Calcium

The chemical element Calcium (Ca), atomic number 20, is the fifth element and the third most abundant metal in the earth’s crust. The metal is trimorphic, harder than Sodium, but softer than Aluminium. A well as Beryllium and Aluminium, and unlike the alkaline metals, it doesn’t cause skin-burns. It is less chemically reactive than alkaline metals and than the other alkaline-earth metals.

Calcium ions solved in water form deposits in pipes and boilers and when the water is hard, that is, when it contains too much Calcium or Magnesium. This can be avoided with the water softeners. In the industry, metallic Calcium is separated from the melted Calcium Chloride by electrolysis. This is obtained by treatment of Carbonated minerals with chlorhydric acid, or like a sub product of the Carbonates Solvay process.

In contact with air, Calcium develops an oxide and nitride coating, which protects it from further corrosion. It burns in the air at a high temperature to produce nitride.

The commercially produced metal reacts easily with water and acids and it produces Hydrogen which contains remarkable amounts of ammonia and hydrocarbides as impurities.

Applications

The metal is used in Aluminium alloys for bearings, as a helper in the Bismuth removal form lead, as well as in controlling graphitic Carbon in melted Iron. It is also used as a deoxidizer in the manufacture of many steels; as a reducing agent in the preparation of metals as Chromium, Thorium, Zirconium and Uranium, and as separating material for gaseous mixtures of Nitrogen and Argon. Calcium is an alloying used in the production of Alluminium, Beryllium, Copper, lead and Magnesium alloys. It is also used in making cements and mortar that are used in builldings.

The Calcium oxide, CaO, is produced by thermal decomposition of Carbonated minerals in furnaces, applying a continuous bed process.  The oxide is used in high intensity light arcs (lime light) for its unusual spectral characteristics and as dehydrating industrial agent. The metallurgic industry extensively uses the oxide during the reduction of ferrous alloys.

The Calcium oxide, Ca(OH)₂, has many applications in which the hydroxyl ion is necessary. In the process of Calcium hydroxide quenching, the volume of blown out lime [Ca(OH)₂] expends to double the initial quantity of quick lime (CaO), fact that makes it useful to break down rocks or wood.

The quick lime is an excellent absorbent for the Carbon dioxide, because it produces Carbonate, which is very insoluble.

The Calcium silicate, CaSi, prepared in an electric oven from lime, silica and reducing Carbonated agents, is useful as a steel-deoxidizing agent. Calcium carbide, CaC₂, is produces when heating up a mixture of lime and Carbon at 3000ºC in an electric oven and it is an acetylate which produces acetylene by hydrolysis. The acetylene is the base material of a great number of important chemicals for the organic industrial chemistry.

The pure Calcium Carbonate occurs in two crystalline forms: calcite, hexagonal shaped, which possesses birrefringent properties, and aragonite, rhombohedric. The natural Carbonates are the most abundant Calcium minerals. The Iceland spar and the calcite are essentially pure Carbonate forms, whilst the marble is impure and much more compact, reason why it can be polished. It’s very demanded as construction material. Although the Calcium Carbonate is very little soluble in water, it is quite soluble if the water contains dissolved Carbon dioxide, for in these solutions it forms biCarbonate when dissolving. This fact explains the cave formation, where the lime stone deposits have been in contact with acid waters.

The Calcium halogenures include phosphorescent fluoride, which is the Calcium compound more abundant and with important applications in spectroscopy. The Calcium Chloride possesses, in the anhydric form, great deliquescence capacity, which makes it useful as industrial dehydrating agent and as sand whirl control factor in roads. Calcium hypochlorite (whitening powder) is produced in the industry when passing Chlorine through a lime solution, and has been used as a whitening agent and as water purifier.

The dehydrated Calcium sulphate is the mineral gypsum, constitutes the bigger portion of Portland concrete, and has been used to reduce the alkalinity of soils. Heating gypsum at high temperatures produces a Calcium sulphate hemihydrate, which is sold with the commercial name of Parisian stucco.

Calcium in the environment

Calcium is the fifth element and the third most abundant metal in the earth’s crust. The Calcium compounds account for 3.64% of the earth’s crust. The distribution of Calcium is very wide; it is found in almost every terrestrial area in the world. This element is essential for the life of plants and animals, for it is present in the animal’s skeleton, in tooth, in the egg’s shell, in the coral and in many soils. Seawater contains 0.15% of Calcium Chloride.

Calcium is always present in every plant, as it is essential for its growth. It is contained in the soft tissue, in fluids within the tissue and in the structure of every animal’s skeleton. The vertebrate’s bones contain Calcium in the form of Calcium fluoride, Calcium Carbonate and Calcium phosphate.

Health effects of Calcium

Calcium is the most abundand metal in the human body: is the main constituent of bones and theets and it has keys metabolic functions.
Calcium is sometimes referred to as lime. It is most commonly found in milk and milk products, but also in vegetables, nuts and beans. It is an essential component for the preservation of the human skeleton and teeth. It also assists the functions of nerves and muscles. The use of more than 2,5 grams of Calcium per day without a medical necessity can lead to the development of kidney stones and sclerosis of kidneys and blood vessels.

A lack of Calcium is one of the main causes of osteoporosis. Osteoporosis is a disease in which the bones become extremely porous, are subject to fracture, and heal slowly, occurring especially in women following menopause and often leading to curvature of the spine from vertebral collapse.

Unlike most of the people think, there is an intense biological activity inside our bones. They are being renewed constantly by new tissue replacing the old one. During childhood and adolescence, there’s more production of new tissue than destruction of the old one, but at some point, somewhere around the 30 or 35  years of age, the process is inverted and we start to loose more tissue than what we can replace. In women the process is accelerated after the menopause (he period marked by the natural and permanent cessation of menstruation, occurring usually between the ages of 45 and 55); this is because their bodies stop producing the hormone known as estrogen, one of which functions is to preserve the osseous mass. 

Evidence suggests that we need a daily intake of 1,000 milligrams of Calcium in order to preserve the osseous mass in normal conditions. This is both for man and pre-menopausic women. The recommended daily intake rises to 1,500 for menopausic woman.

The main Calcium sources are the dairy products, but also nuts, some green vegetables like spinach, and cauliflower, beans, lentils…

Calcium works together with Magnesium to create new osseous mass. Calcium should be taken together with Magnesium in a 2:1 rate, that is to say, if you ingest 1000 mg of Calcium, you should also ingest 500 mg of Magnesium. Some Magnesium sources in the diet are seafood, whole-grains, nuts, beans, wheat oats, seeds and green vegetables.

Other important measures to prevent osteoporosis are:

• Doing regular exercise (at least three times a week)
  
• Taking adequate amounts of Manganese, folic acid, vitamin B₆ , vitamin B₁₂ , omega 3 (it aids Calcium absorption and stimulates new osseous mass production) and vitamin D (it aids Calcium absorption in the small intestine).
  
• Not abusing of sugar, saturated grease and animal proteins
  
• Not abusing of alcohol, caffeine, nor gaseous drinks
  
• Not smoking

Other triggers for osteoporosis are the hereditary factor and the stress.
   

Environmental effects of Calcium

Calcium phosphide is very toxic to aquatic organisms.