it form from ß decayĤ8Ca: atomic weight of this isotope is 47.) Can this isotopes 20 proton, 20 electron and 28 neutron is present. It form from ß decayĤ6Ca: atomic weight of this isotope is 45.9 In this isotope 20 proton, 20 electron and 26 neutron is present It is present 0.004%. It is present 96%Ĥ2Ca: Atomic weight of this isotope is 41.9 In this isotopes 20 proton,20 electron and 22 neutron is present It is present 0.6%Ĥ3Ca: Atomic weight of this isotope is 42.9 In this isotopes 20 proton, 20 electron and 23 neutron is present It is present 0.13%Ĥ4Ca: atomic weight of this isotope is 43.9 In this isotopes 20 proton, 20 electron and 24 neutron is present It is present 2.08%. In this isotopes 20 proton ,20 electron and 20 neutron is present. But is soft in natureĩ) Boiling point : boiling point of calcium is 1484 0 Cġ1) Isotopes: Calcium show 6 stable isotopesĤ0Ca : atomic weight of this isotpresent 39.9 It is placed in 2nd column (group) and 4 th period (row) It is placed in alkaline earth metal seriesĨ) Nature : it is found in solid state. In calcium atom 20 proton and 20 electron is presentĪtomic weight of calcium is 40.08 In calcium atom nucleus 20 proton and 20 neutron is present The name calcium is derived from Latin word ‘ calx ‘ Meaning of this word is lime Lime is a calcium carbonate substanceĢ) Atomic number : atomic number of calcium is 20. Milk, yoghurt, cheese, green vegetables, nuts are rich in calciumĭiscovery : calcium is discovered by Humphrey Davy in 1808 It is less soluble in water It is one of the useful mineral in our body for bones and teeth It is also useful for clotting of blood. It has no shine In daily life it is found in chalk, limestone and marbles. It is found in earth curst in the form of limestone, gypsum and fluorite. It is 5 th mostly found element in earth crust. Atomic Mass, Number, Physical, Chemical properties, Electronic configuration, Valency, Chemical reaction, UsesĬalcium is and 3rd alkaline earth metal. Gypsum (calcium sulfate) is used by builders as a plaster ( Improvements In Or Relating To Calcium Sulphate Plaster Mixes And To Methods Of Applying The Same (1932)), and by nurses for setting bones, as ‘plaster of Paris’.Ĭalcium reacts with water, but less vigorously than sodium and potassium.Calcium – Learn all details regarding Calcium in Periodic Table i.e. When mixed with sand, slaked lime takes up carbon dioxide from the air and hardens as lime plaster: Improvements relating to the preparation of line plaster (1960). It is also used in steel making to remove impurities from the molten iron ore ( Manufacture Of Lime With Low Water Content For Steel Manufacture (1981)). Slaked lime is used to make concrete, ( Impermeable coating material, comprises marble microparticles, slaked lime, white cement, water repellent and concrete retardant (2001)), as a soil conditioner and in water treatment to reduce acidity ( Lime Neutralization Process For Treating Acidic Waters (1995)), and in the chemicals industry. This reacts vigorously with water to give slaked lime (calcium hydroxide) ( Process Of Converting Quicklime Into Powdered Hydrated Lime (1904)). When limestone is heated in kilns it gives off carbon dioxide gas, leaving behind quicklime (calcium oxide) ( Kiln For Burning Or Calcining Limestone (1901)). Natural deposits of limestone (calcium carbonate) can be used directly as a building stone and indirectly for cement.Ĭalcium carbonate can be produced synthetically ( Calcium-Carbonate Manufacture (1916)). Calcium can form many alloys with with numerous metals.
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