Board exam two mark questions in Periodic Classification Of Elements

11th Standard

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Chemistry

Answer any 50 of the following questions
Time : 01:30:00 Hrs
Total Marks : 100

    Part - A

    58 x 2 = 116
  1. The ionisation energy is directly related to metallic character. Explain the variation of metallic character along the period and in the group.

  2. Explain the nature of oxides formed by metals and non metals.

  3. How does the basic and acidic nature of oxides vary along a period and in group?.

  4. How is ionisation energy related to the metallic character? How does the basic nature of hydroxides of alkaline earth metals very down the group?

  5. Account for the difference in size of Na +(95 pm) and Mg+2(65pm) both of which have the same noble gas configuration

  6. Which of the following will have the most electron gain enthalpy and which the least electro negative? P, S, CI, F Explain your answer

  7. Show by chemical reaction, with water, that Na2O is a basic oxide and Cl2O7 is an acidic oxide

  8. What is the basic difference in approach between Mandeleev's periodic law and modem periodic law.

  9. In terms of period and group where would you locate the element with Z = 114

  10. Give the IUPAC names and symbols of the following elements with atomic numbers 123, 126, 134, 148, 150

  11. Calculate the screening constant in Zinc for (i) 4s electron, (ii) for a 3d electron. The electronic configuration of Zinc (30) is (ls)2 (2s, 2p)(3s,3p)8 (3d10) (4s)2

  12. What is the basic difference in approach between Mendeleev's periodic table and modern periodic table?

  13. The element with atomic number 120 has not been discovered so far. What would be the IUPAC name and the symbol for this element? Predict the possible electronic configuration of this element.

  14. Predict the position of the element in periodic table satisfying the electronic configuration (n-l}d2, ns2 where n =5

  15. The first ionisation energy (lE1) and second ionisation energy (lE2) of elements X, Y and Z are given below.

    Element IE1(kJ mol-1) IE2(kJ mol-1)
    X 2370 5250
    Y 522 7298
    Z 1680 3381

    Which one of the above elements is the most reactive metal, the least reactive metal and a noble gas?

  16. The electron gain enthalpy of chlorine is 348 kJ mol-1. How much energy in kJ is released when 17.5 g of chlorine is completely converted into Cl- ions in the gaseous state?

  17. State Johann Dobereiner's law of triads.

  18. Write a note about Chancourtois classification.

  19. State the Newland's law of octaves.

  20. State Mendeleev's periodic law.

  21. Explain about the relationship between the atomic number of an element and frequency of the X-ray emitted from the elements.

  22. What are the anomalies of the long form of periodic table?

  23. Mention the names of the elements with atomic number 101, 102, 109 and 110.

  24. Write a note about the electronic configuration of elements in groups

  25. Give the name and electronic configuration of elements of 1st group and 2nd group.

  26. Write any two characteristic properties of alkali metals

  27. Write any two characteristic properties of alkaline earth metals.

  28. Groups from 13 to 18 in the periodic table are called p-block elements. Give reason.

  29. Why noble gases do not show much of chemical reactivity?

  30. Halogens and chalcogens have highly negative electron gain enthalpies.Why?

  31. What are d-block elements? Why are they called so?

  32. Elements Zn, Cd and Hg with electronic configuration (n-l)d10 ns2 do not show most of transition elements properties. Give reason.

  33. Why Zn, Cd and Hg are considered as soft metals?

  34. Why d-block elements are called as transition elements?

  35. What are f-block elements? How many series are there? Why they are called f-block elements?

  36. What are semi-metals? Give example.

  37. What are periodic properties? Give example

  38. Define ionic radius.

  39. Cationic radius is smaller than its corresponding neutral atom.Justify this statement.

  40. Anionic radius is higher than the corresponding neutral atom.Give reason.

  41. What are isoelectronic icons? Give example.

  42. Define ionization energy. Give its unit

  43. Ionization energy of beryllium is greater than the ionization energy of boron. Why?

  44. Ionization energy of nitrogen is greater than the ionization energy of oxygen. Give reason

  45. Define electron gain enthalpy or electron affinity.Give its unit.

  46. Electron gain enthalpy of F is less negative than Cl. Why?

  47. Electron affinity of oxygen is less negative than sulphur. Justify this statement.

  48. Explain about the factors that affect electronegativity.

  49. Explain about periodic variation of electro negativity across a period.

  50. Explain about the period variation of electronegativity along a group.

  51. Define valency. How is it determined?

  52. On the basis of quantum numbers, justify that the sixth period of the periodic table should have 32 elements.

  53. Why do elements in the same group have similar physical and chemical properties?

  54. How do atomic radius vary in a period and in a group? How do you explain the variation.

  55. Explain why cation are smaller and anions are larger in radii than their parent atoms?

  56. What is basic difference between the terms electron gain enthalpy and electro negativity?

  57. Would you expect the first ionization enthalpies of two isotopes of the same element to be the same or different? Justify your answer.

  58. Write the general electronic configuration of S-, p-, d-, and f-block elements?

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