The pure calcium carbonate (CaC 2) occurs in two crystalline forms Calcite in hexagonal shaped, and Aragonite in rhombohedric shaped. Gypsum is also known as calcium sulfate (CaSO 4) is used by builders as a plaster and by nurses for setting bones, as ‘plaster of Paris’.Ĭalcium carbide (CaC 2) is produces when heating up a mixture of carbon & lime at 3000 ✬ in an electric oven and it is an acetylate which produces acetylene (C 2H 2) by hydrolysis (chemical breakdown of a compound due to reaction with water). When calcium hydroxide mixed with sand, it takes up carbon dioxide (CO 2) from the air and hardens as lime plaster. Slaked lime (Ca(OH) 2) is used to make cement, as a soil conditioner, and in water treatment to reduce acidity, and in the chemical industries, It is also used in steel making process to remove impurities from the molten iron ore. When limestone is heated in kilns (furnace) it gives off carbon dioxide (CO 2) gas leaving behind quicklime (Burnt lime or calcium oxide, CaO), which reacts vigorously with water, and give slaked lime ( calcium hydroxide, Ca(OH) 2). It is also used as an alloying agent for copper, aluminium, beryllium, lead and magnesium alloys, and used as a “getter” for residual gases in vacuum tubes, etc.Ĭalcium compounds are widely used, where vast deposits in limestone ( calcium carbonate, CaCO 3) used directly as a building stone and indirectly for cement. Precipitated by phosphate ions in alkaline solutions:ĥ Ca 2+ (aq) + 3 PO 4 3- (aq) + OH – (aq) → Ca 5(SO 4) 3OH (s) Ĭa ions are precipitated by sulfate ions in neutral to alkaline solutions.Ĭa 2+ (aq) + SO 4 2- (aq) → CaSO 4 (s) Calcium Historyĭiscovery & first isolation: Humphry Davy (1808) in London, England Calcium UsesĪCalcium metal is used as a reducing agent (element or compound that donates electron to another chemical species) in preparing other metals such as uranium, thorium, zirconium etc., and is used as a deoxidizer, desulfurizer, or decarburizer (compound used in a reaction to remove oxygen, sulfur,or carbon) for various ferrous and nonferrous alloys.Ĭalcium silicate also known as calcium orthosilicate (Ca 2SiO 4 or 2CaO.SiO 2) is prepared in an electric oven from silica, lime, and reducing carbonated agents, and it is useful as a steel-deoxidizing agent. In reaction forms Ca 2+ with bicarbonate ion (HCO 3 –), by CO 2 with water at seawater, which contain calcium carbonate::ĬaCO 3 (s) + CO 2 + H 2O → Ca 2+ + 2 HCO 3 –Ĭa ions are precipitated by carbonate ions in netural to alkaline solution:Ĭa 2+ (aq) + CO 3 2- (aq) → CaCO 3 (s) ĪCa ions can be precipitated by strong bases: Reacts with halogens, and forming Calcium (II) halides,where the reactions with fluorine & chlorine are exothermic, and with bromine & iodine are endothermic:Ĭa (s) + F 2 (g) → CaF 2 (s) (Calcium (II) fluoride)Ĭa (s) + Cl 2 (g) → CaCl 2 (s) (Calcium (II) chloride)Ĭa (s) + Br 2 (g) → CaBr 2 (s) (Calcium (II) bromide)Ĭa (s) + I 2 (g) → CaI 2 (s) (Calcium (II) iodide)Ĭa dissolves readily in dilute or concentrated hydrochloric acid (HCl), and forms Ca (II) ions & hydrogen gas:Ĭa (s) + 2 HCl (aq) → Ca 2+ (aq) + 2 Cl – (aq) + H 2 (g) Reacts slowly with water, and forming calcium hydroxide & hydrogen:Ĭa (s) + 2 H 2O (l) → Ca(OH) 2 (aq) + H 2 (g) The metal once ignited, it burn in air, and forms a mixture of white calcium oxide (CaO) & calcium nitride (Ca 3N 2): The metal reacts with oxygen at room temp., and forming a thin layer of CaO, which protect the metal from further oxidation. Isotopes: 40 Ca 41 Ca 42 Ca 43 Ca 44 Ca 45 Ca 46 Ca 47 Ca 48 Ca Isotope Ionization energies: 1st: 589.9 kJ.mol 2nd: 1145 kJ/mol 3rd: 4912.5 kJ/molįace Centered Cubic (FCC) Reactivity of CalciumĮlectron affinity: 2.37 kJ/mol Nuclear Properties of Calcium Sound Speed: 3810 m/s Atomic Properties of Calcium Molar magnetic susceptibility: 0.553×10 -9 m 3/mol Physical Properties of Calciumĭensity: 1.55 g/cm 3 (In solid) 1.378 g/cm 3 (In Liquid at M.P) Mass magnetic susceptibility: 13.8×10 -9 m 3/kg

Volume magnetic susceptibility: 0.00002139 Magnetic susceptibility (x mol): +40×10 -6 cm 3/mol Thermal conductivity: 201 W/(m∙K) Electrical properties of CalciumĪ Electrical type: Conductor Magnetic Properties of Calcium Calcium Electron Configuration Thermal Properties of Calciumĭebye temperature: 230 K (-43.15 oC, -45.67 oF)

Ca element