Bonding molecular orbitals energy levels

Fig. 10.5 A qualitative c + n bonding molecular orbital energy level diagram for Cr(C0)6 based on Figs. 6.11 and 6.16(c) together with the associated discussion. This schematic diagram may be compared with Fig. 10.10 which is a more accurate molecular ener level diagram for Cr(C0)6.

Step 2 Use matching valence-shell atomic orbitals to build bonding and antibonding molecular orbitals and draw the resulting molecular orbital energy-level diagram (Figs. 3.31 and 3.32). 

FIGURE 3.39 The molecular orbital energy-level diagram for the ir-orbitals of benzene. In the ground state of the molecule, only the net bonding orbitals are occupied. 

FIGURE 3.40 The molecular orbital energy-level diagram for SFf, and the occupation of the orbitals by the 12 valence electrons of the atoms. Note that no antibonding orbitals are occupied and that there is a net bonding interaction even though no d-orbitals are involved. 

Draw simple molecular orbital energy-level diagrams to indicate how the bonding in the saline hydrides, such as NaH or KH, differs from that between hydrogen and a light p-block element such as carbon or nitrogen. 

For each of the following, draw a molecular orbital energy level diagram and give the bond order. Tell whether the species would be more or less stable after gaining an electron, (a) 02+ (b) CN (c) S2 (d) NO (e) Be2+. 

Fig. 5.13 Correct molecular orbital energy levels For early elements of the first long row. Some mixing (hybridization) has occurred between the 2r and 2p orbitals. Note that it is somewhat more difficult to keep books" and determine the bond order here ihan in Fig. 5.12 3o- and are clearly bonding (they lie below the atomic orbitals contributing i0 them) 4(7, and 5trR are essentially nonbonding since they lie between the atomic orbitals contributing to them and roughly symmetrically spaced about the center of gravity." The maximum net bond order is therefore one cr bond plus two 7r bonds. The electronic configuration shown is for the Bz molecule. Note the unpaired pi electrons.

Construct a molecular-orbital energy-level diagram for HF. Compare and contrast the bonding and the energy levels in HF and LiH. 

It is important to establish the main similarities and differences in the electronic spectra of isoelectronic metal carbonyls and cyanides and to relate these spectral comparisons to the nature of the M-CN and M—CO bonds. In this paper the electronic spectra of d6 metal carbonyls and cyanides are assigned on the basis of a derived molecular orbital energy level scheme. The differences in the energies erf the single electron molecular orbitals for representative metal hexa-carbonyls and hexacyanides are obtained and a general discussion erf electronic structure is presented. 

Finally, there are tig and tau rb and tt ligand orbital combinations which do not interact with metal orbitals. The molecular orbital energy level scheme expected for the bonding situation described above is shown in Fig. 2. 

FIGURE 3.31 A molecular orbital energy-level diagram for the bonding and antibonding molecular orbitals that can be built from two s-orbitals. The signs of the s-orbitals are depicted by the different shades of blue. 

Draw a molecular orbital energy-level diagram and determine the bond order expected for each of the following species (a) Li2 (b) Li2+ (c) Li2 . State... 

Figure 2.5 Schematic molecular orbital energy level diagram for a transition metal coordination cluster, [ML6]. (a) Energy levels of atomic orbitals of the free cation, M (b) energy levels for the six ligands, L, before bonding (c) molecular orbital energy levels for the octahedral [ML6] cluster.

Figure 11.2 Qualitative molecular orbital energy level diagram for the Fe2+ ion in octahedral coordination. The diagram refers to o-bond formation only.

Figure 11.5 Molecular orbital energy level diagram for pyrite, FeS2 (from Bums Vaughan, 1970). Note the increase of A as a result of Tt-bond formation facilitated in low-spin Fe2+.

Figure 11.6 Molecular orbital energy level diagrams computed for iron octahedrally coordinated to oxygen. Left divalent iron in the [Fe06]-1° cluster (based on Sherman, 1991) right trivalent iron in the [Fe06]-9 cluster (from Sherman, 1985a). Orbital energies have been scaled relative to zero for the non-bonding 6rlu level.

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