Advertisements
Advertisements
प्रश्न
Match the species given in Column I with the hybridisation given in Column II.
| Column I | Column II |
| (i) Boron in [B(OH)4]– | (a) sp2 |
| (ii) Aluminium in [Al(H2O)6]3+ | (b) sp3 |
| (iii) Boron in B2H6 | (c) sp3d2 |
| (iv) Carbon in Buckminsterfullerene | |
| (v) Silicon in \[\ce{SiO^{4-}4}\] | |
| (vi) Germanium in [GeCl6]2– |
Advertisements
उत्तर
| Column I | Column II |
| (i) Boron in [B(OH)4]– | (b) sp3 |
| (ii) Aluminium in [Al(H2O)6]3+ | (c) sp3d2 |
| (iii) Boron in B2H6 | (b) sp3 |
| (iv) Carbon in Buckminsterfullerene | (a) sp2 |
| (v) Silicon in \[\ce{SiO^{4-}4}\] | (b) sp3 |
| (vi) Germanium in [GeCl6]2– | (c) sp3d2 |
Explanation:
(i) Boron in [B(OH)4]– is sp3
(ii) Aluminium in [Al(H20)6]3+ is sp3d2 hybridized
(iii) Boron in B2H6 is sp3
(iv) Carbon in Buckminsterfullerene sp2 is hybridised.
(v) Silicon in \[\ce{SiO^{4-}4}\] is sp3
(vi) Germanium in [GeCl6]2- is sp3d2
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.
What happens when BF3 is reacted with ammonia?
In some of the reactions thallium resembles aluminium, whereas in others it resembles with group I metals. Support this statement by giving some evidences.
Ionisation enthalpy (∆iH1kJ mol–1) for the elements of Group 13 follows the order.
In the structure of diborane ______.
Explain why the following compounds behave as Lewis acids?
BCl3
Explain the following:
Boron does not exist as B3+ ion.
Explain the following:
PbX2 is more stable than PbX4.
Explain the following:
Pb4+ acts as an oxidising agent but Sn2+ acts as a reducing agent.
Explain the following:
Electron gain enthalpy of chlorine is more negative as compared to fluorine.
Identify the compounds A, X and Z in the following reactions:
\[\ce{A + 2HCl + 5H2O -> 2NaCl + X}\]
Identify the compounds A, X and Z in the following reactions:
\[\ce{X ->[Δ][370 K] HBO2 ->[Δ][> 370 K] Z}\]
Describe the general trends in the following properties of the elements in Groups 13 and 14.
Atomic size
Account for the following observations:
Though fluorine is more electronegative than chlorine yet BF3 is a weaker Lewis acid than BCl3
Three pairs of compounds are given below. Identify that compound in each of the pairs which has group 13 element in more stable oxidation state. Give reason for your choice. State the nature of bonding also.
TlCl3, TlCl
Three pairs of compounds are given below. Identify that compound in each of the pairs which has group 13 element in more stable oxidation state. Give reason for your choice. State the nature of bonding also.
InCl3, InCl
Boron fluoride exists as BF3 but boron hydride doesn’t exist as BH3. Give reason. In which form does it exist? Explain its structure.
Which one of the following is the correct statement?
