![]() ![]() Radioactive strontium-90 is produced in nuclear explosions and released during nuclear plant accidents, which is particularly dangerous because it can be absorbed into the bones of young children.įor children exceeded strontium uptake may be a health risk, because it can cause problems with bone growth. In the human body, most of the absorbed strontium is deposited in the bones, In the ratio of strontium to calcium is between 1:1000 and 1:2000 roughly. It is Non-Toxic, Because it is similar to calcium. Strontium titanate (SrTiO 3) is an optical material, which has extremely high refractive index (measure of the bending of a ray of light when passing from one medium into another) and an optical dispersion greater than that of diamond. Strontium chloride hexahydrate (H 12Cl 2O 6Sr) is an ingredient in toothpaste for sensitive teeth. Modern ‘glow-in-the-dark ’ paints and plastics contain strontium aluminate (SrAl 2O 4), where they absorb light during the day and release it slowly for hours afterwards. It high-energy radiation can be used to generate electricity for space vehicles, remote weather stations and navigation buoys. Strontium-90 is a dangerously radioactive isotope, It is a by-product of nuclear reactors and present in nuclear fallout (from whose spent fuel is extracted). It is one of the best high-energy beta-emitters. It also has found use in producing ferrite magnets and in refining zinc. Strontium compounds are used in pyrotechnics and gives the brilliant red colour to fireworks and flares. SStrontim has similar uses of calcium and a brium but it is employed rarely because of its higher cost. Naming: After the mineral strontianite, itself named after Strontian, Scotlandįirst isolation:Humphry Davy (1808) Strontium Uses The metal can also be prepared by electrolysis of a solution of strontium chloride in molten potassium chloride: The sulfate is reduced to the sulfide by the carbothermic reduction: The metal dissolves readily in dilute or concentrated hydrochloric acid (HCl) and forming Sr (II) ions and hydrogen gas. Sr (s) I 2 (g) → SrI 2 (s) (Strontium (ll) iodide) Sr (s) Br 2 (g) → SrBr 2 (s) (Strontium (ll) bromide) Sr (s) Cl 2 (g) → SrCl 2 (s) (Strontium (ll) chloride) Strontium react with Chlorine, bromine, iodine and forming Strontium (II) halides: Strontium reacts slowly with water and forming strontium hydroxide (Sr(OH) 2)and hydrogen gas (H 2). When Ignited, Strontium metal burns in air and reacts with both oxygen and nitrogen, to give a mixture of white strontium oxide (SrO) and strontium nitride (Sr 3N 2) Strontium reacts with oxygen (O 2)and forming a protective layer of SrO on the surface. Isotopes: 82 Sr 83 Sr 84 Sr 85 Sr 86 Sr 87 Sr 88 Sr 89 Sr 90 Sr Isotope Lattice constant: 608.49, 608.49, 608.49 pmįace Centered Cubic (FCC) Reactivity of StrontiumĮlectron affinity: 5.03 kJ/mol Nuclear Properties of Strontium The ionization potential of an atom: 5.67 Poisson ratio: 0.28 Atomic Properties of Strontium ![]() Molar magnetic susceptibility: 0.116×10 -9 m 3/mol Physical Properties of Strontiumĭensity: 2.64 g/cm 3 (In solid) 2.375 g/cm 3 (In Liquid) Mass magnetic susceptibility: 1.32×10 -9 m 3/kg Volume magnetic susceptibility: 0.00000347 Magnetic susceptibility (x mol): -92×10 -6 cm 3/mol Thermal conductivity: 35.4 W/(m∙K) Electrical properties of StrontiumĪ Electrical type: Conductor Magnetic Properties of Strontium The electron transitions which produced lines in the visible spectrum involved atoms rather than ions.Strontium Electron Configuration Thermal Properties of Strontiumĭebye temperature: 147 K (-126.15 oC, -195.07 oF) Because the electron is now at a higher and more energetically unstable level, it falls back down to the original level, but not necessarily in one transition. ![]() When heated, the electrons gain energy and can be excited into any of the empty higher-energy orbitals-7s, 6p, 4d, or any other, depending on the amount of energy a particular electron happens to absorb from the flame. For example, a sodium ion in an unexcited state has the electron configuration 1s 22s 22p 6. Flame colors are produced from the movement of the electrons in the metal ions present in the compounds. That means that each different metal will have a different pattern of spectral lines, and so a different flame color. The exact sizes of the possible jumps in energy terms vary from one metal to another. (right): Submicroscopic view of how electrons move between different energy levels in Na ion \): (left): Na ion emits yellow flame when an electron gets excited and drops back to its ground state. ![]()
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