SELENIUM 217
4. CHEMICAL AND PHYSICAL INFORMATION
4.1 CHEMICAL IDENTITY
Information regarding the chemical identity of selenium and selenium compounds is presented in
Table 4-1.
4.2 PHYSICAL AND CHEMICAL PROPERTIES
Selenium is a non-metal element with atomic number 34 and an atomic mass of 78.96 (Lide 2000).
Selenium belongs to Group 6 (Group VIA) of the periodic table, located between sulfur and tellurium,
and resembles sulfur both in its various forms and in its compounds. The six stable isotopes of selenium
are
74
Se,
76
Se,
77
Se,
78
Se,
80
Se, and
82
Se. These isotopes occur naturally with approximate abundances of
0.87, 9.02, 7.58, 23.52, 49.82, and 9.19%, respectively (Hoffmann and King 1997). Artificial radioactive
isotopes of selenium have also been created by neutron activation. The gamma-emitting isotope
75
Se has
been used in diagnostic applications of medicine (Hoffmann and King 1997). Selenium exists in several
allotropic forms. Three are generally recognized, but as many as six have been claimed (Lide 2000). The
stable form at ordinary room temperatures is the grey or hexagonal form with a melting point of 220.5 EC
(Lide 2000). The other two important forms are red (monoclinic) with a melting point of 221 EC and
amorphous selenium, which exists in black and red forms. Black amorphous selenium is vitreous and is
formed by the rapid cooling of liquid selenium. Red amorphous selenium is colloidal and is formed in
reduction reactions (Hoffmann and King 1997). Important selenium oxidation states are -2, 0, +4, and +6.
The chemical properties of selenium are similar to sulfur. Selenium combines with metals and many
nonmetals directly or in aqueous solution. The selenides resemble sulfides in appearance, composition,
and properties (Hoffmann and King 1997). Selenium may form halides by reacting vigorously with
fluorine and chlorine, but the reactions with bromine and iodide are not as rapid. Selenium does not react
directly with hydrogen fluoride or hydrogen chloride, but decomposes hydrogen iodide to liberate iodine
and yield hydrogen selenide (Hoffmann and King 1997). Selenium reacts with oxygen to form a number
of oxides, the most stable of which is selenium dioxide.
Information regarding the physical and chemical properties of selenium and selenium compounds is
located in Table 4-2.