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1 Bal Bharati Public School,Pitampura HALF YEARLY EXAMINATION CHEMISTRY CLASS-11 th CODE--A Q1Arrange the following molecules in order of increasing covalent character LiCl, LiF, LiBr,LiI Q2 What is the compressibility factor for an ideal gas? Q3 Predict the position of the element in the periodic table having electronic configuration (n-1)d 3 ns 2 for n = 5 Q4 Give any two differences between electron gain enthalpy and electron negativity. Q5 Which of the following will have most negative electron gain enthalpy P, S, Cl, F Q6 Write all the quantum numbers for the 21 st electron of Scandium ( Z= 21) Q7 How many unpaired electrons are present in Cr ( Z= 24) Q8 Name any two green house gases. Q9 Calculate the number of Cl - ions in 100 ml of 0.001M HCl solution. Q10 a) How are 0.50 m Na 2 CO 3 and 0.5 M Na 2 CO 3 different? b) Write the electronic configuration of Cu 2+ ( Z = 29 ) Q11 a) How many electrons in a given atom can have the following quantum number n = 3,l=1 b) Calculate the mass of one atom of silver ( Z = 108 ) Q12a) Write a short note on green house effect? b) What is the cause of ozone depletion state any two harmful effects of ozone depletion? Q13a) Define Law of multiple proportion b) What is the number of molecules present in 18mg of water? Q14 a) List any two properties of Lithium in which it resembles magnesium. What is this relationship called? b) State any two reasons for anomalous behaviour of second period elements Q15 a) What is smog? b) State any two harmful effects of smog? Q16Give reasons for the following: a) Ionisation enthalpy of Be is higher than B b) Size of cation is smaller than that of the neutral atom Q17a) What are transition elements? State any two characteristics of these elements. b) State any merits of Mendeleev periodic table Q18a) What are isoelectronic ions? b) Arrange the following in order of decreasing size O 2-, Mg 2+, F -, Na + Q19 A,B,C are three elements B is an inert gas other than helium. Complete the following table and answer the questions: Element Atomic No. No. Of electrons in the valence shell and group No A Z -- 1 B Z C Z + 1
2 a) Electron affinity of B is zero b) Ionization enthalpy of element C is less than that of element A Q20 Give reasons for the following: a) It is not possible to cool the gas to 0 K b) Vegetables are cooked with difficulty at a hill station. c) The liquid drops assume a spherical shape Q21 The density of 3 molal solution of NaOH is 1.110gml-1.Calculate the molarity of the solution Q22 At 273 K the density of a gaseous oxide at 2 bar is same as that of nitrogen at 5 bar. Calculate the molecular mass of the oxide. Q23 Draw the structures and predict the shape of the following molecules on the basis of VSEPR theory AsF5, BrF5, XeF2. Q24 a) Dipole moment of NH3 is higher than NF3.Explain b) Calculate the formal charge on each atom of NO2 c) Draw Lewis structure to show bonding in HNO3 molecule. Q25 When a photon of frequency 1.0 x 1015 s-1 was allowed to hit a metal surface, an electron having x 10-19J of kinetic energy was emitted. Calculate the threshold frequency of the metal. Show that an electron will not be emitted if a photon of wavelength 600 nm hits the metal surface. Q26 Calculate the wave number for the longest wavelength transition in the Balmer series of atomic hydrogen. Q27a) What mass of solid silver chloride is obtained when 25ml of M AgNO3 reacts with excess of aqueous HCl?( atomic mass of Ag = 108,N = 14,Cl = 35.5,O = 16) b) What volume of 36M and 1M sulphuric acid must be mixed to get 1L of 6M sulphuric acid? Q28 A 4.24mg sample of compound A is completely burnt. It gives 8.45mg of CO2 and 3.46mg of H2O.The molecular mass of the compound was found to be 88u.What is the molecular formula of the compound. Q29a) Give any two difference between real gases and an ideal gas. b) Explain the significance of Vander Waal constants a & b and also give their unit? c) A gas balloon has a volume of 0.5 dm3 at 100 C and 1 bar pressure. What will be the volume of the balloon at 0 C. (assume no change in pressure) Q30 a) Describe the valence bond theory of covalent bond formation by taking an example of hydrogen. b) Arrange the following bonds in order of increasing ionic character N---H, F---H, C---H and O---H c) Draw Lewis structure to show bonding between X and Y ( Atomic no. of X = 13, Y= 7 ).Write the formula of t he compound formed. Q31 Why energy of an electron in an atom is negative? b) Half filled and completely filled orbitals have maximum stability.explain with the help of an example c)calculate de-broglie wavelength of an electron (mass = 9.1 x kg) moving at 1% speed of light.( h = 6.63 x kg m2 s-1)
3 Bal Bharati Public School,Pitampura HALF YEARLY EXAMINATION CHEMISTRY CLASS-11 th CODE--B Q1 Which of the following will have most negative electron gain enthalpy P, S, Cl, F Q2 Predict the position of the element in the periodic table having electronic configuration (n-1)d 3 ns 2 for n = 5 Q3 Give any two differences between electron gain enthalpy and electron negativity. Q4 Arrange the following molecules in order of increasing covalent character LiCl, LiF, LiBr,LiI Q5 What is the compressibility factor for an ideal gas? Q6 Name any two green house gases Q7 How many unpaired electrons are present in Cr ( Z= 24) Q8 Write all the quantum numbers for the 21 st electron of Scandium ( Z= 21) Q9 a) Write a short note on green house effect? b) What is the cause of ozone depletion state any two harmful effects of ozone depletion. Q10a) Define Law of multiple proportion b) What is the number of molecules present in 18mg of water? Q11 a) How are 0.50 m Na 2 CO 3 and 0.5 M Na 2 CO 3 different? b) Write the electronic configuration of Cu 2+ ( Z = 29 ) Q12 a) How many electrons in a given atom can have the following quantum number n = 3,l=1 b) Calculate the mass of one atom of silver ( Z = 108 ) Q13 Calculate the number of Cl - ions in 100 ml of 0.001M HCl solution Q14a)What are transition elements? State any two characteristics of these elements. b) State any two merits of Mendeleev periodic table Q15 a) List any two properties of Lithium in which it resembles magnesium. What is this relationship called? b) State any two reasons for anomalous behaviour of second period elements Q16 a) What is smog? b) State any two harmful effects of smog? Q17Give reasons for the following: c) Ionisation enthalpy of Be is higher than B d) Size of cation is smaller than that of the neutral atom
4 Q18 A,B,C are three elements B is an inert gas other than helium. Complete the following table and answer the questions: Element Atomic No. No. Of electrons in the valence shell and group No A Z -- 1 B Z C Z + 1 a) Electron affinity of B is zero b)ionization enthalpy of element C is less than that of element A Q19 Give reasons for the following: d) It is not possible to cool the gas to 0 K e) Vegetables are cooked with difficulty at a hill station. f) The liquid drops assume a spherical shape Q20a) What are isoelectronic ions? b) Arrange the following in order of decreasing size O2-, Mg2+, F-, Na+ Q21 a) Dipole moment of NH3 is higher than NF3.Explain b) Calculate the formal charge on each atom of NO2 c) Draw Lewis structure to show bonding in HNO3 molecule Q22 Draw the structures and predict the shape of the following molecules on the basis of VSEPR theory AsF5, BrF5, XeF2. Q23 The density of 3 molal solution of NaOH is 1.110gml-1.Calculate the molarity of the solution Q24 At 273 K the density of a gaseous oxide at 2 bar is same as that of nitrogen at 5 bar. Calculate the molecular mass of the oxide. Q25a) What mass of solid silver chloride is obtained when 25ml of M AgNO3 reacts with excess of aqueous HCl?( atomic mass of Ag = 108,N = 14,Cl = 35.5,O = 16) b) What volume of 36M and 1M sulphuric acid must be mixed to get 1L of 6M sulphuric acid? Q26 A 4.24mg sample of compound A is completely burnt. It gives 8.45mg of CO2 and 3.46mg of H2O.The molecular mass of the compound was found to be 88u.What is the molecular formula of the compound Q27 When a photon of frequency 1.0 x 1015 s-1 was allowed to hit a metal surface, an electron having x 10-19J of kinetic energy was emitted. Calculate the threshold frequency of the metal. Show that an electron will not be emitted if a photon of wavelength 600 nm hits the metal surface. Q28 Calculate the wave number for the longest wavelength transition in the Balmer series of atomic hydrogen. Q29 a) Describe the valence bond theory of covalent bond formation by taking an example of hydrogen. b) Arrange the following bonds in order of increasing ionic character N---H, F---H, C---H and O---H c) Draw Lewis structure to show bonding between X and Y ( Atomic no. of X = 13, Y= 7 ).Write the formula of t he compound formed.
5 . Q30a) Why energy of an electron in an atom is negative? b) Half filled and completely filled orbitals have maximum stability.explain with the help of an example c)calculate de-broglie wavelength of an electron (mass = 9.1 x kg) moving at 1% speed of light.( h = 6.63 x kg m2 s-1) Q31a) Give any two difference between real gases and an ideal gas. b) Explain the significance of Vander Waal constants a & b and also give their unit? c) A gas balloon has a volume of 0.5 dm3 at 100 C and 1 bar pressure. What will be the volume of the balloon at 0 C. (assume no change in pressure)
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