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(a) d 2c>a (cc d. a>d 13. lewis acidity of silicon tetrahelides [sifa, sicl4, sibra, sil4] decreasing in the order: a) sila> sibr> siclh> sif (c) sif4> siclĄ> s
(a) D 2C>A (CC D. A>D 13. Lewis acidity of silicon tetrahelides [SiFa, SiCl4, SiBra, Sil4] decreasing in the order: a) Sila> SiBr> SiClh> SiF (C) SiF4> SiClĄ> SiBr4> Sils b) Sil,> SiCl4> SiBr,> SiF, (d) SiFa> SiBr> Sil,> SiCl4 11 Arcanas the hudrida CH. HA CaH HSoin arder af ineraacina acid ctranath Which ana i
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Priyanshu kumar Best Answer
The Lewis acidic properties of the tetrahalides tend to increase as follows: SiI4 < SiBr4 < SiCl4 < SiF4. This trend is attributed to the relative electronegativities of the halogens.
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A Lewis acid is an electron pair acceptor. In SiF4, the Si−F bond electrons are attracted towards F while the attraction is the least in Si−I bond. So Si in SiF4 is most ready to receive/accept electron pairs and hence SiF4 is the strongest Lewis acid
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but sir in case of Boron BI3>BBr3>BCl3>BF3
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here backbonding case occurs
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ok sir got it
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Dinesh khalmaniya 1![best-answer]()
option C A Lewis acid is an electron pair acceptor. In SiF4, the Si−F bond electrons are attracted towards F while the attraction is the least in Si−I bond. So Si in SiF4 is most ready to receive/accept electron pairs and hence SiF4 is the strongest Lewis acid.