W2013CHM2311 Part 4b Notes

2 the poten0al energies given are the average

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Unformatted text preview:   If we were to look at the molecular orbitals, the shapes would be distorted from those of homonuclear diatomics. 4σ* 1π 1π 2s 2s C 2σ* 1σ CO 2s O MO Diagram for CO Some differences from homonuclear diatomics: 2π* 2π* 2p 1.  Atomic orbitals on different atoms have different energies. ↳  e.g., carbon 2s and oxygen 2s 3.  Molecular orbitals are no longer given “g” and “u” symmetry labels due to distor0on in their shapes. 4.  To dis0nguish between orbitals, they are given numbers. The lowest energy σ is 1, the next is 2, etc. Other numbering systems are also frequently used. 3σ 2p energy 2.  If we were to look at the molecular orbitals, the shapes would be distorted from those of homonuclear diatomics. 4σ* 1π 1π 2s 2s C 2σ* 1σ CO 2s O MO Diagram for CO Some differences from homonuclear diatomics: 1.  Atomic orbitals on different atoms have different energies. ↳  e.g., carbon 2s and oxygen 2s 2.  If we were to look at the molecular orbitals, the shapes would be distorted from those of homonuclear diatomics. 3.  Molecular orbitals are no longer given “g” and “u” symmetry labels due to distor0on in their shapes. 4.  To dis0nguish between orbitals, they are given numbers. The lowest energy σ is 1, the next is 2, etc. Other numbering systems are also frequently used. Figure 5- 14 Miessler and Tarr (p136) Energies of Atomic Orbitals General Rule: More electronega0ve atoms have lower energy atomic orbitals. ↳  e.g., the more 0ghtly electrons are held to the nucleus, the lower the energy of the...
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This note was uploaded on 03/28/2014 for the course CHM 2311 taught by Professor Richardson during the Winter '09 term at University of Ottawa.

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