Abstract
The halogens—fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At)—make up group 17 (VIIA) of the elements. Because of their propensity to form salts [the standard potentials (E 0, volts) for the oxidation of halides (2X−→X2 + 2e −) are −3.06, −1.36, −1.07, and −0.54 for fluorine, chlorine, bromine, and iodine, respectively], Berzelius designated these elements as “halogens” (Greek hals, sea salt; gennao, I beget). The halogens make up a particularly well defined family, having the most regular gradation of physical properties of all the families of elements. Thus, an almost perfect doubling of atomic weights on going from one halogen to the next down the periodic table is accompanied by an increase in specific gravity, melting points, and boiling points, and a decrease in water solubility and chemical reactivity (Table 1–1) (Stokinger, 1981). The concentrations of the halogens found in seawater and in the lithosphere are given in Table 1–2.
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© 1991 Plenum Press, New York
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Kirk, K.L. (1991). The Halogens: Discovery, Occurrence, and Biochemistry of the Free Elements. In: Biochemistry of the Elemental Halogens and Inorganic Halides. Biochemistry of the Elements, vol 9A+B. Springer, Boston, MA. https://doi.org/10.1007/978-1-4684-5817-6_1
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DOI: https://doi.org/10.1007/978-1-4684-5817-6_1
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