Why does boron trifluoride behave as a Lewis acid ?
Why does boron trifluoride behave as a Lewis acid ?
The electric configuration of boron is $n s^{2} n p^{1}$. It has three electrons in its valence shell. Thus, it can form only three covalent bonds. This means that there are only six electrons around boron and its octet remains incomplete. When one atom of boron combines with three fluorine atoms, its octet remains incomplete.
Hence, boron trifluoride remains electron-deficient and acts as a Lewis acid.
Similar Questions
Given below are two statements :
Statement $I:$ Upon heating a borax bead dipped in cupric sulphate in a luminous flame, the colour of the bead becomes green.
Statement $II:$ The green colour observed is due to the formation of copper(I) metaborate.
In the light of the above statements, choose the most appropriate answer from the options given below :
Given below are two statements :
Statement $I:$ Upon heating a borax bead dipped in cupric sulphate in a luminous flame, the colour of the bead becomes green.
Statement $II:$ The green colour observed is due to the formation of copper(I) metaborate.
In the light of the above statements, choose the most appropriate answer from the options given below :
- [JEE MAIN 2023]
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