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Account for the following observations. Though fluorine is more electronegative than chlorine yet \(BF_{3}\) is weaker Lewis acid than\( BCl_3\).

Answer

Lewis acids are generally electron-deficient species. In the case of \(BF_3\), the boron has vacant \( 2p\)-orbital and fluorine has one completely filled \( 2p\) orbital. The electron from filled orbital goes to vacant orbital because both of these orbitals belong to the same energy level therefore, they can overlap effectively and form a \(p\pi- \ p\pi\) double bond. This type of bond formation is known as back bonding as shown:
Answer for Account for the following observations. Though fluorine is more electronegative than chlorine yet BF_{3} is weaker Lewis acid than BCl_3.
On the other hand, in the case of \(BCl_3\), there is no effective overlapping of \(2p-\) orbital of boron and \(3p-\) orbital of chlorine. Hence, \( BCl_3\) is more electron deficient species than \(BF_3\). That's why \(BF_{3}\) is a weaker Lewis acid than \(BCl_{3}\).
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