Question:
The Lewis acidity of $BF_3$ is less than $BCl_3$ even though fluorine is more electronegative than chlorine. It is due to
The Lewis acidity of $BF_3$ is less than $BCl_3$ even though fluorine is more electronegative than chlorine. It is due to
Updated On: Jun 20, 2022
- stronger $2p(B)-2p (F) \sigma$ - bonding
- stronger $2p(B)-2p(F) \pi$ - bonding
- stronger $1 p( B )-3 p( Cl ) \sigma$ -bonding
- stronger $2p(B)-3p(Cl) \pi$ - bonding
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The Correct Option is B
Solution and Explanation
Boron and fluorine do not have $d$ -orbitals. Hence, both of these participate in strong $2 p(B)-2 p(F)$ back $\pi$ -bonding. On the other hand, due to large size and availability of vacant $d$ -orbitals, Cl does not participate in such type of back $\pi$ -bonding. Hence, $BF _{3}$ is less acidic than $BCl _{3}$.
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Concepts Used:
Group 13 Elements
Group 13 is commonly known as the Boron Family. The boron family comprises:
- Boron (B)
- Aluminum (Al)
- Gallium (Ga)
- Indium (In)
- Thallium (Tl)
Element 113 (Nihonium) gets the name of ununtrium Uut. Each one of the elements has three electrons in the external shell of their nuclear structure is one of the important and mutual properties of the group.
The general electronic configuration for the group 13 elements is ns2 np1.
Density of Boron Family:
Melting point and Boiling Point:
Electronegativity:
Atomic and Ionic Radii:
Compounds of Group 13 Elements:
- Oxides
- Halides
- Borates
- Boron Hydrides
- Diborane
- Borazine