Sketch the MO energy level diagram for the oxygen anion superoxide and deduce its ground state electronic configurations. Write down the LCAO for each type of MO.
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- 1. Use the orbital approximation to estimate the energy of an Li atom. How does this value compare to the experimental energy of -3.26x10 J? (Use the Aufbau principle to determine the electron configuration and appropriate hydrogenic atomic orbitals).Write out the ground-state electron configurations of Ru2+Explain the difference in energy of the electron in the 3s orbital with that in the 3d orbital for both hydrogenic and polyelectronic systems.
- Give the ground-state electron configu rations of (a) H2 - . (b) Li2, (c) Be2, (d) C2, (e) N2, and (f) O2 .Describe the orbital approximation. How is it related to the atomic electronic configuration. Describe the trends in the periodic table for size, ionization energy and electronegativity.Write the noble gas orbital box electronic configuration of (i) S, and (ii) Ca*.
- Consider a magnesium (Mg) atom that could have an electronic configuration of either [Ne]3s2 or [Ne]3s13p1. Discuss the following: a) Give one argument for why the [Ne]3s2 configuration might be more stable. b) Give one argument for why the [Ne]3s13p1 configuration might be more stable. c) Which configuration does Mg actually adopt and why?Calculate the number of possible microstates for electron configurations 3s23p2; 3s13p3 en 3s03p4. Show the calculationsWith what neutral molecule ClO–is isoelectronic?
- For each of the statements below, indicate whether it is true or false and explain your reasoning. (1 sentence ) 1/ It takes more energy to ionize an electron from the 2s orbital than an electron from the 2p orbital in the Li2+ ion. 2/ The electron affinity of the Ne atom is larger than the electron affinity of the F atom. 3/ K* has a larger radius than Ar. 4/ For a diatomic molecule, in which the internuclear axis is the z-axis, the 3dz? orbital cannot mix with the 2px orbital. 5/ The internuclear distance of O2 increases as it takes an additional electron to become O2".Q2: a- Explain how such a model uses potentials such as a square well and a harmonic oscillator to try and predict the magic numbers. b- Describe what causes the existence of "magic numbers" for protons and neutrons in nuclei. Why are nuclei which have these magie numbers more stable than other nuclei? Draw any analogies with the energy levels of atomic electrons. c- Discuss briefly the failures of the shell model. ofSuppose that the H2+ ion is excited by light so that an electron moves from a lower-energy to a higher energy MO. Would you expect the excited- state H2+ ion to be stable or to fall apart? Explain.