Explain the difference between the and MOs for homonuclear diatomic molecules. How are bonding and antibonding orbitals different? Why are there two MOs and one MO? Why are the MOs degenerate? 3.
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The Pauli exclusion principle No two electrons in an atom can have the same quantum numbers n, l, m , and m l s – this means that an orbital can never have more than two electrons in it The Aufbau or filling principle In multielectron atoms, the electrons fill up the available energy levels (orbitals) starting with the lowest available level Orbital energies The orbitals in a multielectron atom do not have the same size or energy as the corresponding orbitals in a hydrogen atom – this is because the electrons in them experience an effective nuclear charge (Z eff) that is different from 1 (one) Effective nuclear charge Each electron is attracted to the nucleus and repelled by
Author: Steven S. Zumdahl
This textbook survival guide was created for the textbook: Chemistry, edition: 8. The full step-by-step solution to problem: 2 from chapter: 9 was answered by , our top Chemistry solution expert on 11/15/17, 04:25PM. Chemistry was written by and is associated to the ISBN: 9780547125329. The answer to “Explain the difference between the and MOs for homonuclear diatomic molecules. How are bonding and antibonding orbitals different? Why are there two MOs and one MO? Why are the MOs degenerate? 3.” is broken down into a number of easy to follow steps, and 32 words. This full solution covers the following key subjects: mos, explain, Degenerate, diatomic, difference. This expansive textbook survival guide covers 22 chapters, and 2897 solutions. Since the solution to 2 from 9 chapter was answered, more than 279 students have viewed the full step-by-step answer.