W2013CHM2311 Part 4b Notes

As a general rule if e 2 e 1 13 ev then c1 or c2

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: atomic orbital. You can find the valence orbital potenHal energies for 28 elements in Table 5- 2 on p. 144 (also posted on Blackboard Learn) 1.  Poten0al energies are nega0ve because electrons are favourably acracted to the nucleus. 2.  The poten0al energies given are the average energies for all electrons in the same subshell. 3.  The poten0al energies are for the orbitals in the neutral atoms. Energies of Atomic Orbitals and Orbital Interac0ons In homonuclear diatomics, each of the atomic orbitals of equal energy makes an equal contribuBon to the molecular orbitals. ψ*MO = c1ϕ1 – c2ϕ2 Energy ΔE’ ϕ1 ΔE ϕ2 ψMO= c1ϕ1 + c2ϕ2 For homonuclear diatomics, since there is an equal contribu0on to the MOs from the AOs: Energies of Atomic Orbitals and Orbital Interac0ons In heteronuclear diatomics, each of the atomic orbitals makes a different contribuBon to the molecular orbitals. out- of- phase (an0bonding) interac0on ψ*MO = c2ϕ1 – c1ϕ2 ΔE’ Since the coefficient defines the extent of orbital interac0on, for heteronuclear diatomics: Energy ϕ1 ΔE ϕ2 ψMO= c1ϕ1 + c2ϕ2 in- phase (bonding) interac0on Energies of Atomic Orbitals and Orbital Interac0ons In heteronuclear diatomics, each of the atomic orbitals makes a different contribuBon to the molecular orbitals. out- of- phase (an0bonding) interac0on ψ*MO = c2ϕ1 – c1ϕ2 The closer ϕ2 and ϕ1 are in energy, the closer the MO is to a homonuclear diatomic. ΔE’ Energy ϕ1 ↳  If E (ϕ2) = E (ϕ1), then c1 = c2, the equa0on reduces to the equa0on for homonuclear diatomics....
View Full Document

Ask a homework question - tutors are online