The most important calcium compound is calcium carbonate, CaCO3, the major constituent of limestone, marble, chalk, oyster shells, and corals. Calcium carbonate obtained from its natural sources is used as a filler in a variety of products, such as ceramics, glass, plastics, and paint, and as a starting material for the production of calcium oxide. Synthetic calcium carbonate, called “precipitated” calcium carbonate, is employed when high purity is required, as in medicine (antacids and dietary calcium supplements), in food (baking powder), and for laboratory purposes.

Calcium oxide, CaO, also known as lime or more specifically quicklime, is a white or grayish white solid produced in large quantities by roasting calcium carbonate so as to drive off carbon dioxide. At room temperature, CaO will spontaneously absorb carbon dioxide from the atmosphere, reversing the reaction. It will also absorb water, converting itself into calcium hydroxide and releasing heat in the process. The bubbling that accompanies the reaction is the source of its name as “quick,” or living, lime. The reaction of quicklime with water is sometimes used in portable heat sources. One of the oldest known products of a chemical reaction, quicklime is used extensively as a building material. It is sometimes used directly as a fertilizer, although calcium carbonate is usually preferred for that purpose. Large quantities of quicklime are used in various industrial neutralization reactions. Limelights, used in the 19th century in stage lighting, emit a very brilliant white light upon heating a block of calcium oxide to incandescence in an oxyhydrogen flame, hence the expression “to be in the limelight.”

A large amount of calcium oxide also is used as starting material in the production of calcium carbide, CaC2, also known simply as carbide, or calcium acetylide. Colourless when pure (though technical grades are typically grayish brown), this solid decomposes in water, forming flammable acetylene gas and calcium hydroxide, Ca(OH)2. The decomposition reaction is used for the production of acetylene, which serves as an important fuel for welding torches. The drip of water on calcium carbide produces a steady stream of acetylene that is ignited in carbide lamps. Such lamps were commonly used in lighthouse beacons and by miners in the early 20th century and still find some use in spelunking. Calcium carbide also is used to make calcium cyanamide, CaCN2, a fertilizer component and starting material for certain plastic resins.

Calcium hydroxide, also called slaked lime, Ca(OH)2, is obtained by the action of water on calcium oxide. When mixed with water, a small proportion of it dissolves, forming a solution known as limewater, the rest remaining as a suspension called milk of lime. Calcium hydroxide is used as an industrial alkali and as a constituent of mortars, plasters, and cement. It is used in the kraft paper process and as a flocculant in sewage treatment.

Another important compound is calcium chloride, CaCl2, a colourless or white solid produced in large quantities either as a by-product of the manufacture of sodium carbonate by the Solvay process or by the action of hydrochloric acid on calcium carbonate. The anhydrous solid is used as a drying agent and for dust and ice control on roads. Calcium hypochlorite, Ca(ClO2), widely used as bleaching powder, is produced by the action of chlorine on calcium hydroxide. The hydride CaH2, formed by the direct action of the elements, liberates hydrogen when treated with water. Traces of water can be removed from many organic solvents by refluxing them in the presence of CaH2.

Calcium sulfate, CaSO4, is a naturally occurring calcium salt. It is commonly known in its dihydrate form, CaSO4∙2H2O, a white or colourless powder called gypsum. As uncalcined gypsum, the sulfate is employed as a soil conditioner. Calcined gypsum is used in making tile, wallboard, lath, and various plasters. When gypsum is heated to about 120 °C (250 °F), it loses three-quarters of its water, becoming the hemihydrate CaSO41/2H2O, plaster of paris. If mixed with water, plaster of paris can be molded into shapes before it hardens by recrystallizing to dihydrate form. Calcium sulfate may occur in groundwater, causing hardness that cannot be removed by boiling.

Calcium phosphates occur abundantly in nature in several forms and are the principal minerals for the production of phosphate fertilizers and for a range of phosphorus compounds. For example, the tribasic variety (precipitated calcium phosphate), Ca3(PO4)2, is the principal inorganic constituent of bone ash. The acid salt Ca(H2PO4)2, produced by treating mineral phosphates with sulfuric acid, is employed as a plant food and stabilizer for plastics.

The hydrogen sulfite, Ca(HSO3)2, is made by the action of sulfur dioxide on a slurry of Ca(OH)2. Its aqueous solution under pressure dissolves the lignin in wood to leave cellulose fibres and thus finds considerable application in the paper industry.

The fluoride, CaF2, is important to the production of hydrofluoric acid, which is made from CaF2 by the action of sulfuric acid. CaF2 is used in laboratory instruments as a window material for both infrared and ultraviolet radiation.

Timothy P. Hanusa
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bone

bone mineral density, estimate of bone mass. Bone is a rich mineral reservoir, composed mainly of calcium and phosphorous, which together impart hardness, rigidity, and compressive strength to bone. Bone is also dynamic in that it is constantly being broken down and rebuilt. A normal individual has a healthy equilibrium between these two opposing processes. However, when the mineral content of bone is taken away faster than it is added, the bone becomes thin, weak, and prone to fracture.

Bone mineral density tests specifically measure the mineral content in one square centimetre of bone and estimate the risk for fracture. An example of a bone mineral density test is the dual-energy X-ray absorptiometry (DXA) scan, which employs minimal amounts of radiation and is commonly used for osteoporosis (bone-thinning) screening. Other types of clinical tests that are used to determine bone mineral density include those based on the use of single-photon absorptiometry, dual-photon absorptiometry, ultrasound, and quantitative computed tomography.

In order to determine whether a person is affected by a reduction in bone density, bone mineral density testing typically is performed on the individual’s wrists, spine, and hips. In the case of a DXA scan, the results are expressed in two numbers, the Z-score and the T-score. The Z-score is derived by comparing a person’s DXA scan result to a healthy person of similar age and represents the number of standard deviations that the patient may diverge from the normal bone mineral density score for his or her age. The Z-score can sometimes shed light on the underlying cause of bone loss. The T-score is derived by comparing a person’s DXA scan result to that of a healthy young adult of the same sex and race or to that of a healthy young adult woman. A T-score between −1.0 and −2.5 indicates osteopenia (a reduced amount of bone tissue), while a T-score of −2.5 indicates osteoporosis.

Muscles of facial expression, human anatomy, (Netter replacement project - SSC). Human face, human head.
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Characteristics of the Human Body

An integral part of preventing bone fractures associated with osteoporosis is early patient screening and intervention. General guidelines recommend obtaining a bone mineral density test in all women aged 65 and older, regardless of the presence of any other risk factors for osteoporosis. Younger postmenopausal women who have one or more risk factors for osteoporosis (e.g., family history, early estrogen deficiency, endocrine abnormalities) and postmenopausal women who experience fractures may also undergo DXA scan screening.

Bone mineral density testing has been shown to significantly reduce fracture risk. For example, by identifying individuals at greatest risk for osteoporosis and employing early intervention, such as lifestyle modification and medications, the risk of hip and vertebral fractures can be reduced by as much as 50 percent.

Shen-Ying (Richard) Ma Dino Samartzis Francis H. Shen