Advertisements
Advertisements
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 |
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.
APPEARS IN
संबंधित प्रश्न
If B–Cl bond has a dipole moment, explain why BCl3 molecule has zero dipole moment.
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.
Write a balanced equation for Al + NaOH → ?
The most commonly used reducing agent is ______.
Explain why the following compounds behave as Lewis acids?
BCl3
Explain why the following compounds behave as Lewis acids?
AlCl3
When BCl3 is treated with water, it hydrolyses and forms [B[OH]4]– only whereas AlCl3 in acidified aqueous solution forms [Al(H2O)6]3+ ion. Explain what is the hybridisation of boron and aluminium in these species?
Explain the following:
Electron gain enthalpy of chlorine is more negative as compared to fluorine.
Explain the following:
Tl (NO3)3 acts as an oxidising agent.
Account for the following observations:
PbO2 is a stronger oxidising agent than SnO2
