Therithal - Important questions with answers: 11 th Std Class Chemisty

Wednesday 30 March 2016

11 th Std Class Chemisty - Importance questions with Answer Key

11 th Std Class Chemisty - Importance questions with Answer Key

Inorganic Chemistry

UNIT 1. Chemical Calculations

UNIT 2. General Introduction to Metallurgy

Metallurgy - Ores and Minerals -- - Download - Key Answer
Sources from earth, living systems and in sea -- - Download - Key Answer
Metallurgy - Purification of ores -- - Download - Key Answer
Metallurgical processes -- - Download - Key Answer
Metallurgy - Purification of metals -- - Download - Key Answer

UNIT 3. Atomic Structure – I

UNIT 4. Periodic Classification – I

UNIT 5. Group 1 s-Block elements

UNIT 6. Group 2 s-Block elements

Group 2 s - Block Elements -- - Download - Key Answer
Magnesium: Important Ores, Metallurgy, Properties, Uses -- - Download - Key Answer
Compounds of alkaline earth metals -- - Download - Key Answer

UNIT 7. p-Block elements

Physical Chemistry

UNIT 8. Solid state – I

Crystalline solids and Amorphous solids -- - Download - Key Answer
Difference between Crystalline and Amorphous Solids -- - Download - Key Answer
Characteristic parameters and seven classes of unit cell -- - Download - Key Answer
Miller Indices -- - Download - Key Answer

UNIT 9. Gaseous state – I

UNIT 10. Chemical Bonding

UNIT 11. Colligative Properties

UNIT 12. Thermodynamics – I

UNIT 13. Chemical Equilibrium – I

UNIT 14. Chemical Kinetics – I

Organic Chemistry

UNIT 15. Basic Concepts of Organic Chemistry

Basic Concepts Of Organic Chemistry - Introduction -- - Download - Key Answer
Classification of Organic Compounds: open chain, cyclic compounds -- - Download - Key Answer

UNIT 16. Purification of Organic compounds

UNIT 17. Detection and Estimation of Elements

UNIT 18. Hydrocarbons

UNIT 19. Aromatic Hydrocarbons

UNIT 20. Organic Halogen Compounds

Inorganic Chemistry

UNIT 1. Chemical Calculations

1. Can two different compounds have same molecular formula ? Illustrate your answer with two examples.

2. What are the essentials of a chemical equation ?

3. What are the informations conveyed by a chemical equation ?

4. Balance the following equations

Fe + H₂O ® Fe₃O₄ + H₂

Fe₂ (SO₄)₃ + NH₃ + H₂O ® Fe(OH)₃ + (NH₄)₂ SO₄

KMnO₄ + H₂SO₄ ® K₂SO₄ + MnSO₄ + H₂O + O₂

K₂Cr₂O₇ + H₂SO₄ ® K₂SO₄ + Cr₂(SO₄)₃ + H₂O + O₂

UNIT 2. General Introduction to Metallurgy

. Write in one or two sentence

1. Distinguish between ore and mineral with suitable example ?

2. What are the elements obtained from sea water source?

3. What are the different methods of concentration of ores?

4. What is gravity separation ?

5. Name the ores which are concentrated by froth floatation process.

6. Define Metallurgy.

7. What are the major steps involved in the metallurgical process ?

8. What is calcination? Give example.

9. What is the principle involved in Bessemer process ?

10. What is meant by electrolytic refining? Give example.

11. What is anode mud?

12. What do you understand by the following terms (i) roasting (ii) smelting

C. Explain briefly on the following

13. Write short note on source of element in living system.

14. Explain froth flotation process with neat diagram.

15. How electrolytic separation process is useful in the separation of magnetic impurities from nonmagnetic ores? Draw the diagram.

16. How the impurities of ore are removed by chemical method?

17. What is roasting ? Explain different types of roasting with suitable example.

18. What is smelting ? Explain the process with example.

19. What is Zone refining ? Describe the principle involved in the purification of the metal by this method.

20. How nickel is extracted by Mond’s process? Write the various reactions involved in the process.

21. Write short note on mineral wealth of India.

Give a brief account of the mineral wealth of Tamil Nadu.

UNIT 3. Atomic Structure – I

Write in one or two sentence

1. What is the charge of an electron, proton and a neutron ?

2. What is atomic number?

3. What is the maximum number of electrons that an orbital can have?

4. How many orbitals are there in the second orbit? How are they designated?

5. Sketch the shape of s and p-orbital indicating the angular distribution of electrons.

6. What are the charge and mass of an electron?

7. What is an orbital?

8. Give the order of filling of electrons in the following orbitals 3p, 3d,4p, 3d and 6s.

9. What is meant by principal quantum number?

10. How many protons and neutrons are present in ¹⁸₈O?

11. What are the particles generally present in the nuclei of atoms?

12. The atomic mass of an element is 24 and its atomic number is 12. Show how the atom of the element is constituted?

13. How will you experimentally distinguish between a ray of neutron and ray of proton?

14. What is the principal defect of Bohr atom model?

15. Write the complete symbol for : (a) The nucleus with atomic number 56 and mass number 138 ; (b) The nucleus with atomic number 26 and mass number 55 ; (c) The nucleus with atomic number 4 and mass number 9.

16. An atomic orbital has n = 3. What are the possible values of l ?

17. An atomic orbital has l= 3. What are the possible values of m?

18. Give the electronic configuration of chromium. (Z=24).

19. Which energy level does not have p-orbital?

20. An atom of an element has 19 electrons. What is the total number of p-orbital?

21. How many electrons can have s+ ½ in a d-sub-shell?

22. Write the values of l and m for p-orbitals.

23. Which quantum accounts for the orientation of the electron orbital?

24. What is shape of the orbital with (i) n = 2 and l = 0 ; (ii) n = 2 and l = 1?

25. Give the values for all quantum numbers for 2p electrons in nitrogen (Z = 7).

26. Give the electronic configuration of Mn²⁺ and Cu. Atomic number of Cu = 29 and Mn = 25.

27. Explain why the electronic configuration of Cr andCu are written as 3d⁵, 4s¹ and 3d¹⁰ 4s¹ instead of 3d⁴ 4s² and 3d⁹ 4s²?

D. Explain briefly on the following

1. Describe Aufbau principle. Explain its significance in the electronic build up of atoms.

2. Using the s, p, d, notation, describe the orbital with the following quantum numbers? (a) n = 1, l=0; (b) n = 2,l = 0; (c) n = 3, l = 1;

3. (d) n = 4, l =3.

4. Using the a Aufbau principle, write the electronic configuration in the ground state of the following atoms : Boron (Z = 5 ) Neon (Z = 10) and Aluminium (Z = 13).

5. What is Rutherford’s a- ray scattering experiment? What are its conclusions?

6. What are the postulates of Bohr theory of atom?

7. Explain the various quantum numbers which completely specify the electron of an atom.

UNIT 4. Periodic Classification – I

Write in one or two sentence

1. Arrange F, Cl, Br and I in the order of increasing electronic gain enthalpy.

2. Write electronic configurations for the elements of atomic numbers 6 and 14 and from this find out of which group in the periodic table each elements belongs.

3. Which of the following electronic configurations has the lowest ionization enthalpy ? (a) 1s², 2s², 2p⁶ ; (b) 1s², 2s², sp⁶ ; (c) 1s², 2s², 2p⁶ , 3s².

4. State Modern Periodic Law.

5. Why Noble gases have zero electron gain enthalpy?

6. Which of the following pairs of elements would you expect to have lower first ionization enthalpy ? (a) Cl or F ; (b) Cl or S ; (c) K or Ar ; (d)Kr or Xe.

7. Why do elements in the same group have generally similar properties?

7. Name any two transition elements and any two inner transition elements.

8. Arrange the order of increasing atomic volumes in : (a) Li, Na and K; (b) C, N and O ; (c) Ca, Sr and Ba.

9. Name the different blocks of elements in periodic table. Give the general electronic configuration of each block.

10. To which block does the element with configuration 3d¹⁰4s² belongs

11. Why nitrogen has higher I.E. value than oxygen?

12. Out of fluorine and chlorine, which has greater electron gain enthalpy?

13. Why are d-block elements called transition elements?

14. What property did Mendeleev use to classify elements in his periodic table?

15. Among the elements Li, K, Ca, S and Kr which one has the lowest first ionization enthalpy? Which has the highest first ionization enthalpy?

D. Explain briefly the following

1. Why does the first ionization enthalpy would have higher electron gain enthalpy?

2. Which of the following pairs of elements would have higher electron gain enthalpy? (a) N or O ; (b) F or Cl . Explain.

3. Lanthanides and actinides are placed in separate rows at the bottom of the periodic table. Explain the reason for this arrangement ?

4. What do you mean by representative elements? Name the groups of the periodic table, which contain representative elements.

5. Define transition elements. Name the different transition series.

6. Which element of the following pairs have smaller ionization enthalpy? (a) Ca or Be ; (b) Ca or K ; (c) Cl or I. Justify your answer.

7. Why is Na atom bigger than the atoms of both lithium and magnesium ?

8. What do you mean by the term electron gain enthalpy? How does electron gain enthalpy change along a period and in a group?

9. Explain how the elements are arranged in the form of the periodic table.

10. What are normal, transition and inner- transition elements?

11. What are the differences between normal and transition elements?

12. Explain why radii of positive ions are always smaller than the radii of corresponding neutral atoms and why negative ions have larger radii than the corresponding neutral atom.

13. Explain the size of group Cl^- > Na⁺.

14. What is electron gain enthalpy? On what factors does it depend?

15. Give the general variation of electron gain enthalpies in the periodic table.

16. Define the term ionic radius. Justify that the radius of anion is larger than the parent atom.

17. What do you mean by ionization enthalpy? How does it vary across a period and down a group?

18. What is meant by electronegativity? On what factors does it depend?

19. What are the essential features of the periodic table of Mendeleev? Discuss how his table has been modified subsequently.

UNIT 5. Group 1 s-Block elements

Write in one or two sentences

1. What are isotopes? Mention the isotopes of hydrogen.

2. Write a short note on tritium.

3. How does deuterium react with nitrogen?

4. How does deuterium react with metals?

5. Mention the uses of deuterium.

6. How is tritium prepared?

7. How do you convert para hydrogen to ortho hydrogen?

8. How does heavy water react with metals?

9. How is hydrogen peroxide prepared in the laboratory?

10. How is hydrogen peroxide solution concentrated?

11. Write about the reducing property of hydrogen peroxide.

12. Mention two important uses of H₂O₂.

13. Why alkali metals have low melting and boiling points?

14. Why alkali metals have strong electropositive character?

D. Explain briefly on the following

1. How is deuterium obtained by diffusion process?

2. Write about the exchange reactions of deuterium.

3. What are ortho and para hydrogen? Explain.

4. Differentiate between ortho and para hydrogen.

5. Explain the preparation of heavy water.

6. Compare water and heavy water.

7. Explain the oxidizing property of hydrogen peroxide.

8. Explain how liquid hydrogen can be used as a fuel.

9. How is lithium extracted from its ore?

UNIT 6. Group 2 s-Block elements

Write in one or two sentence

1. Mention the reasons for the stabilisation of lower oxidation state of p-block element.

2. Show the electron accepting property of boron trifluoride by giving an example.

3. Give an example of monovalent and trivalent element in group III.

4. Why diamond is hard compared with graphite?

5. Why Boron family has a tendency to form hydrides?

6. Boron does not form B³⁺ ion. Why?

7. Why NH₃ has high boiling point than PH₃?

8. NH₃ is soluble in water whereas other hydrides of group 15 elements are insoluble in water. Why?

9. Which is considered to be "earth's protective umbrella"?

10. Mention any 3 uses of ozone.

11. What are CFC's? Mention its environmental action.

12. What are compound oxides? Give an example.

13. Mention the metal ions present in haemoglobin and myoglobin and state its function.

14. What happens when ozone reacts with

15. a) lead sulphide b) potassium manganate

Explain briefly on the following

1. Explain inert pair effect with suitable example.

2. Give an account of nature of hydrides of 15^th group elements.

3. How is boron extracted from borax?

4. What happens when boron reacts with

conc.H2SO4 b) conc.HNO3 c) SiO2

5. How is borax prepared from colemanite?

6. How borax bead test is helpful in identifying basic radicals in qualitative analysis?

7. Discuss the structural difference between diamond and graphite.

8. Write a short note on fixation of nitrogen.

9. How nitric acid is prepared by ostwald process.

10. Why silicon carbide is used as an abrasive?

11. How molecular oxygen is important for all oxygenated animals?

12. How ozone reacts with the following (a) PbS (b) KmnO4

13. How can you explain the anomalous behaviour of beryllium.

14. How does magnesium occur in nature? How is the metal extracted from its Ore?

15. In the light of metallic bonding account for the following properties of group 2 elements.

a. These are harder than alkali metals

b. These are good conductors of heat and electricity.

16. Why the first ionization energy of alkaline earth metals higher than that of Ist group.

17. Mention the uses of plaster of Paris.

18. How is plaster of paris prepared?

19. How is MgSO4 prepared?

20. Mention the uses of Magnesium?

UNIT 7. p-Block elements

Write in one or two sentence

1. Why the oxides of Group 2 metals have high melting points?

2. Why there is increase in the ionisation potential for forming M³⁺ ion for group 2 metals?

3. Why the ionization potential of M²⁺ is not very much greater than M⁺?

4. Why a precipitate of Mg(OH)2 is not formed when aqueous ammonia, NH₄OH is added to a solution of MgCl₂?

5. List the carbonates and hydroxide of alkaline earth metals in order of their increasing stability and their solution.

6. Why do beryllium halides fume in air?

7. Why group 2 elements are harder than alkali metals?

8. Beryllium halides are covalent whereas magnesium halides are ionic. Why?

9. Why are monoxides of alkaline earth metals are very stable?

10. The basic strength of the oxides of group 2 elements increases from Be to Ba. Why?

D. Explain briefly on the following

1. What are alkaline earth metals? Why are they called so?

2. In what respects Be and Mg differ from all the other metals of group 2.

Physical Chemistry

UNIT 8. Solid state – I

Write in one or two sentence :

1. What governs the packing of particles in crystals?

2. What is meant by ‘unit cell’ in crystallography?

3. How many types of cubic unit cell exits?

4. What are Miller Indices?

5. Mention the number of sodium and chloride ions in each unit cell of NaCl

6. Mention the number of cesium and chloride ions in each unit cell of CsCl

D. Explain briefly on the following :

1. Define and explain the following terms

a) Crystalline solids b) Amorphous solids c) Unit cell

2. Give the distinguishing features of crystalline solids and amorphous solids.

3. Explain the terms Isotropy and Anisotropy.

4. What is the difference between body centred cubic and face centred cubic?

5. Draw a neat diagram for sodium chloride structure and describe it accordingly.

6. Draw a neat diagram for Cesium chloride structure and describe it accordingly.

UNIT 9. Gaseous state – I

Write in one or two sentence

1. Write the mathematical expression for Boyle's law.

2. Compare the partial pressures of gases A and B when 3 moles of A and 5 moles of B mixed in constant volume, and 25^oC and 1 atm pressure.

3. Give the correction factors for the volume and pressure deviation for a Vanderwaal's gas.

4. A sample of an ideal gas escapes into an evacuated container, there is no change in the kinetic energy of the gas. Why?

5. What is the change in temperature when a compressed real gas is allowed to expand adiabatically through a porous plug.

6. Define Boyle's law and Charle's law.

7. What are measurable properties of gases?

8. What is the molar volume of nitrogen at 500K and 600 atm according to ideal gas law?

9. Define Graham's law of diffusion.

10. Give the values of R-gas constant in calories and Joules.

11. What are the units of Vanderwaals constants `a' and `b' ?

12. Write the significance of Vanderwaal's constants.

13. Write the limitations of vanderwaal equation of state.

14. Define Joule-Thomson effect.

15. What is meant by inversion temperature ?

E. Explain briefly on the following

31 At 27^oC, H₂ is leaked through a tiny hole into a vessel for 20 minutes. Another unknown gas at the same T and P as that of H₂ is leaked through the same hole for 20 minutes. After effusion of the gas, the mixture exerts a pressure of 6 atm. The H₂ content of the mixture is 0.7 moles. If volume of the container is 3 litres what is the molecular weight of unknown gas ?

32 Calculate the pressure exerted by 5 moles of CO₂ in one litre vessel at 47^oC using Vanderwaal's equation. Also report the pressure of gas if it behaves ideally in nature. Given that a=3.592 atm lit² mol^-2. b = 0.0427 lit mol^-1

UNIT 10. Chemical Bonding

Write in one or two sentence

1. Arrange NaCl, MgCl₂ and AlCl₃ in the increasing order of covalent character.

2. )LQG 1 DQG Œ ERQGV LQ WKH IROORZLQJ

3. CH₃-CH₃, CH₂=CH₂, CHºCH

4. Among Na⁺, Ca⁺², Mg⁺², Al⁺³ which has high polarising power ?

5. What is the structure of BeCl₂ ?

6. Write the differences between electrovalent and covalent bonds.

7. Give reason : CCl₄ is insoluble in H₂O while NaCl is soluble.

8. sp³ hybridisation is involved in CH₄, H₂O and NH₃. Why are the bond angles different in three cases?

9. Explain the co-ordinate bond formation between BF₃ & NH₃.

10. What is octet rule? Explain with an example.

11. What are the different types of bonds?

12. What is meant by electrovalent bond. Explain the bond formation in AlBr₃ and CaO.

13. Give the electron dot representation for PH₃ and ethane.

14. Write the Lewis dot structures for the following. S, S^2-, P, P^3-, Na, Na⁺, Al and Al³⁺.

15. What are the important features of valence bond theory?

16. What is meant by hybridisation?

17. Define resonance. Give the various resonance structures of CO2 and CO3^2- ion.

Explain briefly on the following

1. Discuss the important properties of electrovalent compounds.

2. Calculate the lattice energy of NaCl using Born-Haber cycle.

3. Explain the important properties of covalent compounds.

4. Discuss the partial covalent character in ionic compounds using Fajan's rule.

5. Explain the polarity of covalent bonds in H₂O and HCl.

6. Discuss the shapes of following molecules : NH₃, H₂O, CH₄, PCl₅ and SO₂.

7. Discuss VSEPR model applied for linear, trigonal planar, tetrahedral and octahedral geometries of molecules.

8. Explain the formation and difference between a sigma bond and a pi-bond. Which has more bond strength?

9. Calculate the lattice enthalpy of CaCl₂ given that the enthalpy of :

Sublimation of Ca in 121 kJ mol^-1

Dissociation of Cl₂ to 2Cl is 242.8 kJ mol^-1

Ionisation of Ca to Ca²⁺ is 2422 kJ mol^-1

Electron gain for Cl to Cl^- is -355 kJ mol^-1

û+_f^(o) overall is -795 kJ mol^-1

UNIT 11. Colligative Properties

Answer the following in one (or) two sentences

1. What are colligative properties?

2. Define relative lowering of vapour pressure.

3. What do you understand by molal elevation of boiling point? What are abnormal solutes?

4. Addition of non-volatile solute always increases the boiling point of the solution. Why?

5. Volatile hydrocarbons are not used in the brakes of automobile as lubricant, but non-volatile hydrocarbon are used as lubricants. Why?

6. Prove that the depression in freezing point is a colligative property.

7. Explain the terms osmosis and osmotic pressure.

8. What are isotonic solutions?

9. What are the advantages of Berkley-Hartley method?

10. Explain how the degree of dissociation of an electrolyte may be

11. determined from the measurement of a colligative property.

Explain briefly on the following

1. Explain the determination of relative lowering of vapour pressure by Ostwald- Walker method?

2. Describe about Beckmann thermometer.

3. Explain the determination of depression in freezing point by Beckmann method.

4. What is elevation of boiling point? Explain its determination by Cottrell's method.

5. Explain the laws of osmotic pressure?

6. Explain its determination by Berkley-Hartley method.

7. What are abnormal colligative properties?

8. Explain with example and write its determination using Van't Hoff factor.

UNIT 12. Thermodynamics – I

Write in one or two sentence:

1. Name the equipment using which heat of combustion of compounds are determined?

2. Energy can be created and be destroyed. State whether this is true or false.

3. Define zeroth law of thermodynamics.

4. Define an adiabatic process.

5. Write the differences between an exothermic and an endothermic process.

6. What are intensive and extensive properties?.

7. Define first law of thermodynamics.

8. Explain thermal and mechanical equilibrium processes.

Explain briefly on the following

1. Describe a bomb calorimeter and explain how heat of formation of an organic compound is determined.

2. Compare the enthalpy changes that occur between the neutralisation of a strong acid and a weak acid by sodium hydroxide. Explain the differences seen.

UNIT 13. Chemical Equilibrium – I

Write in one or two sentence

1. Define law of mass action

2. Write the Kp expression for PCl5(g) < -- >PCl3(g) + Cl2(g)

3. Relate Kp and Kc

4. Give an example of irreversible reaction

5. Reason out why equilibrium concentrations remain constant.

Explain briefly on the following

1. Differentiate irreversible and reversible reactions.

2. Explain the characteristics of a chemical equilibrium.

3. Write a note on heterogeneous equilibrium reaction.

Two moles of H₂ and three moles of I₂ are taken in 2 dm³ vessel and heated. If the equilibrium mixture contains 0.8 moles of HI, calculate Kp and Kc for the reaction HI.

UNIT 14. Chemical Kinetics – I

Write very short answers

1. Define half life period.

2. Name the factors that affect the rate of reaction.

3. What is molecularity?

4. What is a rate determining step?

5. List the factors on which an order of the reaction depend.

6. Write the rate law of pA + qB -- > lC + mD reaction.

7. Define the rate of a reaction.

Explain briefly on the following

1. Compare and contrast the terms, order and molecularity of a reaction.

2. Describe the factors on which the rate of a reaction depends.

3. What is a pseudo order reactions? How do you experimentally determine the pseudo first order rate constant of acid hydrolysis ester reaction?

4. Discuss the rate of the reaction

2N2O5(g) ® 4NO2(g) + O2(g)

Organic Chemistry

UNIT 15. Basic Concepts of Organic Chemistry

. Explain briefly on the following

1. Homolytic and heterolytic fission.

2. Substitution reaction.

3. Addition reaction.

4. Elimination reaction.

5. Polymerisation reaction.

6. Condensation reaction.

7. Hydrolysis.

8. Reduction and oxidation reactions.

9. Electrophilic and Nucleophilic reagents.

10. Carbonium ions and carbanions.

11. Free radicals.

12. Inductive effect.

13. Resonance effect.

UNIT 16. Purification of Organic compounds

Write in one or two sentence

What are the different stages followed during Crystallisation?

Define steam distillation.

What are different types of distillation?

Give the advantages of distillation under reduced pressure.

What are the types of paper chromatography?

Explain briefly on the following

1. Explain the method of purifying a solid organic compound.

2. Write short notes on

a) Fractional crystallisation b) Solvent extraction

3. Explain the purification of compounds by using thin layer chromatography.

4. What are the various principles used in chromatographic separation?

5. Write down the general characteristics of organic compounds.

UNIT 17. Detection and Estimation of Elements

Estimation of carbon and hydrogen

Estimation of nitrogen

Estimation of sulphur

Estimation of halogens

UNIT 18. Hydrocarbons

Explain briefly on the following

1. Mention any five chemical properties of alkanes.

2. Discuss the general methods of preparing alkanes.

3. What is hydroboration?

4. What is ozonolysis?

5. What is witting reaction?

6. What is polymerisation?

7. How is ethylene hydrated?

8. What is the action of ozone on acetylene.

What happens when acetylene is passed through red-hot tube?

UNIT 19. Aromatic Hydrocarbons

Explain briefly on the following

1. How is benzene is prepared commercially?

2. Explain the term aromaticity.

3. Write a note an activating groups in benzene.

4. How would you convert the following?

sodium benzoate to benzene

phenol to benzene

benzene to toluene

5. Write briefly on resonance in benzene.

UNIT 20. Organic Halogen Compounds

Write in one or two sentence

1. What are Lewis acids?

2. What is an electrophilic addition?

3. What is Hunsdiecker reaction?

4. What is Finkelstein reaction?

5. What is Swarts reaction?

Explain briefly on the following

1. Discuss S_N¹ mechanism

2. Discuss S_N² mechanism

3. Discuss E1 elimination

4. Discuss E2 elimination

5. What are the uses of alkyl halides?

6. What are the general reactions of aryl halides.

7. What are aralkyl halides ? How are they prepared?

8. What are Grignard reagents? Discuss its synthetic uses.

9. Discuss the general methods of preparation of alkyl halides.

CHEMISTRY

HIGHER SECONDARY - FIRST YEAR

Syllabus : Higher Secondary - First Year Chemistry

INORGANIC CHEMISTRY

Unit I - Chemical Calculations

Significant figures - SI units - Dimensions - Writing number in scientific notation - Conversion of scientific notation to decimal notation - Factor label method - Calculations using densities and specific gravities - Calculation of formula weight - Understanding Avogadro’s number - Mole concept-mole fraction of the solvent and solute - Conversion of grams into moles and moles into grams - Calculation of empirical formula from quantitative analysis and percentage composition - Calculation of molecular formula from empirical formula - Laws of chemical combination and Dalton’s atomic theory - Laws of multiple proportion and law of reciprocal proportion - Postulates of Dalton’s atomic theory and limitations - Stoichiometric equations - Balancing chemical equation in its molecular form - Oxidation reduction-Oxidation number - Balancing Redox equation using oxidation number - Calculations based on equations. - Mass/Mass relationship - Methods of expressing concentration of solution - Calculations on principle of volumetric analysis - Determination of equivalent mass of an element - Determination of equivalent mass by oxide, chloride and hydrogen displacement method - Calculation of equivalent mass of an element and compounds - Determination of molar mass of a volatile solute using Avogadro’s hypothesis.

Unit 2 - Environmental Chemistry

Environment - Pollution and pollutants - Types of pollution - Types of pollutants - Causes for pollution - Effects of pollution - General methods of prevention of environmental pollution.

Unit 3 - General Introduction to Metallurgy

Ores and minerals - Sources from earth, living system and in sea - Purification of ores-Oxide ores sulphide ores magnetic and non magnetic ores - Metallurgical process - Roasting-oxidation - Smelting-reduction - Bessemerisation - Purification of metals-electrolytic and vapour phase refining - Mineral wealth of India.

Unit 4 - Atomic Structure - I

Brief introduction of history of structure of atom - Defects of Rutherford’s model and Niels Bohr’s model of an atom - Sommerfeld’s extension of atomic structure - Electronic configuration and quantum numbers - Orbitals-shapes of s, p and d orbitals. - Quantum designation of electron - Pauli’s exclusion principle - Hund’s rule of maximum multiplicity - Aufbau principle - Stability of orbitals - Classification of elements based on electronic configuration.

Unit 5 - Periodic Classification - I

Brief history of periodic classification - IUPAC periodic table and IUPAC nomenclature of elements with atomic number greater than 100 - Electronic configuration and periodic table - Periodicity of properties Anomalous periodic properties of elements.

Unit 6 - Group-1s Block elements

Isotopes of hydrogen - Nature and application - Ortho and para hydrogen

1. Heavy water - Hydrogen peroxide - Liquid hydrogen as a fuel - Alkali metals

2. General characteristics - Chemical properties - Basic nature of oxides and hydroxides - Extraction of lithium and sodium - Properties and uses.

Unit 7 - Group - 2s - Block elements

General characteristics - Magnesium - Compounds of alkaline earth metals.

Unit 8 -p- Block elements

General characteristics of p-block elements - Group-13. Boron Group - Important ores of Boron - Isolation of Born-Properties - Compounds of Boron-Borax, Boranes, diboranes, Borazole-preparation. properties - Uses of Boron and its compounds - Carbon group - Group -14 - Allotropes of carbon - Structural difference of graphite and diamond - General physical and chemical properties of oxides, carbides, halides and sulphides of carbon group - Nitrogen

Group-15 - Fixation of nitrogen - natural and industrial - HNO₃-Ostwald process

Uses of nitrogen and its compounds - Oxygen - Group-16 - Importance of molecular oxygen-cell fuel - Difference between nascent oxygen and molecular oxygen - Oxides classification, acidic basic, amphoteric, neutral and peroxide - Ozone preparation, property and structure - Factors affecting ozone layer.

Physical Chemistry

Unit 9 - Solid State - I

Classification of solids-amorphous, crystalline - Unit cell - Miller indices - Types of lattices belong to cubic system.

Unit 10 - Gaseous State

Four important measurable properties of gases - Gas laws and ideal gas equation - Calculation of gas constant ‘‘R” - Dalton’s law of partial pressure - Graham’s law of diffusion - Causes for deviation of real gases from ideal behaviour - Vanderwaal’s equation of state - Critical phenomena - Joule-Thomson effect and inversion temperature - Liquefaction of gases - Methods of Liquefaction of gases.

Unit 11 - Chemical Bonding

Elementary theories on chemical bonding - Kossel-Lewis approach - Octet rule - Types of bonds - Ionic bond - Lattice energy and calculation of lattice energy using Born-Haber cycle - Properties of electrovalent compounds - Covalent bond - Lewis structure of Covalent bond - Properties of covalent compounds - Fajan’s rules - Polarity of Covalent bonds - VSEPR Model - Covalent bond through valence bond approach - Concept of resonance - Coordinate covalent bond.

Unit 12 - Colligative Properties

Concept of colligative properties and its scope - Lowering of vapour pressure - Raoul’s law - Ostwald - Walker method - Depression of freezing point of dilute solution - Beckmann method - Elevation of boiling point of dilute solution - Cotrell’s method - Osmotic pressure - Laws of Osmotic pressure - Berkley-Hartley’s method - Abnormal colligative properties Van’t Hoff factor and degree of dissociation.

Unit 13 - Thermodynamics - I

Thermodynamics - Scope - Terminology used in thermodynamics - Thermodynamic properties - nature - Zeroth law of thermodynamics - Internal energy - Enthalpy - Relation between ‘‘H and “E - Mathematical form of First law - Enthalpy of transition - Enthalpy of formation - Enthalpy of combustion – Enthalpy of neutralisation - Various sources of energy-Non-conventional energy resources.

Unit 14 - Chemical Equilibrium - I

Scope of chemical equilibrium - Reversible and irreversible reactions - Nature of chemical equilibrium - Equilibrium in physical process - Equilibrium in chemical process - Law of chemical equilibrium and equilibrium constant - Homogeneous equilibria - Heterogeneous equilibria.

Unit 15 - Chemical Kinetics - I

Scope - Rate of chemical reactions - Rate law and rate determining step - Calculation of reaction rate from the rate law - Order and molecularity of the reactions - Calculation of exponents of a rate law - Classification of rates based on order of the reactions.

ORGANIC CHEMISTRY

Unit 16 - Basic Concepts of Organic Chemistry

Catenation - Classification of organic compounds - Functional groups - Nomenclature - Isomerism - Types of organic reactions - Fission of bonds - Electrophiles and nucleophiles - Carbonium ion Carbanion - Free radicals - Electron displacement in covalent bond.

Unit 17 - Purification of Organic compounds

Characteristics of organic compounds - Crystallisation - Fractional Crystallisation - Sublimation - Distillation - Fractional distillation - Steam distillation - Chromotography.

Unit 18 - Detection and Estimation of Elements

Detection of carbon and hydrogen - Detection of Nitrogen - Detection of halogens - Detection of sulphur - Estimation of carbon and hydrogen - Estimation of Nitrogen - Estimation of sulphur - Estimation of halogens.

Unit 19 - Hydrocarbons

Classification of Hydrocarbons - IUPAC nomenclature - Sources of alkanes - General methods of preparation of alkanes - Physical properties - Chemical properties - Conformations of alkanes - Alkenes - IUPAC nomenclature of alkenes - General methods of preparation - Physical properties - Chemical properties - Uses - Alkynes - IUPAC Nomenclature of alkynes - General methods of preparation - Physical properties - Chemical properties - Uses.

Unit 20 - Aromatic Hydrocarbons

Aromatic Hydrocarbons - IUPAC nomenclature of aromatic hydrocarbons - Structure of Benzene - Orientation of substituents on the benzene ring - Commercial preparation of benzene - General methods of preparation of Benzene and its homologues - Physical properties - Chemical properties - Uses - Carcinogenic and toxic nature.

Unit 21 - Organic Halogen Compounds

Classification of organic hydrogen compounds - IUPAC nomenclature of alkyl halides - General methods of preparation - Properties - Nucleophilic substitution reactions - Elimination reactions - Uses - Aryl halide - General methods of preparation - Properties - Uses - Aralkyl halides - Comparison arylhalides and aralkyl halides - Grignard reagents - Preparation - Synthetic uses.

CHEMISTRY PRACTICALS FOR STD XI

Knowledge of using Burette, Pipette and use of logarithms is to be demonstrated.

Preparation of Compounds.

Copper Sulphate Crystals from amorphous copper sulphate solutions

Preparation of Mohr’s Salt

Preparation of Aspirin

Preparation of Iodoform

Preparation of tetrammine copper (II) sulphate

Identification of one cation and one anion from the following. (Insoluble salt should not be given)

Cation : Pb⁺⁺, Cu⁺⁺, Al⁺⁺, Mn²⁺, Zn⁺⁺, Ca⁺⁺, Ba⁺⁺, Mg⁺⁺, NH₄⁺.

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

IV. Determination of Melting point of a low melting solid.

Acidimetry Vs Alkalimetry

Preparation of Standard solution of Oxalic acid and Sodium Carbonate solution.

Titration of HCl Vs NaOH

Titration of HCl Vs Na₂CO₃

Titration of Oxalic acid Vs NaOH

Inorganic Chemistry

UNIT 1. Chemical Calculations

UNIT 2. General Introduction to Metallurgy

UNIT 3. Atomic Structure – I

UNIT 4. Periodic Classification – I

UNIT 5. Group 1 s-Block elements

UNIT 6. Group 2 s-Block elements

UNIT 7. p-Block elements

Physical Chemistry

UNIT 8. Solid state – I

UNIT 9. Gaseous state – I

UNIT 10. Chemical Bonding

UNIT 11. Colligative Properties

UNIT 12. Thermodynamics - I

UNIT 13. Chemical Equilibrium - I

UNIT 14. Chemical Kinetics – I

Organic Chemistry

UNIT 15. Basic Concepts of Organic Chemistry

UNIT 16. Purification of Organic compounds

UNIT 17. Detection and Estimation of Elements

UNIT 18. Hydrocarbons

UNIT 19. Aromatic Hydrocarbons

UNIT 20. Organic Halogen Compounds

List of Department

Wednesday 30 March 2016

11 th Std Class Chemisty - Importance questions with Answer Key

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