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emistry = ’ D re ionisation ene Be Page No. 23, Q. No. 3 eany three aii of VS or Page No. 28. Q. No 36. in sp’ hybrdisation by taking BCI, as an ) vefer Page No. 28, Q. No, 42 the molecular orbital electronic tion of oxygen mol : late the bond order. we and fer Page No. 31, Q. No. 55. the following redox reaction b ation number method. , fer Page No. 61, Q. No, 20. 0, + Br-— Mn’ + Br, | What causes the temporary permanent hardness of water? fer Page No. 66, Q. No. 32. Give the composition of water gas. +H, fa) Explain how sodium carbonate (washing _ Soda) is prepared by Solvay process? _ Give the reaction involved in the process. fer Page No. 73, Q. No. 42. How do you prepare Diborane from BF ,? et Page No. 77, Q. No. 20. b) Boric acid behaves as a weak monobasic _ acid. Give reason. fer Page No. 75, Q. No. 4. $e (ili) Smatier size, EPR theory, and it is an empirical formula? An organic pund contain 4.07% of hydrogen, 6 of carbon and 71.65% of chlorine. at is its empirical formula? t. masses H=1,C =12,Cl= of this compound is re of a solvent, what is the lution obtained? fer Page No. 5, Q. No. 52. age No. 7, Q. No. 63. 35.5]. If two dissolved in 5 molarity of the 28. (a) Give any three model of an atom, : ’ Aas. Rotor Page No. 18, Q, No, 60, oo (b) Write the Rudberg squaton calculate va wave number hae “A po rogen spectrum, Wha chine ni for a spectral line appearing in visible region of hydrogen spectrum? Ans. Refer Page No, 18, Q. No, 59. 29, (a) Write the electronic configuration of copper (29) and give the value of n and / for the valence shell electron, Ans. Refer Page No. 18, Q. No. 58. (b) (i) State Pauli’s exclusion principle (ii) State (n + 1) rule. Ans. Refer Page No. 14 and 18, Q, No. 15 and 61, 30. (a) Enlist any three assumptions of Kinetic molecular theory of gases. Ans. Refer Page No. 37, Q. No. 46. (b) A balloon is filled with 2L of air at 300 temperature. What will be the volume o the balloon at 320K temperature? Ans. Refer Page No, 37, Q. No. 48. 31. Define standard enthalpy of formation. Calculate the standard enthalipy of formation of benzene from the following equations. (i) C(s)+0,(g)—+ CO, (g). AH? = —393.5KJmol"' (ii) H, (s) +50, (g)—— H,O(1) AH} = ~285.83KJ mol (iii) H, (1) +750, (g) +60, (g)+3H,0(1) AH” =—3267KJmol ' Ans. Refer Page No, 45 and 43, Q. No, 58. 32. (a) Define (i) Extensive property (ii) Adiabatic process (iii) Entropy. (i) Refer Page No. 42, Q. No, 33. (ii) Refer Page No. 40, Q. No. 1. (iii) Refer Page No. 43, Q. No. 45. (b) State | law of thermodynamics and write the mathematical representation of | law, Ans. Refer Page No. 42, Q. No. 26. Ans. PUE BOARD MODEL 1. State law of ‘Multiple proportions’. Ans. If two elements combine to form two or more Ans, - Write the relationship between K, and K.. Ans, . State ‘Modern Periodic law’. Ans. Ans, - Which is the basic structural unit of silicates? Ans. . What is dry ice? Ans, compound, the masses of one element that ean combine with a fixed mass of the other element, are in the small whole number ratio”. - What will be the volume of 10cm’ of oxygen gas at -273.5°C (absolute zero)? Z2eTO, K, =K, (RT), The properties of the elements are the periodic functions of their atomic numbers, . What is the oxidation state on Mnin KMnO,? Ans. - Write the chemical composition of ‘Plaster of Oxidation state of Mn in KMn0O, is +7. paris’. CaSO, . ; H,O (R,SiO)- Solid CO,,. Write the IUPAC name of CH, - CH, - CH, ~CH-COOH CH, Ans. 2-methyl- pentanoic acid. 10. Draw the Newman projection formula of Ans. eclipsed conformation of ethane, H Quest iON PAPER] “the s.[. unit of amount of su}... it is defined? Ans. Refer Page No. 1, Q: No. 2 Page No. 2 Q. No. 13. for compres; the expression mpressi i haere for one mole of a gas. What ji.) mpressibility factor Z for CO, ai sees at ordinary temperatur; Ans. Refer Page No. 36, Q. No. 37. 13, Dipole moment in BF, is zero. Give rv. Ans. Refer Page No. 20, Q. No. 23. 14. Complete the reaction, (i) CaCO, _~ (ii) Ca(OH), + CO, —++ Ans. Refer Page No. 71, Q. No. 29, 33. 15. Mention any two anamolous beh.\ carbon. Ans. Refer Page No. 83, Q. No. 44. 16. Explain “Wurtz reaction” with eva: Ans. Refer Page No. 70, Q. No. 23. 17, State Markovnikoffs e. following reaction. CH, -CH= CH, ane, Refer Page No, 96, Q. No. 38 and 40 18. How is ozone layer formed in the stratus Name a chief chemical that .. Ans, Refer Page No, 102, Q. No. 15. Compl: (CHC) « ques 5 Ans, Rafer Pag No.6, No.1. (b) What is the chemical used in to remove temporary h; Ans. Lime or Ca (OH), 25. (a) Mention biological muaguesiene sult aan Ans. Refer Page No. 72,Q. No. 38. (b) Name the protest. potassium reacts with o Ans. Potassium superoxide. 26. (a) Diamond is a bad conduct but graphite ra good c Ans. Due ozeeene Due to sp2 hybridisation electrons to conduct vs y. 0h) Whee fe thie waka aa nuclear te eo a Ans. Refer Page No. 65,Q.No.14. 27. (a) D ; he « mpi oxide of iron whieh masa: Fe = 55.8 Ans. Refer No. 8, Q. No | Ans. Refer Page No. 3,Q. No 3) i Aan 4, State Gaylussac’s Aue, Under similar conditions Of temperature and pressure av ever Bases Combine, they dogo in volumes which bear simple whole number ) l Fatlo with each other and : also with the gaseous products. 1, Between CO and CO,, which Ans. CO difuses faster 3. Give relationship between Ans, K) = K. (RT). 4. On what parameter do the elements are ‘¢lassified in the modern periodic table? Ans, Atomic number. 5. What is the oxidation number of sulphur in oe. ;? Aus. Oxidation number of *S’ in H,S.O, is +6. 6. Which element is diagonally related to lithium? Ais. Magnesium (Mz). 1 Give the general electronic configuration of _ peblock elements. Ans. [Nobel gas] ns* np’ ‘ ‘B. What is producer gas? Aus, Mixture of CO+ N. or Carbon monoxide and ar iy ae ’ hey Gaseous volumes, diffuses faster? K, and K , 9% Give an example for a heterocyclic compound. Ams, Furan, Pyrrole, Pyridine [ State Markovnikov’s rule. an unsymmetrical alkene reacts with i etrical molecule, negative part of = PP etMing molecule addsto:he double bonded ca on 4 / gen atoms Contain: # umber ofhydrogena ake ing least num na B 5*2 m8 scientific ’ in the tpress the following in tl Betation. 2 12. Explain (n +2) rule with an example. Ans. Refer Page No, 18, Q. No. 61, 13. Distinguish between a sigma and a Pi bond. Ans. Refer Page No, 27, Q. No. 30, 14. Give any two uses of plaster of paris. Ans. Refer Page No. 72, Q. No, 35, 15. Write reactions to justify amphoteric nature of aluminium, Refer Page No. 76, Q. No. 13. How do you convert Benzene to Benzene hexachloride (BHC)? Refer Page No. 98, Q. No. 58. Ans, 16. Ans. 17, Write any two differences between resonance effect and Electromeric effect. Ans. Refer Page No. 86, Q. No. 53. 18. Howis ozone layer formed in the stratosphere? Name a chief chemical that causes jits depletion. $. Refer Page No. 102, Q. No. 15. - 2 ve % , ‘ 19.(a) What happens when limited amount of CO, gas is passed inte lime water? Give equation. Refer Page No. 71, Q. No. 29 (b) Name the radioactive. Refer Page No. 69, O. No. 3. Explain main postulates of VSEPR theory. Refer Page No. 28, Q. No. 36 Ans. alkali metal which is Ans. 20. Ans. 21. (a) Write electronic configuration of = molecule, What is its magnetic property” Refer Page No 31,Q. No. 54 (b) Define bond angle. Refer Page No, 25,0. No 43 Ans, Ans, ) 0.0048 (ii) 4008 ‘ ns (i) 48% |0° (ij) 8.008 * 10 a SMemistry _ order of their ionic radiys: aN, Mg", Na’, QO» > O* > Na*s Me?** )) State modern IUPAC name number 104, Periodic Ia to the ele orbitals, (1+2 er Page No. 27, Q. No. 31. ) Draw the Shapes of formed by combina atomic orbitals. er Page No. 27, Q. No. 26. |. (a) What are sigma and pibonds? (2+ 1) Refer Page No. 27, Q. No. 29. _ (b) Why is a sigma bona Stronger than a pi bond? fer Page No, 26, Q. No. 13. a) Define dipole moment of a polar bond. Refer Page No. 26, Q. No. 23. __(b) Show that BeF, ‘ee dipole moment. efer Page No. 24, Q. No. 26. ance the redox reaction using oxidation mber method: +Br_, —>MnO,, +BrO,,, (inacidic) molecule has zero Page No. 61, Q. No. 21. i i duction of lain with equations the pro drogen by coal gasification and water gas t reaction. Refer Page No. 46, Q. No. 25 and 26. (a) ati enthalpies and ve re the hydration en . Re ton enthalpies of the alkali + and alkaline earth metals. (2+1) fer Page No. 71, Q. No 22 Give the chemical formula of paris. plaster of W and assign the ment with atomic 8S fi combination of atomic rete mean BMO and ABMO tion of Is and Is a 26. (a) Between boron and aluminiun cannot have covalency more thar Alcan have, Give reason, Ans. Refer Page No. 55, Q. No. 4. (b) Explain the reaction of diborane when it is exposed to air. Ans. Refer Page No, 77, Q. No. 22. | | 27. (a) Define (i) Limiting reagent (ii) Molarity. Ans. Refer Page No. 2, Q. No. 18 and 19, (b) CaCO, decomposes to give CO, gas according to the equation, CaCO,,, > CaO, + CO, , Calculate the mass of CaO, and CO produced on complete decomposition of 5p of CaCO, [Given molar mass of CaO = 56g and CO = 44g] Ans. Refer Page No. 5, Q. No. 46. 28. (a) The atomic number and atomic mass of iron are 26 and 56 respectively. Find the number of protons and neutrons in its atom. (2+3) Ans. Refer Page No. 11, Q. No. 19. (b) Calculate the wave number of the spectral line of shortest wavelength appearing in the Balmer series of H-spectrum (R= 1,09 x 107/m) Ans. Refer Page No. 16, Q. No. 38. 29. (a) For the element with atomic number 24 (i) Write the electronic configuration. (ii) Write the value of n and | for its electron in the valence shell. (iii) How many unpaired electrons are present in it. Ans. Refer Page No. 19, Q. No. 62. (b) State Pauli’s exclusion principle, Is it possible to have the configuration Is’? Ans. Refer Page No. 14, Q. No. 15. Is’ configuration is not possible. 30. (a) Write any three postulates of kinetic theory of gases. @+2) er Page No. 69, Q. No: / Ans. Refer Page No. 37, Q. No, 46 State “Law of definite — tion - The law states that “a given comp: ay | ae ie 5 ss contains exactly the ae oro rents | S oils 2 lecule of w, by weight.” e mass of on, - Mention the type of intermolecu that exists between non-polar - London forces or Dispersion on fore 7 - H is a Lewis base. Give reason, . Because it donates an electron pair. Nitrogen has higher ionization that of oxygen. Give reason. Nitrogen has half filled orbitals more stable than oxygen which partially filled orbitals (2p*) . What is the oxidation state of Mn » I . Which alkali metal is the st agent? Lithium or Li. . Give the composition of water g: , O04 H, (or) a mixture of carbon n hydrogen. Mention the type of hybridiza in diamond. : 3 - Sp . Mention one use of Chromoto; (i) Separation of components (or) : (ii) To test purity of a compo! Draw the staggered conformat H Staggered Conformation Alkanes C,H, Prepared by 1. Hydrogenation Ethene 2. Wurtz reaction CH,Br+2Na+ BrCH, —“= 5, Bremouaealte 3. Decarboxylation CH,COO’Na‘* + NaOH 4. Kolbe's electrolytic method mMopropane Conformane ce conformat: Chain or nuclear CH,CH,CH,CH, & CH Position CH,CH,CH,OHCB, Functional WA CH,CH,OH &CH,OCH, — Metamerism Inductive effect When a covalent bond the electron density is more towards more electronegative} Free CH, <1" <2? < 3° __(stability >lanar: sp* hybridised carbon | x ptical isomerisr | ry he plane polaris: ent direction attached to d system ised carbon ‘ lity orde' | A a Om aniline 4 chron atogmy mM. to graphy ) pfrom base!iic | ‘Om baseline ( or? INE €arth me, Ja, Sr, Ba ar id P Hydration Enthalpy _ (A,,,H of alkaline earth metal is greater than alkali metals due to yy form oxide - ey form hy ar ay |. System 8. Entropy (5) Measure of randomness of dinordemess AH of the system Thermodynamic terms Specified portion of the universe under study 3. Thermodynamic properties §. Equation for work don 6. Laws of thermodyna 7. Hess's Law of constant heat summation Net energy aviable to do useful work Heat change accompanying @ reaction ts AG = AH-TAS always same whether the reaction takes place in one step or in multisteps AS=— 1 QUICK CHAPTER ROUND UP Open system (can exchange both matter and energy) Ex: Hot cup of tea Closed system(can exchange energy but not matter) Ex: A Closed teapot Isolated system Ex: Thermos flask 2. Surroundings (Remaining portion of the universe excluding system ) Intensive (Does not depend on the quantity of matter present in the system) Ex: temperature, density, pressure etc. Extensive (depend on the quantity of matter present in the system) Ex: mass, volume, internal energy, enthalpy, heat capacity, etc. Isothermal process (temperature remains constant AT #0) | 4. Thermodynamic process mr 5% Adiabatic process (no exchange of heat between system and surroundings) Isothermal irreversible expansion of an ideal gas w = ~p,, AV (For free expansion, p,, * 0) Isothermal reversible expansion of an ideal gas w = -2.303nRT log ve Sign convention Work done on the system is +ve, Heat absorbed by the system is ve Work done by the system is -ve, , Heat given out by the system m -ve 1” Law (The energy of an isolated system is constant.) AU=q+w 2” Law (For a spontaneous process, The entropy of the universe is continuously increasing) AS. > 0 3” Law (The entropy of any pure crystalline substance & sero at absolute zero) 9, Gibbs Free Energy (G) AG® = 2. 303RTiogK 10. Criteria for spoatancity If AG < 0 process is spontancous If AG = 0 process is a1 equilibrawn if AG 0 PFOCess ba Moti piaieis hts Uned to predict geor Ip-Ip » Ip-bp bp-bp Sequence of enegy levels * For OIE i. > dls
