sp3 orbitals are similar in shape to p orbitals however one side is much larger than the other - hence you have a lopsided dunbell shape orbital
It is trigonal planar.
trigonal planar
i don't know....... maybe the cation is sp3 hybridization?
In this compound, the central atom, sulfur, has one lone pair and four bond pairs, and it takes the see-saw shape according to VSEPR theory. Its hybridisatio is approximately sp3d
Hi, The nitrogen is glycine is sp3 hybrid. The shape is tetrahedral.
sp3 or 4 sigma bonds
sp3d2
in XeO3 ,Xe shows sp3 but shape is pyramidal because of the presence of a lone pair of electrons on the central xenon atom. This lone pair distorts the shape of the molecule making it pyramidal.
i don't know....... maybe the cation is sp3 hybridization?
In this compound, the central atom, sulfur, has one lone pair and four bond pairs, and it takes the see-saw shape according to VSEPR theory. Its hybridisatio is approximately sp3d
CH3 is a trigonal planar and has a hybridization of sp3
As the CCl4 molecule has a regular tetrahedral shape the hybridisation is sp3
Hi, The nitrogen is glycine is sp3 hybrid. The shape is tetrahedral.
That would be Trigonal Pyramidal in shape and have an sp3 hybridization.
The formula looks like trans- 2-butene. The c atoms working left to right will have sp3 sp2 sp2, sp3 hybridisation. the bond angles will be tetrahedral on the sp3 centers, 120 0 on the sp2 centres which have a planar shape, with all four substituents lying in the same plane. Good picture in wikipedia. The actual bond angles will deviate slightly.
sp3 or 4 sigma bonds
NH2- is sp3 hybridized and there is 2 bonding and 2 lone pair of electron,that's why shape of NH2 is angular.
sp3 is better
sp3d2