A Lewis acid is a molecule that can accept a lone pair of electrons from a Lewis

Question

A Lewis acid is a molecule that can accept a lone pair of electrons from a Lewis base to form an adduct. For example, compounds containing boron are often Lewis acids because the empty p orbital on boron can accept an electron pair, whereas compounds like ammonia (NH3) are Lewis bases because they can donate an electron pair (the lone pair on N in the case of ammonia). The formation of an adduct between a Lewis acid, BX3, and ammonia could be described as: BX3 + :NH3 X3B:NH3 The ability of a Lewis acid to form an adduct with a Lewis basis is dependent (in part) upon how easily the two molecules forming the complex can approach one another. This ability is related to the steric repulsion between molecules. Essentially, if adduct formation requires the groups in the molecules to get too close to one another, steric repulsion will be high and adduct formation will be difficult. Conversely, if the adduct structure allows the groups in the molecules to avoid one another, steric repulsion will be low and adduct formation will be facile. Use concepts related to molecular shape and steric repulsion to predict which of the following molecules can most easily act as a Lewis base to form an adduct with BF3:

a) PF3

b) SF4

c) IF5

Explanation / Answer

answer : a ) PF3

explanation:

BF3 having empty orbital and PF3 haivng lone pair on P. so PF3 can act as lewis base and BF3 can act as lewis acid . there will be coordinate covalent bond is formed between BF3 and PF3

BF3 <---------------PF3

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