Chapter 11: Q11.47CP (page 434)

The sulfate ion can be represented with four S—O bonds or with two S-O and two S=O bonds.
Which representation is better from the standpoint of formal charges?
What is the shape of the sulfate ion, and what hybrid orbitals of S are postulated for the sigma bonding?
In view of the answer to part (b), what orbitals of S must be used for the pi bonds? What orbitals of O?
Draw a diagram to show how one atomic orbital from S and one from O overlap to form a pi bond.

Short Answer

Expert verified

The sulphate ion can be represented by the two S-O and two S=O bonds.
The shape of the sulphate is tetrahedral and the hybrid orbital of S is postulated with s-orbital.
The orbitals used for the formation of pi-bond in sulphate ion is p-orbital.
The diagram between the S-atom and one O-atom to show the pi-bond:

Step by step solution

Bonding

Bonding may be defined as the force of attraction between two or more atoms to form a compound. The molecule can have the same atom and a different atom.

Formal Charge

The formal charge is the charge present on the individual charge of an atom which shows the bonding of the molecule. Here the two S-O single bonds and two S=O double bonds can fulfil the octet of the S-atom.

Sigma Bonding

Sigma bond is the bond between the molecules which is formed by the head-on-overlapping of the hybrid orbitals of the atoms. There are two single bonds S-atom and O-atom forming after the overlap of the s-orbital of both the atom by head-on-overlapping.

Pi Bonding

Pi bond is the bond between the molecules which is formed by the side-on-overlappingof the hybrid orbitals of the atoms. There are two S-atom and O-atom forming after the overlap of the p-orbital of both the atom by side-ways-overlapping.