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
Which one of the following statements is not true regarding diborane ?
Which one of the following statements is not true regarding diborane ?
Given below are the statements about diborane.
$(a)$ Diborane is prepared by the oxidation of $\mathrm{NaBH}_{4}$ with $\mathrm{I}_{2}$.
$(b)$ Each boron atom is in sp $^{2}$ hybridized state.
$(c)$ Diborane has one bridged $3$ centre$-2-$electron bond.
$(d)$ Diborane is a planar molecule.
The option with correct statement(s) is :
Given below are the statements about diborane.
$(a)$ Diborane is prepared by the oxidation of $\mathrm{NaBH}_{4}$ with $\mathrm{I}_{2}$.
$(b)$ Each boron atom is in sp $^{2}$ hybridized state.
$(c)$ Diborane has one bridged $3$ centre$-2-$electron bond.
$(d)$ Diborane is a planar molecule.
The option with correct statement(s) is :
- [JEE MAIN 2021]
Common alum is
Common alum is
The Lewis acid character of boron tri halides follows the order:
The Lewis acid character of boron tri halides follows the order:
- [JEE MAIN 2023]
Which is correct statement about Borax
Which is correct statement about Borax