Are BCl3 and SiCl4 electron deficient c...

Are `BCl_3` and ` SiCl_4` electron deficient compounds ? Explain.

Text Solution

Verified by Experts

`BCl_3` is an electron deficient molecule since boron does not have octet. It can accept an electron pair Lewis bases and act as Lewis acid.
`SiCl_4` is not an electron deficient molecule: Silicon has octet in this compound.

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AlCl_(3) is an electron deficient compound but AlF_(3) is due to

Atomic size of F is smaller than Cl, which makes `AlF_(3)` more covalent

`AlCl_(3)` is a covalent compound while `AlF_(3)` is an ionic

Al in `AlCl_(3)` is `sp^(3)` hybridised but in `AlF_(3), Al` is `sp^(2)` hybridised

`AlCl_(3)` is exists in dimer but `AlF_(3)` does not

Which of the following is electron deficient?

`(BH_(3))_(2)`

`PH_(3)`

`(CH_(3))_(2)`

`(SiH_(3))_(2)`

(A) : Diborane is electron deficient molecule (R): In the formation of diborane molecule, boron atom uses sp^(3) - hybrid orbitals

Both A and R are true and R is the correct explanation of A

Both A and R are true and R is not correct explanation of A

A is true and R is false

A is false and R is true