Molecular shapes of SF4, CF4 and XeF4 are :
Different, with 1, 0 and 2 lone pairs of electrons respectively.
The structure of species can be predicted on the basis of hydridisation which is tern can be know by knowing the number of hybrid orbitals in that species.
For SF4 : S is sp3 hybridised in SF4. Thus SF4 has 5 hybrid orbitals of which only four are used by F, leaving one lone pair of electrons on sulphur (valence electron
For CF4 : C is sp3 hybridised in CF4. Since all the four orbitals of carbon are involved in bond formation, no lone pair is present on C having four valence electrons.
For XeF4 : Xe is sp2d2 hybridised in XeF4. Of the six hybrid orbitals, four form bond with F, leaving behind two pair of electrons on Xe.
The molecule having one unpaired electrons is :
The hydrogen bond is strongest in :
The species in which the central atom uses sp2 hybrid orbitals in its bonding is :
The molecule which has zero dipole moment is :
The molecule which has pyramidal shape is :
Which one is most ionic?
Number of paired electrons in O2 molecule is :
Among the following species, identify the isostructural pairs, .
The correct order of increasing Câ€•O bond length of CO, , is
The common features among the species CN–, CO and NO+ are