14452-75-6 Usage
Description
Calcium is the chemical element with the symbol Ca and atomic number 20. It is a soft grey metallic element belonging to group 2 (formerly IIA) of the periodic table. Calcium is the fifth most abundant element in the Earth's crust and is essential for the growth of living organisms. It is a good conductor of heat and electricity, and it has a low ionization potential and a relatively large atomic radius, making it a very electropositive element.
Uses
Used in Building and Construction:
Calcium is used as an alloy agent for copper and aluminum. It is also used to purify lead and is a reducing agent for beryllium. Calcium oxide was used in ancient times to make mortar for building with stone.
Used in Metallurgy:
Calcium is used to remove carbon and sulfur impurities during the processing of iron, producing a higher-grade iron for use in the manufacture of steel. It is also used as a reducing agent in the preparation of several other important metals.
Used in Agriculture:
Calcium is an important ingredient in the diets of all plants and animals. It is found in the soft tissues and fluids of animals (e.g., blood) as well as in bones and teeth. Calcium is an essential secondary plant nutrient, required for plant cell elongation, cell division, and various anabolic and catabolic processes.
Used in Nutrition:
Calcium makes up about 2% of the human body weight. It contributes to bone and teeth formation, muscle contraction, and blood clotting. It is found in milk, vegetables, and egg yolk.
Used in Chemistry:
Calcium, plasma standard solution is used as a standard solution in analytical chemistry and atomic absorption spectroscopy. It is also used as a single-element standard solution for plasma emission spectrometry.
Used in Environmental Management:
Calcium is the main ingredient of Portland cement and is used to reduce the acid content of soils.
Used in Pharmaceutical Applications:
Calcium is an important element for the nutrition of living organisms, particularly vertebrates. Vitamin D from foods, sunlight, and milk aids in the deposition of calcium in bones and teeth.
Industrial uses:
Calcium and its compounds are employed industrially in fertilizers, foodstuffs, and medicine. It is an essential element in the formation of bones, teeth, shells, and plants. Oyster shells form an important commercial source of calcium for animal feeds.
Agricultural Uses:
Calcium is an essential element for the growth of living organisms. It is a soft grey metallic element belonging to Group 2 (formerly Ⅱ A) of the Periodic Table. It is an important constituent of bones and teeth in animals and is present in blood. It is required for muscle contraction and other metabolic processes. In plants, it is a constituent of the middle lamella and is essential for plant cell elongation, cell division, and various anabolic and catabolic processes.
Isotopes
There are 20 isotopes of calcium, ranging from Ca-35 to Ca-54. Of the sixstable isotopes, Ca-40 makes up 96.941% of the calcium found in the Earth’s crust, andCa-42 = 0.647%, Ca-43 = 0.135%, Ca-44 = 2.086%, Ca-46 = 0.004%, and Ca-48 =0.187% found on Earth. All the other isotopes of calcium are radioactive and are artificially produced with half-lives ranging from a few microseconds to 1×105 years.Radioactive Ca-45 emits beta particles (high-speed electrons) and has a half-life ofabout 163 days. It is used to determine the calcium levels in bones and in soils.
Isotopes
Calcium has four stable isotopes (40Ca and 42Ca
through 44Ca), plus two more isotopes (46Ca and 48Ca)
that have such a long half-lives that for all practical
purposes they can be considered stable. It also has
a cosmogenic isotope, radioactive 44Ca, with a half-life
of 103,000 years. Unlike cosmogenic isotopes that are
produced in the atmosphere, 41Ca is produced by
neutron activation of 40Ca. Most of its production is in
the upper meter or so of the soil column, where the
cosmogenic neutron flux is still sufficiently strong.
41Ca has received much attention in stellar studies
because it decays to 41K, a critical indicator of solar
system anomalies.
A major part (97%) of naturally occurring calcium is
in the form of 40Ca. This isotope is one of the daughter
products of 40K decay, along with 40Ar. While K/Ar
dating has been used extensively in the geological
sciences, the prevalence of 40Ca in nature has impeded
its use in dating. Techniques using mass spectrometry
and a “double-spike” isotope dilution have been used
for K/Ca age dating.
The most abundant isotope, 40Ca, has a nucleus of 20
protons and 20 neutrons. This is the heaviest stable
isotope of any element known that has equal numbers
of protons and neutrons. In supernova explosions,
calcium is formed from the reaction of carbon with
various numbers of alpha particles (helium nuclei), until
this most common calcium isotope (containing 10
helium nuclei) has been formed.
Origin of Name
Its modern name was derived from the word calcis or calx, which is
Latin for “lime.
History
Calcium (Latin word calcis meaning “lime”) was
known as early as the first century when the Ancient
Romans prepared lime as calcium oxide from limestone
and used “slaked lime” as a “whitewash” on various
homes and buildings. Literature dating back to 975 AD
notes that “Plaster-of-Paris” (calcium sulfate), is useful
for setting broken bones. The metal was not isolated
until 1808 when Sir Humphrey Davy of England electrolyzed
a mixture of lime and mercuric oxide, using then
the new “Voltaic Cell” as an energy source. Davy was
trying to isolate calcium. When he heard that Swedish
chemist J?ns Berzelius and his colleague, Pontin, had
prepared calcium amalgam by electrolyzing lime in
mercury, he set up a similar system and was successful.
He worked with electrolysis throughout his life and also discovered/isolated boron, sodium, potassium, magnesium,
calcium, strontium and barium. Calcium metal
was not available on a large scale until the beginning
of the twentieth century.
History
Though lime
was prepared by the Romans in the first century under the
name calx, Calcium was not discovered until 1808. After
learning that Berzelius and Pontin prepared calcium amalgam
by electrolyzing lime in mercury, Davy was able to isolate the
impure metal. Calcium is a metallic element, fifth in abundance
in the Earth’s crust, of which it forms more than 3%. It
is an essential constituent of leaves, bones, teeth, and shells.
Never found in nature uncombined, it occurs abundantly
as limestone (CaCO3), gypsum (CaSO4·2H2O), and fluorite
(CaF2); apatite is the fluorophosphate or chlorophosphate of
calcium. Calcium has a silvery color, is rather hard, and is
prepared by electrolysis of the fused chloride to which calcium
fluoride is added to lower the melting point. Chemically it
is one of the alkaline earth elements; it readily forms a white
coating of oxide in air, reacts with water, burns with a yellowred
flame, largely forming the oxide. The metal is used as a
reducing agent in preparing other metals such as thorium,
The Elements 4-7
uranium, zirconium, etc., and is used as a deoxidizer, desulfurizer,
and inclusion modifier for various ferrous and nonferrous
alloys. It is also used as an alloying agent for aluminum,
beryllium, copper, lead, and magnesium alloys, and serves as a
“getter” for residual gases in vacuum tubes. Its natural and prepared
compounds are widely used. Quicklime (CaO), made by
heating limestone and changed into slaked lime by the careful
addition of water, is the great cheap base of the chemical
industry with countless uses. Mixed with sand it hardens as
mortar and plaster by taking up carbon dioxide from the air.
Calcium from limestone is an important element in Portland
cement. The solubility of the carbonate in water containing
carbon dioxide causes the formation of caves with stalactites
and stalagmites and is responsible for hardness in water.
Other important compounds are the carbide (CaC2), chloride
(CaCl2), cyanamide (CaCN2), hypochlorite (Ca(OCl)2), nitrate
(Ca(NO3)2), and sulfide (CaS). Calcium sulfide is phosphorescent
after being exposed to light. Natural calcium contains
six isotopes. Sixteen other radioactive isotopes are known.
Metallic calcium (99.5%) costs about $200/kg.
Characteristics
Finely powdered calcium metal is flammable in air because it liberates hydrogen from themoisture. It can be extremely reactive in water but can be dissolved in acids. Calcium is harderthan sodium metal, but softer than aluminum. In its elemental form it can be machined (cuton a lathe), extruded (pushed through a die), and drawn (stretched into rods or wires).Calcium is present in a number of products used in our everyday lives. It is found inclassroom chalk, teeth, and bones. About 2% of the human body consists of various forms ofcalcium compounds. Calcium is an essential inorganic element (usually in compound form)for plant and animal life.
Indications
Calcium is the principal extracellular electrolyte regulated
by PTH, calcitonin, and D3. Extracellular calcium
is a critical component of signal transduction across the
plasma membrane, which regulates a wide spectrum of
physiological events including muscle contraction, secretion
of neurotransmitters and hormones, and the action
of growth factors, cytokines, and protein hormones.
Intracellular calcium is an important cofactor in many
enzymatic reactions.
Hazard
The metallic form of calcium, particularly the powdered form, combines with water oroxidizing agents to release hydrogen that may explode, as do the other alkali metals. There aremany useful calcium compounds; some are excellent reducing agents, some are explosive, andothers are essential for life.The radioactive isotope calcium-45 is deposited in bones and teeth as well as other plantand animal tissues. Because our bodies cannot distinguish between Ca-45 and the stable Ca-40, the radioactive isotope Ca-45 is used as a tracer to study diseased bone and tissue. At thesame time, a massive overexposure to Ca-45 can displace the stable form of Ca-40 in animalsand can cause radiation sickness or even death.A few calcium compounds, when in powder or vapor form, are toxic when ingested orinhaled.
Pharmaceutical Applications
Calcium is mostly found in limestone and its related forms, such as chalk, and marble and lime (CaO). Calcium is the most abundant inorganic element in the human body and is an essential key for many physiological
processes. Calcium ions are a critical
factor in several life-defining biochemical processes as well as in the endocrine, neural and renal aspects of
blood pressure homeostasis.
Calcium has the symbol Ca and atomic number 20 and is a soft grey alkaline earth metal. Calcium has
four stable isotopes (40Ca and 42Ca–44Ca) and the metal reacts with water with the formation of calcium
hydroxide and hydrogen.
Check Digit Verification of cas no
The CAS Registry Mumber 14452-75-6 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 1,4,4,5 and 2 respectively; the second part has 2 digits, 7 and 5 respectively.
Calculate Digit Verification of CAS Registry Number 14452-75:
(7*1)+(6*4)+(5*4)+(4*5)+(3*2)+(2*7)+(1*5)=96
96 % 10 = 6
So 14452-75-6 is a valid CAS Registry Number.
14452-75-6Relevant articles and documents
New Fourier transform infrared emission spectra of CaH and SrH: Combined isotopomer analyses with CaD and SrD
Shayesteh, Alireza,Walker, Kaley A.,Gordon, Iouli,Appadoo, Dominique R.T.,Bernath, Peter F.
, p. 23 - 37 (2004)
In a search for the infrared spectra of gaseous CaH2 and SrH2, we obtained new Fourier transform infrared emission spectra of CaH and SrH, but no evidence of the metal dihydrides. The vibration-rotation bands from v=1→0 to v=4→3 of 40CaH and 88SrH, and the v=1→0 band of 87SrH and 86SrH were observed in the X2Σ+ ground electronic states. The new data were combined with the previous ground state data, obtained from diode laser infrared and pure rotational spectra, and the spectroscopic constants for v=0 to 4 of 40CaH and 88SrH were determined. In addition, the Dunham constants and the Born-Oppenheimer breakdown correction parameters were obtained using the previous ground state data for CaD and SrD in combined isotopomer fits. The equilibrium vibrational constants (ωe) for CaH and SrH were found to be 1298.400(1) and 1207.035(1)cm-1, respectively, while the equilibrium rotational constants (Be) are 4.277043(4) and 3.673495(4)cm-1. The equilibrium bond distances (re) were determined to be 2.0023603(9) A? for CaH and 2.1460574(10) A? for SrH.
