Give reasons for the following
a) [SiF6]^2- is known where as [Sicl6]^2- is not known.
b) Diamond is covalent yet has high melting point
c) Pb x, is more stable than pb X4 (x = CI, Br)
d) Boron is unable to form BF6^3-
e) BF3 behaves as lewis acid.
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A.Due to smaller size of F as compared to Cl , six small F atoms can be easily accommodated around Si atom while Cl cannot since F are present in smaller 2p orbital and Cl are present in larger 3p orbital therefore interaction of F lone pair electron with d-orbitals of silicon are stronger in F as compared Cl
:b.diamond has three dimensional c-c bond
C .due to innert pair effect and oxidation state of +2 pbx is more stable
D.Boron does not have d orbitals. Because of this, it is not possible for the element to expand on its octet. This, in turn, causes the maximum covalence of boron to be restricted to 4. Beyond this value, boron will become unstable and not be able to form [BF
6
]
3−
ions.
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