Q1. What is the wavelength in nm and the frequency of light emitted when the electron in the hydrogen atom undergoes transition from an energy level with n=4 to an energy level with n=2? In which region of the electromagnetic spectrum will this line lie? (Rydberg constant =109,677cm-1) Q2. The electronic configurations of some neutral atoms are given below:1s2 2s2 (ii) 1s2 2s2 2p1 (iii) 1s2 2s2 2p4 (iv) 1s2 2s2 2p3. Q3. After writing their orbital electronic configuration, find the number of unpaired electrons present in phosphorus (Z=15) Chromium (z=24) and copper (Z=29). Q4. Which of these electronic configuration would be expected to have the highest:IE1 b) IE2 c) IE3 d) IE4. Q5. the following in order of decreasing Van der Waals’ radii: Cl, H, O, N. Explain. Q6. Arrange the following in order of increasing radii: a) I, I+, I- b) C, N, Si, P c) O2-, N3-, S2-, F-. Q7. Estimate the difference in energy between the first and the second Bohr orbit for a hydrogen atom. At what minimum atomic number, a transition from n=2 to n=1 energy level would results in the emission of X-rays with ʎ=3*10^-8 m? Which hydrogen-like species does the atomic number correspond to?Q8. Calculate the wavelength of the radiation emitted producing a line in the Lyman series when an electron falls from fourth stationary state in hydrogen atom. (RH=1.1*10^7 m-1). Q9. Arrange the elements with the following electronic configurations in order of increasing electron affinity. 1s2 2s2 2p5 (ii) 1s2 2s2 2p4 (iii) 1s2 2s2 2p3 (iv) 1s2 2s2 2p6 3s2 3p4. Q10. Arrange the following elements in order of decreasing electron affinity: B, C, N and O. Q11. A solid mixture weighing 5.00 g containing lead nitrate and sodium nitrate was heated below 6000C until the mass of the residue was constant. If the loss of mass is 28%, find the mass of lead nitrate and sodium nitrate in the mixture. (Atomic weights of Pb=207, Na=23, N=14, O=16). (1/60) Q12. Calculate the volume of hydrogen liberated at STP when 500 cm3 of 0.5 N sulphuric acid reacts with excess of zinc. (H=1, O=16, S=32). (1/61) Q13. One litre of oxygen at STP is made to react with 3 litres of carbon monoxide at STP. Calculate the weight of each substance found after the reaction. Which one is the limiting reactant? (1/62) Q14. Concentrated sulphuric acid is 98% by mass and has a density of 1.84 gcm-3. What volume of the concentrated acid is required to make 5.0 L of 0.500 M H2SO4 solution? Q15. 0.01 M solution of acetic acid is 1.34% ionized at 298K. What is the ionization constant of acetic acid?Q16. A 0.01M ammonia solution has the degree of dissociation of 0.0135. Calculate the concentrations of NH4+ and HO- formed and the dissociation constant Kb. Q17. Balance the following redox equation using redox half equation method:K2Cr2O7 (aq) + 3 SO2(g) + H2SO4 (aq) -- Cr2(SO4)3 + K2SO4 (aq) + H2O (l)HNO3 (aq) + I2 (aq) - NO2 (g) + HIO3 (aq) + 4 H2O (l) 2 FeCl2 (aq) + 2 HCl (aq) + H2SO4 (aq) -- FeCl3 (aq) + SO2 (g) + H2O (l)

Question

Q1. What is the wavelength in nm and the frequency of light emitted when the electron in the hydrogen atom undergoes transition from an energy level with n=4 to an energy level with n=2? In which region of the electromagnetic spectrum will this line lie? (Rydberg constant =109,677cm-1) Q2. The electronic configurations of some neutral atoms are given below:1s2 2s2  (ii) 1s2 2s2 2p1   (iii) 1s2 2s2 2p4  (iv) 1s2 2s2 2p3. Q3. After writing their orbital electronic configuration, find the number of unpaired electrons present in phosphorus (Z=15) Chromium (z=24) and copper (Z=29). Q4. Which of these electronic configuration would be expected to have the highest:IE1  b) IE2    c) IE3     d) IE4. Q5. the following in order of decreasing Van der Waals’ radii: Cl, H, O, N. Explain. Q6. Arrange the following in order of increasing radii: a) I, I+, I-   b) C, N, Si, P   c) O2-, N3-, S2-, F-. Q7. Estimate the difference in energy between the first and the second Bohr orbit for a hydrogen atom. At what minimum atomic number, a transition from  n=2 to n=1 energy level would results in the emission of X-rays with ʎ=3*10^-8 m? Which hydrogen-like species does the atomic number correspond to?Q8. Calculate the wavelength of the radiation emitted producing a line in the Lyman series when an electron falls from fourth stationary state in hydrogen atom. (RH=1.1*10^7 m-1). Q9. Arrange the elements with the following electronic configurations in order of increasing electron affinity.  1s2 2s2 2p5  (ii) 1s2 2s2 2p4   (iii) 1s2 2s2 2p3   (iv) 1s2 2s2 2p6 3s2 3p4. Q10. Arrange the following elements in order of decreasing electron affinity: B, C, N and O. Q11. A solid mixture weighing 5.00 g containing lead nitrate and sodium nitrate was heated below 6000C until the mass of the residue was constant. If the loss of mass is 28%, find the mass of lead nitrate and sodium nitrate in the mixture. (Atomic weights of Pb=207, Na=23, N=14, O=16). (1/60) Q12. Calculate the volume of hydrogen liberated at STP when 500 cm3 of 0.5 N sulphuric acid reacts with excess of zinc. (H=1, O=16, S=32). (1/61) Q13. One litre of oxygen at STP is made to react with 3 litres of carbon monoxide at STP. Calculate the weight of each substance found after the reaction. Which one is the limiting reactant? (1/62) Q14. Concentrated sulphuric acid is 98% by mass and has a density of 1.84 gcm-3. What volume of the concentrated acid is required to make 5.0 L of 0.500 M H2SO4 solution? Q15.  0.01 M solution of acetic acid is 1.34% ionized at 298K. What is the ionization constant of acetic acid?Q16. A 0.01M ammonia solution has the degree of dissociation of 0.0135. Calculate the concentrations of NH4+ and HO- formed and the dissociation constant Kb. Q17. Balance the following redox equation using redox half equation method:K2Cr2O7 (aq) + 3 SO2(g) + H2SO4 (aq) -- Cr2(SO4)3 + K2SO4 (aq) + H2O (l)HNO3 (aq) + I2 (aq) - NO2 (g) + HIO3 (aq) + 4 H2O (l) 2 FeCl2 (aq) + 2 HCl (aq) + H2SO4 (aq) -- FeCl3 (aq) + SO2 (g) + H2O (l)

Accepted Answer

Since you have asked multiple question, we will solve the first questionfor you. If you want any…