Calcium Chemische Eigenschaften,Einsatz,Produktion Methoden
ERSCHEINUNGSBILD
GL?NZENDES SILBERWEISSES METALL (AN FRISCHEN SCHNITTFL?CHEN); VERF?RBT SICH BL?ULICH GRAU AN FEUCHTER LUFT.
PHYSIKALISCHE GEFAHREN
Entzündet sich in feinverteilter Form an der Luft.
CHEMISCHE GEFAHREN
Reagiert mit Wasser, Alkohol und verdünnten S?uren unter Bildung leichtentzündlichen Wasserstoffs. Reagiert mit Halogenen. Brennt an der Luft. Kontakt mit Alkalihydroxiden oder -carbonaten kann Explosionen verursachen.
ARBEITSPLATZGRENZWERTE
TLV nicht festgelegt (ACGIH 2005).
MAK nicht festgelegt (DFG 2005).
WIRKUNGEN BEI KURZZEITEXPOSITION
WIRKUNGEN BEI KURZZEITEXPOSITION: Die Substanz reizt die Augen.
LECKAGE
Alle Zündquellen entfernen. Verschüttetes Material in Beh?ltern sammeln. NICHT in die Kanalisation spülen. Reste sorgf?ltig sammeln. An sicheren Ort bringen. NICHT mit S?gemehl oder anderen brennbaren Absorptionsmitteln binden. Pers?nliche Schutzausrüstung: Vollschutzanzug mit umgebungsluftunabh?ngigem Atemschutzger?t.
R-S?tze Betriebsanweisung:
R15:Reagiert mit Wasser unter Bildung hochentzündlicher Gase.
S-S?tze Betriebsanweisung:
S8:Beh?lter trocken halten.
S24/25:Berührung mit den Augen und der Haut vermeiden.
S43:Zum L?schen . . . (vom Hersteller anzugeben) verwenden (wenn Wasser die Gefahr erh?ht, anfügen: "Kein Wasser verwenden").
Chemische Eigenschaften
Calcium is a silvery-white metal when freshly cut, which tarnishes to a blue-gray color in air. It can also be found as a powder.
Calcium cations (Ca2+ ) and calcium salts are among the most commonly encountered substances in water, arising mostly from dissolution of minerals. Calcium often is the most abundant cation in river water. Among the most common calcium minerals are the two crystalline forms of calcium carbonate-calcite and aragonite (CaCO 3 , limestone is primarily calcite), calcium sulfate (the dehydrated form, CaSO4 , is anhydrite; the hydrated form, CaSO4.2H2O, is gypsum), calcium magnesium carbonate (CaMg(CO3) 2 , dolomite), and, less often, calcium fluoride (CaF2 , fluorite).
Physikalische Eigenschaften
Bright, silvery-white metal; face-centered cubic crystal structure (α = 0.5582 nm) at ordinary temperatures, transforming to body-centered cubic form (α = 0.4407) at 430°C; density 1.54 g/cm
3 at 20°C; hardness 2 Mohs, 17 Brinnel (500 kg load); melts at 851°C; vaporizes at 1,482°C; electrical resistivity 3.43 and 4.60 microhm-cm at 0° and 20°C, respectively; modulus of elasticity 3-4x106 psi; mass magnetic susceptibility +1.10x10-6 cgs; surface tension 255 dynes/cm; brick-red color when introduced to flame (flame test); standard reduction potential E° = -2.87V.
Verwenden
Calcium is used as a deoxidizer for copper,steel, and beryllium in metallurgy; to hardenlead for bearing; and in making alloys.
Definition
Alkaline-earth element of atomic number 20, group
IIA of the periodic table. Aw 40.08. Valence 2. Six
stable isotopes.
Vorbereitung Methode
Calcium may be obtained by electrolytic or thermal reduction of its salts.Electrolytic reduction involves electrolysis of partially molten calcium chloride at 780° to 800°C in a graphite lined steel vessel. The method requires precise control of temperature and current. The solid deposit of metal produced may contain entrapped salt and impurities such as chlorine and nitrogen. It is re-melted to reduce impurity levels.
Currently, thermal reduction processes have replaced the electrolysis method. The starting material in these methods is limestone, which is calcined to produce calcium oxide. The latter is ground, mixed and compacted with aluminum, and reduced at temperatures between 1,000° to 1,200°C under vacuum. Calcium vapors formed in low yield under such thermodynamic conditions are transferred from the reactor and condensed in cool zones, thus shifting the equilibrium to allow formation of more calcium vapors. The reactions are as follows:
4Ca + 2Al → CaOAl
2O
3 + 3Ca (vapor)
6Ca + 2Al → 3CaOAl
2O
3 + 3Ca (vapor).
Allgemeine Beschreibung
A silvery, soft metal that turns grayish white on exposure to air. Used in metallurgy.
Air & Water Reaktionen
Pyrophoric ignites in air when finely divided, then burns with crimson flame [Merck 11th ed. 1989]. Calcium rapidly decomposes in water, the heat of reaction is sufficient that hydrolysis released hydrogen may ignite [Lab. Gov. Chemist 1966].
Reaktivit?t anzeigen
Boron trifluoride reacts with incandescence when heated with alkali metals or alkaline earth metals except magnesium [Merck 11th ed. 1989]. Calcium reacts violently with acids [Lab. Govt. Chemist 1965]. Finely divided Calcium burns spontaneously in chlorine at elevated temperatures [Mellor 3:637, 638, 651 1946-47]. Finely divided or massive Calcium burns spontaneously in fluorine at ordinary temperatures. Calcium is incompatible with metal oxides, alkali metal hydroxides, chlorine fluorides, dinitrogen tetraoxide, and sulfur(with sulfur reacts explosively when ignited) [Bretherick, 5th Ed., 1995].
Hazard
Evolves hydrogen with moisture.
Flammable in finely divided state. Fire and
explosion hazard when heated or on contact with
strong oxidizing agents.
Health Hazard
Calcium is an essential nutrient for plants and animals, essential for bone, nervous system, and cell development. Recommended daily intakes for adults are between 800 and 1200 mg/day. Most of this is obtained in food; drinking water typically accounts for 50–300 mg/day, depending on the water hardness and assuming inges- tion of 2 L/day. Calcium in food and water is essentially nontoxic. A number of stud- ies suggest that water hardness protects against cardiovascular disease. One possible adverse effect from ingestion of high concentrations of calcium for long periods of time may be a greater risk of kidney stones. The presence of calcium in water decreases the toxicity of many metals to aquatic life. Stream standards for these met- als are expressed as a function of hardness and pH. Thus, the presence of calcium in water is beneficial and no limits on calcium have been established for protection of human or aquatic health.
Brandgefahr
Produce flammable gases on contact with water. May ignite on contact with water or moist air. Some react vigorously or explosively on contact with water. May be ignited by heat, sparks or flames. May re-ignite after fire is extinguished. Some are transported in highly flammable liquids. Runoff may create fire or explosion hazard.
Mechanism of action
About 48% of serum calcium is ionic, ca 46% is bound to blood proteins, the rest is present as diffusible complexes, e.g., of citrate. The calcium ion level must be maintained within definite limits.
Bones act as a reservoir of certain ions, in particular Ca2+ and PO4
3-, which readily exchange between bones and blood. Bone structure comprises a strong organic matrix combined with an inorganic phase which is principally hydroxyapatite, 3Ca3(PO4)2·Ca(OH)2. Bones contain two forms of hydroxyapatite. The less soluble crystalline form contributes to the rigidity of the structure. The crystals are quite stable, but because of the small size present a very large surface area available for rapid exchange of ions and molecules with other tissues. There is also a more soluble intercrystalline fraction. Bone salts also contain small amounts of magnesium, sodium, carbonate, citrate, chloride, and fluoride. Osteoporosis is reported to result when bone resorption is relatively faster than bone formation. The calcium ion, necessary for blood-clot formation, stimulates release of bloodclotting factors from platelets.
m?gliche Exposition
Calcium is used as a raw material for
aluminum, copper, and lead alloys.
Carcinogenicity
No studies on the carcinogenicity
of elemental calcium were noted. The carcinogenicity of
calcium chromate is attributed solely to intracellular soluble
chromium.
l?uterung methode
Clean the metal by washing it with ether to remove adhering paraffin, file the surface in an argon-filled glove box, and wash it with ethanol containing 2% of conc HCl. Then wash it with dry ethanol, dry it in a vacuum and store it under pure argon [Addison et al. J Chem Soc 3868 1962].
Inkompatibilit?ten
Forms hydrogen gas on contact with air;
finely divided material or dust may ignite spontaneously. A
strong reducing agent; reacts violently with water, acids,
strong oxidizers (such as chlorine, bromine, and fluorine),
alkaline carbonates, dinitrogen tetroxide; halogenated
hydrocarbons; lead chloride, halogens, alkaline hydroxides,
oxygen, silicon, sulfur, chlorine, fluorine, chlorine trifluoride, and many other substances. Reacts with water to produce flammable hydrogen gas
Calcium Upstream-Materialien And Downstream Produkte
Upstream-Materialien
Downstream Produkte
