English
Karnataka Board PUCPUC Science Class 11

Write a balanced equation for B2H6 + NH3 → - Chemistry

Advertisements
Advertisements

Question

Write a balanced equation for B2H6 + NH3 → ?

One Line Answer

Solution

\[\ce{3B_2H_6  + 6NH_3 -> 3[BH_2(NH_3)_2]^+[BH_4]- -> \underset{Borazene}{2B3N3H6} + 12H2}\]

shaalaa.com
Group 13 Elements - The Boron Family
  Is there an error in this question or solution?
Chapter 11: The p-Block Elements - EXERCISES [Page 333]

APPEARS IN

NCERT Chemistry - Part 1 and 2 [English] Class 11
Chapter 11 The p-Block Elements
EXERCISES | Q 11.31 - (vi) | Page 333

RELATED QUESTIONS

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


Write a balanced equation for Al + NaOH → ?


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.


Which of the following oxides is acidic in nature?


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


The most commonly used reducing agent is ______.


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?

BCl3


Explain why the following compounds behave as Lewis acids?

AlCl3


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:

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


Match the species given in Column I with properties given in Column II.

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

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

Ionisation enthalpy


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

Metallic character


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.

InCl3, InCl


Boron compounds behave as Lewis acids because of their ______.


A group 13 element ‘X’ reacts with chlorine gas to produce a compound XCl3. XCl3 is electron deficient and easily reacts with NH3 to form \[\ce{Cl3X –> NH3}\] adduct; however, XCl3 does not dimerize X is ______.


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×