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Chapter 6 Electronic Structure of Atoms

This chapter explores the electronic structure of atoms, including orbital diagrams, Hund's rule, and anomalies in the periodic table. Learn how to represent orbitals and electrons, understand the rules governing electron arrangement, and discover the irregularities that occur in certain elements.

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Chapter 6 Electronic Structure of Atoms

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  1. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 6Electronic Structureof Atoms John D. Bookstaver St. Charles Community College St. Peters, MO  2006, Prentice Hall, Inc.

  2. Orbital Diagrams • Each box represents one orbital. • Half-arrows represent the electrons. • The direction of the arrow represents the spin of the electron.

  3. Hund’s Rule “For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximized.”

  4. Periodic Table • We fill orbitals in increasing order of energy. • Different blocks on the periodic table, then correspond to different types of orbitals.

  5. Some Anomalies Some irregularities occur when there are enough electrons to half-fill s and d orbitals on a given row.

  6. Some Anomalies For instance, the electron configuration for copper is [Ar] 4s1 3d5 rather than the expected [Ar] 4s2 3d4.

  7. Some Anomalies • This occurs because the 4s and 3d orbitals are very close in energy. • These anomalies occur in f-block atoms, as well.

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