Question
Why does $\mathrm{BF}_3$ behave as Lewis acid?
✓
Answer
In $\mathrm{BF}_3$ there are six electrons around Boron after sharing with fluorine atoms and hence Boron is electron deficient. B in $\mathrm{BF}_3$ can accept lone pair of electrons in the vacant 2 p orbital of Boron and so behaves as Lewis acid as its octet is not complete.
Need a full question paper?
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
Explore more
Similar questions
Give IUPAC name of:
Write the principle of Le-Beil and Van't Hoff.
Write the significance of a plus and a minus sign shown in representing the orbitals.
What is the importance of measuring BOD of a water body?
Give the IUPAC name of the following compound $\text{CH}_3-\text{CH}-\text{C}-\text{CH}-\text{CH}_3\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ | \ \ \ \ \ \ \ \ \ \| \ \ \ \ \ \ |\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Br} \ \ \ \ \ \ \text{O} \ \ \ \ \ \text{CH}_3$
→List the quantum numbers ( $m_l $ and I) of electrons for 3d orbital.
→Why is CO more toxic than $\mathrm{CO}_2$?
→A and B belong to same group of periodic table. 'A' has higher atomic number than B. Which will have lower ionisation energy and why?
The entropy of $Mg ^{+2}$ ion in aqueous solution will be more before hydration or after hydration.
→Why eclipsed and staggered forms of ethane cannot be isolated at room temperature?