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प्रश्न
Match the species given in Column I with the properties mentioned in Column II.
| Column I | Column II |
| (i) \[\ce{BF^{-}4}\] | (a) Oxidation state of central atom is +4 |
| (ii) AICI3 | (b) Strong oxidising agent |
| (iii) SnO | (c) Lewis acid |
| (iv) PbO2 | (d) Can be further oxidised |
| (e) Tetrahedral shape |
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उत्तर
| Column I | Column II |
| (i) \[\ce{BF^{-}4}\] | (e) Tetrahedral shape |
| (ii) AICI3 | (c) Lewis acid |
| (iii) SnO | (d) Can be further oxidised |
| (iv) PbO2 | (b) Strong oxidising agent |
Explanation:
(i) \[\ce{BF^{-}4}\]: Tetrahedral shape, sp3 hybridisation, regular geometry.
(ii) AlCl3: Octet of Al not complete, acts as Lewis acid.
(iii) SnO: Sn2+ can show +4 oxidation state.
(iv) PbO2: Due to inert pair effect, Pb4+ is less stable than Pb2+ and hence acts as strong oxidising agent.
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संबंधित प्रश्न
Aluminium trifluoride is insoluble in anhydrous HF but dissolves on the addition of NaF. Aluminium trifluoride precipitates out of the resulting solution when gaseous BF3 is bubbled through. Give reasons.
What do you understand by inert pair effect?
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Which of the following statements are correct. Answer on the basis of Figure.
(i) The two birdged hydrogen atoms and the two boron atoms lie in one plane;
(ii) Out of six B – H bonds two bonds can be described in terms of 3 centre 2-electron bonds.
(iii) Out of six B – H bonds four B – H bonds can be described in terms of 3 centre 2 electron bonds;
(iv) The four-terminal B – H bonds are two centre-two electron regular bonds.
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Aluminium dissolves in mineral acids and aqueous alkalies and thus shows amphoteric character. A piece of aluminium foil is treated with dilute hydrochloric acid or dilute sodium hydroxide solution in a test tube and on bringing a burning matchstick near the mouth of the test tube, a pop sound indicates the evolution of hydrogen gas. The same activity when performed with concentrated nitric acid, reaction doesn’t proceed. Explain the reason.
Explain the following:
Pb4+ acts as an oxidising agent but Sn2+ acts as a reducing agent.
Explain the following:
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Identify the compounds A, X and Z in the following reactions:
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| Column I | Column II |
| (i) Diborane | (a) Used as a flux for soldering metals |
| (ii) Galluim | (b) Crystalline form of silica |
| (iii) Borax | (c) Banana bonds |
| (iv) Aluminosilicate | (d) Low melting, high boiling, useful for measuring high temperatures |
| (v) Quartz | (e) Used as catalyst in petrochemical industries |
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Though fluorine is more electronegative than chlorine yet BF3 is a weaker Lewis acid than BCl3
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