Covalent Bond Formation-Molecular Orbital MO Method

2 COVALENT BOND FORMATION-MOLECULAR ORBITAL (MO) METHOD [Pg.13]

Two parallel p orbitals overlap side-by-side to form a pi (tt) bond. Fig. 2-3(u), or a n bond. Fig. 2-3(6). The bond axis lies in a nodal plane (plane of zero electronic density) perpendicular to the cross-sectional plane of the tt bond. [Pg.13]

Single bonds are a bonds. A double bond is one a and one it bond. A triple bond is one a and two TT bonds (a tt and a if the triple bond is taken along the j -axis). [Pg.13]

Although MO s encompass the entire molecule, it is best to visualize most of them as being localized between pairs of bonding atoms. This description of bonding is called linear combination of atomic orbitals (LCAO). [Pg.13]

Problem 2.2 What type of MO results from side-to-side overlap of an s and a p orbital [Pg.13]

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