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What Is the Physical State of Strontium Chapter 6 Review

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Chemic element, symbol Sr and diminutive number 38

Strontium, 38 Sr
Strontium destilled crystals.jpg
Strontium
Pronunciation

  • ( STRON-tee-É™m)

  • ( STRON-shee-É™m)
Appearance argent white metallic; with a stake yellow tint[1]
Standard atomic weight A r, std(Sr) 87.62(1) [2]
Strontium in the periodic table
Hydrogen Helium
Lithium Glucinium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silvery Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
Ca
↑
Sr
↓
Ba
rubidium ← strontium → yttrium
Diminutive number (Z) 38
Grouping grouping 2 (alkali metal earth metals)
Menstruum period 5
Block s-block
Electron configuration [Kr] 5s2
Electrons per crush 2, eight, eighteen, 8, 2
Physical properties
Phase atSTP solid
Melting point 1050 One thousand ​(777 °C, ​1431 °F)
Humid point 1650 K ​(1377 °C, ​2511 °F)
Density (almostr.t.) 2.64 g/cmthree
when liquid (atm.p.) 2.375 g/cm3
Estrus of fusion 7.43 kJ/mol
Heat of vaporization 141 kJ/mol
Molar estrus capacity 26.4 J/(mol·K)
Vapor pressure
P (Pa) 1 x 100 1 m 10 k 100 k
at T (K) 796 882 990 1139 1345 1646
Diminutive backdrop
Oxidation states +1,[3] +two (a strongly basic oxide)
Electronegativity Pauling scale: 0.95
Ionization energies
  • 1st: 549.five kJ/mol
  • 2nd: 1064.two kJ/mol
  • tertiary: 4138 kJ/mol
Atomic radius empirical: 215 pm
Covalent radius 195±10 pm
Van der Waals radius 249 pm

Color lines in a spectral range

Spectral lines of strontium
Other backdrop
Natural occurrence primordial
Crystal structure ​face up-centered cubic (fcc)

Face-centered cubic crystal structure for strontium

Thermal expansion 22.v Âµm/(k⋅K) (at 25 °C)
Thermal electrical conductivity 35.4 W/(m⋅Thousand)
Electrical resistivity 132 nΩ⋅m (at 20 °C)
Magnetic ordering paramagnetic
Tooth magnetic susceptibility −92.0×10−6  cm3/mol (298 K)[iv]
Young's modulus xv.seven GPa
Shear modulus six.03 GPa
Poisson ratio 0.28
Mohs hardness 1.5
CAS Number 7440-24-half dozen
History
Naming after the mineral strontianite, itself named after Strontian, Scotland
Discovery William Cruickshank (1787)
First isolation Humphry Davy (1808)
Main isotopes of strontium
Iso­tope Abun­trip the light fantastic toe Half-life (t 1/two) Disuse way Pro­duct
82Sr syn 25.36 d ε 82Rb
83Sr syn 1.35 d ε 83Rb
β+ 83Rb
γ –
84Sr 0.56% stable
85Sr syn 64.84 d ε 85Rb
γ –
86Sr nine.86% stable
87Sr 7.00% stable
88Sr 82.58% stable
89Sr syn 50.52 d ε 89Rb
β− 89Y
90Sr trace 28.90 y β− 90Y
 Category: Strontium
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Strontium is the chemical element with the symbol Sr and atomic number 38. An alkaline earth metal, strontium is a soft silverish-white yellowish metallic element that is highly chemically reactive. The metallic forms a night oxide layer when it is exposed to air. Strontium has physical and chemic backdrop similar to those of its two vertical neighbors in the periodic table, calcium and barium. It occurs naturally mainly in the minerals celestine and strontianite, and is generally mined from these.

Both strontium and strontianite are named after Strontian, a village in Scotland near which the mineral was discovered in 1790 by Adair Crawford and William Cruickshank; it was identified as a new element the next year from its cherry-red-red flame test color. Strontium was starting time isolated as a metallic in 1808 by Humphry Davy using the and then newly discovered process of electrolysis. During the 19th century, strontium was more often than not used in the production of sugar from saccharide beets (meet strontian procedure). At the peak of production of television receiver cathode ray tubes, as much as 75% of strontium consumption in the United states was used for the faceplate glass.[5] With the replacement of cathode ray tubes with other display methods, consumption of strontium has dramatically declined.[5]

While natural strontium (which is mostly the isotope strontium-88) is stable, the synthetic strontium-90 is radioactive and is 1 of the most dangerous components of nuclear fallout, as strontium is captivated by the body in a similar manner to calcium. Natural stable strontium, on the other mitt, is not hazardous to health.

Characteristics [edit]

Strontium is a divalent silverish metallic with a pale yellow tint whose properties are mostly intermediate between and like to those of its group neighbors calcium and barium.[6] Information technology is softer than calcium and harder than barium. Its melting (777 °C) and boiling (1377 °C) points are lower than those of calcium (842 °C and 1484 °C respectively); barium continues this downward trend in the melting signal (727 °C), but not in the boiling point (1900 °C). The density of strontium (ii.64 g/cm3) is similarly intermediate between those of calcium (1.54 g/cmiii) and barium (three.594 g/cmiii).[seven] Three allotropes of metallic strontium exist, with transition points at 235 and 540 °C.[8]

The standard electrode potential for the Srii+/Sr couple is −two.89 V, approximately midway between those of the Ca2+/Ca (−2.84 V) and Ba2+/Ba (−ii.92 V) couples, and close to those of the neighboring alkali metals.[nine] Strontium is intermediate between calcium and barium in its reactivity toward water, with which it reacts on contact to produce strontium hydroxide and hydrogen gas. Strontium metal burns in air to produce both strontium oxide and strontium nitride, merely since it does not react with nitrogen beneath 380 °C, at room temperature, it forms just the oxide spontaneously.[vii] Besides the simple oxide SrO, the peroxide SrO2 can exist made by straight oxidation of strontium metallic under a high pressure of oxygen, and there is some evidence for a yellow superoxide Sr(O2)2.[10] Strontium hydroxide, Sr(OH)2, is a stiff base, though it is not every bit strong as the hydroxides of barium or the brine metals.[11] All four dihalides of strontium are known.[12]

Due to the big size of the heavy s-block elements, including strontium, a vast range of coordination numbers is known, from 2, 3, or 4 all the style to 22 or 24 in SrCdeleven and SrZn13. The Sr2+ ion is quite big, so that high coordination numbers are the dominion.[thirteen] The large size of strontium and barium plays a meaning part in stabilising strontium complexes with polydentate macrocyclic ligands such equally crown ethers: for instance, while 18-crown-half-dozen forms relatively weak complexes with calcium and the alkali metals, its strontium and barium complexes are much stronger.[14]

Organostrontium compounds contain 1 or more strontium–carbon bonds. They have been reported every bit intermediates in Barbier-type reactions.[15] [16] [17] Although strontium is in the same group equally magnesium, and organomagnesium compounds are very usually used throughout chemistry, organostrontium compounds are not similarly widespread considering they are more difficult to brand and more reactive. Organostrontium compounds tend to be more similar to organoeuropium or organosamarium compounds due to the similar ionic radii of these elements (Sr2+ 118 pm; Eutwo+ 117 pm; Sm2+ 122 pm). Most of these compounds can simply be prepared at depression temperatures; bulky ligands tend to favor stability. For example, strontium dicyclopentadienyl, Sr(CfiveH5)2, must exist fabricated past directly reacting strontium metal with mercurocene or cyclopentadiene itself; replacing the CvH5 ligand with the bulkier C5(CH3)5 ligand on the other hand increases the compound's solubility, volatility, and kinetic stability.[18]

Because of its extreme reactivity with oxygen and water, strontium occurs naturally only in compounds with other elements, such as in the minerals strontianite and celestine. It is kept under a liquid hydrocarbon such as mineral oil or kerosene to preclude oxidation; freshly exposed strontium metal apace turns a yellow color with the formation of the oxide. Finely powdered strontium metal is pyrophoric, meaning that it will ignite spontaneously in air at room temperature. Volatile strontium salts impart a bright cherry-red color to flames, and these salts are used in pyrotechnics and in the product of flares.[vii] Like calcium and barium, as well as the alkali metals and the divalent lanthanides europium and ytterbium, strontium metal dissolves straight in liquid ammonia to give a dark bluish solution of solvated electrons.[6]

Isotopes [edit]

Natural strontium is a mixture of 4 stable isotopes: 84Sr, 86Sr, 87Sr, and 88Sr.[7] Their affluence increases with increasing mass number and the heaviest, 88Sr, makes upwardly about 82.6% of all natural strontium, though the abundance varies due to the product of radiogenic 87Sr equally the girl of long-lived beta-decomposable 87Rb.[19] This is the basis of rubidium–strontium dating. Of the unstable isotopes, the primary disuse manner of the isotopes lighter than 85Sr is electron capture or positron emission to isotopes of rubidium, and that of the isotopes heavier than 88Sr is electron emission to isotopes of yttrium. Of special annotation are 89Sr and 90Sr. The sometime has a one-half-life of l.6 days and is used to treat os cancer due to strontium's chemic similarity and hence ability to replace calcium.[20] [21] While ninetySr (half-life 28.xc years) has been used similarly, it is likewise an isotope of concern in fallout from nuclear weapons and nuclear accidents due to its product as a fission product. Its presence in bones tin cause bone cancer, cancer of nearby tissues, and leukemia.[22] The 1986 Chernobyl nuclear accident contaminated virtually 30,000 km2 with greater than x kBq/mii with 90Sr, which accounts for about 5% of the xcSr which was in the reactor core.[23]

History [edit]

Strontium is named later on the Scottish village of Strontian (Gaelic Sròn an t-Sìthein), where it was discovered in the ores of the lead mines.[24]

In 1790, Adair Crawford, a dr. engaged in the preparation of barium, and his colleague William Cruickshank, recognised that the Strontian ores exhibited properties that differed from those in other "heavy spars" sources.[25] This allowed Crawford to conclude on page 355 "... it is probable indeed, that the scotch mineral is a new species of earth which has not hitherto been sufficiently examined." The doctor and mineral collector Friedrich Gabriel Sulzer analysed together with Johann Friedrich Blumenbach the mineral from Strontian and named it strontianite. He also came to the conclusion that it was distinct from the witherite and contained a new earth (neue Grunderde).[26] In 1793 Thomas Charles Hope, a professor of chemistry at the University of Glasgow studied the mineral[27] [28] and proposed the proper name strontites.[29] [30] [31] He confirmed the earlier piece of work of Crawford and recounted: "... Because information technology a peculiar earth I idea it necessary to give it an name. I have chosen it Strontites, from the place information technology was institute; a manner of derivation in my stance, fully every bit proper as any quality information technology may possess, which is the present fashion." The element was eventually isolated by Sir Humphry Davy in 1808 past the electrolysis of a mixture containing strontium chloride and mercuric oxide, and announced past him in a lecture to the Royal Club on 30 June 1808.[32] In keeping with the naming of the other alkaline earths, he inverse the name to strontium.[33] [34] [35] [36] [37]

The start large-scale application of strontium was in the production of carbohydrate from sugar beet. Although a crystallisation process using strontium hydroxide was patented by Augustin-Pierre Dubrunfaut in 1849[38] the big scale introduction came with the improvement of the process in the early on 1870s. The German sugar industry used the procedure well into the 20th century. Before Earth War I the beet sugar manufacture used 100,000 to 150,000 tons of strontium hydroxide for this process per year.[39] The strontium hydroxide was recycled in the procedure, merely the need to substitute losses during production was loftier enough to create a significant demand initiating mining of strontianite in the Münsterland. The mining of strontianite in Germany ended when mining of the celestine deposits in Gloucestershire started.[xl] These mines supplied virtually of the earth strontium supply from 1884 to 1941. Although the celestine deposits in the Granada bowl were known for some time the big scale mining did not kickoff before the 1950s.[41]

During atmospheric nuclear weapons testing, it was observed that strontium-ninety is one of the nuclear fission products with a relatively high yield. The similarity to calcium and the gamble that the strontium-90 might become enriched in bones made research on the metabolism of strontium an important topic.[42] [43]

Occurrence [edit]

The mineral celestine (SrSO4)

Strontium usually occurs in nature, being the 15th well-nigh abundant element on Globe (its heavier congener barium existence the 14th), estimated to average approximately 360 parts per 1000000 in the Earth's crust[44] and is found chiefly equally the sulfate mineral celestine (SrSO4) and the carbonate strontianite (SrCOthree). Of the ii, celestine occurs much more frequently in deposits of sufficient size for mining. Considering strontium is used nigh often in the carbonate form, strontianite would be the more than useful of the two common minerals, just few deposits take been discovered that are suitable for development.[45] Because of the fashion information technology reacts with air and h2o, strontium simply exists in nature when combined to class minerals. Naturally occurring strontium is stable, but its synthetic isotope Sr-xc is only produced past nuclear fallout.

In groundwater strontium behaves chemically much like calcium. At intermediate to acidic pH Sr2+ is the dominant strontium species. In the presence of calcium ions, strontium normally forms coprecipitates with calcium minerals such equally calcite and anhydrite at an increased pH. At intermediate to acidic pH, dissolved strontium is spring to soil particles by cation exchange.[46]

The mean strontium content of ocean water is 8 mg/l.[47] [48] At a concentration between 82 and 90 μmol/fifty of strontium, the concentration is considerably lower than the calcium concentration, which is normally between 9.half dozen and 11.6 mmol/l.[49] [50] It is nevertheless much higher than that of barium, 13 Î¼g/fifty.[7]

Production [edit]

Grey and white world map with China colored green representing 50%, Spain colored blue-green representing 30%, Mexico colored light blue representing 20%, Argentina colored dark blue representing below 5% of strontium world production.

Strontium producers in 2014[51]

The three major producers of strontium every bit celestine as of 2015 are Mainland china (150,000 t), Spain (ninety,000 t), and Mexico (70,000 t); Argentina (ten,000 t) and Kingdom of morocco (2,500 t) are smaller producers. Although strontium deposits occur widely in the United states, they take non been mined since 1959.[51]

A large proportion of mined celestine (SrSO4) is converted to the carbonate by ii processes. Either the celestine is straight leached with sodium carbonate solution or the celestine is roasted with coal to class the sulfide. The second stage produces a dark-coloured material containing mostly strontium sulfide. This so-called "black ash" is dissolved in water and filtered. Strontium carbonate is precipitated from the strontium sulfide solution by introduction of carbon dioxide.[52] The sulfate is reduced to the sulfide by the carbothermic reduction:

SrSO4 + two C → SrS + 2 CO2

Nigh 300,000 tons are processed in this way annually.[53]

The metal is produced commercially by reducing strontium oxide with aluminium. The strontium is distilled from the mixture.[53] Strontium metal tin also exist prepared on a small calibration by electrolysis of a solution of strontium chloride in molten potassium chloride:[9]

Sr2+ + ii
e −
→ Sr
2 Cl− → Cltwo + two
e −

Applications [edit]

Cathode ray tube (CRT) display made from strontium and barium oxide-containing drinking glass. This application used to swallow most of the world's production of strontium.

Consuming 75% of product, the principal use for strontium was in glass for colour telly cathode ray tubes,[53] where it prevented X-ray emission.[54] [55] This application for strontium has been failing because CRTs are being replaced by other display methods. This decline has a meaning influence on the mining and refining of strontium.[45] All parts of the CRT must absorb X-rays. In the cervix and the funnel of the tube, lead glass is used for this purpose, but this blazon of glass shows a browning effect due to the interaction of the X-rays with the glass. Therefore, the front panel is made from a different glass mixture with strontium and barium to absorb the 10-rays. The average values for the drinking glass mixture adamant for a recycling study in 2005 is 8.5% strontium oxide and x% barium oxide.[56]

Because strontium is and so like to calcium, it is incorporated in the bone. All 4 stable isotopes are incorporated, in roughly the same proportions they are constitute in nature. However, the actual distribution of the isotopes tends to vary greatly from one geographical location to another. Thus, analyzing the bone of an individual can help determine the region information technology came from.[57] [58] This arroyo helps to identify the ancient migration patterns and the origin of commingled homo remains in battlefield burial sites.[59]

87Sr/86Sr ratios are commonly used to make up one's mind the probable provenance areas of sediment in natural systems, particularly in marine and fluvial environments. Dasch (1969) showed that surface sediments of Atlantic displayed 87Sr/86Sr ratios that could exist regarded as bulk averages of the 87Sr/86Sr ratios of geological terrains from side by side landmasses.[60] A good example of a fluvial-marine system to which Sr isotope provenance studies have been successfully employed is the River Nile-Mediterranean system.[61] Due to the differing ages of the rocks that institute the majority of the Bluish and White Nile, catchment areas of the changing provenance of sediment reaching the River Nile Delta and Eastward Mediterranean Sea can exist discerned through strontium isotopic studies. Such changes are climatically controlled in the Belatedly Fourth.[61]

More recently, 87Sr/86Sr ratios have as well been used to determine the source of aboriginal archaeological materials such as timbers and corn in Chaco Coulee, New Mexico.[62] [63] 87Sr/86Sr ratios in teeth may as well be used to track animal migrations.[64] [65]

Strontium aluminate is oftentimes used in glow in the dark toys, as it is chemically and biologically inert.[ citation needed ]

red fireworks

Strontium salts are added to fireworks in order to create reddish colors

Strontium carbonate and other strontium salts are added to fireworks to give a deep cherry colour.[66] This same effect identifies strontium cations in the flame test. Fireworks consume most v% of the world's production.[53] Strontium carbonate is used in the manufacturing of hard ferrite magnets.[67] [68]

Strontium chloride is sometimes used in toothpastes for sensitive teeth. 1 popular brand includes x% full strontium chloride hexahydrate by weight.[69] Small-scale amounts are used in the refining of zinc to remove small amounts of lead impurities.[7] The metal itself has a limited use every bit a getter, to remove unwanted gases in vacuums by reacting with them, although barium may also be used for this purpose.[ix]

The ultra-narrow optical transition between the [Kr]5s2 1South0 electronic basis country and the metastable [Kr]5s5p 3P0 excited state of 87Sr is i of the leading candidates for the future re-definition of the 2d in terms of an optical transition as opposed to the current definition derived from a microwave transition between different hyperfine ground states of 133Cs.[70] Current optical diminutive clocks operating on this transition already surpass the precision and accuracy of the current definition of the 2d.

Radioactive strontium [edit]

89Sr is the active ingredient in Metastron,[71] a radiopharmaceutical used for bone hurting secondary to metastatic os cancer. The strontium is processed like calcium past the body, preferentially incorporating information technology into bone at sites of increased osteogenesis. This localization focuses the radiation exposure on the cancerous lesion.[21]

RTGs from Soviet-era lighthouses

ninetySr has been used as a power source for radioisotope thermoelectric generators (RTGs). 90Sr produces approximately 0.93 watts of heat per gram (information technology is lower for the course of 90Sr used in RTGs, which is strontium fluoride).[72] Notwithstanding, 90Sr has one 3rd the lifetime and a lower density than 238Pu, another RTG fuel. The main reward of 90Sr is that it is cheaper than 238Pu and is found in nuclear waste. The Soviet Matrimony deployed nearly 1000 of these RTGs on its northern coast as a power source for lighthouses and meteorology stations.[73] [74]

Biological role [edit]

Strontium
Hazards
GHS labelling:

Pictograms

 GHS02: Flammable GHS07: Exclamation mark

Indicate word

 Danger

Take a chance statements

 H261, H315

Precautionary statements

 P223, P231+P232, P370+P378, P422 [75]
NFPA 704 (fire diamond)

two

0

2

Due west

Chemical compound

Acantharea, a relatively large grouping of marine radiolarian protozoa, produce intricate mineral skeletons composed of strontium sulfate.[76] In biological systems, calcium is substituted to a small extent by strontium.[77] In the human body, well-nigh of the absorbed strontium is deposited in the bones. The ratio of strontium to calcium in man bones is between one:1000 and 1:2000, roughly in the same range as in the claret serum.[78]

Effect on the human trunk [edit]

The man body absorbs strontium as if it were its lighter congener calcium. Because the elements are chemically very like, stable strontium isotopes exercise not pose a pregnant wellness threat. The average human has an intake of almost two milligrams of strontium a day.[79] In adults, strontium consumed tends to adhere only to the surface of bones, but in children, strontium can supervene upon calcium in the mineral of the growing bones and thus lead to bone growth problems.[80]

The biological half-life of strontium in humans has variously been reported as from 14 to 600 days,[81] [82] one,000 days,[83] xviii years,[84] 30 years[85] and, at an upper limit, 49 years.[86] The wide-ranging published biological one-half-life figures are explained by strontium's complex metabolism within the body. Nevertheless, by averaging all excretion paths, the overall biological half-life is estimated to be almost eighteen years.[87] The emptying charge per unit of strontium is strongly afflicted past age and sex, due to differences in bone metabolism.[88]

The drug strontium ranelate aids os growth, increases bone density, and lessens the incidence of vertebral, peripheral, and hip fractures.[89] [90] Even so, strontium ranelate also increases the risk of venous thromboembolism, pulmonary embolism, and serious cardiovascular disorders, including myocardial infarction. Its apply is therefore now restricted.[91] Its beneficial effects are likewise questionable, since the increased bone density is partially caused by the increased density of strontium over the calcium which information technology replaces. Strontium likewise bioaccumulates in the body.[92] Despite restrictions on strontium ranelate, strontium is still independent in some supplements.[93] [94] There is not much scientific evidence on risks of strontium chloride when taken by rima oris. Those with a personal or family history of blood clotting disorders are advised to avoid strontium.[93] [94]

Strontium has been shown to inhibit sensory irritation when applied topically to the skin.[95] [96] Topically practical, strontium has been shown to accelerate the recovery rate of the epidermal permeability barrier (skin barrier).[97]

Nuclear waste [edit]

Strontium-90 is a radioactive fission production produced by nuclear reactors used in nuclear ability. It is a major component of loftier level radioactive waste and spent nuclear fuel. Its 29-year half life is short plenty that its disuse heat has been used to ability arctic lighthouses, but long enough that it tin accept hundreds of years to decay to rubber levels. Exposure from contaminated water and food may increment the run a risk of leukemia, bone cancer[98] and primary hyperparathyroidism.[99]

Remediation [edit]

Algae has shown selectivity for strontium in studies, where almost plants used in bioremediation have not shown selectivity betwixt calcium and strontium, often condign saturated with calcium, which is greater in quantity and also present in nuclear waste product.[98]

Researchers accept looked at the bioaccumulation of strontium by Scenedesmus spinosus (algae) in simulated wastewater. The study claims a highly selective biosorption capacity for strontium of S. spinosus, suggesting that it may be appropriate for use of nuclear wastewater.[100]

A report of the pond alga Closterium moniliferum using non-radioactive strontium establish that varying the ratio of barium to strontium in water improved strontium selectivity.[98]

See also [edit]

References [edit]

  1. ^ Greenwood and Earnshaw, p. 112
  2. ^ "Standard Atomic Weights: Strontium". CIAAW. 1969.
  3. ^ Colarusso, P.; Guo, B.; Zhang, K.-Q.; Bernath, P. F. (1996). "High-Resolution Infrared Emission Spectrum of Strontium Monofluoride" (PDF). J. Molecular Spectroscopy. 175 (1): 158. Bibcode:1996JMoSp.175..158C. doi:x.1006/jmsp.1996.0019.
  4. ^ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemic Rubber Company Publishing. pp. E110. ISBN0-8493-0464-4.
  5. ^ a b "Mineral Resource of the Calendar month: Strontium". U.S. Geological Survey. 8 December 2014. Retrieved xvi August 2015.
  6. ^ a b Greenwood and Earnshaw, pp. 112–13
  7. ^ a b c d e f C. R. Hammond The elements (pp. iv–35) in Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Printing. ISBN0-8493-0486-5.
  8. ^ Ropp, Richard C. (31 December 2012). Encyclopedia of the Alkaline Earth Compounds. p. xvi. ISBN978-0-444-59553-9.
  9. ^ a b c Greenwood and Earnshaw, p. 111
  10. ^ Greenwood and Earnshaw, p. 119
  11. ^ Greenwood and Earnshaw, p. 121
  12. ^ Greenwood and Earnshaw, p. 117
  13. ^ Greenwood and Earnshaw, p. 115
  14. ^ Greenwood and Earnshaw, p. 124
  15. ^ Miyoshi, N.; Kamiura, K.; Oka, H.; Kita, A.; Kuwata, R.; Ikehara, D.; Wada, Yard. (2004). "The Barbier-Type Alkylation of Aldehydes with Alkyl Halides in the Presence of Metallic Strontium". Bulletin of the Chemical Society of Japan. 77 (2): 341. doi:10.1246/bcsj.77.341.
  16. ^ Miyoshi, N.; Ikehara, D.; Kohno, T.; Matsui, A.; Wada, M. (2005). "The Chemistry of Alkylstrontium Halide Analogues: Barbier-type Alkylation of Imines with Alkyl Halides". Chemical science Letters. 34 (6): 760. doi:10.1246/cl.2005.760.
  17. ^ Miyoshi, Northward.; Matsuo, T.; Wada, Yard. (2005). "The Chemistry of Alkylstrontium Halide Analogues, Part 2: Barbier-Type Dialkylation of Esters with Alkyl Halides". European Journal of Organic Chemistry. 2005 (twenty): 4253. doi:10.1002/ejoc.200500484.
  18. ^ Greenwood and Earnshaw, pp. 136–37
  19. ^ Greenwood and Earnshaw, p. nineteen
  20. ^ Halperin, Edward C.; Perez, Carlos A.; Brady, Luther W. (2008). Perez and Brady's principles and do of radiations oncology. Lippincott Williams & Wilkins. pp. 1997–. ISBN978-0-7817-6369-one . Retrieved 19 July 2011.
  21. ^ a b Bauman, Glenn; Charette, Manya; Reid, Robert; Sathya, Jinka (2005). "Radiopharmaceuticals for the palliation of painful bone metastases – a systematic review". Radiotherapy and Oncology. 75 (3): 258.E1–258.E13. doi:10.1016/j.radonc.2005.03.003. PMID 16299924.
  22. ^ "Strontium | Radiation Protection | US EPA". EPA. 24 April 2012. Retrieved 18 June 2012.
  23. ^ "Chernobyl: Cess of Radiological and Health Touch, 2002 update; Affiliate I – The site and blow sequence" (PDF). OECD-NEA. 2002. Retrieved iii June 2015.
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  26. ^ Sulzer, Friedrich Gabriel; Blumenbach, Johann Friedrich (1791). "Ãœber den Strontianit, ein Schottisches Foßil, das ebenfalls eine neue Grunderde zu enthalten scheint". Bergmännisches Journal: 433–36.
  27. ^ "Thomas Charles Promise, MD, FRSE, FRS (1766-1844) - School of Chemistry". www.chem.ed.ac.u.k..
  28. ^ Doyle, W.P. "Thomas Charles Promise, MD, FRSE, FRS (1766–1844)". The University of Edinburgh. Archived from the original on 2 June 2013.
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Bibliography [edit]

  • Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN978-0-08-037941-8.

External links [edit]

  • WebElements.com – Strontium
  • Strontium at The Periodic Table of Videos (Academy of Nottingham)

brownentreirs.blogspot.com

Source: https://en.wikipedia.org/wiki/Strontium

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