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

Which of the following oxides is acidic in nature?

Advertisements
Advertisements

प्रश्न

Which of the following oxides is acidic in nature?

पर्याय

  • B2O3

  • Al2O3

  • Ga2O3

  • In2O3

MCQ
Advertisements

उत्तर

B2O

Explanation:

B2O3 is acidic in nature. It reacts with basic oxides to form metal borates. Acidic nature decreases on moving down the group.

shaalaa.com
  या प्रश्नात किंवा उत्तरात काही त्रुटी आहे का?
पाठ 11: The p-block Elements - Multiple Choice Questions (Type - I) [पृष्ठ १३४]

APPEARS IN

एनसीईआरटी एक्झांप्लर Chemistry [English] Class 11
पाठ 11 The p-block Elements
Multiple Choice Questions (Type - I) | Q 4 | पृष्ठ १३४

संबंधित प्रश्‍न

How can you explain higher stability of BClas compared to TlCl3?


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


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


Write a balanced equation for Al + NaOH → ?


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 \[\ce{MF^{3-}6}\]?


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.


Dry ice 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


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.


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

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.

Atomic size


Account for the following observations:

Though fluorine is more electronegative than chlorine yet BF3 is a weaker Lewis acid than BCl3 


Boron compounds behave as Lewis acids because of their ______.


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


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×