Question

The first description of covalent bonding was provided by Lewis in terms of the sharing of electron pairs between atoms and related the process to the attainment of noble gas configuration by reacting atoms. While a single covalent bond is formed by sharing of an electron pair between two atoms, multiple bonds result from the sharing of two or three electron pairs. Some bonded atoms have additional pairs of electrons not involved in bonding. The VSEPR model was used for predicting the geometrical shapes of molecules. The valence bond (VB) approach to covalent bonding is basically concerned with the energetics of covalent bond formation about which the Lewis and VSEPR models are silent. Basically the VB theory discusses bond formation in terms of overlap of orbitals. For explaining the characteristic shapes of polyatomic molecules Pauling introduced the concept of hybridization of atomic orbitals. The molecular orbital (MO) theory describes bonding in terms of the combination and arrangement of atomic orbitals to form molecular orbitals that are associated with the molecule as a whole. (i) The pair of molecule that exhibit only sp2 hybridisation is a) H2O, C2H4 b) BH3, C2H4 c) NH3, C2H2 d) CH4, C2H2 (ii) Using MO theory, predict which of the following species has shortest bond length? a) O2- b) O2 2- c) O2 2+ d) O2 + (iii) The correct order of energies of molecular orbitals of N2 is a) (2py) < ( 2pz )< (*2px) = (*2py) b) (2py) > ( 2pz )>(*2px) = (*2py) c) (2py) < ( 2pz )> (*2px) = (*2py) d) (2py) > ( 2pz )< (*2px) = (*2py) (iv) The shape of PH3, SCl4, ClF3 according to VSEPR theory respectively are a) Pyramidal , T- shaped , Tetrahedral b) Bent , Seesaw shaped , linear c) Pyramidal , Seesaw shaped , T- shaped d) Linear , planar , trigonal bipyramidal (v) Based on H-N-H bond angle, the order of the following molecule and ions would be a) NH4+ > NH3> NH2- b) NH3 > NH4+ > NH2- c) NH4+ > NH2- > NH3 d) NH2- >NH4+ > NH3​

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