For molecules containing atoms with electrons in p orbitals, energy-level diagrams become more complex. Core electrons are usually omitted from MO energy level diagrams. Discuss with your group or the class the following: (a) Why are core electrons usually omitted? For the second-row diatomics what is the lowest MO formed from valence shell orbitals? (b) Describe how molecular orbitals are formed from atomic orbitals. Would you expect them to be higher or lower in energy than o (sigma) molecular orbitals? (c) As the nuclear charge increases, the energies of all orbitals are lowered, as shown in the figure below for homonuclear diatomics. Why does this happen?

For molecules containing atoms with electrons in p orbitals, energy-level diagrams become more complex. Core electrons are usually omitted from MO energy level diagrams. Discuss with your group or the class the following: (a) Why are core electrons usually omitted? For the second-row diatomics what is the lowest MO formed from valence shell orbitals? (b) Describe how molecular orbitals are formed from atomic orbitals. Would you expect them to be higher or lower in energy than o (sigma) molecular orbitals? (c) As the nuclear charge increases, the energies of all orbitals are lowered, as shown in the figure below for homonuclear diatomics. Why does this happen?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

could you anwer this?
Relate the energies of the orbitals found (these we will use for building Molecular Orbital energy level diagrams) to Z*, also known as Zeff, determined by Slater’s rules Please show calculations for the following: H (1s electron) He (1s electron)
The existence of compounds of the noble gases was once a great surprise and stimulated a great deal of theoretical work. Sketch the molecular orbital energy level diagram for XeF and deduce its ground state electron configurations. Is XeF likely to have a shorter bond length than XeF+?
4. Amphotericin B is a polyene antifungal agent. In the molecule, 6 C-C single bonds and 7 C=C double bonds alternate along a chain of 14 C atoms; see a schematic of the structure of the molecule below. OH OH HO O OH OH OH OH O,,.. OH HO" ОН OH NH₂ Each C atom contributes 1 p electron to the 77 orbitals in the conjugated system giving 14 electrons that move along the molecule. Assuming an average inter-nuclear distance of 140 pm, and that, in the ground state of amphotericin B, each quantum state is occupied by two electrons, use the particle-in-a-box model to calculate (a) the energy separation between the highest occupied state and the lowest unoccupied state, and (b) the frequency of the radiation required to produce a transition between the two states.
Draw the Lewis structure of CH₃CCH and then choose the appropriate set of hybridization states for the three central atoms. Your answer choice is independent of the orientation of your drawn structure.
Draw a labelled diagram showing the atomic orbitals for C and O on each side and the molecular orbitals for CO in the middle. The diagram should clearly show: /) which atomic orbitals combine to form each molecular orbital, ii) the relative position (increasing energy going up the page) of the molecular orbitals and the locations of electrons in the atomic orbitals and the molecular orbitals. Use your diagram to determine the following: • What is the bond order? Explain how you obtained this number from your MO diagram. The calculation must be presented. • Is the molecule diamagnetic or paramagnetic? Explain how you deduced this from your MO diagram. • From the following three possibilities, CO+, CO, CO-, determine which has the strongest bond? Explain with reference to your MO diagram.
Explain from the position of Molecular Orbital Theory the change of dissociation energy (energy required to split the bond Ed) for the following: F2 molecules have Ed =155 kJ/mol O2 molecules have Ed= 493/ kJ/mol N2 molecules have Ed= 945 kJ/mol
ST 9C.2- Calculate the energy (in eV) of an antibonding molecular orbital for the molecule XY (with X being more electronegative) given the information below. Note how much closer (a little bit higher) it is to the energy of Y's atomic orbital than X's atomic orbital. a (X) = -11.2 eV a (Y) = -8.8 eV B = -1.0 eV Type your answer...
(a) Using the molecular orbital model, write the valence electron configuration for CN and use it to calculate the bond order. Is the species paramagnetic? Bond order = Paramagnetic? (b) Using the molecular orbital model, write the valence electron configuration for CO and use it to calculate the bond order. Is the species paramagnetic? Bond order = Paramagnetic?
(d) In the formation of CO, the 2s orbital from C and 2p orbital from O could also participate in the formation of σ molecular orbital. Explain why this is possible?
6. For heteronuclear diatomic molecules, the energy-level diagrams of the molecular orbitals need to be modified via calculation. For both NO and CN', the order of molecular orbitals are similar to that of O,. Write electron configurations of NO and CN including core electrons, starting with o1,'01,*². Which bond is stronger? (hint: bond order)
the options for atom B are linear, tetrahedral, or trigonal planar. Betwwen those would it be tetrahedral or trigonal planar?