - Colloids - Preparation of colloids - Properties of colloids - Emulsions.

Unit 13 - Electrochemistry - I

Conductors, insulators and semi conductors - Theory of electrical conductance - Theory of strong electrolytes - Faraday's laws of electrolysis - Specific resistance, specific conductance, equivalent and molar conductance - Variation of conductance with dilution - Kohlraush's law - Ionic product of water, pH and pOH - Buffer solutions - Use of pH values.

Unit 14 - Electrochemistry - II

Cells - Electrodes and electrode potentials - Construction of cell and EMF - Corrosion and its preventions - commercial production of chemicals - Fuel cells.

Unit 15 - Isomerism in Organic Chemistry

Geometrical isomerism - Conformations of cyclic compounds - Optical isomerism - Optical activity - Chirality - Compounds containing chiral centres - D-L and R-S notation - Isomerism in benzene.

Unit 16 - Hydroxy Derivatives

Nomenclature of alcohols - Classification of alcohols - General methods of preparation of primary alcohols - Properties Methods of distinction between three classes of alcohols 1°, 2° and 3°) - Methods of preparation of dihydric alcohols. (glycol) - Properties - Uses - Methods of preparation of trihydric alcohols - Properties - Uses - Aromatic alcohols - Methods of preparation of benzyl alcohol - Properties - Uses - Phenols - Manufacture of phenols - Properties - Chemical properties - Uses of Phenols.

Unit 17 - Ethers

Ethers - General methods of preparation of aliphatic ethers - Properties - Uses - Aromatic ethers - Preparation of anisole - Reactions of anisole - Uses.

Unit - 18 Carbonyl Compounds

Nomenclature of carbonyl compounds - Comparison of aldehydes and ketones - General methods of preparation of aldehydes - Properties - Uses Aromatic aldehydes - Preparation of benzaldehyde - Properties - Uses - Ketones - general methods of preparation of aliphatic ketones (acetone) - Properties - Uses - Aromatic ketones - preparation of acetophenone- Properties - Uses - preparation of benzophenone - Properties.

Unit 19 - Carboxylic Acids

Nomenclature - Preparation of aliphatic monocarboxyli c acids - formic acid - Properties - Uses - Tests for carboxylic acid - Monohydroxy mono carboxylic acids - Lactic acid - Sources - Synthesis of lactic acid - Aliphatic dicarboxylic acids - preparation of dicarboxylic acids - oxalic and succinic acids - Properties - Strengths of carboxylic acids - Aromatic acids - Preparation of benzoic acid - Properties - Uses - Preparation of salicylic acid - Properties - Uses - Derivatives of carboxylic acids - Preparation of acid chloride - acetyl chloride (CH3COCl) - Preparation - Properties - Uses - Preparation of acetamide - Properties - Preparation of acetic anhydride - Properties - Preparation of esters- methyl acetate - Properties.

Unit - 20 Organic Nitrogen Compounds

Aliphatic nitro compounds - Preparation of aliphatic nitroalkanes - Properties - Uses - Aromatic nitro compounds - Preparation - Properties - Uses - Distinction between aliphatic and aromatic nitro compounds - Amines - Aliphatic amines - General methods of preparation - Properties - Distinction between 1°, 2°, and 3° amines - Aromatic amines - Synthesis of benzylamine - Properties - Aniline-preparation - Properties - Uses - Distinction between aliphatic and aromatic amines - Aliphatic nitriles - Preparation - properties - Uses - Diazonium salts - Preparation of benzene diazoniumchloride - Properties.

Unit 21 - Biomolecules

Carbohydrates - structural elucidation - Disaccharides and polysaccharides - Proteins - Amino acids - structure of proteins - Nucleic acids - Lipids.

Unit 22 - Chemistry in Action

Medicinal chemistry - Drug abuse - Dyes - classification and uses - Cosmetics - creams, perfumes, talcum powder and deodorants - chemicals in food - Preservatives artificial sweetening agents, antioxidants and edible colours - Insect repellant - pheromones and sex attractants - Rocket fuels - Types of polymers, preparation and uses.

CHEMISTRY PRACTICALS FOR STD XII

Detection of Nitrogen, Halogen and Sulphur in organic compounds.

Detection of Functional groups present in organic compounds.

a) Saturation and Unsaturation

b) Aromatic and aliphatic

c) Aldehydes, carboxylic acids, diamides, phenolic groups-(Nature

of any one functional group is identified)

Qualitative analysis

Determination of two cations and two anions in a given mixture.

Cations: Pb++, Cu++, Al3+, Fe3+, Zn2+, Mn2+, Ca++, Ba2+, Mg2+, NH4+

Anions: Borate, Sulphide, Sulphate, Carbonate, Nitrate, Chloride, Bromide.

(Insoluble and interfering ions are to be excluded. Also, two cations of

the same group and anions of the following)

Combinations such as (Cl- + Br-) and (CO32- + C2O42-) Should be

avoided.

Volumetric analysis

a) Permanganometry

1. Titration of Oxalic acid Vs KMnO4

2. Titration of ferrous ammonium sulphate against KMnO4 solution.

b) Dichrometry

1. Standardization of K2Cr2O7 solution.

2. Any one estimation using K2Cr2O7 as one of the oxidant.

Report should contain two acid radicals and two basic radicals, without

mentioning the name of the salt.

Confirmatory tests should be exhibited.

Inorganic Chemistry

UNIT 1 : Atomic Structure - II

UNIT 2 : Periodic Classification - II

UNIT 3 : p - Block Elements

UNIT 4 : d - Block Elements

UNIT 5 : f - Block Elements

UNIT 6 : Coordination Compounds and Bio-Coordination Compounds

UNIT 7 : Nuclear Chemistry

Physical Chemistry

UNIT 8 : Solid State - II

UNIT 9 : Thermodynamics - II

UNIT 10 : Chemical Equilibrium – II

UNIT : 11 Chemical Kinetics II

UNIT : 12 Surface Chemistry

UNIT : 13 Electro Chemistry I

UNIT : 14 Electro Chemistry II

Organic Chemistry

UNIT : 15 Isomerism in Organic Chemistry

UNIT : 16 Hydroxy Derivatives

UNIT : 17 Ethers

UNIT : 18 Carbonyl Compounds

UNIT : 19 Carboxylic Acids

UNIT : 20 Organic Nitrogen Compounds

UNIT : 21 Biomolecules

UNIT : 22 Chemistry in Action

List of Department

Wednesday 30 March 2016

12 th Std Class Chemisty - Importance questions with Answer Key

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