Molecular oibital diagrams

Fig. 11.52 Molecular oibital diagram for a tetrahedral ML4 complex, showing possible ligand-to-metal charge transfer (LMCT) transitions.

Fig. 16.60 Qualitative molecular oibital diagram for dinuclear rhenium and molybdenum complexes. All of the bonding molecular orbitals are filled for [Ke2Clx]"- (c) and a bond order of 4 results from one a. two it. and one 6 bond. When electrons are added to the 6 level, the bond order is reduced as shown for (dl and (e). Removing elections from the S bond also leads to a lower bond order as shown by (a) and (b). (Taken in part from Cotton. F. A.

Practice Probiem B Given that BeO is diamagnetic, ase a molecular oibital diagram to determine whether the orbitals are ordered like those of Be2 or those of O2. 

Figure 3.2. Simplified molecular oibital diagram for the energy levels in Tl2Pt(CN)4-...

Figure 4.12. Simplified molecular oibital diagram for dimers.

FIGURE 5.9. Assembly of the oibital diagram for tetrahedral H4 from those of two units. (The solid lines in this diagram which are asspdated with the geometrical figures are used to help the reader visualize the molecular geometry. The "bonds between connected atoms, usually depicted by lines have been left off for clarity.)... 

We can do similar analyses of the molecules Li2 and Bc2. (The Li and Be atoms have ground-state electron configurations of [He]2s and [He]2s, respectively.) The 2s atomic oibitals also combine to form the corresponding cr and tr molecular orbitals. Figure 9.14 shows the molecular orbital diagrams and bond orders for Li2 and Be2. 

Figure 4.24. Simplified molecular orbital diagram for a metal-metal bonded dimer showing the d oibitals that are used to obtain the intermetallic bonds, and the energy level of these orbitals.

Prepare a molecular orbital energy level diagram for SH , including sketches of the orbital shapes and the number of electrons in each of the oibitals. If a program for calculating molecular orbitals is available, use it to confirm your predictions or to explain why they differ. 

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