Sweep up and shovel. Keep in suitable, closed containers for disposal. Reference to other sections For disposal see section Precautions for safe handling Avoid contact with skin and eyes. Avoid formation of dust and aerosols. Further processing of solid materials may result in the formation of combustible dusts. The potential for combustible dust formation should be taken into consideration before additional processing occurs.
Provide appropriate exhaust ventilation at places where dust is formed. For precautions see section 2. Conditions for safe storage, including any incompatibilities Keep container tightly closed in a dry and well-ventilated place.
Keep in a dry place. Exposure controls Appropriate engineering controls Handle in accordance with good industrial hygiene and safety practice. Wash hands before breaks and at the end of workday. Skin protection Handle with gloves. Gloves must be inspected prior to use.
Use proper glove removal technique without touching glove's outer surface to avoid skin contact with this product. Dispose of contaminated gloves after use in accordance with applicable laws and good laboratory practices. Wash and dry hands. Full contact Material: Nitrile rubber Minimum layer thickness: 0. This recommendation is advisory only and must be evaluated by an industrial hygienist and safety officer familiar with the specific situation of anticipated use by our customers.
It should not be construed as offering an approval for any specific use scenario. Body Protection Complete suit protecting against chemicals, The type of protective equipment must be selected according to the concentration and amount of the dangerous substance at the specific workplace.
Respiratory protection Where risk assessment shows air-purifying respirators are appropriate use a full-face particle respirator type N US or type P3 EN respirator cartridges as a backup to engineering controls.
If the respirator is the sole means of protection, use a full-face supplied air respirator. Control of environmental exposure Do not let product enter drains. Information on basic physical and chemical properties Appearance Form: powder, pieces, or solid in various forms Odor No data available Odor Threshold No data available pH Reactivity No data available Chemical stability Stable under recommended storage conditions.
Possibility of hazardous reactions No data available Conditions to avoid Avoid moisture. Incompatible materials acids, Water Hazardous decomposition products Other decomposition products- No data available In the event of fire: see section 5.
NTP: No component of this product present at levels greater than or equal to 0. OSHA: No component of this product present at levels greater than or equal to 0. Reproductive toxicity No data available Specific target organ toxicity -single exposure Inhalation-May cause respiratory irritation. Specific target organ toxicity -repeated exposure No data available Aspiration hazard No data available Additional Information RTECS: EW Cough, Shortness of breath, Headache, Nausea, Vomiting To the best of our knowledge, the chemical, physical, and toxicological properties have not been thoroughly investigated.
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See more Calcium products. Calcium atomic symbol: Ca, atomic number: 20 is a Block S, Group 2, Period 4 element with an atomic weight of The number of electrons in each of Calcium's shells is [2, 8, 8, 2] and its electron configuration is [Ar]4s 2.
Upon exposure, many soldiers underwent choking and even suffocation, and their eyes were especially susceptible to the forces of calcium oxide. During the Middle Ages, many took advantage of this weapon, using it against naval forces. Carried by the speed and distance of a catapult, trebuchet, or some other kind of ballista, calcium oxide could easily affect every crewmember of a ship.
This was detailed by Thirteenth Century writer Giles of Rome :. This situation is very dangerous in naval warfare because fighting men in such war see themselves threatened with death from every quarter. Wherefore, if the eyes of the fighting men in such a battle are so irritated by powdered lime that they cannot see, they can easily either be slain by their enemies or submerged in the water.
Another dreadful maritime war application of calcium oxide might have been its inclusion in the secret recipe of Greek Fire , a mysterious substance still not entirely understood. Greek Fire was an incendiary mixture used by Eastern Roman Emperors to face against naval power, and it first appeared in the Seventh Century CE to defend Constantinople against an invading fleet.
This material was basically liquid fire; it was hurled at enemies through siphons, burning on contact. As it was inextinguishable, the chemical fireball spread quickly, even continuing to burn on water and it should sound familiar to Game of Thrones fans. Today, the primary uses of calcium oxide differ from its history in warfare and more closely resemble its original application. Like in the pyramids and the Great Wall, quicklime is still a strong component of different materials. Lime is a common chemical used in iron and steel manufacturing , acting as a flux in purifying steel in electric arc furnaces EAF and basic oxygen furnaces BOF.
In addition to removing impurities, calcium oxide reduces refractory wear and gunning, and can provide a foaming slag for long arc operation. The resulting slaked lime is used for mortar, plaster, and cement in buildings and other structures. Biological role. Calcium is essential to all living things, particularly for the growth of healthy teeth and bones.
Calcium phosphate is the main component of bone. The average human contains about 1 kilogram of calcium. Children and pregnant women are encouraged to eat foods rich in calcium, such as milk and dairy products, leafy green vegetables, fish and nuts and seeds.
Natural abundance. It is not found uncombined in nature, but occurs abundantly as limestone calcium carbonate , gypsum calcium sulfate , fluorite calcium fluoride and apatite calcium chloro- or fluoro-phosphate. Hard water contains dissolved calcium bicarbonate. When this filters through the ground and reaches a cave, it precipitates out to form stalactites and stalagmites. Help text not available for this section currently. Elements and Periodic Table History. Lime calcium oxide, CaO was the useful material obtained by heating limestone and used for centuries to make plaster and mortar.
In , Humphry Davy tried to reduce moist lime by electrolysis, just as he had done with sodium and potassium, but he was not successful.
Davy tried using more lime in the mixture and produced more of the amalgam from which he distilled off the mercury leaving just calcium.
Atomic data. Glossary Common oxidation states The oxidation state of an atom is a measure of the degree of oxidation of an atom. Oxidation states and isotopes. Glossary Data for this section been provided by the British Geological Survey. Relative supply risk An integrated supply risk index from 1 very low risk to 10 very high risk. Recycling rate The percentage of a commodity which is recycled. Substitutability The availability of suitable substitutes for a given commodity.
Reserve distribution The percentage of the world reserves located in the country with the largest reserves. Political stability of top producer A percentile rank for the political stability of the top producing country, derived from World Bank governance indicators. Political stability of top reserve holder A percentile rank for the political stability of the country with the largest reserves, derived from World Bank governance indicators.
Supply risk. Relative supply risk 5. Young's modulus A measure of the stiffness of a substance. Shear modulus A measure of how difficult it is to deform a material. Bulk modulus A measure of how difficult it is to compress a substance. Vapour pressure A measure of the propensity of a substance to evaporate. Pressure and temperature data — advanced.
Listen to Calcium Podcast Transcript :. You're listening to Chemistry in its element brought to you by Chemistry World , the magazine of the Royal Society of Chemistry. This week it's the turn of the element that gives us cement, plaster of Paris, our own bones, hard teeth and hard water. Milk, cheese, yogurt, spinach, almonds. What element do they all have in common? It's calcium of course! But whilst most off us immediately think of food when someone mentions calcium and I personally hold the old milk TV adverts accountable for this , it actually has a far bigger role in our lives than that.
Calcium is all around us. It is the 5th most abundant element in the earth's crust, occurring widely as calcium carbonate which is more commonly known as limestone. It is also the fifth most abundant dissolved ion in seawater. Calcium was named after the Latin term calx meaning lime, and is a reactive silvery metallic element found in Group 2 of the periodic table.
It was first isolated in in England when Sir Humphry Davy electrolyzed a mixture of lime and mercuric oxide. Today we obtain calcium through the electrolysis of a fused salt such as calcium chloride. Once exposed to air, elemental calcium rapidly forms a grey-white oxide and nitride coating.
Unlike magnesium, calcium is quite difficult to ignite, but once lit, it burns with a brilliant high-intensity red flame. The compounds of calcium are however much more useful than the element itself.
Literature dating back to AD shows that plaster of Paris which is calcium sulphate was used even then for setting broken bones. Calcium oxide also known as lime or quicklime is a major component of mortar and cement. The production of cement using calcium oxide has long been known; it was used by the Romans and also the Egyptians who built the Great Pyramid of Giza and Tutankhamen's tomb. Calcium fluoride is also well known for being insoluble and transparent over a wide range of wavelengths, making it useful for making cells and windows for infrared and ultraviolet spectrometers.
Our drinking water also contains calcium ions - more so in so called hard water areas. Hard water is the term used for water with a high proportion of calcium and magnesium 2 plus ions. The calcium usually enters the water as it flows past either calcium carbonate, from limestone and chalk, or calcium sulfate, from other mineral deposits.
Whilst some people do not like the taste, hard water is generally not harmful to your health. Although it does make your kettle furry!
Interestingly, the taste of beer something dear to my heart seems related to the calcium concentration of the water used, and it is claimed that good beer should have a calcium concentration that is higher than that of hard tap water. Calcium is what is known as an essential element, meaning that it is an element which is absolutely necessary for life processes. Which is what the old milk TV adverts were trying to tell us after all. Calcium is used to produce the minerals contained in bones, shells and teeth through a process called biomineralisation.
Calcium phosphate also known as hydroxyapatite is the mineral component of bones and teeth and is a particularly good example of how organisms fabricate 'living' composite materials.
Indeed, the different properties such as stiffness of bone are produced by varying the amount of organic component, mostly a fibrous protein called collagen, with which hydroxyapatite is associated.
The bone in our body functions not only as a structural support, but also as the central Ca store. Thus, during pregnancy, bones tend to be raided for their Ca in a process called demineralisation.
Bone does not last forever; a serious medical problem is osteoporosis which is the decalcification of bone. This loss of bone mass which occurs with increasing age makes bones more susceptible to breaking under stress and it occurs mainly in older people, especially women. Calcium ions also play a crucial role in higher organisms as an intracellular messenger. Calcium is also very important in helping blood to clot. When bleeding from a wound suddenly occurs, platelets gather at the wound and attempt to block the blood flow.
Calcium, vitamin K, and a protein called fibrinogen help the platelets to form a clot. If your blood is lacking calcium or one of these other nutrients, it will take longer than normal for your blood to clot. The ability to detect extremely small amounts of an element can be a very useful adaptation for an animal if that element is important to it.
For example, hermit crabs, which inhabit second hand shells and change to newer, bigger shells as they grow, have the ability to recognise shells suitable for occupation not only by feeling for them, but apparently also by measuring the minute amount of calcium carbonate that is dissolved in the water around a shell.
They can readily distinguish natural shells containing calcium carbonate from calcium-bearing replicas made from calcium sulphate. The concentration of calcium detected by the hermit crab is in the order of 4ppm or less, which is amazingly low. So from strong teeth and bones, through to good tasting beer and ensuring hermit crabs find their perfect home -you can see that calcium really is an essential element.
Well, I'm very at home with my hard water, and the local beer tastes quite good too, although I do get through quite a few kettles - indeed Russell Hobbs probably owe their buoyant share price just down to me.
Well, maybe. Next week, if you were an element which one would you be? If I had to choose a person to represent gold, then I guess it might be an ambitious young stockbroker, a bit flashy, and not great at forming relationships. For helium - an airy-fairy blonde with a bit of a squeaky voice, but with aspirations to join the nobility. And for boron?
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