2nd Year Chemistry Chapter 4 Group VA and Group VIA Elements Notes

chemistry 12th notes chapter No 4

1. Which of the following shows phosphorescence?


2. Nitric acid, Sulphuric acid and Caustic soda can be transported in a container made up of:


3. H₂SO₄ produces:


4. Atomic number of Te is:


5. Phosphorous shows oxidation state (+3) in which of the following:


6. Which of the following species has the maximum number of unpaired electrons?


7. H₂SO₄ the sugar becomes black due to:


8. Gold dissolve in Aqua regia to give:


9. Laughing gas is chemically


10. Which one of the following elements occur free in nature:


11. Yellow colour of Nitiric Acid is due to the presence of:


12. Most of the sulphuric acid is manufactured in world is by:


13. NO₂ is called


14. Arsenic oxides are removed during manufacture of H₂SO₄ by passing through:


15. The lowest ionization energy is possessed by:


16. In Pyrite burner, the gas produced is:


17. Orthophosphoric acid is:


18. The composition of oleum is:


19. Indicate the formula of metaphosphoric acid is:


20. Which of the following gas is evolved when copper reacts with dil HNO₃?


21. Which catalyst is used in lead chamber process?


22. Which element is the most abundant in the earth’s crust:


23. The element whose inorganic minerals are not much abundant in earth crust:


24. Which one of the following molecules is paramagnetic in nature?


25. The percent by volume of N₂ in air is:


26. Which of the following phosphorus is most reactive:


27. In group VA the most electronegative element is:


28. Which of the following statement is incorrect?


29. Which one of the following is an amphoteric oxide:


30. Which of the following is a white hygroscopic powder:


31. Which catalyst is used in contact process?


32. HNO₂ acts as an/a:


33. Out of all the elements of group VA, the highest ionization energy is possessed by


34. Red phosphorous can be obtained from white Phosphorous by:


35. Which one the following elements occur free in nature:


36. Out of all the elements of group VIA, the highest melting and boiling points is shown by the elements


37. Which one of the following compounds is not known:


38. Among group VA elements, the most electronegative element is


39. Which of the following is used at the tips of match stick:


40. The catalyst used in manufacturing of H₂SO₄ by Contact process is:


41. SO₃ is not directly dissolved in water to get Sulphuric acid because:


42. Ortho-phosphoric acid has melting point:


43. Which of the following metal reacts with HNO₃:


44. FeSO₄ forms brown ring with:


45. Which is a laughing gas:


46. In group V-A element the most electronegative element is:


47. What is the number of electrons present in the valence shell of P in PCl₃ ?


48. HNO₂ is:


49. Which of the following is a reddish brown gas:


50. Free nitrogen and oxygen are present in atmosphere but they do not react with each other under normal conditions because


51. Nitrous acid is a:


52. Formula of Gibbsite is:


53. Ozone is not:


54. H₂SO₄ has great affinity for water because:


55. Cinnabar is:


56. The substance which is attracted by the magnetic field is called:


57. Aqua Regia is:


58. The percentage of N in NH₃:


59. At 18 ͦC the specific gravity of H₂SO₄ is:


60. The composition of Aqua Regla is:


61. SO₃ is not absorbed in water directly to from H₂SO₄ because


62. Phosphorus pentoxide is used as:


63. Phosphorus helps the growth of:


64. The contact process for the manufacturing of H₂SO₄ was developed by:


65. Oleum is:


66. Which of the following elements is most metallic:


67. P₂O₅ is heated with water to get:


68. Oxidation of NO in air produces:


69. Oxidation of NO in air produces:


70. When red phosphorous is heated with HNO₃ it forms:


71. HNO₃ is:


72. A strong triple bond is present between two nitrogen atoms in a molecule and therefore nitrogen gas is:


73. The most electronegative element in group-VA is


74. The brown gas formed when metal reduces HNO₃ is:


75. Which of the following gives brown ring with FeSO₄?


76. The compound N₂O causes disease:


77. Which of the following is not correct about Phosphorous?


78. Molecular formula of white phosphorous is:


79. “Lead” in lead pencil is:


80. Which of the following elements does not show the phenomena of allotropy?


81. In which compound of nitrogen, the oxidation state of N is (+1):


82. Which metal is rendered passive by HNO₃?


83. Chemical formula of laughing gas is


84. The anhydride of nitric acid is:


85. The structure of white phosphorus is:


86. In which substance nitrogen is not present:


87. The given element gives NO gas with dil HNO₃:


88. Bone ash contains:


Short Questions

“1. Complete and balance the following chemical equation.
KMnO₄+ FeSO₄+ H₂SO₄ —–>”
2. Describe “Ring test for the confirmation of the presence of nitrate ions in solution?
3. Give four dissimilarities of oxygen and sulphur.
4. Give reactions to justify that H₃PO₃ is a reducing agent?
5. Give the advantages of contact process for the manufacture of sulpuric acid?
6. Give the name and formulas of oxyacids of phosphorus and indicate the oxidation number of phosphorus in them?
7. Give the names and formulas of various oxides of phosphorus?
8. Give the names of four elements which do not react with nitric acid.
9. Give two reactions of sulphuric acid which show its oxidizing behaviour.
10. Give two reactions which show oxidizing behaviour of NO.
11. Gives the reactions of HNO₃ in which it acts as an oxidizing agent?
12. H₃PO₃ is dibasic acid although it has three hydrogen atoms in that. Give reasons?
13. How a brown couloured gas NO₂ is prepared from:
14. How allotropy is associted with nitrogen and phosphorus?
15. How dilute HNO₃ can be concentrated on commercial scale?
16. How do you compare the elements of the group VI-A in their physical states?
17. How do you compare the properties of white and red phosphorus?
18. How do you compare the structures of N₂O and NO?
19. How do you compare the structures of PCI₃ and NH₃?
20. How do you justify that N₂O is a supporter of combustion?
21. How does aqua regia dissolve gold?
22. How does H₂SO₄ act as a dehydrating reagent?
23. How does HNO₂ act as reducing agent?
24. How does HNO₂ acts as an oxidizing agent?
25. How does nitrogen differ from its family members in physical state atomicity and variety of oxidation states?
26. How does oxygen differ from its own family members especially sulphur?
27. How does oxygen occur in nature?
28. How does P₂O₃ react with water in cold and hot state?
29. How does P₂O₅ react with water in cold and hot state?
30. How does phosphorus occur in the form of minerals in plants and animal tissues?
31. How does sulphur occur in nature?
32. How H₃PO₄ is affected at high temperature?Is it a tribasic acid?
33. How KmnO₄ and K₂Cr₂O₇ react with H₂SO₄ ?
“34. How NO₂ is prepared from:
a. Lead nitrate
b. Cu+HNO₃ “
35. How PCI₃ and PCI₅ react with alcohols and carboxylic acids?
36. How sulphur can increase its oxidation number but oxygen can not?
37. How the involvement of d-orbital increases the oxidation number of phosphorus?
38. How the melting and boiling points for the elements of group V-A vary down the group?
39. i) pbNO₃ ii) Cu and HNO₃
40. Justify that conc. H₂SO₄ is a dehydrating agent.
41. Justify that NO acts as an oxidizing agent?
42. Justify that P₂O₅ is the dehyderating reagent?
43. Justify that sulphuric acid is king of chemicals.
44. Mention the catalytic condition for the emanufacture of H₂SO₄ in contact process?
45. Mention various allotropic forms for the elements of group VI-A?
46. Name three allotropic forms of phosphorus.
47. NO₂ is a strong oxidizing agent. Prove with the help of two examples.
48. P₂O₅ is powerful dehydrating agent. Give two examples.
49. What are the optimum condition for the manufacture of H₂SO₄ in the contact tower?
50. What happens when NO₂ is dissolved in water?
51. What is aqua regia and how does it dissolve the noble metals?
52. What is aqua regia?
53. What is meant by fuming nitric acid?
54. What is the action of heat on orthophosphoric acid? Write chemical equation also.
55. What is the effect of temperature on N₂O₄?
56. What is the general occurrence of elements of group V-A?
57. What is the rection of No with FeSO₄ solution?
58. What type of oxides are mostly given by the elements of group V-A?
59. Why SO₃ is dissolved in sulphuric acid and not in water?
60. Why SO₃ gas is dissovled in H₂SO₄ but not in water in contact process?
61. Why the elements of VIA other than oxygen show more than two oxidation states?
62. Why the outermost p-sub-shells of group V-A elements are extra stable?
63. Write any four properties of sulphuric acid.
64. Write any four uses of Nitric acid.
65. Write down the equation for the reaction between conc. H₂SO₄ and copper and explain what type fo rection is it?
66. Write down the formulas and names of oxyacids of nitrogen posphorus,arsenic and antimony with oxidation number +5?
67. Write down the name formulae and colours of oxides of nitrogen along with the oxidation states of nitrogen in them?
68. Write down the reaction involved in the preparation on HNO₃ by Birckland Eyde’s process?
69. Write down two chemical reactions which show that sulphuric acid is a dehydrating agent?
70. Write two points of dissimilarities of oxygen and sulphur.
71. Write two reactions of preparation of nitrous acid.

Long Questions

“1. What happen when dil HNO₃ and conc. HNO₃ react with following?
(i) Cu (ii) Hg (iii) Sn (iv) Zn”
2. How is nitric acid prepared industrially? Give all equations involved.
3. Describe eight points of similarities of oxygen with sulphur.
4. How sulphuric acid is manufactured by contact process on industrial scale?
5. Write preparation and two reactions of HNO₂.
6. Write down four similarities and four differences between oxygen and sulphur.
7. H₂SO₄ is a dehydrating agent and oxidizing agent, prove this truth by giving two examples of each.
8. Write down two reactions in which HNO₂ acts as an oxidizing agent and two reactions in which HNO₂ acts as reducing agent.
9. Discuss reactions of Sulphuric Acid as a Dehydrating Agent.
10. Explain the cathode coating and anode coating of iron.

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