मराठी
कर्नाटक बोर्ड पी.यू.सी.पीयूसी विज्ञान इयत्ता ११

In the structure of diborane ______.

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प्रश्न

In the structure of diborane ______.

पर्याय

  • All hydrogen atoms lie in one plane and boron atoms lie in a plane perpendicular to this plane.

  • 2 boron atoms and 4 terminal hydrogen atoms lie in the same plane and 2 bridging hydrogen atoms lie in the perpendicular plane.

  • 4 bridging hydrogen atoms and boron atoms lie in one plane and two terminal hydrogen atoms lie in a plane perpendicular to this plane.

  • All the atoms are in the same plane.

MCQ
रिकाम्या जागा भरा
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उत्तर

In the structure of diborane 2 boron atoms and 4 terminal hydrogen atoms lie in the same plane and 2 bridging hydrogen atoms lie in the perpendicular plane.

Explanation:

Four terminal hydrogen atoms and two boron atoms lie in the same plane and two hydrogen atoms forming bridges lie in a plane perpendicular to the rest of the molecule.

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पाठ 11: The p-block Elements - Multiple Choice Questions (Type - I) [पृष्ठ १३५]

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एनसीईआरटी एक्झांप्लर Chemistry Exemplar [English] Class 11
पाठ 11 The p-block Elements
Multiple Choice Questions (Type - I) | Q 10 | पृष्ठ १३५

संबंधित प्रश्‍न

If B–Cl bond has a dipole moment, explain why BCl3 molecule has zero dipole moment.


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Which of the following oxides is acidic in nature?


Ionisation enthalpy (∆iH1kJ mol–1) for the elements of Group 13 follows the order.


A compound X, of boron reacts with NH3 on heating to give another compound Y which is called inorganic benzene. The compound X can be prepared by treating BF3 with Lithium aluminium hydride. The compounds X and Y are represented by the formulas.


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.


Explain why the following compounds behave as Lewis acids?

AlCl3


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Explain the following:

PbX2 is more stable than PbX4.


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.


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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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Ionisation enthalpy


Describe the general trends in the following properties of the elements in Groups 13 and 14.

Nature of halides


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AlCl3 , AlCl


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