39Apply VSEPR to find their shapes...except SF4, they are square planar(which means equal bond lengths). Due to lone pair in S, the bond angle decreases.
1..IN WHICH OF THE FOLLOWING BONDS re not equal
1.SF4 2.SiF4
3.XeF4 4..BF4
GIVE EXPLANATION [2]
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5 Answers
39
29SF4 -- see-saw shaped compound sp3d hybridisation so it has two kinds of S-F bonds axial and equatorial
XeF4 Square planar sp2d
SiF4 sp3 it's tetrahedral and not square planar
and BF4- also tetrahedral sp3
In square planar compounds hybridisation is sp2d so they involve participation of d-orbitals whereas in tetrahedral compounds hybridisation is sp3 and they do not have participation of d-orbitals..
1square planar compounds hybridisation is not sp2d govind its dsp2 na??
1
SF4--->sp3d
SiF4---->sp3
Acc to VSEPR
(6+4)/2=5 and 1 lone pair => see saw shape....here the see saw shape is a bit hindered due to presence of lone pair electrons
XeF4----> sp3d2
acc to VSEPR
(8+4)/2=6 and 2 lone pairs => square planar
BF4- -----> sp3
Acc to VSEPR
(3+4+1)/2=4 and 0 lone pairs => tetrahedral shape
Each angle of tetrahedral = 109.5°
Each Angle of square planar= 90°
Angles of see saw shape = http://en.wikipedia.org/wiki/Sulfur_tetrafluoride