Which is best sp2 or sp3

The best example is the alkanes. All the carbon atoms in an alkane are sp 3 hybridized with tetrahedral geometry. The carbons in alkenes and other atoms with a double bond are often sp 2 hybridized and have trigonal planar geometry. The triple bond , on the other hand, is characteristic for alkynes where the carbon atoms are sp -hybridized.

There a few common exceptions to what we have discussed about determining the hybridization state and they are mostly related to the method where we look at the bonding type of the atom.

For example, in the carbon dioxide CO 2 , the carbon has two double bonds, but it is sp -hybridized. And the reason for this is the fact that the steric number of the carbon is two there are only two atoms of oxygen connected to it and in order to keep two atoms at o , which is the optimal geometry, the carbon needs to use two identical orbitals. This is only possible in the sp hybridization. The other two 2p orbitals are used for making the double bonds on each side of the carbon.

Here the carbon has only single bonds and it may look like it is supposed to be sp 3 hybridized. However, the carbon in these type of carbocations is sp 2 hybridized. Again, for the same reason, that its steric number is 3 sp 2 — three identical orbitals. One exception with the steric number is, for example, the amides.

What is the orbital hybridization in BrCl3? What is the orbital hybridization theory? What hybridization is involved in the carbon-carbon bonds? See all questions in Orbital Hybridization. Impact of this question views around the world. You can reuse this answer Creative Commons License.

So each double bond bring the degree of the p level down by 1. An atom with a triple bond and one lone pair has two regions of electron density. Therefore, its hybridization would be sp one orbital per region of electron density. The sigma bond between to the carbon atoms is formed from overlap of sp hybrid orbitals from each carbon atom. They do not have cylindrical symmetry.

If you rotate the bond about the bond axis, you will see that the nodal plane has rotated as well. Sigma bond is a chemical bond formed by the linear or co-axial overlapping of the atomic orbitals of two atoms. A pi bond is a type of covalent bond that exists between atoms where the electrons are on top and bottom of the axis connecting the nuclei of the joined atoms.

If a bond between two atoms is broken when one atom is rotated around the bond axis, that bond is called a pi bond. Pi bonds are formed from the overlap of parallel p orbitals on adjacent atoms. They are not formed from hybrid orbitals. Begin typing your search term above and press enter to search. Press ESC to cancel.