SOE Symmetry Overlap Energy Assignment

SOE: Symmetry–Overlap–Energy à Bonding and antibonding molecular orbitals Adapted from Clayden et al., Organic Chemistry (Oxford University Press, 2000), page 96. © Copyright Oxford University Press, 2007. Atoms interact by overlap of their atomic orbitals (AO's). If the AO's overlap in-phase, electron density is enhanced between the atoms and so the Coulomb energy decreases as the atoms approach. If the AO's overlap out-of-phase, electron density is depleted between the atoms and so the Coulomb energy increases as the atoms approach. For both in-phase and out-of-phase overlap, since the molecular orbital (MO) electron wave is confined to smaller region, and so has smaller wavelength, as the atoms approach the kinetic energy increases. Upper left: In-phase (bonding) AO combination energies: Coulomb contribution (lower, blue curve); kinetic energy contribution (upper, red curve); and total energy (middle, yellow curve). Upper right: Out-of-phase (antibonding) AO combination: Coulomb contribution (middle, blue curve); kinetic energy contribution (lower red curve); and total energy (upper, yellow curve). The small circles compare the energies of the separated atoms (the zero of energy) and total energy at the placed at the bond length (the minimum of the total energy of the in-phase total energy). Lower left: In-phase (bonding) AO combination total energy (blue, lower curve), :and out-of-phase (antibonding) AO combination (red, upper curve). The small circles compare the energies of the separated atoms (the zero of energy) and total energy at the placed at the bond length (the minimum of the total energy of the inphase total energy). Lower right: Correlation diagram relating the energies of the AO's when the atoms are wide apart with the energies of the MO's formed from the in-phase IMObond ) and out-of-phase (MOantibond ) overlap. The small circles on the diagrams compare the energies of the separated atoms (the zero of energy) and total energy at the bond length (the minimum of the in-phase total energy). The correlation diagram (lower right) is a compact way of representing this comparison. The middle part of the correlation diagram corresponds to the atoms separated by the bond distance; the left and right parts corresponds to the atoms far enough apart that there is no overlap of their AO's and so no bonding or antibonding effect on total energy. Here are questions about the energy of MO's formed from the combination of AO's as atoms approach one another. 1. The kinetic energy of the antibonding combination of a pair of AO's is ... A greater than that for the bonding combination B about the same that for the bonding combination C less than that for the bonding combination 2 The total energy of the antibonding combination of a pair of AO's is ... A never negative B has a minimum near the bond distance C about the same as for the bonding combination D is smaller the larger the separation E A and D 3 The potential energy of the antibonding combination of a pair of AO's is ... A never negative B about zero C about the same as for the bonding combination 4 As a pair of atoms approach from a large separation, initially the energy resulting from in-phase overlap of their AO's ... A goes up, due to increased kinetic energy. B goes down, due to enhancement of electron density between C goes up, due to depletion of electron density between the D None of the above 5 As a pair of atoms approach from a large separation, initially the energy of the MO resulting from out-of-phase overlap of their AO's ... A goes down, due to decreased kinetic energy. B goes down, due to enhancement of electron density between C goes up, due to depletion of electron density between the D None of the above 6 A pair of atoms approach from a large separation, and the resulting MO has equal amounts of in-phase and out-of-phase overlap of their AO's. The result is that initially the total energy ... A goes up, due to increased kinetic energy. B goes down, due to enhancement of electron density between C goes up, due to depletion of electron density between the D None of the above à Symmetry If AO's have only in-phase or only out-of-phase overlap, we say they have correct symmetry. If AO's have equal amounts of in-phase and out-of-phase overlap, we say they have incorrect symmetry. Adapted from Clayden et al., Organic Chemistry (Oxford University Press, 2000), page 103. © Copyright Oxford University Press, 2007. 7 Which pairs of AO's on different atoms have correct symmetry? A 1s + 1s B 1s + 2s C both D neither 8 Which pairs of AO's on different atoms have correct symmetry? Assume z is along bond axis. A 1s + 2pz B 1s + 2py C both D neither 9 Which pairs of AO's on different atoms have correct symmetry? Assume z is along bond axis. A 2s + 2pz B 2s + 2py C both D neither 10 Which pairs of AO's on different atoms have correct symmetry? Assume z is along bond axis. A 2pz + 2pz B 2pz + 2py C both D neither 11 Which pairs of AO's on different atoms have correct symmetry? Assume z is along bond axis. A 2px + 2py B 2px + 2px C both D neither à Overlap If AO's have correct symmetry, then we consider next how much they overlap. The greater the overlap, the greater the energy change, relative to the AO energies, when the atoms are at the bond length separation. 12 Arrange the pairs of AO's in Li2 according to increasing overlap when the atoms are at the lowest energy separation (the bond length). A 1s + 1s < 2s + 2s < 1s + 2s B 1s + 2s < 1s + 1s < 2s + 2s C 1s + 1s < 1s + 2s < 2s + 2s à Energy Finally, once we know the pair of AO's with correct symmetry and greatest overlap, we consider relative AO energies. The bonding/antibonding effect will be greatest for AO's closest in energy. Adapted from Clayden et al., Organic Chemistry (Oxford University Press, 2000), page 103. © Copyright Oxford University Press, 2007. 13 Arrange the pairs of AO's in Li2 according to increasing energy change at the bond length. A 1s + 1s < 2s + 2s < 1s + 2s B 1s + 2s < 1s + 1s < 2s + 2s C 1s + 1s < 1s + 2s < 2s + 2s 14 Which pair of AO's in HF will interact most strongly? Assume z is along the bond axis. A H 1s + F 1s B H 1s + F 2s C H 1s + F 2pz D H 1s + F 2py E C and D 15 Assume AO1 and AO2 have correct relative symmetry, greatest overlap, and are closest in energy. AO1 has IE = 5 eV and AO2 has IE = 6 eV. Which of the following is true? Adapted from Clayden et al., Organic Chemistry (Oxford University Press, 2000), page 102. © Copyright Oxford University Press, 2007. A Bonding MO has more AO1 than AO2 C Antibonding MO is almost entirely AO1 E A and D B Bonding MO has more AO2 than AO1 D Antibonding MO is almost entirely AO2 F B and C 16 AO1 has IE = 3 eV and AO2 has IE = 12 eV. Which of the following is true? Adapted from Clayden et al., Organic Chemistry (Oxford University Press, 2000), page 101. © Copyright Oxford University Press, 2007. A Bonding MO is almost entirely AO1 B Bonding MO is has a little more AO2 than AO1 C Antibonding MO is almost entirely AO1 D Antibonding MO has a little more AO1 than AO2 E None of the above F B and C 17 The bond pair in Na:F is in the Na 3s + F 2pz MO. The bond pair in H:F is in the H 1s + F 2pz MO. Which of the following is true? A The bond pair is almost entirely on the F of HF. B The bond pair is almost entirely on the H of HF. C The bond pair is almost entirely on the F of NaF. D The bond pair is almost entirely on the Na of NaF. E A and D 18 Na 3s has IE = 5.1 eV. H 1s has IE = 13.6 eV. F has IE = 17.4 eV. NaF is more ionic than HF because ... A Na 3s has lower IE than does H 1s B F 2pz has higher IE than does H 1s C Na 3s has lower IE than does F 2pz D F 2pz has higher IE than does Na 3s 19 A key concept in chemistry is that it is the valence electrons on different atoms that interact with one another, rather than the core electrons. What is the best explanation for this? A Adjacent valence electron waves have the greatest in-phase or out-of-phase overlap. B Adjacent valence electron waves have the same energy. C Core electron clouds have the wrong symmetry. D Core electron clouds move with the wrong frequency.