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Explain why the following compounds behave as Lewis acids? AlCl3

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प्रश्न

Explain why the following compounds behave as Lewis acids?

AlCl3

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उत्तर

AlCl3 forms a covalent bond with chlorine by forming three single bonds of chlorine as aluminium has three electrons in its valence shell and act as an electron-deficient compound and act as lewis acid.

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पाठ 11: The p-block Elements - Multiple Choice Questions (Type - I) [पृष्ठ १३८]

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एनसीईआरटी एक्झांप्लर Chemistry Exemplar [English] Class 11
पाठ 11 The p-block Elements
Multiple Choice Questions (Type - I) | Q 25.(ii) | पृष्ठ १३८

संबंधित प्रश्‍न

Suggest reasons why the B–F bond lengths in BF3 (130 pm) and `"BF"_4^(-)` (143 pm) differ.


How would you explain the lower atomic radius of Ga as compared to Al?


The geometry of a complex species can be understood from the knowledge of type of hybridisation of orbitals of central atom. The hybridisation of orbitals of central atom in [Be(OH)4] and the geometry of the complex are respectively.


The exhibition of highest co-ordination number depends on the availability of vacant orbitals in the central atom. Which of the following elements is not likely to act as central atom in \[\ce{MF^{3-}6}\]?


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.


The most commonly used reducing agent is ______.


Cement, the important building material is a mixture of oxides of several elements. Besides calcium, iron and sulphur, oxides of elements of which of the group (s) are present in the mixture?


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 the following:

Boron does not exist as B3+ ion.


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:

\[\ce{X ->[Δ][370 K] HBO2 ->[Δ][> 370 K] Z}\]


Complete the following chemical equations:

\[\ce{Z + 3 LiAlH4 -> X + 3LiF + 3AlF_3}\]

\[\ce{X + 6H2 -> Y + 6H2}\]

\[\ce{3X + 3O2 ->[Δ] B2O3 + 3H2O}\]


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–  

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

Atomic size


Account for the following observations:

PbO2 is a stronger oxidising agent than SnO2 


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.

AlCl3 , AlCl


Boron fluoride exists as BF3 but boron hydride doesn’t exist as BH3. Give reason. In which form does it exist? Explain its structure.


A nonmetallic element of group 13, used in making bullet proof vests is extremely hard solid of black colour. It can exist in many allotropic forms and has unusually high melting point. Its trifluoride acts as Lewis acid towards ammonia. The element exihibits maximum covalency of four. Identify the element and write the reaction of its trifluoride with ammonia. Explain why does the trifluoride act as a Lewis acid.


Boron compounds behave as Lewis acids because of their ______.


Taking stability as the factor, which one of the following represents the correct relationship?


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