Home
Class 11
CHEMISTRY
Boron, the first member of group 13 (p-b...

Boron, the first member of group 13 (p-block) is a typical non-metal. H exists in two allotropic forms. The compounds of boron are mainly electron deficient as well as Lewis acids. For example, all the trihalides of boron `(BX_(3))` are Lewis acids. The expected order of acidic strength based on the electro negativity of halogen atoms is : `BF_(3)gtBC l_(3)gtBBr_(3)gtBl_(3)`. But the actual order is the reverse. This is explained with the help of the concept of back bonding `(p pi- p pi)` . Among the hydrides of boron. diborane has a bridged structure.
Among the halides of the elements of group 13, the one which is most acidic is:

A

`BF_(3)`

B

`AlCl_(3)`

C

`BCl_(3)`

D

`BBr_(3)`.

Text Solution

Verified by Experts

`BBr_(3)` is maximum acidic because `p pi- p pi` back bonding is the minimum.
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • P BLOCK ELEMENTS (GROUP 13 AND 14 )

    DINESH PUBLICATION|Exercise Straight obj.|17 Videos

  • P BLOCK ELEMENTS (GROUP 13 AND 14 )

    DINESH PUBLICATION|Exercise Select the correct answer|24 Videos

  • ORGANIC CHEMISTRY - SOME BASIC PRINCIPLES & TECHNIOUES

    DINESH PUBLICATION|Exercise PURIFICATION & CHARACTERISATION OF ORGANIC COMPOUNDS|38 Videos

  • PHYSICAL AND CHEMICAL EQUILIBRIA

    DINESH PUBLICATION|Exercise ULTIMATE PREPARATORY PACKAGE|13 Videos

Similar Questions

Explore conceptually related problems

Boron, the first member of group 13 (p-block) is a typical non-metal. H exists in two allotropic forms. The compounds of boron are mainly electron deficient as well as Lewis acids. For example, all the trihalides of boron (BX_(3)) are Lewis acids. The expected order of acidic strength based on the electro negativity of halogen atoms is : BF_(3)gtBC l_(3)gtBBr_(3)gtBl_(3) . But the actual order is the reverse. This is explained with the help of the concept of back bonding (p pi- p pi) . Among the hydrides of boron. diborane has a bridged structure. Which of the following statements of group 13, the one which is most acidic is:

Boron, the first member of group 13 (p-block) is a typical non-metal. H exists in two allotropic forms. The compounds of boron are mainly electron deficient as well as Lewis acids. For example, all the trihalides of boron (BX_(3)) are Lewis acids. The expected order of acidic strength based on the electro negativity of halogen atoms is : BF_(3)gtBC l_(3)gtBBr_(3)gtBl_(3) . But the actual order is the reverse. This is explained with the help of the concept of back bonding (p pi- p pi) . Among the hydrides of boron. diborane has a bridged structure. In the reaction: BF_(3)+3LiBH_(4)rarr3liF+X is

Knowledge Check

  • The order of acidic strength of boron trihalides

    A
    `BF_(3) lt BCl_(3) lt BBr_(3) lt BI_(3)`
    B
    `BI_(3) lt BBr_(3) lt BCl_(3) lt BF_(3)`
    C
    `BCl_(3) lt BBr_(3) lt BI_(3) lt BF_(3)`
    D
    `BBr_(3) lt BCl_(3) lt BF_(3) lt BI_(3)`

  • The order of acidic strenght boron trihalides is:

    A
    `BF_(3)ltBCl_(3)ltBBr_(3)ltBl_(3)`
    B
    `Bl_(3)ltBBr_(3) ltBCl_(3)ltBF_(3)`
    C
    `BCl_(3)ltBBr_(3)ltBl_(3)ltBF_(3)`
    D
    `BBr_(3)ltBCl_(3)ltBF_(3)ltBl_(3)`

  • The unexpected order of acidic strength of the trihalides of boron can best be explained by.

    A
    `p pi-p pi` beack bonding
    B
    Hybridisation
    C
    Trigonal planar structure
    D
    None of the above

    • Similar Questions

    Explore conceptually related problems

    Boron, the first member of group 13 (p-block) is a typical non-metal. H exists in two allotropic forms. The compounds of boron are mainly electron deficient as well as Lewis acids. For example, all the trihalides of boron (BX_(3)) are Lewis acids. The expected order of acidic strength based on the electro negativity of halogen atoms is : BF_(3)gtBC l_(3)gtBBr_(3)gtBl_(3) . But the actual order is the reverse. This is explained with the help of the concept of back bonding (p pi- p pi) . Among the hydrides of boron. diborane has a bridged structure. The two types of bonds in diboran e are covalent and q

    Why is BF_(3) a Lewis acid?

    The correct order of Lewis acidic strength of boron trihalides :

    Why boron forms electron deficient compounds?

    The power of halides of boron to act as Lewis acids decreases in the order

    Home
    Profile