Lithium
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| Lithium | |||||||
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| General Info | |||||||
| Atomic Symbol | Li | ||||||
| Atomic Number | 3 | ||||||
| Atomic Weight | 6.941 g/mol6.941 amu | ||||||
| Chemical series | [[Alkali metals]] | ||||||
| Appearance | silvery white/grey 
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| Group, Period, Block | 1, 2, S | ||||||
| Electron configuration | 1s2, 2s1 | ||||||
| Electrons per shell | 2, 1 
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| CAS number | [[CAS number::[7439-93-2]]] | ||||||
| Physical properties | |||||||
| Phase | {{{phase}}} | ||||||
| Density | 0.534 g/ml | ||||||
| Melting point | {{{melting}}}warning.png"{{{melting}}}" is not a number. | ||||||
| Boiling point | {{{boiling}}}warning.png"{{{boiling}}}" is not a number. | ||||||
| Isotopes of Lithium | |||||||
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| All properties are for STP unless otherwise stated. | |||||||
Lithium (comes form the Greek word lithos which means stone), is the 3rd element. Lithium is one of the most abundant elements in the world even thought it does not exist in its natural form.You might not think lithium plays a big rule in the world we live in today, but it does. Lithium has many uses; it brought us to space, powered pace makers, and even helps people live a normal life day in and day out
Contents |
Properties
Lithium is located in group 1 even though it has some property of alkaline-Earth metals It is has a single valence electron. Lithium is an unstable substance that is will to lose electrons to become positive. Because lithium reacts with water extremely easily it does not exist as a free element on Earth. Lithium is also extremely soft; you are able to cut lithium with a knife. When lithium is not exposed to air it as a soft silvery- lustrous metal. [1] Lithium is also very light is able to float in water. Lithium is also very flammable, when place over it flame it burns at high tempters, its flames is white. Lithium will also burn when it comes in compact with water. It is the only metal that reacts with nitrogen. Lithium metal is also very corrosive; you need to be carefully when you come in contact with it because it is very have corrosive. Lithium is not found in lithium humans
Occurrences
Lithium does not exist in tits free form, although lithium is widely distributed. Lithium is also found in most igneous rocks, and in brines. Lithium is contained most highly in the minerals spodumene, lepidslite, amblygonite, spodumemen, and petalite. Chile is the worlds largest lithium producer; Argentina is the second largest producer. These two nations mine most of their product from brine pools.
Uses
Lithium is used in the making of batteries. The reason why lithium is used in batteries is because of its lightweight and being capable of creation twice as much power then a standard dry cell battier of 1.5v.
Lithium plays a big role in medical field. Lithium carbonate, lithium citrate, and lithium orotate are used in the treatment of bipolar disorder. The benefit of using lithium salt is that they treat both mania and depression unlike the traditional treatments. Lithium also has the capability to use as a treatment in migraine disease and cluster headaches.
Lithium is also use in 7up, and hundreds of other soft drinks and in a few beers.
History
Lithium was discover by Jose Bonifacio de Anoada I silva a Brazilian scientist in Sweden at the end of the 1700’s. Two men, William Jomas Brande, and Sir Humphry Davy first isolated lithium. These two men used electrolysis to isolate Lithium. Lithium was first used in commercial production was in 1923, the product was a lithium metal
Lithium pharmacology
History
John Cade an Australian psychiatrist discoed what the true use of Lithium was in 1949. He did this b giving lithium urate, and lithium salts to animals, when given to animal it tranquilized them. And after this drug as reformed it was used in controlling mania in chronically hospitalized patients. But after a few mishaps these drugs were discounted, Lithium was not used in the US in tell it was approved by the United States Food and Drug Administration in 1970 for the treatment of manic illness.
Treatment
Lithium is mostly used in the treatment of bipolar disorder. When lithium is used in treatments it is used with anti-psychotic drugs, because Lithium can take several weeks to have full effects. Lithium still has many other uses in the medical field; some of these are migraine, um polar, depression, and cycloid psychosis. Lithium is so versatile it can be used on young children, to as young as four.
Mechanism of Action
Nobody knows why Lithium is capable of being used as a mood-stabilizing drug.
Lithium toxicity and side effects
When lithium is used in the treatment of bipolar the dosages in 15-20mg per kg of the patients body weight; this is such a height dosage that the patient needs to be monitored during treatment. Not all of Lithium long-term effect are know, the ones that are know is that it causes histological and functional changes in the kidney, The results of overdose can be sever but most common is effect are: confusion, diarrhea, lethargy; severe tremors, and upset stomach.
Levels In Humans
Blood/mg dm-3: 0.004
Bone/p.p.m: 1.3
Liver/p.p.m: 0.025
Muscle/p.p.m: 0.023
Daily Dietary Intake: 0.1-2 mg
Total Mass In Avg. 70kg human: 7 mg [2]
Isotopes
- Main Article: Isotopes
Naturally lithium contains two stable isotopes 6Li and 7Li. 7Li is the most abundantly in the nature taking up about 92.5% of the natural abundance. There are seven radioisotopes , with 8Li being the most stable with a half-life’s that is less the 8.6ms. The isotope with the shortest life time is the isotope 4Li, because it decays very rapidly and has a life time of 7.58043x10-23 s. The most unstable isotope is the 11Li. This is so unstable that it has a nuclear halo of two neutrons.[3]
| nuclide symbol | Z(p) | N(n) | isotopic mass (u) | half-life | nuclear spin | representative isotopic composition (mole fraction) | range of natural variation (mole fraction) |
|---|---|---|---|---|---|---|---|
| excitation energy | |||||||
| 4Li | 3 | 1 | 4.02719(23) | 91(9)−24 s [6.03 MeV] | 2- | ||
| 5Li | 3 | 2 | 5.01254(5) | 370(30)−24 s [~1.5 MeV] | 3/2- | ||
| 6Li | 3 | 3 | 6.015122795(16) | STABLE | 1+ | [0.0759(4)] | 0.07714-0.07225 |
| 7Li | 3 | 4 | 7.01600455(8) | STABLE | 3/2- | [0.9241(4)] | 0.92275-0.92786 |
| 8Li | 3 | 5 | 8.02248736(10) | 840.3(9) ms | 2+ | ||
| 9Li | 3 | 6 | 9.0267895(21) | 178.3(4) ms | 3/2- | ||
| 10Li | 3 | 7 | 10.035481(16) | 2.0(5)−21 s [1.2(3) MeV] | (1-,2-) | ||
| 10m1Li | 200(40) keV | 3.7(15)−21 s | 1+ | ||||
| 10m2Li | 480(40) keV | 1.35(24)−21 s | 2+ | ||||
| 11Li | 3 | 8 | 11.043798(21) | 8.75(14) ms | 3/2- | ||
| 12Li | 3 | 9 | 12.05378(107)# | <10 ns | |||
Compounds
Lithium chloride
Preparation
To make lithium chloride you need to cause a chemical reaction with Lithium Hydroxide and Hydrochloride acid or Lithium carbonate with hydrochloric acid.
Uses
The main use of Lithium Chloride is in the making of lithium metal. They did this by electrolysis of a LiCl/KC1 melt at 450 C, In the 1940’s Lithium Chloride was used instead of salt, but was soon discontinued because of toxic effects.
Properties
| Solubility of LiCl in various solvents (g LiCl / 100g of solvent at 25° C) | |
|---|---|
| H2O | 55 |
| Liquid ammonia | 3.02 |
| Liquid sulfur dioxide | 0.012 |
| Methanol | 21 - 41 |
| Formic acid | 27.5 |
| Sulfolane | 1.5 |
| Acetonitrile | 0.14 |
| Acetone | 0.83 |
| Formamide | 28.2 |
| Dimethylformamide | 11 - 28 |
| Reference: Burgess, J. Metal Ions in Solution (Ellis Horwood, New York, 1978) ISBN 0-85312-027-7 | |
Lithium Bromide
Properties Lithium bromide has a melting point 552s c, and a bowling point 1265 c. Lithium Bromide has an appearance of white crystalline powder. Lithium Bromide has a moral mass of 86.845 g/mol and a density and phase of 3.464 g/cm3, solid
Uses Lithium Bromide was first use a sedative in the early 1900s, but after a few tragedies caused by this when several patients with heart problems die when they tried to use Lithium Bromide as a salt substitute if the 1940s. As of know Lithium Bromide is only used in air conditioning. [5]
Lithium niobate
Properties Lithium nibate is formed when you add oxygen, niobium, and lithium. Lithium niobate is a soiled material that is colorless. Lithium niobate has a melting point of 1257 °C and has a density of 4,65 g/cm³.
Uses Lithium niobate is used in laser frequency doubling, birefringent,Q-switching devices for lasers, acousto-optic devices, and in the manufacture of optical waveguides. [6]
Lithium Hydride
Properties Lithium hydride has a grayish white tint to it, it is odorless and is a crystalline solid. Lithium Hydroxide has a melting point of 689 c and a density of 780 kilo grams per cubic meter. Lithium Hydride is also extremely flammable.
Uses Lithium Hydride is most common use is in hydrogen generators. It is used as a coolant and a shielding when used in nuclear reactors. [7]
Lithium hydroxide
Properties Lithium hydroxide is white, and is a hygroscopic crystalline material. Lithium Hydroxide is extremely soluble it is soluble in water and in ethanol.
Uses Lithium Hydroxide has many uses it is used in purification of gases and air battery electrolyte, ceramics and in an all purpose lubricating grease. [8]
Related References
- Lithium Wikipedia
- The essentialsWeb Elements
- Lithium UCC
