Explain why $${BF}_{3}$$ behaves as a lewis acid.
$$\text{Boron trifluoride }BF_3\text{ behaves as Lewis acid because it is an electron-deficient species and it can accept}$$ $$\text{electron pair.}$$ Here we see Boron configuration is $$1s^22s^22p^1$$ and $$\text{vacant p-orbital}$$ exist, which indicates that mean $$BF_3$$ has the tendency to accept lone pair, hence $$BF_3$$ is $$lewis \ acid.$$