About Calcium information

8/10/2019 About Calcium information

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Calcium

Ca lcium, 20 Ca

Spectral lines of calcium

General properties

Name, symbol calcium, CaPronunciation / klsim/

KAL-see- m

Appearance dull gray, silverCalcium in the periodic table

Mg

CaSr

potassium calciu m scandium

Atomic number 20Standard atomicweight

40.078(4)

Elementcategory alkaline earth metal

Group , block group 2 (alkaline earth metals),s-block

Period period 4Electronconfiguration

[Ar] 4s2

per shell 2, 8, 8, 2

Physical properties

Phase solid

Melting point 1115 K (842 C, 1548 F)Boiling point 1757 K (1484 C, 2703 F)Density near r.t. 1.55 gcm3

liquid, at m.p. 1.378 gcm3

From Wikipedia, the free encyclopedia

This article is about t he m etallic ele ment . For the place, see Calcium, New

York .

Calcium is a chemical elementwithsymbol Ca and atomicnumber 20. Calcium is asoftgray alkaline earth metal, and isthe fifth-most-abundant

element by mass in theEarth'scrust. Calcium is also the fifth-most-abundant dissolvedion inseawater by bothmolarity andmass, after sodium, chloride,magnesium, and sulfate.[2]

Calcium is essential for livingorganisms, in particular incell

physiology, where movement ofthe calcium ionCa2+ into andout of thecytoplasm functionsas a signal for many cellularprocesses. As a major materialused in mineralization ofbone,teeth and shells, calcium is themost abundantmetal by massin manyanimals.

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2/20

Heat of fusion 8.54 kJmol1

Heat ofvaporization

154.7 kJmol1

Molar heatcapacity

25.929 Jmol1K1

vaporP (Pa) 1 10 100 1 k 10 k 100 kat T (K) 864 956 1071 1227 1443 1755

Atomic properties

Oxidation states +2 , +1[1] (a stronglybasicoxide)

Electronegativity Pauling scale: 1.00Ionizationenergies

1st: 589.8 kJmol12nd: 1145.4 kJmol13rd: 4912.4 kJmol1(more)

Atomic radius empirical: 197pmCovalent radius 17610 pmVan der Waalsradius

231 pm

Miscellanea

Crystalstructure

face-centered cubic (fcc)

Speed of soundthin rod, at 20 C

3810 ms1

Thermalexpansion

22.3 mm1K1 (at 25 C)

Thermalconductivity

201 Wm1K1

Electricalresistivity

at 20 C: 33.6 nm

Magneticordering

diamagnetic

Young'smodulus

20 GPa

Shear modulus 7.4 GPaBulk modulus 17 GPaPoisson ratio 0.31Mohs hardness 1.75Brinell hardness 167 MPaCAS number 7440-70-2

History

Discovery andfirst isolation

Humphry Davy (1808)

Most stable isotopes

Main article:Isotopes of calcium

Contents [hide]1 Notable characteristics

1.1 H and K lines2 Compounds3 Isotopes

3.1 Isotope fractionation4 Geochemical cycling5 History6 Occurrence7 Applications

7.1 Calcium compounds8 Nutrition

8.1 Dietary supplements8.2 Bone health8.3 Cardiovascular impact8.4 Cancer

9 Hazards and toxicity10 See also11 References12 Further reading13 External links

Notable

characteristicsIn chemical terms, calcium isreactive and soft for a metal;though harder thanlead, it canbe cut with a knife with difficulty.It is a silvery metallic elementthat must be extracted byelectrolysis from a fusedsaltlikecalcium chloride.[3] Once

produced, it rapidly forms agray-whiteoxide and nitridecoating when exposed to air. Inbulk form (typically as chips or"turnings"), the metal issomewhat difficult to ignite,more so even than magnesiumchips; but, when lit, the metalburns in air with a brilliant high-intensity orange-red light.Calcium metal reacts withwater, generating hydrogen gasat a rate rapid enough to be

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Hawai`i

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iso NA half-life DM DE (MeV) DP40Ca 96.941%>5.91021

y( + +) 0.194 40Ar

41Ca trace 1.03105y

41K

42Ca 0.647% 42Ca is stable with 22neutrons43Ca 0.135% 43Ca is stable with 23 neutrons

44Ca 2.086% 44Ca is stable with 24 neutrons45Ca syn 162.7 d 0.258 45Sc46Ca 0.004% >8.81022

y( ) 0.988 46Ti

47Ca syn 4.536 d 0.694,1.99

47Sc

1.297 48Ca 0.187% 4.31019

y 4.274 48Ti( ) 0.0058 48Sc

Decay modes in parentheses are predicted, buthave not yet been observedview talk edit references

Flame test. Brick-red colororiginates from calcium.

noticeable, but not fast enough at roomtemperature to generate much heat, making ituseful for generating hydrogen.[4] In powderedform, however, the reaction with water isextremely rapid, as the increased surface area

of the powder accelerates the reaction with thewater. Part of the reason for the slowness of the calciumwater reaction is aresult of the metal being partly protected by insoluble whitecalcium hydroxide.In water solutions of acids, where this salt is soluble, calcium reacts vigorously.

With a density of 1.55 g/cm3, calcium is the lightest of the alkaline earth metals;magnesium (specific gravity 1.74) and beryllium (1.84) are denser thoughlighter in atomic mass. From strontium onward, the alkali earth metals becomedenser with increasing atomic mass.

Calcium has twoallotropes.[5]Calcium has a higher electrical resistivity thancopper or aluminium, yet weight-for-weight, due to its much lower density, it is a much better conductor thaneither. However, its use in terrestrial applications is usually limited by its highreactivity with air.

Calcium salts are colorless from any contribution of the calcium, and ionicsolutions of calcium (Ca2+) are colorless as well. As withmagnesium salts andother alkaline earth metal salts, calcium salts are often quite soluble in water.

Notable exceptions includecalcium hydroxide, calcium sulfate (unusual forsulfate salts), calcium carbonate and tricalcium phosphate. With the exceptionof calcium sulfate, even the insoluble calcium salts listed are in general moresoluble than thetransition metal counterparts. When in solution, the calcium ionvaries remarkably to the human taste, being reported as mildly salty, sour,

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"mineral-like" or even "soothing." It is apparent that many animals can taste, ordevelop a taste, for calcium, and use this sense to detect the mineral insalt licksor other sources.[6] In human nutrition, soluble calcium salts may be added totart juices without much effect to the average palate.

Calcium is the fifth-most-abundant element by mass in the human body, whereit is an important cellular ionic messenger with many functions. Calcium also

serves as a structural element in bone. It is the relatively high-atomic-numbercalcium in the skeleton that causes bone to be radio-opaque. Of the humanbody's solid components after drying and burning of organics (as for example,after cremation), about a third of the total "mineral" mass remaining is theapproximately one kilogram of calcium that composes the average skeleton (theremainder being mostly phosphorus and oxygen).

H and K lines

Visible spectra of many stars, including theSun, exhibit strongabsorption lines

of singly ionized calcium. Prominent among these are the H-line at 3968.5and the K line at 3933.7 of singly ionized calcium, or Ca II. When observingthe Sun, or stars with low temperatures, the prominence of the H and K lines inthe visible spectra can be an indication of strong magnetic activity in thechromosphere. Measurement of periodic variations of these active regions canalso be used to deduce the rotation periods of these stars.[7]

CompoundsSee also Category:Calcium compounds .

Calcium, combined withphosphate, forminghydroxylapatite, is the mineralportion of human and animal bones and teeth. The mineral portion of somecorals can also be transformed into hydroxylapatite.

Calcium hydroxide (slaked lime) is used in many chemical refinery processesand is made by heatinglimestone at high temperature (above 825 C) and thencarefully adding water to it. When lime is mixed with sand, it hardens into amortar and is turned intoplaster by carbon dioxide uptake. Mixed with other

compounds, lime forms an important part ofPortland cement.Calcium carbonate (CaCO3) is one of the common compounds of calcium. It isheated to form quicklime (CaO), which is then added to water (H2O). This formsanother material known as slaked lime (Ca(OH)2), which is an inexpensive basematerial used throughout the chemical industry. Chalk, marble, and limestoneare all forms of calcium carbonate.

When water percolates throughlimestone or other solublecarbonate rocks, itpartially dissolves the rock and causes cave formation with their characteristicstalactites and stalagmites, and also formshard water. Other important calciumcompounds arecalcium nitrate, calcium sulfide, calcium chloride, calciumcarbide, calcium cyanamide and calcium hypochlorite.

A few calcium compounds where calcium is in the oxidation state +1 have also

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been investigated recently.[1]

IsotopesMain article: Isotopes of calcium

Calcium has five stableisotopes (40Ca, 42Ca, 43Ca, 44Ca and 46Ca), plus onemore isotope (48Ca) that has such a long half-life that for all practical purposes it

can also be considered stable. The 20% range in relative mass among naturallyoccurring calcium isotopes is greater than for any other element excepthydrogen and helium. Calcium also has acosmogenic isotope, radioactive 41Ca,which has ahalf-life of 103,000 years. Unlikecosmogenic isotopes that areproduced in theatmosphere, 41Ca is produced byneutron activation of 40Ca.Most of its production is in the upper metre or so of the soil column, where thecosmogenic neutron flux is still sufficiently strong.41Ca has received muchattention in stellar studies because it decays to41K, a critical indicator of solar-system anomalies.

Ninety-seven percent of naturally occurring calcium is in the form of40Ca. 40Cais one of the daughter products of40K decay, along with40Ar. WhileKAr datinghas been used extensively in thegeological sciences, the prevalence of40Ca innature has impeded its use in dating. Techniques usingmass spectrometry anda double spike isotope dilution have been used forK-Ca age dating.

The most abundant isotope,40Ca, has a nucleus of 20protons and 20neutrons. This is the heaviest stable isotope of any element that has equalnumbers of protons and neutrons. In supernova explosions, calcium is formedfrom the reaction of carbon with various numbers of alpha particles (heliumnuclei), until the most common calcium isotope (containing 10 helium nuclei)has been synthesized.[citation needed ]

Isotope fractionation

As with the isotopes of other elements, a variety of processes fractionate, oralter the relative abundance of, calcium isotopes.[8] The best studied of theseprocesses is the mass-dependentfractionation of calcium isotopes thataccompanies the precipitation of calcium minerals, such ascalcite, aragoniteand apatite, from solution. Isotopically light calcium is preferentially incorporatedinto minerals, leaving the solution from which the mineral precipitated enrichedin isotopically heavy calcium. At room temperature the magnitude of thisfractionation is roughly 0.25 (0.025%) per atomic mass unit (AMU). Mass-dependent differences in calcium isotope composition conventionally areexpressed the ratio of two isotopes (usually44Ca/ 40Ca) in a sample comparedto the same ratio in a standard reference material.44Ca/ 40Ca varies by about1% among common earth materials.[9]

Calcium isotope fractionation during mineral formation has led to severalapplications of calcium isotopes. In particular, the 1997 observation by Skulanand DePaolo[10] that calcium minerals are isotopically lighter than the solutionsfrom which the minerals precipitate is the basis of analogous applications in
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Travertine terraces Pamukkale,Turkey

medicine and in paleooceanography. In animals with skeletons mineralized withcalcium the calcium isotopic composition of soft tissues reflects the relative rateof formation and dissolution of skeletal mineral. In humans changes in thecalcium isotopic composition of urine have been shown to be related to changesin bone mineral balance. When the rate of bone formation exceeds the rate ofbone resorption, soft tissue44Ca/ 40Ca rises. Soft tissue44Ca/ 40Ca falls whenbone resorption exceeds bone formation. Because of this relationship, calciumisotopic measurements of urine or blood may be useful in the early detection ofmetabolic bone diseases likeosteoporosis.[11]

A similar system exists in the ocean, where seawater44Ca/ 40Ca tends to risewhen the rate of removal of Ca2+ from seawater by mineral precipitationexceeds the input of new calcium into the ocean, and fall when calcium inputexceeds mineral precipitation. It follows that rising44Ca/ 40Ca corresponds tofalling seawater Ca2+ concentration, and falling44Ca/ 40Ca corresponds to risingseawater Ca2+ concentration. In 1997 Skulan and DePaolo presented the first

evidence of change in seawater44

Ca/ 40

Ca over geologic time, along with atheoretical explanation of these changes. More recent papers have confirmedthis observation, demonstrating that seawater Ca2+ concentration is notconstant, and that the ocean probably never is in steady state with respect toits calcium input and output.[12][13] This has important climatological implications,as the marine calcium cycle is closely tied to thecarbon cycle (see below).

Geochemical cyclingCalcium provides an important link betweentectonics, climate and the carboncycle. In the simplest terms, uplift of mountains exposes Ca-bearing rocks tochemical weathering and releases Ca2+ into surface water. This Ca2+ eventuallyis transported to the ocean where it reacts with dissolved CO2 to formlimestone. Some of this limestone settles to the sea floor where it isincorporated into new rocks. Dissolved CO2, along withcarbonate andbicarbonate ions, are referred to asdissolved inorganic carbon (DIC).

The actual reaction is more complicatedand involves the bicarbonate ion

(HCO3) that forms when CO2 reactswith water at seawaterpH:

Ca2+ + 2HCO3 CaCO3(limestone) + CO2 + H2O

Note that at ocean pH most of the CO2produced in this reaction is immediately

converted back into HCO3. The reactionresults in a net transport of onemolecule of CO2 from the ocean/atmosphere into thelithosphere.[14]

The result is that each Ca2+ ion released by chemical weathering ultimatelyremoves one CO2 molecule from the surficial system (atmosphere, ocean, soils
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'Ain Ghazalfigure

and living organisms), storing it in carbonate rocks where it is likely to stay forhundreds of millions of years. The weathering of calcium from rocks thus scrubsCO2 from the ocean and atmosphere, exerting a strong long-term effect onclimate.[15] Analogous cycles involving magnesium, and to a much smallerextent strontium and barium, have the same effect.

As the weathering of limestone (CaCO3) liberates equimolar amounts of Ca2+

and CO2, it has no net effect on the CO

2 content of the atmosphere and ocean.

The weathering ofsilicate rocks likegranite, on the other hand, is a net CO2sink because it produces abundant Ca2+ but very little CO2.

HistoryLime as building material was used since prehistoric timesgoing as far back as 7000 to 14000 BC.[16] Significantstatues made fromlime plaster date back into the 7millennia BC were found in'Ain Ghazal.[17] The first datedlime kiln dates back to 2500 BC and was found inKhafajahmesopotamia.[18][19] Calcium (fromLatin calx , genitivecalcis , meaning "lime")[20] was known as early as the firstcentury when theAncient Romans prepared lime ascalciumoxide. Literature dating back to 975 AD notes thatplaster ofparis (calcium sulfate), is useful for setting broken bones. Itwas not isolated until 1808 inEngland whenSir HumphryDavy electrolyzed a mixture of lime andmercuric oxide.[21]

Davy was trying to isolate calcium; when he heard thatSwedish chemistJns Jakob Berzelius and Pontin preparedcalcium amalgam by electrolyzing lime in mercury, he tried it himself. He workedwith electrolysis throughout his life and also discovered/isolatedsodium,potassium, magnesium, boron and barium. Calcium metal was not available inlarge scale until the beginning of the 20th century.

OccurrenceSee also Category:Calcium minerals .

Calcium is not naturally found in its elemental state. Calcium occurs mostcommonly insedimentary rocks in the mineralscalcite, dolomite and gypsum. Italso occurs inigneous and metamorphic rocks chiefly in thesilicate minerals:plagioclases, amphiboles, pyroxenes and garnets.

ApplicationsCalcium is used[22]

as a reducing agent in the extraction of other metals, such asuranium,zirconium, and thorium.as a deoxidizer, desulfurizer, or decarbonizer for variousferrous andnonferrousalloys.as an alloying agent used in the production ofaluminium, beryllium, copper,
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lead, and magnesium alloys.in the making ofcements and mortars to be used inconstruction.in the making ofcheese, where calciumions influence the activity ofrenninin bringing about thecoagulation of milk.

Calcium compoundsSee also Category:Calcium compounds .

Calcium carbonate (CaCO3) is used in manufacturingcement and mortar,lime, limestone (usually used in the steel industry) and aids in production inthe glass industry. It also has chemical and optical uses as mineralspecimens intoothpastes, for example.Calcium hydroxide solution (Ca(OH)2) (also known aslimewater) is used todetect the presence of carbon dioxide by being bubbled through a solution.It turns cloudy where CO2 is present.Calcium arsenate (Ca3(AsO4)2) is used ininsecticides.

Calcium carbide (CaC2) is used to makeacetylene gas (for use in acetylenetorches forwelding) and in the manufacturing ofplastics.Calcium chloride (CaCl2) is used inice removal anddust control on dirtroads, in conditioner forconcrete, as an additive in cannedtomatoes, and toprovide body forautomobile tires.Calcium citrate (Ca3(C6H5O7)2) is used as a food preservative.Calcium cyclamate (Ca(C6H11NHSO3)2) is used as a sweetening agent inseveral countries. In the United States it is no longer permitted for usebecause of suspected cancer-causing properties.[23]

Calcium gluconate (Ca(C6H11O7)2) is used as a food additive and invitaminpills.Calcium hypochlorite (Ca(OCl)2) is used as a swimming pool disinfectant, asa bleaching agent, as an ingredient indeodorant, and inalgaecide andfungicide.Calcium permanganate (Ca(MnO4)2) is used in liquid rocket propellant,textile production, as a water sterilizing agent and in dental procedures.Calcium phosphate (Ca3(PO4)2) is used as a supplement foranimal feed,fertilizer, in commercial production fordough and yeast products, in themanufacture ofglass, and in dental products.Calcium phosphide (Ca3P2) is used infireworks, rodenticide, torpedoes andflares.Calcium stearate (Ca(C18H35O2)2) is used in the manufacture ofwaxcrayons, cements, certain kinds ofplastics and cosmetics, as a foodadditive, in the production of water resistant materials and in the productionof paints.Calcium sulfate (CaSO42H2O) is used as common blackboard chalk, as well

as, in its hemihydrate form better known as Plaster of Paris.Calcium tungstate (CaWO4) is used in luminouspaints, fluorescent lightsand inX-ray studies.Hydroxylapatite (Ca5(PO4)3(OH), but is usually written Ca10(PO4)6(OH)2)
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Recommended adequate intake by the

IOM for calcium: [24][25]

Age Calcium (mg/day)

06 months 200

712 months 260

13 years 700

48 years 1000918 years 1300

1950 years 1000

5170 years (male) 1000

5170 years (female) 1200

71+ years 1200

makes up seventy percent ofbone. Also carbonated-calcium deficienthydroxylapatite is the main mineral of whichdental enamel and dentin arecomprised.

NutritionMain articles: Calcium in biology , Calcium metabolism and Disorders of

calcium metabolism Calcium is an important component ofa healthy diet and a mineralnecessary for life. TheNationalOsteoporosis Foundation says,"Calcium plays an important role inbuilding stronger, denser bones earlyin life and keeping bones strong andhealthy later in life." Approximately 99percent of the body's calcium isstored in the bones and teeth.[26] Therest of the calcium in the body hasother important uses, such as someexocytosis, especiallyneurotransmitter release, and musclecontraction. In theelectricalconduction system of the heart,calcium replaces sodium as the mineral that depolarizes the cell, proliferatingthe action potential. In cardiac muscle, sodium influx commences an actionpotential, but during potassium efflux, the cardiac myocyte experiences calciuminflux, prolonging the action potential and creating a plateau phase of dynamicequilibrium. Long-termcalcium deficiency can lead torickets and poorbloodclotting and in case of a menopausal woman, it can lead toosteoporosis, inwhich the bone deteriorates and there is an increased risk of fractures. While alifelong deficit can affect bone and tooth formation, over-retention can causehypercalcemia (elevated levels of calcium in the blood), impaired kidney

function and decreased absorption of other minerals.[27][28]

Several sourcessuggest a correlation between high calcium intake (2000 mg per day, or twicethe U.S.recommended daily allowance, equivalent to six or more glasses ofmilk per day) andprostate cancer.[29] High calcium intakes or high calciumabsorption were previously thought to contribute to the development of kidneystones. However, a high calcium intake has been associated with a lower riskfor kidney stones in more recent research.[30][31][32] Vitamin D is needed toabsorb calcium.

Dairy products, such as milk and cheese, are a well-known source of calcium.Some individuals are allergic to dairy products and even more people, inparticular those of non Indo-European descent, arelactose-intolerant, leavingthem unable to consume non-fermented dairy products in quantities larger thanabout half a liter per serving. Others, such asvegans, avoid dairy products for
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500 milligram calcium supplementsmade fromcalcium carbonate

ethical and health reasons.

Many good vegetable sources of calcium exist, includingseaweeds such askelp, wakame and hijiki; nuts and seeds likealmonds, hazelnuts, sesame, andpistachio; blackstrapmolasses; beans (especiallysoy beans); figs; quinoa; okra;rutabaga; broccoli; dandelion leaves; andkale. In addition, several foods anddrinks, such asorange juice, soy milk, tofu, breakfast cereals, and breads areoftenfortified with calcium.[33]

Numerous vegetables, notablyspinach, chard and rhubarb have a high calciumcontent, but they may also contain varying amounts ofoxalic acid that bindscalcium and reduces its absorption. The same problem may to a degree affectthe absorption of calcium fromamaranth, collard greens, and chicory greens.This process may also be related to the generation ofcalcium oxalate.

An overlooked source of calcium is eggshell, which can be ground into a powderand mixed into food or a glass of water.[34][35][36]

The calcium content of most foods can be found in the USDA National NutrientDatabase.[37]

Dietary supplements

Calcium supplements are used toprevent and to treat calciumdeficiencies. Office of DietarySupplements (National Institutes ofHealth) recommends that no more than

600 mg of supplement should be takenat a time because the percent of calciumabsorbed decreases as the amount ofcalcium in the supplement increases.[24]

It is therefore recommended to spreaddoses throughout the day.[38] Recommended daily calcium intake for adultsranges from 1000 to 1300 mg.[38] Calcium supplements may have side effectssuch as bloating and constipation in some people. It is suggested that taking thesupplements with food may aid in nullifying these side effects.[38]

Vitamin D is added to some calcium supplements. Proper vitamin D status isimportant because vitamin D is converted to a hormone in the body, which theninduces the synthesis of intestinal proteins responsible for calciumabsorption.[39]

The absorption of calcium from most food and commonly used dietarysupplements is very similar.[40] This is contrary to what many calciumsupplement manufacturers claim in their promotional materials.Milk is an excellent source of dietary calcium for those whose bodies tolerateit because it has a high concentration of calcium and the calcium in milk isexcellently absorbed.[40]

Soymilk and other vegetable milks are usually sold with calcium added sothat their calcium concentration is as high as in milk.
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Also different kind of juices boosted with calcium are widely available.Calcium carbonate is the most common and least expensive calciumsupplement. It should be taken with food, and depends on low pH levels(acidic) for proper absorption in the intestine.[41] Some studies suggests thatthe absorption of calcium from calcium carbonate is similar to the absorptionof calcium from milk.[42][43]

Antacids frequently contain calcium carbonate, and are a commonly used,inexpensive calcium supplement.Coral calcium is a salt of calcium derived from fossilized coral reefs. Coralcalcium is composed of calcium carbonate and trace minerals.Calcium citrate can be taken without food and is the supplement of choicefor individuals with achlorhydria or who are taking histamine-2 blockers orproton-pump inhibitors.[44] Calcium citrate is about 21% elemental calcium.1000 mg will provide 210 mg of calcium. It is more expensive than calciumcarbonate and more of it must be taken to get the same amount of calcium.

Calcium phosphate costs more than calcium carbonate, but less thancalcium citrate.Microcrystalline Hydroxyapatite (MH) is one of several formsof calcium phosphate used as a dietary supplement. Hydroxyapatite is about40% calcium.Calcium lactate has similar absorption as calcium carbonate,[45] but is moreexpensive. Calcium lactate and calcium gluconate are less concentratedforms of calcium and are not practical oral supplements.[44]

Bone health

Calcium supplementation can have a small effect in improvingbone mineraldensity. This is of no meaningful benefit to health in children, but inpost-menopausal women the risk ofvertebral fractures may be reduced.[46][47]

Cardiovascular impact

A study investigating the effects of personal calcium supplement use oncardiovascular risk in theWomens Health Initiative Calcium/Vitamin DSupplementation Study (WHI CaD Study) found a modestly increased risk ofcardiovascular events, particularlymyocardial infarction in postmenopausalwomen. A broad recommendation of calcium/vitamin D supplements is thereforenot warranted.[48] In contrast, the authors of a 2013 literature review concludedthat the benefits of calcium supplementation, such as on bone health, appear tooutweigh any risk calcium supplementation may theoretically pose to thecardiovascular health.[49]

Cancer

Overall, there is no strong evidence calcium supplementation helps prevent

cancer in people: some studies suggest it might decrease the risk, but otherssuggest it might increase the risk. TheNational Cancer Institute, part of theNational Institutes of Health, does not recommend the use of calciumsupplements to prevent any type of cancer, due to the lack of evidencesupporting its use for this purpose.[50]
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There is weak evidence calcium supplementation might have a preventativeeffect against developingcolorectal adenomatouspolyps, but the evidence isinsufficient to recommend such supplementation as a beneficial practice.[51]

Hazards and toxicityCompared with other metals, the calcium ion and most calcium compoundshave low toxicity. This is not surprising given the very high natural abundance ofcalcium compounds in the environment and in organisms. Calcium poses fewserious environmental problems, with kid

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