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XII CHEMISTRY, OUT OF FOCUS IMPORTANT QUESTIONS AND ANSWERS, , CHAPTER, , 1, , SOLID, , STATE, , PREPARED BY: YOOSAFALI T K , GHSS VARAVOOR , 9947444175, YOUTUBE CHANNEL: CHEM DSM, ==================================================================, 1. Write two examples for covalent solids., Ans: Diamond, Silica, 2. Classify the following in to ionic solids and molecular solids : Sodium chloride , ice , Solid NH 3 , Zinc chloride, Ans: Ionic solids :- Sodium chloride , Zinc chloride, Molecular solids :- ice , Solid NH3, 3. Solid A is very hard, insulator in solid as well as in molten state and melts at extremely high temperature . What, type of solid is it?, Ans : Covalent solids OR Network solids, 4. Which type of solids are electrical conductors , malleable and ductile ?, Ans : Metallic solids, 5. Which of the following forms a molecular solid on solidified ?, ( Silicon carbide , Calcium fluoride , Silica , Methane ), Ans : Methane, 6. Select the covalent solid or network solid which conduct electricity and soft (Diamond, Graphite, Quartz, SiC), Ans : Graphite, 7. Which are two types of three dimensional close packing?, (a) Hexagonal close packing(hcp):-ABAB.. type , Co-ordination number →12, (b) Cubic close packing(ccp):-ABCABC… type., Co-ordination number →12, 8. What is Co-ordination number ?, The number of nearest neighbouring particles (spheres) in a crystal close packing is called co-ordination, number., In hcp and ccp, co-ordination number is 12., 9. What is the co-ordination number of particles present in fcc crystal structure?, Ans: 12 [fcc = ccp, for ccp C.N = 12], 10. In magnesium crystal, the layers of atoms are being stacked in a pattern ABABAB…… type of arrangement. Name, the close packed structure., Ans: Hexagonal close packing (hcp)

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11. What are Interstitial voids?, The vacant spaces inside the crystal lattice are interstitial voids (voids)., The voids surrounded by the four spheres are called tetrahedral voids., The voids surrounded by the six spheres are called octahedral voids., 12. If the number of particle=N,, Octahedral void=N,, Tetrahedral void=2N,, Total void= N+2N=3N, 13. What is Packing efficiency ?, It is the percentage of total space filled by the particles., For simple cubic, packing efficiency is 52.4%, For body centred cubic, packing efficiency is 68 %, For face centred cubic, packing efficiency is 74 %, Most efficient is face centered cubic, 14. What is the co-ordination number of particles present in fcc crystal structure?, Ans: 12 [fcc = ccp, for ccp C.N = 12], 15. In magnesium crystal, the layers of atoms are being stacked in a pattern ABABAB…… type of arrangement. a), Name the close packed structure., Ans: Hexagonal close packing (hcp), 16. Write an equation for the calculation of density of a crystal from its structure?, 𝒛𝑴, ∴ 𝑫𝒆𝒏𝒔𝒊𝒕𝒚 𝒐𝒇 𝒖𝒏𝒊𝒕 𝒄𝒆𝒍𝒍 , 𝒅 =, 𝑵𝑨 𝒂𝟑, d= density , M =atomic mass , a = edge lenth , N A = Avogadro’s number ( 6.022 X 1023) ,, z = number of particles (For simple cubic, z=1 , For bcc ,z = 2 , For fcc , z = 4), , ============================================================================, , CHAPTER 2, , SOLUTIONS, , PREPARED BY : YOOSAFALI T K,GHSS VARAVOOR(8040) , THRISSUR(DT), , 9947444175, , YOUTUBE CHANNEL: CHEM DSM, , ====================================================================, 1. Number of moles of the solute per kilogram of the solvent is: Molarity, 2. Define mole fraction, Mole fraction is the ratio of number of moles of one component to the total number of moles of the solution., 𝑵𝒖𝒎𝒃𝒆𝒓 𝒐𝒇 𝒎𝒐𝒍𝒆𝒔 𝒐𝒇 𝒔𝒐𝒍𝒖𝒕𝒆, 𝒏, 𝑴𝒐𝒍𝒆 𝒇𝒓𝒂𝒄𝒕𝒊𝒐𝒏 𝒐𝒇 𝒔𝒐𝒍𝒖𝒕𝒆(𝑿𝑩 ) =, = 𝑩, 𝑻𝒐𝒕𝒂𝒍 𝒏𝒖𝒎𝒃𝒆𝒓 𝒐𝒇 𝒎𝒐𝒍𝒆𝒔 𝒐𝒇 𝒔𝒐𝒍𝒖𝒕𝒊𝒐𝒏, , 𝒏𝑨 𝒏𝑩, , 3. Number of moles of solute in one litre of the solution is : Molarity, 4. Molarity, 5. Molarity (M), molality (m) and mole fraction (x) are some methods for expressing concentration of solutions., a) Which of these are temperature independent?, Ans: Molality (m) and Mole fraction (x), b) Which is temperature dependent, Ans: Molarity (M)

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CHAPTER, , 3, , ELECTROCHEMISTRY, , PREPARED BY: YOOSAFALI T K , GHSS VARAVOOR(8040),THRISSUR (DT), , 9947444175, , YOUTUBE CHANNEL: CHEM DSM, , ============================================================================, 1. What is Electrochemical cell (galvanic cell) ?, A device that converts chemical energy to electrical energy is called electrochemical cell (galvanic cell)., e.g., Daniel cell., 2. With the help of diagram and equations explain Daniel cell (electrochemical cell), , Anode→ Zinc rod dipped in ZnSO4, Cathode→ Copper rod dipped in CuSO4, Anode and cathode are connected by wire and volt meter externally and by salt bridge internally., , At anode (oxidation), Zn→ Zn2+ + 2eAt cathode (reduction) Cu2+ + 2e-→ Cu, Overall reaction, Zn + Cu2+ → Zn2+ + Cu, Representation of Daniell cell is Zn | Zn2+ || Cu2+ | Cu, 3. What is electrode potential ?, The tendency of an electrode to lose or gain electron is called electrode potential., 4. What is Cell potential or EMF or Electro motive force of a cell?, It is the potential difference between the two electrodes in a galvanic cell., , EMF=Higher reduction potential − Lower reduction potential, = E cathode − E anode, = E right − E left, 5. Describe about standard Hydrogen Electrode (SHE) OR Normal hydrogen electrode (NHE)., It consists of a platinum wire sealed in to a glass tube carrying a platinum foil at one end., The electrode is placed in 1 molar acid solution., Pure hydrogen gas at 1 bar pressure is bubbled through the solution at 298 K.

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The electrode potential of SHE is taken as zero., It can act as both anode and cathode., If SHE acts as anode, ½ H2 → H+ + eIf SHE acts as cathode H+ + e-→ ½ H2, SHE is used to calculate the potential of an electrode., When SHE is used as cathode , it is represented as, H+/H2,Pt, When SHE is used as anode, it is represented as, Pt, H 2/ H+, 6. What is specific conductance or conductivity?, Specific conductance or conductivity of an electrolyte is the conductance of a column of solution of length 1, cm and area of cross section 1 cm2, , 𝛋 =, , 𝟏 𝟏 𝒍, =, 𝛒, 𝑹 𝑨, , 𝒐𝒉𝒎 𝟏 𝒄𝒎, , 𝑺𝒑𝒆𝒄𝒊𝒇𝒊𝒄 𝒄𝒐𝒏𝒅𝒖𝒄𝒕𝒂𝒏𝒄𝒆 , 𝛋 =, , 𝟏, , 𝑶𝒓, , 𝑺𝒄𝒎, , 𝟏, , 𝒄𝒆𝒍𝒍 𝒄𝒐𝒏𝒔𝒕𝒂𝒏𝒕, 𝑴𝒆𝒂𝒔𝒖𝒓𝒆𝒅 𝒓𝒆𝒔𝒊𝒔𝒕𝒂𝒏𝒄𝒆, , 7. What are the factors affecting conductivity of electrolytic solutions?, (I), Strong electrolytes ionize completely and conduct electricity to a large extent., (II), Conductivity of electrolytic solutions increases with temperature., 8. What is molar conductivity and give the relation connecting specific conductance (κ) and molar conductance, (Ʌm) ?, Molar conductivity is the conductance of the solution containing one mole of the electrolyte kept between, two electrodes at a distance of unit length., , 𝐌𝐨𝐥𝐚𝐫 𝐜𝐨𝐧𝐝𝐮𝐜𝐭𝐢𝐯𝐢𝐭𝐲, Ʌ𝐦 =, , 𝐊, 𝑲 𝑿 𝟏𝟎𝟎𝟎, =, 𝐂, 𝑴𝒐𝒍𝒂𝒓𝒊𝒕𝒚, , 9. State Faraday’s laws of electrolysis., (I), Faraday’s first law :The mass of substance liberated (or deposited) at the electrode is directly proportional to the quantity of, electricity passed through the electrolyte solution., , i.e. , w α Q, (II), , But Q= It, , w= mass of the substance formed I = current, t = time, Z= electrochemical equivalent, Faraday’s second law :When the same quantity of electricity is passed through different electrolytes , the masses of substances, formed at the electrodes are proportional to their respective chemical equivalent masses., When the same quantity of electricity is passed through CuSO4 and AgNO3 soluions connected in series,, , 𝑴𝒂𝒔𝒔 𝒐𝒇 𝒄𝒐𝒑𝒑𝒆𝒓, 𝟑𝟏. 𝟕, =, 𝑴𝒂𝒔𝒔 𝒐𝒇 𝒔𝒊𝒍𝒗𝒆𝒓, 𝟏𝟎𝟖, 31.7 = equivalent mass of Cu , 108 = equivalent mass of Ag., 10. What is Faraday?, Charge of one mole electron is called Faraday. 1 F = 96500 C, For the reduction of 1 mol Na+ , 1 F ( 96500 C ) electricity is required., For the reduction of 1 mol Cu2+ , 2F ( 2 X 96500 C ) electricity is required., For the reduction of 1 mol Al3+ , 3F ( 3 X 96500 C ) electricity is required.

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11. What are the products obtained when aqueous NaCl and molten NaCl is electrolysed., When aqueous solution of NaCl is electrolysed, hydrogen gas is liberated at cathode , chlorine gas is liberated at, anode and sodium hydroxide is deposited in the cell., , 2 NaCl + 2 H2O → 2 NaOH + H2 + Cl2, When molten NaCl is electrolysed, sodium is deposited at the cathode and chlorine gas is liberated at anode ., , 2 NaCl → 2 Na + Cl2, 12. What are primary batteries? Give examples, Ans: These are batteries which cannot be recharged or reused., Examples: Dry cell, Mercury cell, 13. What are the anode, cathode and electrolyte of Dry cell?, Anode→ Zinc container, Cathode→ graphite rod surrounded by MnO2 and carbon powder, Electrolyte→ paste of ammonium chloride and zinc chloride, 14. In mercury cell, cell potential 1.35 remain constant during its life .Why?, Because the overall reaction does not involve any ion in solution ., 15. Explain electro chemical theory of corrosion (Rusting of iron)., , Rust is Fe2O3 .x H2O ( Hydrated ferric oxide ), In rusting of iron,, Anode→ pure iron, Cathode→ impure iron, Electrolyte→ CO2 dissolved in H2O forms carbonic acid (H2CO3) .It gives H+ ion, , At anode 2 (Fe → Fe2+ + 2 e− ), At cathode O2 + 4 H+ +4 e−→ 2 H2O, Adding these equations, 2 Fe + O2 + 4 H+ → 2 Fe2+ + 2 H2O, The ferrous ions are further oxidized by atmospheric oxygen to form rust, Fe2O3 .x H2O, 16. What are the methods used to prevent corrosion., (I), Covering the surface with paint or by some chemicals (e.g. bisphenol), (II), Provide a sacrificial electrode of another metal (like Mg, Zn etc.), , ===========================================================================, CHAPTER 4, , CHEMICAL KINETICS, , ================================================================ ==, 1. What is zero order reaction and give example, A reaction is said to be zero order if the rate is independent of the concentration of the reactants., Examples for zero order reaction: Decomposition of ammonia on platinum surface at high pressure, Rate = k[NH3]0

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2. Give the integrated rate equation of zero order reaction., , ∴ 𝐓𝐡𝐞 𝐢𝐧𝐭𝐞𝐠𝐫𝐚𝐭𝐞𝐝 𝐫𝐚𝐭𝐞 𝐞𝐪𝐮𝐚𝐭𝐢𝐨𝐧, 𝐤 =, 3., , [𝐑 𝟎 ] − [𝐑], 𝐭, , [R0] = initial concentration of reactant, [R] = concentration of reactant at time t., Draw graph of zero order reaction, Straight line plot between [R] vs time, , 4. Half life period of a zero order reaction is directly proportional to the initial concentration of the reactant. Give, its equation, Half life period for zero order reaction is 𝐭 𝟏/𝟐, , =, , [𝑹𝟎 ], 𝟐𝒌, , 5. What are Pseudo first order reactions and give examples?, Reactions which appear to be of higher order but actually follow first order kinetics are called pseudo first, order reactions., Examples:, (I), The hydrolysis of ethyl acetate in the presence of dilute acids, (II), Inversion of cane sugar in the presence of dilute acid., 6. With the help of graph, explain the effect of catalyst on rate of a reaction., , A catalyst provides an alternate path for the reaction with lower activation energy. Hence the rate of the reaction, increases., , ==========================================================================, ==============================================================, ==========================================================================

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CHAPTER, , 5, , SURFACE CHEMISTRY, , PREPARED BY: YOOSAFALI T K , GHSS VARAVOOR , 9947444175, YOUTUBE CHANNEL: CHEM DSM, ===============================================================, 1. What are the difference between adsorption and absorption?, , 2., , Adsorption, , Absorption, , Higher concentration of the substance on the surface, Surface phenomena, The rate is high at the beginning and then decreases., Examples: (i) Water on silica gel, (ii)Chalk in contact with litmus solution, , Substances are uniformly distributed in the bulk, Bulk phenomena, Rate is same throughout the process, Examples: (i)Water on calcium chloride, (ii)Sponge in contact with water, , Explain the Mechanism of adsorption., During adsorption energy is released due to the decrease of residual force of attraction. So adsorption is, exothermic ( ∆H = -ve)., During adsorption molecules are adsorbed on the surface and so entropy decreases ( ∆ S = −ve)., For a spontaneous process, ∆G must be negative (∆G = −ve)., So, , ∆H = −ve , ∆ S = −ve, ∆G = −ve, , 3. Give some Applications of adsorption., (i), Decolourisation sugar solution using coconut charcoal., (ii), Heterogeneous catalysis., (iii), Adsorption chromatography., 4. Explain the adsorption theory of heterogeneous catalysis, (I), Diffusion of reactant molecules to the surface of the catalyst., (II), Adsorption of reactant molecules at the active site on the surface of the catalyst., (III), Occurrence of chemical reaction on the surface of the catalyst through the formation of an, intermediate., (IV), Desorption of the products from the surface of the catalyst, (V), Diffusion of the products away from the surface of the catalyst, 5. What are activity and selectivity of a catalyst?, , Activity of a catalyst :- The ability of a catalyst to accelerate a chemical reaction is called activity., Selectivity of a catalyst:-The ability of a catalyst to direct a chemical reaction to form a particular, product is called selectivity., , CO + 3 H2, CO + 3 H2, , 𝑵𝒊, , → CH4 + H2O, 𝑪𝒖,𝒁𝒏𝑶,𝑪𝒓𝟐 𝑶𝟑, , ⎯⎯⎯⎯⎯⎯⎯⎯⎯, , ,, CH3OH, , 6. What are Shape selective catalysis?, The catalytic reaction that depends upon the pore structure of the catalyst and the size of the reactant and, product molecule is called shape selective catalysis. Such catalysts are called shape selective catalysts., Example: Zeolites.

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7. What are characteristics of enzyme catalysis?, Enzymes are biological catalyst that can accelerate many bio chemical reactions in living organisms., (i), Enzymes are highly efficient., (ii), Enzymes are highly specific. i.e., Each enzyme can catalyse only one biochemical reaction. It cannot, catalyse other bio chemical reactions., 8. Explain the mechanism of enzyme catalysis (Lock and key model)., , E + S →ES* (Activated complex), ES* → E + P, 9. What are Colloids ?, A colloid is a heterogeneous system in which the diameter of the particles of dispersed phase is between 1nm, and 1000nm. Eg. Starch water, Starch→ dispersed phase,, Water → dispersion medium, The substance dispersed (small amount) is called dispersed phase., The medium in which dispersion takes place (large amount) is called dispersion medium, 10. Name the colloid in which dispersed phase is liquid and dispersion medium is solid. (i) Sol (ii) Foam (iii) Emulsion, (iv) Gel, Ans: Gel, 11. Explain any chemical methods for the preparation of lyophobic colloids with suitable examples. [SAY 2018], (I), Oxidation : Sulphur sol is prepared by oxidation of solution of hydrogen sulphide with sulphur dioxide., SO2 + 2H2S → 3S(sol) + 2H2O, (II), Hydrolysis: Ferric hydroxide sol is prepared by adding ferric chloride to boiling water., FeCl3 + 3H2O → Fe(OH)3 + 3 HCl, 12. Bredig’s arc method (Electrical disintegration method) is used for the preparation of colloid. Explain, Metal sols like gold sol, silver sol, platinum sol can be prepared by this method., In this method both dispersion and condensation takes place., It is prepared by striking an electric arc between the electrodes of the metal immersed in the dispersion, medium., The intense heat produced vapourises the metal which then condenses to form particles of colloidal size., 13. Peptisation is a method of preparation of sols. Write a general procedure for peptisation., Conversion of precipitate in to colloid by adding suitable electrolytes is called peptization., Example: Ferric hydroxide sol is prepared by adding ferric chloride to ferric hydroxide precipitate., 14. Which are purification methods of colloids?, Dialysis , Electrodialysis , Ultrafiltration, 15. Explain the different Properties of colloids (i) Brownian movement (ii) Coagulation, (I), , Brownian movement :-The random and continuous movement of colloidal particles in a dispersion, medium is called Brownian movement., It is due to the unbalanced collision of the colloidal particles by the molecules of the dispersion medium., , (II), , Coagulation :- The process of settling of colloidal particles is called coagulation( precipitation)., Deltas are formed near river mouth due to coagulation., Coagulation is done by the following ways (i) By electrophoresis (ii) by mixing two opposite charged sols, (iii) by boiling (iv) By persistent dialysis (v) by the addition of electrolytes

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16. What is Helmhotz electrical double layer ?, In the preferential adsorption of ions from solutions, sol particles adsorb positive ion or negative ion from, solution ad a stationary layer is formed. This charged particle attract counter ion from solution and opposite, charged mobile layer is formed. The combination of two opposite charged layers around the sol particle is, called Helmhotz electrical double layer., 17. What is Zeta potential or electro kinetic potential ?, The potential difference between the stationary layer and diffused mobile layer around the sol particles in a, colloid is known as zeta potential, 18. State Hardy-Schulze rule with the help of example., Opposite charged electrolyte is required for coagulation., The higher the valency of the ion, greater the coagulation power, Example : For positive charged sol, the efficiency of anions follow the order PO43- > SO42- > ClFor negative charged sol, the efficiency of cations follow the order, , Al 3+ > Mg2+ > Na+, , 19. The ion that is more effective for the coagulation of negatively charged As 2S3 sol. (a) Al3+ (b) PO4 3- (c) SO4 2- (d), Na+, Ans: (a) Al3+, 20. What is Protective colloid ?, The unstable lyophobic colloids can be made stable by adding small amount of lyophilic sol., The lyophilic colloid used for this purpose is called protective colloid., Example. Starch sol can protect gold sol., 21. Why lyophilic colloids are used as protective colloids?, Ans: Lyophilic colloids are stable, 22. Give some applications of colloids., (i), Electrical precipitation of smoke by Cottrell precipitator., (ii), Rubber latex (negative charge) is coagulated by adding formic acid., 23. Identify the target electrode of Fe(OH)3 sol, As2S3 sol and starch during the electrophoresis experiment., Fe(OH)3 →Positive sol → Negative electrode (Cathode), As2S3 sol and starch → Negative sols → Positive electrode (Anode), 24. Identify the ions used for the coagulation of As2S3 sol. K+,Cl-,SO42- , Mg2+ . Name the law behind this, For As2S3 sol (Negative sol ) , Positive ions are required for coagulaton., Hardy –Shulze rule, , ============================================================================, PREPARED BY: YOOSAFALI T K , GHSS VARAVOOR (8040), THRISSR (DT), YOUTUBE CHANNEL : CHEM DSM, , =======================================================

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6 GENERAL PRINCIPLES AND PROCESSES OF ISOLATION OF, ELEMENTS, PREPARED BY: YOOSAFALI T K , GHSS VARAVOOR (8040), THRISSR (DT), , =======================================================, 1. Chief ores of some metals, , Metals, , Ores, , Iron, Haematite(Fe2O3 ), Magnetite (Fe3O4), Copper, Copper pyrites(CuFeS2 ), Malachite (CuCO3. Cu(OH)2 ), Aluminium, Bauxite(Al2O3 .x H2O ), Zinc, Zinc blende(ZnS) , Calamine(ZnCO3 ), 2. What is Metallurgy?, The extraction of metals from the ore is called metallurgy., 3. Give a brief note on Ellingham diagram., Ellingham diagram is the graphical representation of standard Gibbs energy change and Temperature of oxide, formation., For the reduction of metal oxides, it is coupled with another oxide formation reaction., If the Gibbs energy value is more negative, the reduction with that metal or nonmetal is possible., Ellingham diagram is used to select better reducing agent., Any metal can reduce the oxides of other metals which lie above in the Ellingham diagram., 4. Explain the following refining processes : (a) Distillation (b) Liquation (c) Zone refining, (I), (II), (III), , Distillation :- For the purification of zinc and mercury (low boiling metals) , distillation is used., Liquation :- For the purification of lead and tin (low melting metals), liquation is used., Zone refining :-, , This method is used to purify semiconductors like Germanium, Silicon and Gallium., Principle of this method is that the impurities are more soluble in melt than solid metal., A circular mobile heater is placed at one end of a rod of impure metal. The molten zone moves along with, heater. As the heater moves, pure metal crystallize out. Impurities are collected at one end. Process is, repeated several times. End is cut off., Ultrapure semiconductors are produced by this method., , 5. EXTRACTION OF IRON (in blast furnace), , Haematite, lime stone and coke are raw materials used in the blast furnace in the extraction of iron., The above are introduced from the top and blast of hot air is passed from bottom of the furnace., Coke combines with oxygen, forms carbon dioxide first and then carbon monoxide., , 2 C + O2 → 2 CO, , Carbon monoxide is the reducing agent in the blast furnace., The reduction reaction in the blast furnace is, , Fe2O3 + 3 CO → 2 Fe + 3 CO2, , The molten iron formed in the blast furnace contains 4 % carbon and some impurities like sulphur,, silicon etc. This impure form of iron is called pig iron., Lime stone decomposes to give Calcium oxide and Calcium oxide is the flux in the blast furnace., The slag formed in the blast furnace is calcium silicate (CaSiO 3), CaO + SiO2 → CaSiO3 (Slag formation reaction in the blast furnace), Flux, Gangue, Slag

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6. What is cast iron and pig iron?, The molten iron formed in the blast furnace contains 4 % carbon and some impurities like sulphur,, silicon etc. This impure form of iron is called pig iron., Cast iron has lower carbon content (about 3 % ) and is hard and brittle., Cast iron is formed by heating pig iron with scrap iron and coke using hot air blast., 7. Purest form of iron is wrought iron., 8. What is the role of lime stone (CaCO3) in the extraction of iron?, Ans: Lime stone decomposes to give Calcium oxide and Calcium oxide is the flux in the blast furnace., ====================================================================================================================, , CHAPTER 7 : THE p – BLOCK ELEMENTS, PREPARED BY : YOOSAFALI T K , GHSS VARAVOOR (8040) , 9947444175, YOUTUBE CHANNEL: CHEM DSM, , ============================================================================, 1. Thermal stability of hydrides decreases from NH3 to BiH3 and so reducing character increases from NH3 to BiH3, 2. H2S is less acidic than H2Te . Why? ., Due to decrease in bond dissociation enthalpy down the group, acidic character increases., 3. Why is H2O a liquid and H2S is gas ?, In H2O hydrogen bond is possible. Not possible in H2S, 4. NH3 has higher boiling point than PH3. Why?, It is because ammonia molecules are associated through inter molecular hydrogen bonding., 5. Acidity order of hydrohalic acid :-, , HF < HCl < HBr < HI, Since HI has the weakest bond dissociation enthalpy, it ionizes readily in aqueous solution and behaves as, strongest acid., , NITROGEN FAMILY, 6. The ionization enthalpy of nitrogen family members are higher than that of oxygen family members. Why?, It is due to stable half filled electronic configuration. (ns 2 np3), 7. Oxidation states of nitrogen family :The common oxidation states of these elements are -3 , +3 and +5., -3 oxidation state decreases down the group due to increase in size and metallic character., The stability of +5 oxidation state decreases and +3 oxidation state increases down the group due to inert pair, effect., Nitrogen shows variable oxidation states from -3 to +5, , (-3 , -2, -1 , 0 , +1 , +2 , +3 , +4 , +5 ), , 8. Nitrogen does not form pentahalides. Why?, Nitrogen(2s2 2p3) has no d- orbitals in its valence shell to expand its covalency beyond four., 9. Give some anomalous properties in which nitrogen differ from the rest of the members., (I), Nitrogen is gas, others are solids, (II), , Nitrogen forms pπ_ pπ multiple bond. (N≡ N ) , while others not.

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(III), Nitrogen does not show pentavalency, while others show., (IV), Nitrogen is diatomic, while others polyatomic., 10. How nitrogen is prepared in the laboratory?, By the thermal decomposition of sodium azide or barium azide., 11. Nitrogen is less reactive at room temperature. Why?, Because of its high bond dissociation enthalpy. It is due to triple bond(N≡N ), 12. Different oxides of nitrogen., (I), Dinitrogen oxide or Nitrous oxide (N2O) :- It is known as laughing gas., (II), Nitrogen oxide or Nitric oxide (NO) :- It is paramagnetic due to the presence of odd electron., (III), Nitrogen dioxide(NO2) :- It exist as dimer on cooling dueto the presence of odd electron on nitrogen., (IV), Dinitrogen tetroxide(N2O4) :- It is the dimer of nitrogen dioxide, (V), Dinitrogen pentoxide (N2O5) :- Its covalency is 4, 13. Which are the allotropes of phosphorus? Explain each., , (i), , White phosphorus:It consist of discrete P4 tetrahedral., It is highly reactive due to strained structure, , (ii), , Red phosphorus:-, , (iii), , It is polymeric, consists of chains of P4 tetrahedra linked through P-P bonds., Black Phosphorus:- It has two forms (i) Alpha black phosphorus (ii)Beta black phosphorus, , 14. How is phosphine is prepared?, (I), Phosphine is prepared by the reaction of calcium phosphide with water or dilute hydrochloric acid., , Ca3P2 +6 H2O→ 2 PH3 + 3 Ca(OH)2, Ca3P2 +6 HCl→ 2 PH3 + 3 CaCl2, (II), , In the laboratory, Phosphine is prepared by heating white phosphorus with concentrated sodium, hydroxide solution in an inert atmosphere of carbon dioxide., , P4 + 3 NaOH + 3 H2O→ PH3 + 3 NaH2PO2, 15. PH3 (Phosphine) is base. Explain with example., PH3 is base due to the presence of lone pair of electrons, , PH3 + HCl → PH4Cl

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Uses of phosphine: In Holme’s signal, In smoke screen, 16. Name the important oxo acids of phosphorus and draw their structures., , H3PO2 is a reducing agent due to the presence of PH bonds in its structure., H3PO4 is tribasic acid due to the presence of three OH bonds and H3PO3 is dibasic acid due to the presence of two, OH bonds., 17. What happens when H3PO3 is heated ?, On heating orthophosphorus acid undergoes disproportionation to form orthophosphoric acid and phosphine., , 4 H3PO3 → 3 H3PO4 + PH3, OXYGEN FAMILY, 18.Oxidation states of oxygen family :Oxygen shows -2 oxidation state except in peroxides (-1) and in OF 2 (+2) while others form positive oxidation, states +2, +4 and +6., +4 and +6 are common., On going down the group,+6 decreases and +4 increases due to inert pair effect., 19. Give some anomalous properties in which oxygen differ from the rest of the members, (I), Oxygen is diatomic gas while others are poly atomic solids., (II), Hydride of oxygen (H2O) is liquid while other hydrides of this family are gases., 20. How oxygen is prepared in the laboratory?, (I), Industrially, by the electrolysis of water., (II), By the thermal decomposition of chlorates, permanganates etc., 21., , Preparation of ozone :-, , In the laboratory, ozone is prepared by passing a silent (sparkless ) electric discharge through pure dioxygen in, an apparatus called ozonizer. Ozone (O3) is Pale blue gas with pungent smell., , 3 O2 → 2 O3, 22. Ozone is powerful oxidizing agent. Why? Give example., Because it liberates nacent oxygen., , O3→O2 + [O]

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Ozone oxidizes black lead sulphide to white lead sulphate., , PbS + 4[O] → PbSO4, 23. How will you estimate ozone?, When ozone react with an excess of potassium iodide solution, iodine is liberated that can be titrated against a, standard solution of sodium thiosulphate. This is a quantitative test for estimating ozone gas., , 24.Allotropes of sulphur: -Rhombic sulphur (α) and Monoclinic sulphur (β), Rhombic sulphur (α), Monoclinic sulphur (β), It is prepared by evaporating a solution of roll, sulphur in carbon di sulphide., Most stable, , It is prepared by melting rhombic sulphur and then, cooling., It is stable only above 369 K, , 25. How is SO2 prepared in the laboratory?, , (i), (ii), , S + O2 → SO2, Sulphite + dilute sulphuric acid → SO2, , 26. SO2 is a reducing agent. Give reactions., SO2 decolourise the acidified potassium permanganate solution. This test is used to detect the presence of SO 2, , HALOGENS, 27. Halogens have maximum negative electron gain enthalpy in the respective period. Why?, Halogens have the smallest size in their respective period and therefore high nuclear charge., As a result, they readily accept one electron to acquire noble gas electronic configuration., 28. Oxidation states of halogen family:All the halogens show -1 oxidation state., Fluorine , the most electronegative element show -1 oxidation state only., However Cl, Br, and I shows +1, +3, +5, +7 also., 29. Give some anomalous properties in which fluorine differ from the rest of the members., (I), Fluorine, the most electronegative element show -1 oxidation state only. However Cl, Br, and I shows +1,, +3, +5, +7 also., (II), HF is low boiling liquid due to association of HF molecules by hydrogen bonding. Other hydrogen halides, are gases., 30. How chlorine is manufactured on large scale?, (I), , Deacon’s process :- By oxidation of hydrogen chloride gas with oxygen in the presence of CuCl 2, catalyst., , (II), , Electrolytic process:- Chlorine is produced by the electrolysis of brine solution(NaCl solution)., , Chlorine is produced at anode., 31. Explain the action of chlorine on alkali.

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With cold and dilute alkalies, chlorine produces a mixture of chloride and hypochlorite., With hot and concentrated alkalies , chlorine produces a mixture of chloride and chlorate., 32. Explain the action of chlorine on ammonia, With excess ammonia , chlorine gives nitrogen and ammonium chloride., With excess chlorine, ammonia gives nitrogen tri chloride( explosive)., 33. What is Bleaching powder? How is it prepared?, Bleaching powder is a mixture of calcium chloride and calcium hypochlorite., It is prepared by passing chlorine gas through dry slaked lime., , Ca(OH)2 + 2 Cl2 → Ca(OCl)2 + CaCl2 + 2 H2O, 34. Explain the Bleaching action of chlorine., Bleaching action of chlorine is due to oxidation., , Cl2 + H2O → 2 HCl + [O], Coloured substance + [O] → Colourless substance, Bleaching action of chlorine is permanent. It bleaches vegetable matter in the presence of moisture, 35. Name Poisonous gases prepared from chlorine., Phosgene, Tear gas, Mustard gas., 36. How will you prepare hydrochloric acid? Give its uses., , 2 NaCl +H2SO4→ Na2SO4+ 2 HCl, Uses: (i) In the manufacture of glucose (ii) As a laboratory reagent, 37. What is Aqua regia? Give its use, Aqua regia is a mixture of concentrated hydrochloric acid and concentrated nitric acid in the ratio 3 :1 ., It is used for dissolving noble metals like gold, platinum., 38. Draw the structures of oxo acids of chlorine., , (I), (II), (III), (IV), , HOCl ,Hypochlorous acid, HClO2 , Chlorous acid, HClO3 , Chloric acid, HClO4 , Perchloric acid

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UNIT 8, THE d AND f BLOCK ELEMENTS, PREPARED BY : YOOSAFALI T K , GHSS VARAVOOR(8040) , 9947444175, YOUTUBE CHANNEL : CHEM DSM, ===========================================================================, 1. What are Transition elements? Zinc, Cadmium and Mercury of group 12 are not Transition elements. Why?, Transition elements are elements having incompletely filled d –orbitals in their free state or in any one of, their oxidation states., Zinc, Cadmium and Mercury of group 12 have completely filled d –orbitals in their free state (d 10) and in their, common oxidation states. So they are not transition elements., 2. Copper, Silver and gold atoms have completely filled d orbitals (d10). But they are transition elements. Why?, Because they have incompletely filled d configuration in any one of its oxidation state., 3. Explain the variation of atomic and ionic radii of transition elements., Atomic and ionic radii of transition elements decrease from left to right in a period due to increase in nuclear, charge. But in the middle decrease in very small due to screening effect of inner d electrons., At the end of the series, atomic radii increase slightly due to inter electronic repulsion., The elements of 4d series and 5d series have similar size due to lanthanoid contraction., 4. Explain melting and boiling point of transition elements., Transition elements have very high melting and boiling point due to the presence of strong metallic bonding, in them., Greater the number of unpaired electrons, stronger the bonding and higher the melting point and enthalpy of, atomisation., Tungsten has highest melting point among the d –block elements, 5. Explain the variation of ionization energy of transition elements., Along a transition series ionization enthalpy increases due to increase in nuclear charge. But it is not regular., The elements of 5 d series have high ionization energy than 3d and 4 d series. This is due to lanthanoid, contraction and poor shielding effect of inner 4f electrons., The second ionization energy of chromium and copper are unusually high due to stable electronic, configuration of 3d5 and3d10 respectively., 6. Why transition elements show variable oxidation states?, Due to the participation of both ns and (n-1) d electrons for compound formation due to small difference in, energies of ns and (n-1) d orbitals ., Manganese ,Mn ( 3d5 4s2) shows largest number of oxidation states among 3d series from +2 to +7., It is due to the participation of two 4s electrons and five 3d electrons for bond formation., The common oxidation states of first transition series is +2 (except for scandium +3)., Scandium does not exhibit variable oxidation state. Only +3., Transition elements show zero oxidation state in metal carbonyls., 7. Transition elements form interstitial compounds. Explain., The transition metal atoms and their crystal structures has interstitial voids and can accommodate small, atoms like hydrogen, boron and nitrogen etc. These are non stoichiometric compounds., Eg:- Nitrides, Carbides, Borides, Hydrides.

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8., , 9., , 10., , 11., , Interstitial compounds: (i) Have high melting point than pure metals.(ii) Are very hard (iii) Retain metallic, conductivity (iv) Are chemically inert., Why transition elements form alloys?, The transition metals are quite similar in size and, therefore, the atoms of one metal can easily replaced by, other atoms of the other metal in its crystal lattice., Examples for alloys are brass (Cu + Zn) , bronze (Cu + Sn), stainless steel (Fe + Cr + Ni + C)., Describe the method of preparation of potassium permanganate from pyrolusite ore., Potassium permanganate is prepared from pyrolusite ore (MnO 2), Pyrolusite ore is fused with potassium hydroxide in the presence of air, potassium manganate is formed., Potasium manganate is then oxidized by electrolysis to potassium permanganate., Give some uses of potassium permanganate, (i), It is used as primary standard in volumetric analysis, (ii), It is used as oxidizing agent., Draw structures of manganate and permanganate ions., , 12. Potassium permanganate is powerful oxidizing agent in acidic medium. Give examples., When Potassium permanganate act as oxidizing agent in acidic medium, it gets reduced to Mn 2+ salt., (I), Acidified K MnO4 oxidises ferrous salt to ferric salt., (II), Acidified K MnO4 oxidises iodide to iodine., (III), Acidified K MnO4 oxidises oxalic acid or oxalate ion to carbon dioxide., 13. What happens when potassium permanganate is heated?, When heated potassium permanganate decomposes at 513 K to form potassium manganate , manganese, dioxide and oxygen., 14. Oxidation states of lanthanoids :-The most common oxidation state of lanthanoids is +3. But some of them, exhibit +2 and +4. Cerium exhibit +4 oxidation state because Ce4+ has the electronic configuration of noble gas, Xenon., , Ce: [Xe] 4f1 5d1 6s2, , Ce4+ : [Xe], , 15. Colour of lanthanoids is due to f-f transition., , 16. Oxidation states of actinoids :-Actinoids show a greater range of oxidation states than lanthanoids., This due to the fact that 5f, 6d and 7s levels are of comparable energies. However +3 oxidation state, is most common among all lanthanoids (except Thorium). Thorium shows +4 oxidation state. Th 4+ :, [Rn], The maximum oxidation state shown by actinoids increases from Th (+4) to Np and Pu (+7) and then, decreases as the atomic number increases.

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17. What are the similarities of lanthanoids and actinoids?, (I), Both the series are formed by progressi, progressive, ve filling of f orbitals and both show +3 oxidation, state predominantly., (II), The elements of both the series are electropositive and highly reactive., (III), Lanthanoid contraction and actinoid contraction are due to the poor shielding of 4f and 5f, electrons respectively., (IV), Most of their ions are paramagnetic and form complexes., 18. What are the differences between lanthanoids and actinoids?, Lanthanides, Actinides, Besides common oxidation state of +3,, Besides common oxidation state of +3,, lanthanides show +2 and +4 states., actinides show +4, +5,+6 and +7 states., The tendency to form complex is less., The tendency to form complex is greater., Except promethium, all elements are, All elements are radioactive., non-radioactive., Lanthanide compounds are less basic., Actinide compounds are more basic., , ========================================================, =============================================================================, =====================, , CHAPTER, , 9, , COORDINATION COMPOUNDS, , PREPARED BY: YOOSAFALI T K , GHSS VARAVOOR , 9947444175, YOUTUBE CHANNEL, CHANNEL: CHEM DSM, ================================================================, 1. What are ligands ? What is the condition to be ligand ?, The neutral molecules or ions which surround the central metal atoms are called ligands., Every ligand should contain at least one electron pair., 2. How will you classify ligands depending on the number of electron pairs donated by atoms? Explain each., (I), Mono dentate ligands provide, de one electron pair per molecule or ion., e.g. NH3 , H2O , CO , Cl- , F- , OH- , NO2- , SCN(II), Di dentate ligands(bidentate ligand) provide two electron pair per molecule or ion., e.g. Oxalate ion (ox),, Ethylene diamine (en) or ethane, ethane-1,2 –diamine, , (III), , Poly dentate ligands provide several pair of electrons per molecule or ion., e.g. EDTA ion

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3. What are Ambidentate ligands and Chelating ligands?, Ambidentate ligands :-Certain, tain mono dentate ligands are capable of ligating through two different atoms present, in it. They are called ambidentate ligands. E.g. NO2− , SCN-−, Chelating ligands:- When a didentate ligand or polydentate ligand is attached by two or more atoms to the, central metal ion and forms a ring structure, the ligand is called chelating ligand. The resulting complex is called, chelates, , 4. What are Homoleptic complexes and Heteroleptic complexes ?, Homoleptic complexes:- Complexes in which the metal atom is linked only to one type of ligands are called, homoleptic complexes. E.g [Co(NH3)6]3+, Heteroleptic complexes :- Complexes in which the metal atom is linked only to more than one type of ligands are, called heteroleptic complexes. E.g [Co(NH3)4 Cl2]+, 5. What is Coordination number?, The total number of ligand donor atoms to which the metal is directly bonded., [Co(NH3)5 (SO4)]Br → Its coordina on number is 6, [CoCl2(en)2]+, → Its coordina on number is 6, 6. What are the postulates of Werner’s theory, (I), In coordination compounds, metal atom exhibit two types of valancies, primary valency and secondary, valancy., (II), The primary valency is ionisable and secondary valency is non ionisable., (III), The primary valancies are satisfied by negative ions and secondary valancies are satisfied by negative ion or, neutral molecules (ligands)., (IV), Every metal atom or ion has a fixed number of secondary valancies equal to its co ordination number., (V), The primary valancies are non directional. The secondary valancies are directional and directed towards, fixed corners of a regular geometry and give shape to the molecule., 7. What are the important features, atures of valence bond theory., (I), The central metal atom provides a number of empty orbitals ,which is equal to the co ordination number of, the central metal ion., (II), The appropriate emptyy atomic orbitals of the metal h, hybridise, ybridise to form a set of equivalent hybridized, orbitals with definite geometry., Coordination number, Hybridisation, Geometry, eometry, 4, sp3, tetrahedral, 4, dsp2, Square planar, 3 2, 2 3, 6, sp d or d sp, octahedral, (III), The empty hybridized orbitals of the central metal atom overlap with the filled orbitals of the ligand to, form metal – ligand coordinate bonds., 8. With the help of valence bond theory, explain the geometry and magnetism of [Co(NH 3)6]3+., Co is in +3 oxidation state , 3 d6 configuration, , In the presence of ligands ( ammonia) pairing will takes place.

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d2sp3 hybridisation,, ridisation, Octahedral complex ., , Inner d orbitals are used for hybridization, so it is iinner orbital complex ., No unpaired electron, it is diamagnetic ., 9. With the help of valence bond theory, explain the magnetic property, inner orbital complex and geometry of, [Fe(CN)6]3- ., Fe is in +3 oxidation state , 3 d5 configuration, , In the presence of ligands( cyanide ions) pairing will takes place., , d2sp3 hybridisation, Octahedral co, complex ., Inner d orbitals are used for hybridization, so it is Inner orbital complex., Unpaired electron is present, so it is paramagnetic., 310. [FeF6] is an outer orbital complex or high spin complex. Prove., Fe is in +3 oxidation state , 3 d5 configuration., , In the presence of ligands ( fluoride ions), pairing will not takes place., Sp3 d2 hybridisation , Octahedral complex., Outer d orbitals are used for hybridization, so it is Outer orbital complex, Large number of unpaired elec, electrons, So high spin complex. It is paramagnetic, 11. With the help of VBT,, explain [Ni(CN)4]2-is square planar complex and [NiCl4] 2- is tetrahedral., , [Ni(CN)4]2-, , Here Ni is in +2 oxidation state, state, 3 d8 configuration., , In the presence of ligands (cyanide ions), pairing will takes place., , dsp2 hybridisation .Square, Square planar geometry., No unpaired electron, it is diamagnetic., , [NiCl4] 2-, , Here Nii is in +2 oxidation state, state, 3 d8 configuration., , In the presence of ligands (chloride ions), pairing will not takes place., sp3 hybridisation , Tetrahedral geometry., Unpaired electrons are present , it is paramagnetic.

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12. With the help of valence bond theory, explain [Ni(CO) 4]is is tetrahedral and diamagnetic., Ni is in 0 oxidation state, , 3 d8 4 s2 configuration., In the presence of ligands ( carbon monoxide),, pairing will takes place.sp, sp3 hybridisation,, tetrahedral geometry. No unpaired electron, it is, diamagnetic., , 13. What are the limitations of valence bond theory, theory?, (I), It does nott explain the colour exhibited by coordination compounds., (II), In certain cases, the experimentally observed values of magnetic moment do not fully agree, ag, with the, values calculated from valence bond theory., 14. Explain the crystal field theory of complexes using oc, octahedral complexes, CFT assumes the ligands to be point charges and the interaction between ligands and central metal ion is purely, electrostatic. There are five degenerate d orbitals. When ligands approach, the energy of five d orbitals increase,, the degeneracy, eneracy will loss and split in to two sets. This is called crystal field splitting., In octahedral complexes, ligands approach through the axis and the orbitals lie in the axis (eg → dx2-y2 and dz2 ), gets repelled more and its energy is more increased., The other d orbitals which lie in between the axes are lowered in energy ( t 2g →dxy , dxz , dyz )., The energy difference between the two sets of orbitals (t 2g and eg) are called crystal field splitting energy (∆o)., , 15. What are Spectro chemical series ?, The ligands can be arranged according to the magnitude of crystal field splitting ((∆o) and is called spectro chemical, series., The ligands lying above H2O are called strong field ligands and those below H2O are called weak field ligands., I- < Br- < Cl- < F- < OH- < H2O < NH3 < en < CN- < CO, 16. With the help of crystal field theory, explain colour of [Ti(H 2O)6]3+, Ti (3d2 4s2) , Here Ti3+ (3d1), → t12g e0g, For the excitation of electron from t 2g orbital to eg orbital, green and yellow light are absorbed., The complimentary colour is purple.

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17. Write electronic configuration of d4 system using crystal field theory in low spin complexes and high spin, complexes., 4, , 0, , 3, , 1, , In low spin complexes t 2g e g ,, In high spin complexes t 2g e g, 18. The hexa aqua manganese (II) ion contain five unpaired electrons, while the hexa cyanido manganese (II) ion, contain only one unpaired electron. Explain using crystal field theory., In hexa aqua manganese (II) ion, manganese is in +2 oxidation state. 3d5 configuration., Here ligand is water, weak field ligand and the crystal field splitting is low., 3, , 2, , So the electronic configuration is t 2g e g .So five unpaired electrons., 𝑴𝒂𝒈𝒏𝒆𝒕𝒊𝒄 𝒎𝒐𝒎𝒆𝒏𝒕 = 𝒏(𝒏, 𝒏 + 𝟐= 𝟓(𝟓 + 𝟐) = √𝟑𝟓 = 5.92, In hexa cyanido manganese (II) ion, manganese is in +2 oxidation state. 3d5 configuration., Here ligand is cyanide,, strong field ligand and the crystal field splitting is high., 5, , 0, , So the electronic configuration is t 2g e g .So only one unpaired electron., 𝑴𝒂𝒈𝒏𝒆𝒕𝒊𝒄 𝒎𝒐𝒎𝒆𝒏𝒕 = 𝒏(𝒏, 𝒏 + 𝟐= 𝟏(𝟏 + 𝟐) = √𝟑 = 1.73, 19. Explain the crystal field splitting in tetrahedral co, complexes., , In tetrahedral complexes, ligands approach the metal ion through a position in between the axes and the t 2g orbitals, get repelled more and its energy is increased than e g orbitals.., The magnitude of tetrahedral splitting will be less than octahedral splitting. ∆t =(4/9) ∆o . So in tetrahedral, complexes high spin complexes are formed., 20. What are the merits of cystal field theory, theory?, (I), It can explain colour of the coordination compounds, (II), It can explain magnetic properties., 21. What are the limitations of crystal field theory?, (I), Since ligands are considered as point charges in crystal field theory, anionic ligands are supposed to exert, greater splitting effect. But many of the anionic ligands are weak field ligands., (II), It considers metal-ligand, ligand bond as ionic and does not take in to account the covalent nature of the bond, , 22. What are the factors which govern the st, stability of complexes?, (I), Greater the charge on the central metal ion , greater the stability of the complexes., K3[Fe(CN)6] is more stable than K 4[Fe(CN)6], (II), Greater the strength of the ligand, greater the stability of the comp, complexes., K4[Fe(CN)6] is more stable than K 4[FeCl6]

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4. Boiling point of alcohols and phenols are higher than haloakanes, hydrocarbons etc. Why?, Due to inter molecular hydrogen bonding, 5. Compare Boiling point of alcohols, (I), As length of alcohols increases, boiling point increases, due to increase in Vander walls force of attraction., Example: Methanol < Ethanol < propanol < Butan, Butanol, (II), As branch of alcohols increases, boiling point decreases, due to decrease in Vander walls force of, attraction. Example: Butan-2-ol, ol < Butan, Butan-1-ol, 6. Lower alcohols are soluble in water. Why?, Lower alcohols form hydrogen bond with water molecules., 7. What is esterification. Give example., Alcohol or phenol reacts with acids, acid chlorides or acid anhydrides gives ester is called esterification, R–OH + R’ –COOH, , 𝑯, , R–O, O CO R’ + H2O, , 𝑷𝒚𝒓𝒊𝒅𝒊𝒏𝒆, , R–OH + R’ –COCl ⎯⎯⎯⎯⎯, R–O, O CO R’ + HCl, 8. Explain the acidity of alcohols, The acidity of alcohols is due to the polar nature of O, O-H bond., An electron releasing alkyl groups increases electron density on oxygen tending to decrease the polarity of, O-H, H bond. This will reduce the acid strength., Acidity decreases in the order, , Alcohols react with active metals give hydrogen gas and alkoxide. This reaction shows that alcohol is acidic., 𝟐 𝑹𝑶𝑯 + 𝟐 𝑵𝒂 → 𝟐𝑹𝑶𝑵𝒂 + 𝑯𝟐, 9. Alcohols are weaker acids than water. Explain, It is explained by the reaction of water with alkoxide., , R-O- + H-O-H → R-O-H, H + OHBase, Acid, This reaction shows that water is a better proton donor (i.e. Water is stronger acid than alcohols), 10. Phenol, enol is weakly acidic. Explain with example., Phenol react with active metals like Na gives hydrogen., Phenol react with alkali like NaOH gives salt and water., Both these reaction shows that phenol is acidic., Reaction with alkali shows that phenol is more acidic than alcohols., , ,, 11. Why phenol is more acidic than alcohols?, (I), In phenol, due to resonance develop a partial positive charge on oxygen and it tries to attract the electron, pair of O-H, H bond. This makes the O, O-H bond weak and the hydrogen atom can be easily released as proton, (II), Phenoxide ion is also resonance stabilized and so release of proton is easy.

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12. Compare the acidity of phenols, Electron releasing group decreases acidity of phenol., Electron withdrawing group increases acidity of phenol., As the number of electron withdrawing group increases acidity of phenols also increases., e.g. 4-methyl phenol < phenol<3-nitrophenol<, nitrophenol< 3,5, 3,5- dinitrophenol < 2,4,6-trinitrophenol, 13. Acidity order : Alcohols < water < Phenols, 14. What happens when zinc, inc is added to phenol?, , Phenol + Zinc → Benzene, enzene, , 15. Explain bromination reaction of phenol, (i), Bromination:On bromination with bromine in CCl4 or CS2, phenol gives, ortho and para bromophenol., , On bromination with bromine water, phenol gives 2,4,6tribromophenol, , 16. Explain the following name reactions ., (a), , Kolbe’s reaction :-, , 𝑪𝑶𝟐, , Phenol + NaOH → Sodium phenoxide ⎯, , Salicylic acid, , 17. How will you distinguish alcohol and phenols?, (i), Phenol reacts with alkali. Alcohol does not., (ii), Phenol gives violet color with neutral ferric chloride. Alcohol does not., 18. Methanol is known as wood spirit. How is it manufactured?, Methanol is manufactured by passing a mixture of carbon monoxide and hydrogen through a catalytic mixture of, ZnO and Cr2O3 at a pressure of 200 atm to 300atm and temperature of 573 K to673 K, , Use of methanol: (i) solvent for paints or varnishes,(ii) in the manufacture of formaldehyde, (iii)for, denaturation of ethanol

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2. Glucose is water soluble . Why?, Due, ue to the formation of hydrogen bond with –OH groups., 3. What are the limitations of open structure of glucose?, (i), D-glucose does not undergo certain reactions of aldehydes. For example, it does not give the Schiff’s test,, 2,4- dinitro phenyl hydrazine test and it does not react with NaHSO 3., (ii), Glucose penta acetate does not react with hydroxylamine indicating the absence of free –CHO group., (iii), Glucose exist in two crystalline forms alpha D(+) glucose and Beta D (+) glucose., It cannot be explained by open structure., 4. Draw the cyclic structure of glucose., , What are Anomers ? Give example for it., A pair of stereo isomeric ring forms of a sugar which differ in configuration at C, C-1, 1 (anomeric carbon) are called, anomers. Thus alpha D(+) glucose and Beta D (+) glucose are anomers, 6. Structure of fructose., Fructose has molecular formula C6H12O6 .Fructose is Ketohexose. It is laevorotatory and belong to D-series, D, 5., , 7. What are Proteins ?, Proteins are complex nitrogeneous organic compounds of high molecular mass found in living systems., Chemically all proteins are polymer of alpha aminoacids., Proteins, oteins are polypeptides having molecular mass more than 10000., 8. What are amino acids?, Aminoacids are compounds containing both amino and carboxyl groups., Aminoacids are formed by the hydrolysis of proteins.

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9. Classify amino acids in to neutral, acidic and basic., Aminoacids containing one amino group and one –COOH, COOH group are neutral aminoacids, E.g. glycine and alanine, Aminoacids containing one amino group and two –COOH, COOH group are acidic aminoacid., E.g. aspartic acid and glutamic acid, Aminoacids containing two amino group and one –COOH, COOH group are basic aminoacid., E.g. lysine argynine and histidine., 10. Which is an optically inactive amino acid found in proteins., Glycine, 11. What are essential and non essential amino acids?, There are 20 aminoacids required for the synthesis of proteins., Aminoacids which the human body cannot synthesise are called essential aminoacids. These must be supplied, suppli, through diet. E.g., Lysine, valine etc., Aminoacids which the human body can synthesise are calle, called, d non essential aminoacids. These are not essential in, the diet. E.g. glycine, alanine etc., 12. What are zwitter ion?, Since amino acids contain both basic and acidic groups ,, they neutralize each other forming a dipolar ion called, zwitter ion., 13. The melting, ng point and solubility in water of amino acids are higher than halo acids. Explain., The amino acids exist as zwitter ion. Due to this polar structure, the molecules have strong dipoledipole dipole, interaction. So they have higher melting point. Due to polar st, structure, they strongly interact with water, molecules and so water soluble., 14. What is peptide linkage?, Peptides are amides formed by the reaction of amino group of one amino acid molecule with the carboxyl, group of another amino acid with the elimination of water molecules., The –CO-NH- bond connecting the amino acids is called peptide linkage or peptide bond., 15. Differentiate between globular and fibrous proteins., , Fibrous proteins, , Globular proteins, , Here poly peptide chains lie side by side to form fibre, like structures., They are insoluble in water, e.g. Keratin ( present in hair , wool), myosine (present in muscles), , Here poly peptide chains coil around or folded, to give a spherical shape, They are soluble in water, e.g. insulin (hormone),, albumin (in egg white), , 16. Explain the structure of protein., , Primary structure, Secondary stucture, Tertiary structure, Quarternary, structure, , It explains which aminoacids are present and sequence of amino acids, Folding of poly peptide chain results to α, α-helix and β-pleated, pleated structure, Three dimens, dimensional, ional folding results fibrous and globular shape., Spatial arrangement of poly peptide sub units

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17. What are Vitamins ? Which is the vitamin synthesized in the body?, Vitamins are organic compounds required in the diet in small amounts to perform specific biological functions for, maintenance of normal growth and health., Vitamin-D is syntesised in the body., 18. How will you classify vitamins?, (i), Water soluble vitamins . e.g. vitamin B ,C, (ii), Fat soluble vitamins . e.g. Vitamin A, D. E, K, 19. Vitamins and deficiency deseases, , Vitamins, , Deficiency deseases, , Vitamin A (Retinol), Night blindness,Xerophthalmia, Vitamin B1 (Thiamine), Beri-beri, Vitamin B2 (Riboflavin), Cheilosis, Vitamin B6 (Pyridoxine), Convulsions, Vitamin B12 (Cyano cobalamine), Pernicious anaemia, Vitamin C (Ascorbic acid), Scurvy, Vitamin D (sunshine vitamin), Rickets, Vitamin E (Antisterility vitamin), Sterility, muscular weakness, Vitamin K, Increased blood clotting time, 20. Vitamin C cannot be stored in our body. Why?, Because it is soluble in water and readily excreted through urine., 21. What are nucleic acids?, Nucleic acids are polymer of nucleotides. So they are called poly nucleotides., Nucleic acids are two types (i) Deoxyribo nucleic acid(DNA) (ii) Ribo nucleic acid(RNA), 22. What are nucleoside and nucleotide?, Nucleoside :- Pentose sugar + nitrogeneous base, Nucleotide :- Pentose sugar + nitrogeneous base + Phosphate ester linkage, 23. Explain the structure of nucleic acid., , Primary structure gives the information regarding the sequence of various nucleotides in the chain of nucleic acid., The secondary structure of DNA is double stranded α-helix structure., The two chains of double helix are held by hydrogen bonds between specific bases., Adenine in one helix is paired with thymine by two hydrogen bonds., Cytosine in one helix is paired with guanine with three hydrogen bonds., RNA has single stranded α-helix structure., 24. What are the difference between DNA and RNA?, , Deoxy ribo nucleic acid (DNA), , Ribo nucleic acid (RNA), , Pentose sugar is β-D-2- deoxy ribose, Pentose sugar is β-D -ribose, Bases are adenine, thymine, cytosine and guanine, Bases are adenine , uracil, cytosine and guanine, DNA has double stranded α-helix structure., RNA has single stranded α-helix structure., DNA controls the heredity(Genetic information is stored, RNA controls the synthesis of proteins, in DNA), DNA undergo replication, RNA does not undergo replication, 25. What products would be formed when a nucleotide from DNA containing thymine is hydrolysed?, Thymine, 2- deoxy D(-) ribose and phosphoric acid, 26. Three types of RNA are (i) Ribosomal RNA (ii) Messenger RNA (iii)Transfer RNA

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CHAPTER 15, , POLYMERS, , PREPARED BY: YOOSAFALI T K , GHSS VARAVOOR , 9947444175, ================================================================, 1. Which is the monomer of PVC ( Poly vinyl chloride) ? Give its use., Its monomer is vinyl chloride., It is used for the manufacture of rain coats, hand bags, vinyl flooring, water p, pipes, ipes etc., , 2. Which is the monomer of Poly styrene? Give its use., Its monomer is Styrene ., It is used as insulator, wrapping material, manufacture of toys, radio and television cabinets., 3. What is Teflon.?? How is it prepared ? Give its use ., Poly tetrafluoroethene, ethene is called Teflon (PTFE)., , 4., , 6., , 7., , 8., , It is formed by the polymerization of tetra fluoro ethene in the presence of catalyst and at high pressure. It is, resistant to heat and chemicals., It is used in non stick frying pans and also used in making oil seals and gaskets, Name a synthetic wool. How is it formed?, Poly acrylo nitrile (PAN) is a synthetic wool. It is known as orlon or acrilan., It is formed by the polymerization of acrylonitrile (vinyl cyanide) in the presence of peroxide catalyst., 5. Name a polyester.. . How is it formed?, Terylene (Dacron) is a polyester. It is produced by heating ethylene glycol and terephthalic acid., It is used in the manufacture of fabrics and as glass reinforcing materials., Which are phenol formaldehyde, hyde polymers?, (i), Novolac :- It is linear polymer . It is used in paints., (ii), Bakelite :- It is a cross linked polymer. It is used for making combs, electrical switches , and handles of, various utensils., Give examples for synthetic rubbers (artificial rubber). Explain each., (i), Buna-S :- Buna –SS is prepared by treating butadiene and styrene in the presence of sodium. . It is used, for the manufacture of autotyres, footwear components, cable insulation etc, (ii), Buna –N :- It is a copolymer of butadiene and acrylonitr, acrylonitrile., ile. It is resistant to the action of petrol,, lubricating oil etc. it is used in making oil seals, tank lining etc., (iii), Neoprene :- It is produced by the free radical polymerization of chloroprene., What are Biodegradable polymers ? Give examples for it., Biodegradable polymers are the polymers which are degraded by microorganisms within a suitable period of time, so that they and their degradation products do not cause serious effects on the environment., Examples :-, , (i), (ii), , Poly β-hydroxybutyrate, hydroxybutyrate-co-β-hydroxy valarate (PHBV)., Nylon 2 –nylon 6, , ===============================================================, ====================================================================

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CHAPTER, , 16, , CHEMSTRY, , IN EVERYDAY, , LIFE, , PREPARED BY: YOOSAFALI T K , GHSS VARAVOOR , 9947444175, YOUTUBE CHANNEL: CHEM DSM, ================================================================, 1. What are Enzyme inhibitors ? Explain each ., Enzyme inhibitors :-Drugs which inhibit the active sites of enzyme are called enzyme inhibitors., These are two types, competitive inhibitors and allosteric inhibitors., Competitive inhibitors :- Drugs compete with the natural substrate for their attachment on the active sites of the, enzymes. Such drugs are called competitive inhibitors., Allosteric inhibitors :- Some drugs do not bind to the active sites of the enzyme, but bind to a different site called, allosteric site , changes the shape of the active site and so substrate cannot recognize it., 2. What are Antagonists and Agonist? When these are used?, Antagonists :-Drugs that bind to the receptor site and inhibit its natural function are called antagonists., These are useful when blocking of message is required., Agonist :-Drugs that mimic the natural messenger by switching on the receptor, these are called agonist., These are useful when there is lack of natural chemical messenger., 3. What are Antibiotics?, Drugs which in low concentration inhibit the growth or destroy micro organism by intervening in their, metabolic processes. These are anti microbial drugs ., Example : Penicillin, 4. What are bactericidal antibiotic and bactereostatic antibiotic with examples?, Antibiotics which kill microorganism or bacteria are called bactericidal antibiotics., e.g. penicillin, ofloxacin , aminoglycosides., Antibiotics which inhibit the growth of microorganism or bacteria are called bacteriostatic antibiotics., e.g. erythromycin, tetracycline , chloramphenicol etc., 5. Explain broad spectrum antibiotic, narrow spectrum antibiotic and limited spectrum antibiotics., Antibiotics which kill or inhibit a wide range of bacteria are called broad spectrum antibiotics., E.g. ampicillin, amoxicillin, chloramphenicol, vancomycin , ofloxacin, Antibiotics which are effective against only gram positive bacteria or gram negative bacteria are called narrow, spectrum antibiotics. E.g. penicillin G, If an antibiotic is effective against only a single organism or disease is called limited spectrum antibiotics., E.g. dysidarizine ( Towards certain type cancer cells), 6. Which are artificial sweeteners . Explain each., (i), Saccharin :- It is ortho sulpho benzimide. 550 times sweeter than sucrose. It can be taken by diabetic, patients because it is excreted from the body through urine without any change., (ii), Aspartame :- 100 times sweet. It is methyl ester of dipeptide formed from aspartic acid and phenyl alanine., It is used in cold foods and in soft drinks because it unstable at high temperature., (iii), Alitame :- 2000 times sweeter than cane sugar. Control of sweetness is difficult., (iv), Sucrolose :- It is the tri chloro derivative of sucrose. It is stable at cooking temperature., 7. What are Food preservatives ? Give examples, Food preservatives prevent spoilage of food due to microbial growth., E.g. Sodium benzoate, common salt , vinegar , oils, sugar

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8. What are Soaps ? How is it manufactured ?, Soaps are the sodium or potassium salts of long chain fatty acids., Soap is formed by the saponification reaction of oil or fat with sodium hydroxide or potassium hydroxide., 9. What are Synthetic detergents ? Classify them ., Synthetic detergents are cleansing agents which have all the properties of soaps, but actually do not contain any, soap., They can be used in both soft water and in hard water., Detergents are highly branched, not readily biodegradable and so cause pollution problems., These are three types, (i), Anionic detergents :- In this anionic part has cleansing action. These are mainly used for house hold, works. E.g. sodium lauryl sulphate, sodium dodecyl benzene sulphonate., (ii), Cationic detergents : -These are quaternary ammonium salt and cationic part has cleansing action., Cationic detergents have germicidal properties. It is used in hair conditioners., E.g. cetyl trimethyl ammonium bromide, (iii), Non ionic detergents :- It contain no ions. Liquid dish washers contain non-ionic detergents., E.g. The ester formed from polyethylene glycol and stearic acid., , =============================================================================, PREPARED BY:, YOOSAFALI T K, GHSS VARAVOOR (8040), THRISSUR (DT), MOBILE : 9947444175, , YOUTUBE CHANNEL: CHEM DSM, , =========================================================