Chemical Bonding And Molecular Structure

The hybridisation of one , one and three -orbitals on a central atom gives rise to five orbitals, three equatorial and two axial. This hybridisation uses one , one and all three of the orbitals and shape of the molecule becomes trigonal bipyramidal.

-Linear shape.

When two atoms come close to each other, there is overlapping of atomic orbitals. This overlap may be positive, negative or zero depending upon the properties of overlapping of atomic orbitals.

The electronegativity of elements helps in predicting polarity of the molecule. If the electron egativities are equal (or difference is 0) the bond is non-polar covalent. If the difference in electron eg activities between the two atoms is but then the bond is polar-covalent. If the difference in electron eg activities between the two atoms is or greater, the bond is ionic.

Anions of the acids and are and respectively
Their structures can be explained as follows:
has planar structure It has nitrogen as a central atom without lone pair, whidi is bonded to three oxygen atoms. Its hybridisation can be predicted by
Where = number of valence electrons
= number of monovalent ion
= cationic charge
- anionic charge
Hybridisation

has tetrahedral structure. It has phosphorus as a central atom without lone pair which is bonded to four oxygen atoms. Its hybridisation can be predicted as

has tetrahedral structure. It has phosphorus as a central atom without lone pair which is bonded to four oxygen atoms. Its hybridisation can be predicted as