COVALENT OR MOLECULAR HYDRIDES

Covalent or molecular hydrides. Dihydrogen forms, molecular compounds with most of the P block elements, examples are CH4, methane, MH3 ammonia, H2O, water, and HF, hydrogen fluoride. Molecular hydrides are further classified according to the relative numbers of electrons and bonds in their Lewis structure into one electron deficient, two electron precise and three electron which hydrides. Diboron, B2H6 is an example of Lewis structure. In fact, all elements of group 13 will form electron deficient compounds. All elements of group 14 form, electron precise compounds. Example, CH4 methane. Which are tetrahedral in geometry. Electron precise compounds have the required number of electrons to write there Lewis structure. Electron rich hydrates have excess electrons which are present as lone pairs. Elements of group 15 to 17 form such compounds. They behave as Lewis bases that is electron donors, the presence of lone pairs on highly electronegative atoms like nitrogen, oxygen and fluorine. In hydrides, results in hydrogen bond formation between the molecules, this leads to the association of molecule.