FUPRE CHM 111 (INORGANIC CHEMISTRY) PAST QUESTIONS 2015/2016

1. Give the last five transition element in the transition series
2. The half life of ¹¹₆C is 20.3 min, how long will it take for 95.0%of a sample to decay?
3. How is positron emitted in a nuclear reaction? This diagram shows the electrolytic extraction of aluminium from bauxite. Use the diagram to answer question 4-6.
 4. Identify A ands E
5. What are the constituent of B?
6. What is the physical state of D?
7. What method is used for the extraction of magnesium from seawater?
8. Give the formula of Borax .
9. Which of the element in group 1A forms a stable nitride? Name and give the formula of the nitride.
10. Name one element that’s appears in group 1A that is not an alkali metal
11. Why is potassium more reactive than lithium?
12. What is the cause of the anomalous behavior of lithium?
13. Why is aluminium metal not extracted by carbon reduction of its oxide?
14. In a reaction with a non-metal, each alkali metal atom____A____its outer electron and becomes an____B_____with a____C____charge.
15. Indicate which ion in the following pair is larger in size. 1.      . (a) N^2- or F^-  (b) Mg²⁺ or Ca²⁺  (c) Fe²⁺ or Fe³⁺  

 16. Define inert pair effect
17. Write the theoretical expression for determination of electronegativity
18. Write the three degenerate orbitals of the p-subshell
19. How many unpaired electron are in one atom of iron, ⁵⁶₂₆Fe?
20. What is the atomic number of an element with the following electronic configuration: 1.      1S² 2S² 2P⁶ 3S² 4S² 3d¹⁰

21. How many neutrons and protons are contained in the atom of gold, ¹⁹⁷₇₉Au?
22. List the four quantum numbers
23. Write the number of electrons and charge of the ion, ⁵³₂₅Mn²⁺
24. To which group of the periodic table does the element with the following electronic configuration belong to? Ne 3S² 3P2
25. State the hund’s rule.
26. What are the shape and bond angle of beryllium hydride,    BeH₂?

27. Define hybridization
28. List the hybrid orbitals of carbon atom when it undergoes hybridization.
29. What is the maximum number of electrons in the principal quantum number, n=4?
30. What is periodicity?
31. What is the total number of values of subsidiary quantum number when the principal quantum number is 4?
32. Arrange the first ionization energy, I1 second ionization energy; second ionization energy, I2; third ionization energy, I3 in order of decreasing energy.
33. X(g) + e- →X(g) + energy. What name is given to the energy?
34. What is the representative name for the group IIA elements?
35. Which of the following element is not a d-block element: Sc, Ne, V, Ni, Cu and Zn?
36. How are atomic radius and effective nuclear charge related to electronegativity?
37. Ammonia has a bond angle of 107.3⁰  while methane has a bond angle of 109.5⁰. why the difference in their structural geometries?
38. Write the excited state configuration of carbon atom
39. In which blocks of the periodic table do these elements belong to; Na, Sc and Cl.
40. Why are +4 ions in group IVA or XIV unknown?
41. In chromium the 3d⁴4S²  electron configuration is less stable than the  3d⁵4S¹; why?
42. How many unpaired electrons are in one atom of iron?
43. How many neutrons and protons are contained in the atom of gold, ¹⁹⁷₇₉Au?
44. Write the values of the magnetic quantum number, Ml for the value of subsidiary quantum number, l=3.
45. Write the formula of the compound formed between sodium and a group VII element, X.
46. What is the standard unit of radioactivity?
47. What is nuclear fission?
48. What is the atomic number of a particle?
49. Give two ways of determining a stable nucleus.
50. Which transition metal has the highest number of oxidation state?
51. When is a transition metal said to be paramagnetic?
52. A nuclide of the element rutherfordium, is formed by the nuclear reaction of californium-249, ²⁴⁹₉₈Cfand carbon-12, ¹²₆C with the emission of four neutrons. This new nucliderapidly decays by emitting an alpha particle. Write the equation for each of these nuclear reactions.
53. The half life of ¹⁹₈O is 29s. what fraction of the isotope originally present would be left after 10.0s?
54. Write the nuclear equation for the following process: two deuterium ions undergoing fusion to give ³₂He  and a neutron.
55. An alkaline earth metal (group IIA) is radioactive. It undergoes decay by emitting three alpha particles in succession. In what periodic table group is the resulting elements found?
56. Name the two impurities found in the ore of bauxite.
57. What happens when i) sodium ii) boron are exposed to air?
58. Give three examples of group IVA elements.
59. Why are the alkali metals not found in the elemental state.
60. Give the chemical formula of cryolite.
61. List the general procedures for extraction of metals.
62. Why is the polarizing power of group IIA much greater than group IA?
63. Give two reasons why it is difficult to prepare elemental boron in a high state of purity
64. List the pairs of elements in group IA-IVA that show diagonal relationship
65. Boron react readily with steam to form compound A and liberate gas B. write a chemical balanced equation for this reaction.
66. The mass of one mole of electron in milligram is_(assume mass of one electron to be (9.1x10^-31kg).
67. Copper prefers the electronic configuration [Ar] 4S¹3d¹⁰.
68. The colour of manganese (Mn) compound in +7 oxidation state is?
69. The most important oxidation state of iron are?
70. Transition metals form metal complexes with________

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