Chemistry

4.40. Bond order is defined as one half the difference between the number of electrons present in the bonding and the antibonding orbitals i.e.

Bond order (B.O.) = ½ (Nb–Na)

4.39. When hydrogen is attached with highly electronegative element in a covalent bonding the electrons of the covalent bond are shifted towards the more electronegative atom. Thus, a partially positively charged hydrogen atom forms a bond with the other more electronegative atom. This bond is known as a hydrogen bond. Hydrogen bond is stronger than the van there Waals forces.

4.38. P has ground state valence shell electronic configuration 3s²3p³ and the first excited state valence shell electronic configuration is 3s¹3p³3d¹. P undergoes sp³d hybridization and has trigonal bipyrami geometry. Because axial bond pairs suffer more repulsive interaction from the equatorial bond pairs, therefore axial bonds have been found to be slightly longer and hence slightly weaker than equatorial bond.

4.37. Molecular orbitals are represented by wavefunctions. A positive sign in an orbital indicates a positive wavefunction while a negative sign in an orbital shows a negative wavefunction.

4.36. O₂: Bond order = 2, paramagnetic
O₂⁺: Bond order = 2.5, paramagnetic
O₂^–: Bond order = 1.5, paramagnetic
O₂^2-: Bond order = 1, diamagnetic
Order of relative stability is
O₂⁺ > O₂ > O₂^– > O₂^2-
(2.5) (2.0) (1.5) (1.0)