The metal atoms are held together by the interactions of the valence electrons (outermost electrons) and the positive metallic ions. The electrons are free to move throughout the solid (sea of electrons) because the valence electrons are not bound between metal ions. Such an arrangement is called the metallic bond, to distinguish it from the covalent bond, in which electrons are shared between one another (Fig. 4–1).
KeywordsCorrosion Rate Electrode Potential Valence Electron Metallic Bond Galvanic Corrosion
Unable to display preview. Download preview PDF.
- L. V. Azàroff, Introduction to Solids, chapters 4 and 5, McGraw-Hill Book Co., New York, 1960.Google Scholar
- M. G. Fontana and N. O. Greene, Corrosion Engineering, McGraw-Hill Book Co., New York, 1967.Google Scholar
- A. G. Guy, Essentials of Materials Science, chapter 2, McGraw-Hill Book Co., New York, 1976.Google Scholar
- A. G. Guy, Physical Metallurgy for Engineers, Addison-Wesley, Reading, Massachusetts, 1962.Google Scholar
- L. H. Van Vlack, A Textbook of Materials Technology, chapters 3–6, Addison-Wesley, Reading, Massachusetts, 1973.Google Scholar
- L. H. Van Vlack, Materials Science for Engineers, chapters 6 and 22, Addison-Wesley, Reading, Massachusetts, 1970.Google Scholar