First Yr Passing Package 2022-2023 PDF

Subject: I PU Chemistry (2022-23) PASSING PACKAGE 1. Classification of elements and periodicity in properties 1.State modern periodic law. Ans: “The physical and chemical properties of the elements are periodic functions of their atomic number”. 2. Name the ele...

Subject: I PU Chemistry (2022-23) PASSING PACKAGE 1. Classification of elements and periodicity in properties 1.State modern periodic law. Ans: “The physical and chemical properties of the elements are periodic functions of their atomic number”. 2. Name the element having highest negative electron gain enthalpy. Ans: Chlorine (Cl) 3. Name the element having highest electronegativity. Ans: Fluorine (F) 4. What is the IUPAC name of the element with atomic number 120 (any number >100)? Ans: Un-bi-nilium 5. What are isoelectronic species? Out of Mg2+ and O2- which one has smaller ionic radius ? Ans: Species which have same number of electrons but different number of protons. Mg2+ 6. Define ionization enthalpy? How does it vary along the period and down the group of the periodic table? Ans: “ Amount of energy required to remove the outermost electron from a gaseous atom” Along the period: Increases Down the group: Decreases 7. Define electron gain enthalpy? How does it vary along the period and down the group? Ans: “ Energy change involved when an electron is added to an isolated neutral gaseous atom’ Along the period: More and more negative Down the group: Less negative 8. Define Electronegativity? How does it vary along the period and down the group? Ans: “ Ability of an atom in a molecule to attract the shared pair of electrons towards itself”  Along the period: Increases Down the group: Decreases 9. Define atomic radius? How does it vary along the period and down the group? Ans: “ Distance between the centre of the nucleus and the outermost shell of an electron” Along the period: Decreases Down the group: Decreases 2. Some Basic Concepts of Chemistry 1. Write any three postulates of Daltons atomic theory. Ans: (i) Matter consist of indivisible atoms (ii) All the atoms of a given element have identical properties including identical mass. (iii) Compounds are formed when atoms of different elements combine in a fixed ratio. (iv) Chemical reaction involve reorganization of atoms. These are neither created nor destroyed. 2. What is homogeneous mixture? Give an example. Ans: In this the component completely mix with each other and its composition is uniform throughout. Example : Salt solution, Sugar solution etc 3. What is heterogeneous mixture ? Give an example. Ans: In this composition is not uniform throughout. Example: Mixture of salt and sugar, oil and water etc 4. State law of definite proportion. Ans: ‘Given compound always contains exactly the same proportion of element by weight’ 5. Define molarity. Ans: No.of moles of the solute present in one litre of the solution. 6. Define molality. Ans: No.of moles of the solute present in one kg of the solvent. 7. How many significant figures are in (any number) Ans Ans (i) 0.0025 - 2 (v) 500.0 - 4 (ii) 208 -3 (vi) 2.0034 - 5 (iii) 5005 - 4 (vii) 0.0410- 3 (iv) 126000 – 3 (viii) 0.2500- 4 (ix) 6.023 ×1023 - 4 8. Express the following numbers in scientific notation (any number) Ans Ans (i) 232.508 - 2.32508 ×102 (vi) 500.0 - 5×102 -4 (ii) 0.00016 - 1.6 ×10 (vii) 6.0012 - 6.0012×100 (iii) 234000 - 234000×105 (viii) 0.00055 - 5.5×10-4 3 (iv) 8008 - 8.008 ×10 (ix) 0.0027 - 2.7×10-3 -3 (v) 0.0048 - 4.8 ×10 (x) 0.0019 - 1.9 ×10-3 9. Express (i) 25°C in Kelvin (any number) (ii) 25°C in Fahrenheit (any number) Ans: (i) K= 273 + °C K = 273 + 25 = 298K (ii) ℉ = 95 °C + 32 9 = × 25 + 32 = 77℉ 5 10. A compound contains 4.07% hydrogen, 24.27% carbon, 71.65% chlorine. Its molar mass is 98.96g. What are its empirical and molecular formula? ( Ans: M.F C2H4Cl2). 11. An organic compound containing 40%carbon, 6.67% hydrogen, and rest of oxygen has the molar mass 180 g/mol. Find out the empirical and molecular formula. (Ans: M.F. C6H12O6) 12. An organic compound contains 40% carbon, 6.66% hydrogen and 53.34% oxygen and its molecular mass is 60. Calculate its empirical and molecular formula. 13. An unknown compound was found to contain 47% potassium, 14.5% carbon and 38.5% oxygen. What is its empirical formula. If its molar mass is 166.2 g/mol. What is its molecular formula? (Ans: M.F : K2C2O4) 14. A sample of a compound contains 48.97% carbon , 2.73% hydrogen and 48.3% chlorine and its molar mass is 147 g/mol. Calculate its molecular formula. 15. A compound with molecular mass of 34 g/mol is known to contain 5.88% hydrogen and 94.12% oxygen. Find the molecular formula of the compound. ( Ans: M.F : H2O2 ). 3. Structure of atom 1. Write any four postulates of Bohrs atomic theory. Ans: (i) Electrons revolve around the nucleus in certain circular paths called orbits (ii) The energy of an electron in the orbit does not change with time. 𝑛ℎ (iii) The angular momentum of an electron in given orbit can be expressed as 𝑚𝑣𝑟 = 2𝜋 (iv) If an electron jump from higher energy level to lower energy level, energy is emitted and when electron jump from lower energy level to higher, energy is absorbed. 2. Write any three limitations of Bohrs atomic theory Ans: i. It is applicable only to hydrogen atom or uni electron systems. ℎ ii. Does not explain why the angular momentum of an electron is an integral multiple of 2𝜋 iii. It fails to explain the fine structure of spectral lines. 3. Mention the significance of four quantum numbers. Ans: i. Principal quantum number- It indicates the size of an orbit ii. Azimuthal Q.No. – It indicates shape of an orbital  iii. Magnetic Q.No. – It indicates orientation of an orbitals in space iv. Spin Q.No – It indicates orientation of the spin of the electron 4. What are the experimental observation made by Rutherford during his scattering experiment? Ans: i. Most of the alpha particles passed through the gold foil undeflected. ii. A small fraction of the alpha particles was deflected by small angles. iii. A very few alpha particles bounced back. 5. State Hund’s rule. Ans: “ Electron pairing in p,d, and f orbitals cannot occur until all orbitals of a given subshell contains one electron each” 6. State Pauli’s exclusion principle. Ans: “ Only two electrons may exist in the same orbital and these electrons must have opposite spin” 7. State Heisenberg’s uncertainity principle. Write its mathematical form. Ans: “ It is impossible to determine simultaneously , the exact position and exact velocity of an electron” ℎ Mathematical form : ∆𝑥 × ∆𝑃 ≥ 4𝜋 8. Using s,p,d notations ,describe the orbital with the following quantum numbers. (i) n=1, l=0 (ii) n=3, l=1 (iii) n=4, l=2 (iv) n=5, l=3 Ans: (i) 1s (ii) 3p (iv) 4d (iv) 5f 𝑒 9. Name the fundamental particle of an atom that has highest value for its ratio. 𝑚 Ans: Electrons. 10. What are isotopes? Ans: The atoms with same atomic number but different mass number are called isotopes. 11. What are isobars? Ans: Isobars are the atoms with same mass number but different atomic number. Problems: 12. Calculate (a) wave number and (b) frequency of yellow radiation having wave length 5800 A°. Ans: (a) ⋋= 5800A° = 5800 ×10-10m. 1 1 𝜗= = −10 = 1.724 ×106 m-1 ⋋ 5800 ×𝑥10 m 𝑐 3×108 (b) Frequency 𝜐 = = = 5.172 × 1014 s-1 𝜆 5800×10−10 13. Yellow light emitted from a sodium lamp has a wavelength (𝜆) of 580nm. Calculate the frequency and wave number of the yellow light. 14. Calculate the wavenumber for the shortest wavelength transition in the Balmer series of the hydrogen spectrum. Ans: For Balmer series shortest wavelength transition is from n1=2 and n2=∞ 1 1 1 1 𝜐=𝑅 [ − ] = 1.09 × 107 [ − ] = 2.725×106 m-1 𝑛1 2 𝑛2 2 22 ∞ 4. Chemical Bonding and Molecular Structure 1. Explain sp or sp2 or sp3 hybridization with an example. 2. Write any four postulates of VSEPR theory. Ans: (i) The geometry of the molecule depends upon the total number of electron pairs present around the central atom (ii) Electron pairs in the valence shell repel one another since their electron clouds are negatively charged. (iii) The pairs of electrons tend to occupy the position in space that minimize repulsion and maximize distance between them. (iv) Where two or more resonance structure can represent a molecule, the VSEPR model is applicable to any structure. 3. Write the electronic configuration of H2 or Li2 or He2 or C2 or O2 molecule. What is its bond order and magnetic property ? 4. Define hydrogen bonding. Mention the compound showing intermolecular and intra molecular hydrogen bonding. Ans: ‘Electrostatic attraction between hydrogen and more electronegative atom (O,N and F) is called hydrogen bonding. Intermolecular H-bonding : HF, H2O, ethanol, methanol etc Intramolecular H-bonding : o-nitro phenol, o-nitro benzoic acid 5. Write any two limitations of octet rule. Ans: (i) Expanded octet of central atom. (ii) The rule failed to predict relative stability of molecules. (iii) The theory does not account for the shape of the molecule 6. Write any two differences between sigma and pi bond. Ans: Sigma bond Pi bond 1. The bond is formed by axial overlap 1. The bond is formed by side wise of the atomic orbitals overlap of the atomic orbitals 2. Strong bond 2. Comparatively weak bond 3. Sigma bond can be formed alone 3. The pi bond can be formed along with pi bond 7. What is ionic bond ? Write any three favourable factors for the formation of ionic bond. Ans: The bond formed by the electrostatic attraction between positive and negative ions is called ionic bond Favourable factors : (i) Donor atom must have low ionization enthalpy  (ii) Acceptor atom must have high electron gain enthalpy. (iii) High lattice enthalpy 5. Equlibrium 1. Define Lewis acid and base. Give an example. Ans: Lewis acid: Species which accept electron pair. Ex: AlCl3, BF3, FeBr3 etc Lewis base: Species which donate electron pair. Ex: NH3, H2O etc 2. Define Bronsted acid and base ? Identify the two conjugate acid base pairs in the following + - NH 3 + HCl NH4 + Cl Ans: An acid is a proton donor while base is a proton acceptor. Conjugate acid base pairs: i.NH3 and NH4+ ii. HCl and Cl- 3. What are buffer solutions ? Give an example for an acidic buffer. Ans: A buffer solution is a solution which resists change in pH on dilution or an addition of small amounts of a strong acid or an alkali. Ex: Mixture of acetic acid and sodium acetate (CH3COOH/CH3COONa) 4. What is common ion effect ? Give an example. Ans: The suppression of the dissociation of a weak electrolyte by adding a strong electrolyte containing a common ion is called the common ion effect. Ans: i. CH3COOH and CH3COONa ii NH4Cl and NH4OH 5. State LeChateliers principle. Ans: ‘If a system in equilibrium is subjected to a change in temperature, pressure or concentration, the equilibrium shift in such a way as to minimize the effect of change’. 6. What is homogeneous equilibrium ? Give an example Ans: The equilibrium reaction in which reactants and products are present in same phase. Ex: N2(g) + 3H2(g) 2NH3(g) 7. What is heterogeneous equilibrium? Give an example. Ans: The equilibrium reaction in which reactants and products are present in different phases Ex: BaCO3(s) BaO(s) + CO2(g) 8. Using LeChateliers principle ,explain the effect of (a) Addition of CH4 (b) Addition of CS2 (c) Removal of S2 (d) Removal of H2S On the equlibrium CH 4 (g) + 2S2 (g) CS2 (g) + 2H2S (g) Ans: (a)Favours forward reaction (b)Favours backward reaction (c) Favours backward reaction (d) Favours forward reaction 9.Explain the effect of pressure , concentration and temperature on N2(g) + 3H2(g) 2NH3(g) ΔH= - X kJ , using LeChateliers principle. 10.What is the effect of temperature change of the following equilibrium  2NO 2(g) N2O4(g) ΔH= -57.2 kJ/mol Ans: a. Increase in temperature favours backward reaction b. decrease in temperature favours forward reaction. 11. Give the relation between Kp and Kc for the equilibrium N2(g) + 3H2(g) 2NH3(g) Ans: 𝐾𝑝 = 𝐾𝑐 (RT)-2 (Δn = 2-4 = -2) 12. Give an example for the reaction in which Kp =Kc Ans: 2HI (g) H2(g) +I2(g) 13.Write the expression for Kc for the equilibrium N2(g) + 3H2(g) 2NH3(g) [𝑁𝐻3 ] 2 Ans: 𝐾𝑐 = [𝑁2 ][𝐻2 ]3 14. What is meant by conjugated acid-base pair ? Write the conjugate acids for CN- and H2O. Ans: A pair of an acid and a base which differ by a proton is called a conjugate acid –base pair. Conjugate acid of CN- is HCN Conjugate acid of H2O is H3O+ 35. Write the relationship between Kp and Kc. Ans: 𝐾𝑝 = 𝐾𝑐 (RT)Δn 6. p-block element 1. Mention the type of hybridization of carbon in diamond. Ans: sp3 2. Write the molecular formula of inorganic benzene. Ans: B3N3H6 3. Write the basic structural unit in silicates. Ans: SiO42- 4. Give any two structural differences between diamond and graphite. 5. Graphite is good conductor of electricity but diamond is bad conductor of electricity. Give reason. Ans: Because graphite contain one free electron but in diamond no free electrons are present. 6. What is dry ice ? Ans: Solid carbon dioxide. 7. How is diborane prepared from BF3 ? Ans: Treating boron trifluoride with lithium aluminium hydride. 4BF 3 + 3LiAlH 4 2B2H6 8. Write any three anomalous behavior of carbon. 9. Name a crystalline form of carbon which resembles soccer ball? Ans: Fullerence 10. Write the structure of Diborane. 7. Hydrocarbons 1. Explain mechanism of chlorination of methane. 2. Explain Wurtz reaction with an example Or How is n-butane obtained from bromoethane ? Write equations dry ether Ans: 2C2H5Br + 2Na C2H5 -C2H5 + 2NaBr ethyl bromide butane sodium bromide (bromo ethane) 3.Explain dehydrohalogenation reaction with an example. Cl alc. KOH Ans: CH3 -CH2 CH2 =CH2 + KCl + H2O ethyl chloride ethene (chloro ethane) 4. How is ethyne converted into benzene ? Give equation. red hot iron tube Ans: 3 CH = CH 873K ethyne benzene 5.State Markonikov’s rule. Ans: It states that “ when unsymmetrical reagent adds to unsymmetrical alkene , then the negative part of the reagent is added to doubly bonded carbon atom contains least number of hydrogen atoms” 6.Explain Friedel-Craft alkylation with an example. Anhydrous CH3 AlCl3 Ans: + CH3Cl methyl chloride + HCl Benzene Toluene 7. Draw the structure of cis and trans isomer of But-2-ene. H3C CH3 H3C H Ans: C C C C H H H CH3 Cis but -2 -ene Trans but -2 -ene 8. Draw the staggered conformation of ethane. 9. Draw the eclipsed conformation of ethane. 10. Name the reagent used for dehydrohalogenation of haloalkanes. Ans: Alcoholic potash (Alc. KOH) 11. Name the reagent used in decarboxylation. Ans: Sodalime (NaOH +CaO) 12. Explain mechanism of chlorination of benzene. 13. Explain mechanism of nitration of benzene 8. Redox reactions: 1. Define oxidation in terms of electron. 2. Define reduction in terms of electron. 3. Calculate the oxidation number of (i) Mn in KMnO4 and MnO2 (ii) Cr in Cr2O72- (iii) O in H2O2 and OF2 (iv)Fe in Fe3O4 4. Balance the redox equation using oxidation number method. (i)Cr2O72- + SO32- Cr3+ + SO42- (acidic medium ) (ii) Cr2O72- + Fe2+ Fe3+ + Cr3+ (acidic medium ) - - (iii)MnO4 + Br MnO2 + BrO3- (basic medium ) (iv) MnO4- + I- MnO2 + I2 ( basic medium) 2- (v) Cr2O7 + SO2 Cr3+ + SO42- (acidic medium ) 9. Environmental Chemistry 1. What is greenhouse effect ? Ans: The increase in temperature of atmosphere due to presence of gases like CH4, CO2 and water vapour, which absorbs infrared radiation. 2. How is ozone layer formed in stratosphere ? Name a chief chemical that causes its depletion. Ans: Due to action of UV radiation on oxygen Chief Chemical: CFC or chlorine containing compounds. 3. Name two gases which are responsible for green house effect. Ans: CO2 and CH4 4.What is meant by BOD ? What is its significance ? Ans: The amount of oxygen required by bacteria to breakdown the organic matter present in certain volume of a sample of water. Significance: BOD is measure of amount of organic matter in water. 5. Write any two common chemicals of photochemical smog. Ans: Acrolein and formaldehyde. 6. Which acid not present in acid rain ? HNO3 , H2SO4, CH3COOH, H2CO3 Ans: CH3COOH 7. What is acid rain ? How it is harmful to the environment ? Ans: When the pH of a rain water is below 5.6 due to presence of oxides of sulphur and nitrogen in the atmosphere is called acid rain. Harmful effects: It toxic to aquatic life and damages buildings 8. What is smog ? Mention one harmful effect of smog. Ans: Smog is a mixture of smoke , dust particles and small drops of fog Harmful effects: irritate nose and throat 9. What is the full form of DDT and BOD ? Ans: DDT- dichloro diphenyl trichloro ethane BOD- biochemical oxygen demand 10. Which part of the atmosphere contains ozone layer ? Ans : Stratosphere 10. Thermodynamics 1. State first law of thermodynamics. Write its mathematical form. 2. What is intensive property? Give an example 3. What is extensive property ? Give an example. 4. Define entropy. Write its SI unit. 5. Write Gibb’s equation.Explain the terms in it. 6. What are the criteria for spontaneity? 7. Write the relation between Cp and Cv. Problems: 8. Calculate the enthalpy of formation of benzene. Given, the enthalpy of combustion of carbon and hydrogen are -393.5 kJ/mol and -285.83kJ/mol respectively. Also it is found that during the combustion of benzene 3267 kJ/mol of heat is liberated. 9. Calculate the standard enthalpy of combustion of methane, given the standard enthalpy of combustion of carbon and hydrogen are -393.5kJ/mol and -285.83kJ/mol resply. Standard enthalpy of formation of methane is -75.16kJmol 10. Calculate the enthalpy of combustion of methyl alcohol from the following given data Standard enthalpy of formation of carbon dioxide ,water and methyl alcohol are -393.5kJ/mol and - 285.83kJ/mol and -238.86kJ/mol resply 11. Calculate the enthalpy of formation of methane from the following data C(g)+ O2(g) CO2(g) ∆H= -393.5kJ H2(g) + 1/2O2(g) H2O(l) ∆H= -285.8kJ CH4(g) + 2O2(g) CO2(g) +2H2O(l) ∆H=-890kJ 12. Calculate the total workdone when 1 mole of a gas expands isothermally and reversibly from an initial value of 20dm3 to a final value of 40dm3 at 298K 11. States of matter 1. Write any four postulates of Kinetic molecular theory. Ans: (i) Gases are made up of extremely small particles called atoms and molecules.  (ii) the volume occupied by molecule is negligible when compared to the total volume occupied by the gas (iii) There are no intermolecular force between the gas molecules (iv)The collisions are perfectly elastic. (v)The collision of gas molecule with the container walls exert the pressure. 2. State Boyle’s law. Give its mathematical form. Ans: ‘At constant temperature, the pressure of a fixed amount of gas inversely proportional to its volume’ 1 𝑃 ∝ (at const T) 𝑉 3. State Charle’s law. Give its mathematical form. Ans: ‘At constant pressure, the volume of a fixed amount of a gas is directly proportional to its absolute temperature’ 𝑉 ∝ 𝑇 (at const P) 4. Calculate the value of gas constant R in SI unit. Ans: One mole of a gas occupies 22.7 L (22.7× 10-3 m3) at STP ( 1 bar pressure (105 pascal) and 273.15 K temperature) We know that, ideal gas equation PV =nRT 𝑃𝑉 𝑅= 𝑛𝑇 (105 𝑝𝑎𝑠𝑐𝑎𝑙)×(22.7×10−3 𝑚3 ) 𝑅= (1𝑚𝑜𝑙)×(273.15𝐾) R= 8.314 J/K/mol 5. State Dalton’s law of partial pressure. Ans: It states that “ the total pressure exerted by a mixture of non-reactive gases is equal to the sum of the partial pressures exerted by individual gases at constant temperature and volume” 6.Write Vanderwaals equation for one mole of a gas and name any two terms in it. 𝑎 Ans: ( 𝑝 + 2 )(𝑉 − 𝑏) = 𝑅𝑇 𝑉 Where T is temperature, a and b are called vanderWaals constant. 7. Write any two differences between ideal and real gases. Ans: Real gases Ideal gases 1. Does not obey ideal gas 1. Obeys ideal gas equation equation 2. Can be liquefied 2. Cannot be liquified 3. There are weak force of 3. There are no intermolecular attraction between gas force of attraction between gas molecules molecules. 8. Write the expression for the compressibility factor (Z) for one mole of a gas and name the terms in it. What is the value of Z for an ideal gas ?  PV Ans: 𝑍 = Where P is pressure, V is volume and T is temperature RT For an ideal gas Z=1 12.Organic Chemistry-Some Basic Principles and Techniques: 1. Give an example for (i) Heterocyclic compound (ii) Alicyclic compound. Ans: (i) Furan, pyrrole, pyridine etc (ii) Cyclopropane, cyclobutane etc 2. Explain position isomerism with an example. Ans: Compounds having same molecular formula but differ in position of the same functional group. Example: (i) 1-butene and 2-butene (ii) propan-1-ol and propan-2-ol 3. Explain functional isomerism with an example. Ans: Compounds having same molecular formula but different functional group. Example: (i) propanone and propanal (ii) Dimethyl ether and ethyl alcohol 4. Explain Chain isomerism with an example. Ans: Compounds having same molecular formula but different number of carbon atoms in the parent chain Example: (i)n-butane and iso butane (ii) n-butanol and iso-butanol 5. Explain metamerism with an example. Ans: Compounds having same molecular formula but different alkyl groups on either side of the functional group. Example: Ethoxyethane and methoxy propane 6. What are nucleophiles ? Give an example. Ans: Electron rich species are called nucleophlies. Example: H2O, Cl-, OH- etc 7. What are electrophiles ? Give an example. Ans: Electron deficient species are called electrophiles. Example : H+, Cl+, AlCl3 etc 8. What is homologues series ? Give any three characteristics. Ans: Homologues series is a series of structurally related compounds differing by –CH2 group. Characteristics: (i) They can be prepared by similar methods. (ii) All the members of a series should have the same functional group. (iii) They have similar chemical properties 9. What is carbocation? Among alkyl carbocation, which one is more stable ? Ans: The positively charged ions in which carbon carries a positive charge. Ex: CH3 + Tertiary carbocation is more stable 10. How is sulphur detected using sodium fusion extract of the given compound ? Ans: On heating sodium fusion extract(SFE) with sodium nitroprusside , appearance of a violet color indicates the presence of sulphur. 11. How is nitrogen detected using sodium fusion extract of the given compound ? Ans: The sodium fusion extract is boiled with iron sulphate and then acidified with concentrated sulphuric acid. The formation of Prussian blue colour indicates the presence of nitrogen. 12. How do you estimate carbon and hydrogen in an organic compound using Liebig’s method? 13. Explain Carius method of estimation of halogens. 14. Write any two differences between resonance effect(mesomeric ) and inductive effect. Ans: Resonance effect Inductive effect 1. It take place in conjugated system 1. It take place in saturated system 2. It involves delocalization of pi electrons. 2. It does not involves delocalization of electrons. 3. It is a strong effect 3. It is weak effect 15. Write any two differences between inductive effect and electromeric effect. Ans: Inductive effect Electromeric effect 1. It is a permanent effect 1. It is a temporary effect 2. This occurs in saturated system 2. This occurs in unsaturated system 3.Attacking reagent is not required 3. Take place only in the presence of attacking reagent 16. For the compound CH=C -CH=CH -CH 3 (i) Write its complete structure (ii) Identify the number of sigma and pi bonds. (iii) Identify the hybridization of each carbon atom. (iv) Write the bond line formula of the compound (v) Mention whether the compound saturated or unsaturated. Br 17. For the compound CH3 -CH -CH 2 -CH3 (i) Write its bond line formula (ii) What is the hybridization of carbon attached to bromine. (iii) How many sigma bonds are present in it. Br. Ans: (i). (ii) Sp3 (iii) 13 13. s-block elements: 1. Write any two anomalous behaviour of lithium. 2. Write any two anomalous behaviour of beryllium. 3. Which alkali metal is strongest reducing agent? 4. Name the radioactive alkali metal. 5. Name the radioactive alkaline earth metal. 6. When carbon dioxide is passed through limewater ,it turns milky? Give the chemical reaction. 7. How does milk of lime reacts with chlorine? Write the chemical reaction.  8. Write the chemical formula of plaster of paris. 9. Explain the preparation of sodium hydroxide by Castner Kellenr cell. TOO Important Questions: 1. Write any three postulates of Bohr’s atomic theory 2. Write any two limitations of Bohr’s atomic theory. 3. Write any three postulates of kinetic molecular theory of gases. 4. Mention the significance of each four quantum numbers. 5. Calculation of empirical and molecular formula. 6. Explain sp or sp2 or sp3 hybridisation with an example. 7. Write the electronic configuration of Li2 or He2 or N2 or O2 and calculate its bond order. 8. Define ionisation enthalpy, electronegativity or electron gain enthalpy. How does it vary along a period and down the group ? 9. Balance the redox equation using oxidation number method. 10. Explain the mechanism of nitration of benzene or chlorination of benzene. 11. Explain position , chain and functional isomerism with an example. 12. Explain Wurtz, Friedel craft and dehydrohalogenation reaction with an example. 13. Write any two differences between diamond and graphite. 14. Write any two differences between pi bond and sigma bond. 15. Write any two differences between electromeric effect and inductive effect. 16. State Boyle’s law, Charle’s law, Markonikov’s rule, Lechateliers principle, modern periodic law. 17. What are isoelectronic species ? Give an example. 18. What is common ion effect and buffer solution. Example 19. Define Lewis base and acid, Bronsted base and acid, conjugate acid base pair. 20. Define entropy and write its SI unit 21. Intensive property and extensive property. Example 22. Enthalpy calculation problem 23. Define Hydrogen bond.Example. 24. Scientific notation, significant numbers, 25. Molarity , molality 26. Temporary hardness and permanent hardness, 27. Anomalous behaviour of lithium and beryllium 28. Estimation of C and H by Liebigs method.