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HALF YEARLY EXAMINATION 2017-18CLASS XI SUB : CHEMISTRYBLUE PRINT S NO NAME OF THE UNITVSA1 MARKSVSA 2 MARKSSA 3 MARKSVALUE BASED 4 MARKSLA 5 MARKSTOTAL MARKS1BASIC CONCEPTS OF CHEMISTRY1(1)1(2)1(3)1(4)?102STRUCTURE OF ATOM?1(2)3(9)??113CLASSIFICATION OF ELEMENTS & PERIODICITY IN PROPERTIES ?1(2)2(6)??84CHEMICAL BONDING &MOLECULAR STRUCTURE ??2(6)?1(5)115STATES OF MATTER2(2)?2(6)??86THERMODYNAMICS1(1)1(2)1(3)?1(5)117EQUILIBRIUM1(1)1(2)1(3)?1(5)118??????709TOTAL NO OF QUESTIONS (26)551213? (B K SHARMA PGT CHEMISTRY K V BHEL JAGDISHPUR)1.Some Basic Concepts of Chemistry 1. Round off up to 3 significant figure (a) 1.235( b) 1.225 Ans. (a) 1.24 (b) 1.222. What is the S.I. unit of Density? 3. What do mean by Mole fraction? 4. Define one mole? Ans. One mole is the amount of a substance that contains as many particles as there are atoms in exactly 12 g of the carbon-12. 5. State the number of significant figures in each of the following: (i) 208.91 (ii) 0.00456 (iii) 453 (iv) 0.346 6. How are 0.50 mol Na2CO3 and 0.50 M Na2CO3 different? 7.What is the percentage of carbon, hydrogen and oxygen in ethanol? Ans C=52.14% O=34.73% 8. What do mean by molarity .Calculate the molarity of NaOH in the solution prepared by dissolving its 4 g in enough water to form 250 mL of the solution. Ans. 0.4 M 9. Define –(a) Average atomic mass (b) Molecular mass (c) Formula mass 10. Express the following in the scientific notation with 2 significant figures- (a) 0.0048 (b) 234,000 (c) 200.0 11. Calculate the number of atoms in each of the following (i) 52 moles of Ar (ii) 52 u of He (iii) 52 g of He Ans. (i) 3.131 × 1025 atoms of Ar (ii) 13 atoms of He (iii) 78.286 x 1023 atoms of He 4 12. What is the difference between empirical and molecular formula? A compound contains 4.07 % hydrogen, 24.27 % carbon and 71.65 % chlorine. Its molar mass is 98.96 g. What are its empirical and molecular formulas? Ans. molecular formula is C2H4Cl2 13.Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation: N2(g) + H2(g) → 2NH3(g) (i) Calculate the mass of ammonia produced if 2.00 × 103 g dinitrogen reacts with 1.00 × 103 g of dihydrogen. (ii) Will any of the two reactants remain unreacted? (iii) If yes, which one and what would be its mass? 14. A welding fuel gas contains carbon and hydrogen only. Burning a small sample of it in oxygen gives 3.38 g carbon dioxide, 0.690 g of water and no other products. A volume of 10.0 L (measured at STP) of this welding gas is found to weigh 11.6 g. Calculate (i) empirical formula, (ii) molar mass of the gas, and (iii) molecular formula. 15. What is the difference between 160 cm and 160.0 cm 16. In the combustion of methane, what is the limiting reactant and why? 17. What is AZT? Ans. AzidothymidineBASIC CONCEPTS OF CHEMISTRY (VALUE BASED QUESTIONS)Q1. Two friends Riya and Pooja were discussing that which is better for expressing the concentration of a solution: Molality or Molarity ?Pooja told Riya that Molality is considered better for expressing the concentration as compared to Molarity and explained the reason as well.What would be the explanation of Pooja?(ii) What are the units of molarity & molality?(iii) What is the difference between molality & molarity?Q2. Mohan learnt the term mol in his chemistry class. He discussed the term mol with her elder sister Anshika. Anshika explained about and then Mohan got satisfied.What was the probable answer given by Anshika ?What for term mol stands?What values are associated with Anshika?Q3.Radhika ,Supriya and Hema were asked by the PGT chemistry to find the mass of a metal piece independently one by one using the same balance and same weight box. Each student was asked to take three observations. The students reported their result as shown in the following table:If the actual mass of the metal piece is 1.325g and the permitted uncertainty in the measurement is 0.001g, answer the following questions:Whose measurement is both accurate and precise? Justify your answer.Whose measurement is precise and not accurate Justify your answer?Whose measurements are neither accurate nor precise? Justify your answer. Mention the associated value or values with these observations.2.Structure of Atom 1 Neutrons can be found in all atomic nuclei except in one case. Which is this atomic nucleus and what does it consists of? Ans. Hydrogen atom. It consists of only one proton. 2. Calculate wave number of yellow radiations having wavelength of 5800 A0. 3. What are the values of n and l for 2p orbital? Ans. n=2 and l= 1 4. Which of the following orbitals are not possible? 1p, 2s, 3f and 4d Ans. 1p and 3f are not possible. 5. Write the electronic configuration of the element having atomic number 24,296. State Pauli Exclusion Principle. 7. When α- rays hit a thin foil of gold, very few α- particles is deflected back. What does it prove? Ans. There is a very small heavy body present within the atom. 8. What is the difference between a quantum and a photon? Ans. The smallest packet of energy of any radiation is called a quantum whereas that of light is called photon. 9.Write the complete symbol for the atom with the given atomic number (Z) and mass number(A). (a) Z = 17, A = 35 (b) Z = 92 , A = 233 10. Using s,p,d and f notation, describe the orbital with the following quantum numbers- 11.How many electrons in an atom have the following quantum numbers? a. n=4, ms= -1/2 b. n =3 , l=o Ans. (a) 16 electrons (b) 2 electrons. 12. An element with mass number 81 contains 31.7 % more neutrons as compared to protons. Assign the atomic symbol. 13. (i) The energy associated with the first orbit in the hydrogen atom is -2.18 x 10-18J/atom. What is the energy associated with the fifth orbit (ii) Calculate the radius of Bohr’s fifth orbit for hydrogen atom. 14. (a)What is the lowest value of n that allows g orbitals to exist? (b)An electron is in one of the 3d orbitals, Give the possible values of n,l and ml for this electron. Ans.(a) minimum value of n= 5 (b)n=3, l=2, ml = -2, -1, 0, +1, +2 15. State (a)Hund’s Rule of maximum Multiplicity (b) Aufbau Principle (c) n+l rule 16. Write the 3 points of difference between orbit and orbital.17.State Heisenberg’s uncertainty principle. Calculate the uncertainty in the position of an electron if the uncertainty in its velocity is 5.7 x 105 m/s. 18. An atom of an element contains 29 electrons and 35 neutrons. Deduce (i)the number of protons and (ii) the electronic configuration of the element (iii) Identify the element . 19. State photo electric effect. The work function for caesium atom is 1.9 eV. Calculate (a) the threshold wavelength and (b) the threshold frequency of the radiation. If the caesium element is irradiated with a wavelength 500 nm, calculate the kinetic energy and the velocity of the ejected photoelectron. 20. Arrange the electron (e), protons (p) and alpha particle (α) in the increasing order for the values of e/m (charge/mass). Ans.. α<p < e3.Classification of Elements Q1. Select the species which are iso-electronic (same number of electron) with each other. (1) Ne (2) Cl- (3) Ca2+ (4) Rb+ Q.2. What the elements of a group have common among them? Ans- They has same number of electrons in the valence shell. Q.3. What the s- and p- block elements are collectively called? Ans- Representative elements. Q.4. State the modern periodic law. Ans- The physical and chemical properties of the elements are the periodic function of their atomic numbers. Q.5. Name the groups of elements classified as s-, p- and d- blocks. Ans- s- block = 1,2 (including He), p- block= 13 to 18 (except He), d- block= 3 to 12. Q.6. Define the term ionisation enthalpy. Ans- The energy required to remove the outer most electron from the valence shell of an isolated gaseous atom is called as ionisation enthalpy. Q.7.In how many groups and periods the elements in modern periodic table are classified? Ans- In 18 groups and 7 periods.Q.8. Describe the two merits of long form periodic table over the Mendeleev’s periodic table? Q.9. It relates the position of an element in the periodic table with its electronic configuration. Q.10. What is a period in the periodic table? How do atomic sizes change in a period with an increase in atomic number? Ans- The horizontal rows in periodic table are called as periods. The atomic sizes decrease in a period with an increase in atomic number. Q.11. What is meant by periodicity in properties of elements? What is the reason behind this? Q.12. How do atomic radii vary in a group and a period? Ans- In group- Atomic size increases on moving from top to bottom. In period- Atomic size decreases on moving left to right in a period. Q.13. Arrange the following in the order of increasing radii: (a) I, I+, I- (b) O, N,P Ans- (a) I+< I < I+ (b) O < N< P14. Name the factors which affect the ionisation enthalpy of an element. Ans- (i) Size of atom or ion (ii) Nuclear charge (iii) Electronic configuration (iv) Screening effect (v) Penetration effect of the electrons Q.15. Noble gases have zero electron gain enthalpy values. Explain. Ans- Because the outer most shell of noble gases is completely filled and no more electrons can be added. Q.16. The first ionisation enthalpy of magnesium is higher than that of sodium. On the other hand, the second ionisation enthalpy of sodium is very much higher than that of magnesium. Explain. Q.17. Explain why are cations smaller and anions larger in size than their parent atoms? Q.18. Consider the following species: N3–, O2–, F–, Na+, Mg2+ and Al3+ (a) What is common in them? (b) Arrange them in the order of increasing ionic radii. Ans- (a) the same number of electrons (10 electrons). Hence, the given species are isoelectronic. (b) Al3+< Mg2+< Na+< F–< O2–< N3–4-Chemical Bonding Q.1. What is the total number of sigma & pi bonds in the following ? (a) C2H2 (b) C2H4 Q.2. Write the significance of a plus and a minus sign shown in representing the orbitals. Ans- Molecular orbitals are represented by wave functions. A plus sign in an orbital indicates a positive wave function while a minus sign in an orbital represents a negative wave function. Q.3. How do you express the bond strength in terms of bond order? Q.4. Arrange the bonds in order of increasing ionic character in the molecules: LiF, K2O, N2, SO2 and ClF3. Ans- N2< SO2< ClF3< K2O < LiF. Q.5. Which type of bond is formed when the atoms have zero difference in electronegativity? Ans- Covalent bond.Q.6. Define hydrogen bond. Is it weaker or stronger than the van der Waals forces? Q.7. Although geometries of NH3 and H2O molecules are distorted tetrahedral, bond angle in water is less than that of ammonia. Discuss.Q.8. Which out of NH3 and NF3 has higher dipole moment and why?Q.9. Explain the important aspects of resonance with reference to the CO32-ion.Q10. Write the resonance structures for SO3, NO2 .Q.11. Although both CO2 and H2O are triatomic molecules, the shape of H2O molecule is bent while that of CO2 is linear. Explain this on the basis of dipole moment.Q.12. Use molecular orbital theory to explain why the Be2 molecule does not exist.Q13. Write the Lewis dot structure of CO molecule.Q.14. Write the Lewis structure of the nitrite ion and ozone also calculate formal charge.Q.15. Distinguish between a sigma and a pi bond.Q.16. Draw diagrams showing the formation of a double bond and a triple bond between carbon atoms in C2H4 and C2H2 molecules.Q.17. Describe the hybridisation in case of PCl5. Why are the axial bonds longer as compared to equatorial bonds?Q.18. What is meant by the term bond order? Calculate the bond order of: N2, O2, and.O2+ O2-Also compare the relative stability of the following species and indicate their magnetic propertiesQ.19. Discuss the shape of the following molecules using the VSEPR model: BeCl2, BCl3, SiCl4, AsF5, H2S, PH3Q.20. Which hybrid orbitals are used by carbon atoms in the following molecules? CH3–CH3; (b) CH3–CH=CH2; (c) CH3-CH2-OH; (d) CH3-CHO (e) CH3COOHQ.21. Apart from tetrahedral geometry, another possible geometry for CH4 is square planar with the four H atoms at the corners of the square and the C atom at its centre. Explain why CH4 is not square planar?Q.22. Describe the change in hybridisation (if any) of the Al atom in the following reaction. AlCl3+Cl- AlCl4-Q.23Is there any change in the hybridisation of B and N atoms as a result of the followingreaction ? BF3 ??NH3 ?????F B3NH35-States of Matter 1. At what condition surface tension vanishes? Ans- (At critical temperature)2. Why Helium is used in balloons in place of hydrogen? Ans-(He is incombustible)3. At what temperature below which a gas does not obey ideal gas law? (Below Boyle Temperature)4. At what temperature the volume of a gas is supposed to be zero? (At absolute zero temp.)5 What is the molar volume at 0oC and 1 bar pressure? (22400 ml.)6. Name the temp. above which a gas can’t be liquefied by any amount of pressure. (Tc)7. What is the effect of increase of temp.on surface tension and viscosity in a liquid? (Both decreases)8. In terms of Charles’ law explain why –273 °C is the lowest possible temperature.9. Why vegetables are cooked with difficulty at hill station. 10. What is the value of Z (compressibility factor) for an Ideal gas? (For ideal gas Z=1)Q.11 How do you convert pressure in atmosphere in to SI unit.(1atm = 101325 Pa or Nm-2, 1 bar = 105 Pa)Q.12 What type graph will you get when PV is plotted against P at constant temperature. Q.13 What would have happened to the gas if the molecular collisions were not elastic? Q.14 At a particular temperature, why is vapour pressure of acetone less than of ether? Q.15 Why liquids diffuse slowly as compared to gases? Q.16 What would be the SI unit for quantity PT2V2/n ? (Nm4K2mol-1)Q.17 Why does sharpened edge becomes smooth on heating up tomelting point? Ans On heating the glass it melts and take up rounded shape at edges which has minimum surface area. b/c of surface tension. Q.18 For real gases the relation b/w P,V,T is given by vander Waal’s equation, write it for n moles? Q.19 What correction is applied to obtain pressure of dry gas with the total pressure & aqueous tension? (P(dry gas) = P(Total) - Aqueous tension)Q.20 Name two phenomena that can be explained on the basis of surface tension.Q.21 Calculate temperature of 4.0 moles of gas occupying 5dm3 volume at 3.32 bar. (R= 0.083 bar dm3 k-1 mol-1)Q.22 Critical temperature of CO2 and CH4 gases are 31.10C and - 81.90C respectively. Which of these has strong intermolecular forces & why?Q.23 Calcutate the total pressure in mixture of 4g of O2 and 2gm. Of H2 can fixed to a total volume of IL at 0o C. (R = 0.0821) L atm. Mol-1Q.24 A mixture of dihydrogen and dinitrogen at 1 bar pressure contains 20% by weight of H2. Calculate partial pressure of H2.Q25. Pressure of 1 g of an ideal gas A at 27 °C is found to be 2 bar. When 2 g of anotherideal gas B is introduced in the same flask at same temperature the pressure becomes 3 bar. Find a relationship between their molecular masses.Q26 The drain cleaner, Drainex contains small bits of aluminum which react with caustic soda to produce dihydrogen. What volume of dihydrogen at 20 °C and one bar will be released when 0.15g of aluminum reacts?Q.27. (a)Why aerated water bottles kept under water during summer? (b) Which property of liquid is responsible for spherical shape of drop? (c) Why is moist air lighter than dry air? (d) Define aqueous tension? (e) What is units of a and b which are vander waal’s constant? Ans (a) To reduce temperature so to reduce pressure, other wise bottle may burst. (b) Surface Tension. (c) Moist air has water vapours which lowers vapour density, so it is lighter. (d) It is pressure of water vapours at given T. (e)Unit of a in atm. L2mol-2, b is L mol-1.6-Thermodynamics 1. State First Law of thermodynamics. 2. What is a thermodynamic state function? 3. Give enthalpy (H) of all elements in their standard state.(In standard state enthalpies of all elements is zero)4. From thermodynamic point to which system the animals and plants belong? (Open system)5. Predict the sign of Δ S for the following reaction: CaCO3(s) → CaO (s) + CO2 (g) (ΔS is positive or entropy increases) 6. For the reaction, Cl2(g) → 2 Cl (g); What will be the sign of ΔH and Δ S? (Both -ve)7. State Hess’s Law for constant heat summation? 8. What is Gibb’s Helmhaltz equation? (Δ G = Δ H – T Δ S )9. Define extensive properties. 10. A real crystal has more entropy than an Ideal Crystal. Why?11. Given: N2(g) + 3 H2 (g) → 2 NH3 (g); ΔrH0 = - 92.4 kJmol-1. What is the standard enthalpy of formation of NH3(g) ? (46.2 kJ mol-1)12. Predict the entropy change in- (i) A liquid crystallizes into solid (Entropy decreases)(ii) Temperature of a crystallize solid raised from OK to 115K (Entropy increase)13. Why standard entropy of an elementary substance is not zero whereas standard enthalpy of formation is taken as zero? 14. Many thermodynamically feasible reactions do not occur under ordinary conditions. Why? Note:- Question from NCERT BOOK 6.5,6.11,6.14,6.15,6.17,6.197-Equilibrium 1. Mention the factors that affect equilibrium constant. Ans. Temperature, pressure, and molar concentration of reactants and products, catalyst.2. Write conjugate acids of H2O & NH3. 3. Write Kc for the gaseous reaction- N2 + 3H2? 2NH34. Out of H2O & H3O+which is stronger acid?5. Write relationship between Kp and Kc for the gaseous reaction - N2 + O2? 2NO6. What is effect of catalyst on equilibrium constant ?Kc?? 7. What is meant by conjugate acid –base pairs? Ans. The acid base pair that differs only by one proton is called conjugate acid base pair. 8. Classify the following bases as strong and weak bases: NaHCO3, NaOH, KOH, Ca(OH)2, Mg(OH)2. Ans:-strong base: NaOH, KOH ; weak bases: NaHCO3,Ca(OH)2, Mg(OH)2. 9.The conc.of H+ion in a sample of soft drink is 3.8 × 10–3M. What is its pH ? Ans: 2.42 10. The species: H2O, HCO3–, HSO4– and NH3 can act both as Bronsted acids and bases.For each case give the corresponding conjugate acid and conjugate base.11. Explain Lewis acids and bases with suitable examples. 12. Describe the effect of : a) addition of H2 ,b) addition of CH3OH ,c) removal of CO d) removal of CH3OH on the equilibrium of the reaction: 2H2(g) + CO (g )?CH3OH (g)13. A mixture of 1.57 mol of N2, 1.92 mol of H2 and 8.13 mol of NH3 is introduced into a 20 L reaction vessel at 500 K. At this temperature, the equilibrium constant,Kc for the reaction N2 (g) + 3H2 (g) ? 2NH3 (g) is 1.7 × 102. Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?Note:- Question from NCERT BOOK Solved and Unsolved ................
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