Difference between revisions of "Lithium"
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{{Infobox element | {{Infobox element | ||
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| − | |image name= | + | |image name= Lithium metal sheet from an Energizer battery by NurdRage.jpg |
|image alt= | |image alt= | ||
| − | |image size= | + | |image size=300 |
| − | |image name comment= | + | |image name comment=Lithium metal from an Energizer battery |
|image name 2= | |image name 2= | ||
|image alt 2= | |image alt 2= | ||
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|heat vaporization ref= | |heat vaporization ref= | ||
|heat vaporization comment= | |heat vaporization comment= | ||
| − | |heat capacity= | + | |heat capacity=24.86 |
|heat capacity ref= | |heat capacity ref= | ||
|heat capacity comment= | |heat capacity comment= | ||
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|heat capacity 2 ref= | |heat capacity 2 ref= | ||
|heat capacity 2 comment= | |heat capacity 2 comment= | ||
| − | |vapor pressure 1= | + | |vapor pressure 1=797 |
| − | |vapor pressure 10= | + | |vapor pressure 10=885 |
| − | |vapor pressure 100= | + | |vapor pressure 100=995 |
| − | |vapor pressure 1 k= | + | |vapor pressure 1 k=1144 |
| − | |vapor pressure 10 k= | + | |vapor pressure 10 k=1337 |
| − | |vapor pressure 100 k= | + | |vapor pressure 100 k=1610 |
|vapor pressure ref= | |vapor pressure ref= | ||
|vapor pressure comment= | |vapor pressure comment= | ||
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|oxidation states=+1 | |oxidation states=+1 | ||
|oxidation states ref= | |oxidation states ref= | ||
| − | |oxidation states comment= | + | |oxidation states comment=(a strongly basic oxide) |
|electronegativity=0.98 | |electronegativity=0.98 | ||
|electronegativity ref= | |electronegativity ref= | ||
|electronegativity comment= | |electronegativity comment= | ||
| − | |ionization energy 1= | + | |ionization energy 1=520.2 |
|ionization energy 1 ref= | |ionization energy 1 ref= | ||
|ionization energy 1 comment= | |ionization energy 1 comment= | ||
| − | |ionization energy 2= | + | |ionization energy 2=7298.1 |
|ionization energy 2 ref= | |ionization energy 2 ref= | ||
|ionization energy 2 comment= | |ionization energy 2 comment= | ||
| − | |ionization energy 3= | + | |ionization energy 3=11815 |
|ionization energy 3 ref= | |ionization energy 3 ref= | ||
|ionization energy 3 comment= | |ionization energy 3 comment= | ||
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|ionization energy ref= | |ionization energy ref= | ||
|ionization energy comment= | |ionization energy comment= | ||
| − | |atomic radius= | + | |atomic radius=152 |
|atomic radius ref= | |atomic radius ref= | ||
|atomic radius comment= | |atomic radius comment= | ||
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|atomic radius calculated ref= | |atomic radius calculated ref= | ||
|atomic radius calculated comment= | |atomic radius calculated comment= | ||
| − | |covalent radius= | + | |covalent radius=128±7 |
|covalent radius ref= | |covalent radius ref= | ||
|covalent radius comment= | |covalent radius comment= | ||
| − | |Van der Waals radius= | + | |Van der Waals radius=182 |
|Van der Waals radius ref= | |Van der Waals radius ref= | ||
|Van der Waals radius comment= | |Van der Waals radius comment= | ||
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|speed of sound ref= | |speed of sound ref= | ||
|speed of sound comment= | |speed of sound comment= | ||
| − | |speed of sound rod at 20= | + | |speed of sound rod at 20=6000 |
|speed of sound rod at 20 ref= | |speed of sound rod at 20 ref= | ||
|speed of sound rod at 20 comment= | |speed of sound rod at 20 comment= | ||
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|thermal expansion ref= | |thermal expansion ref= | ||
|thermal expansion comment= | |thermal expansion comment= | ||
| − | |thermal expansion at 25= | + | |thermal expansion at 25=46 |
|thermal expansion at 25 ref= | |thermal expansion at 25 ref= | ||
|thermal expansion at 25 comment= | |thermal expansion at 25 comment= | ||
| − | |thermal conductivity= | + | |thermal conductivity=84.8 |
|thermal conductivity ref= | |thermal conductivity ref= | ||
|thermal conductivity comment= | |thermal conductivity comment= | ||
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|thermal diffusivity ref= | |thermal diffusivity ref= | ||
|thermal diffusivity comment= | |thermal diffusivity comment= | ||
| − | |electrical resistivity= | + | |electrical resistivity=9.28·10<sup>-8</sup> |
|electrical resistivity unit prefix= | |electrical resistivity unit prefix= | ||
|electrical resistivity ref= | |electrical resistivity ref= | ||
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|Curie point ref= | |Curie point ref= | ||
|Curie point comment= | |Curie point comment= | ||
| − | |magnetic ordering= | + | |magnetic ordering=Paramagnetic |
|magnetic ordering ref= | |magnetic ordering ref= | ||
|magnetic ordering comment= | |magnetic ordering comment= | ||
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|tensile strength ref= | |tensile strength ref= | ||
|tensile strength comment= | |tensile strength comment= | ||
| − | |Young's modulus= | + | |Young's modulus=4.9 |
|Young's modulus ref= | |Young's modulus ref= | ||
|Young's modulus comment= | |Young's modulus comment= | ||
| − | |Shear modulus= | + | |Shear modulus=4.2 |
|Shear modulus ref= | |Shear modulus ref= | ||
|Shear modulus comment= | |Shear modulus comment= | ||
| − | |Bulk modulus= | + | |Bulk modulus=11 |
|Bulk modulus ref= | |Bulk modulus ref= | ||
|Bulk modulus comment= | |Bulk modulus comment= | ||
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|Vickers hardness ref= | |Vickers hardness ref= | ||
|Vickers hardness comment= | |Vickers hardness comment= | ||
| − | |Brinell hardness= | + | |Brinell hardness=5 |
|Brinell hardness ref= | |Brinell hardness ref= | ||
|Brinell hardness comment= | |Brinell hardness comment= | ||
| − | |CAS number= | + | |CAS number=7439-93-2 |
|CAS number ref= | |CAS number ref= | ||
|CAS number comment= | |CAS number comment= | ||
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|prediction date ref= | |prediction date ref= | ||
|prediction date= | |prediction date= | ||
| − | |discovered by= | + | |discovered by=Johan August Arfwedson |
|discovery date ref= | |discovery date ref= | ||
| − | |discovery date= | + | |discovery date=1817 |
| − | |first isolation by= | + | |first isolation by= William Thomas Brande |
|first isolation date ref= | |first isolation date ref= | ||
| − | |first isolation date= | + | |first isolation date=1821 |
|discovery and first isolation by= | |discovery and first isolation by= | ||
|named by= | |named by= | ||
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|engvar= | |engvar= | ||
}} | }} | ||
| − | '''Lithium''' is a an [[alkali metal]], the lightest metal and least dense solid element at room temperature, with the atomic number 3. It is soft, silvery-white metal, with a density of 534 kg/m<sup>3</sup>. It is highly reactive, and it is usually stored in mineral oil. However, because of its extremely low density, it floats in mineral oil, storing the metal proves to be difficult. | + | '''Lithium''' is a an [[alkali metal]], the lightest metal and least dense solid element at room temperature, with the atomic number 3 and symbol '''Li'''. It is soft, silvery-white metal, with a density of 534 kg/m<sup>3</sup>. It is highly reactive, and it is usually stored in [[[mineral oil]]. However, because of its extremely low density, it floats in mineral oil, storing the metal proves to be difficult. |
==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| − | Lithium, like all the alkali metals reacts violently with water, releasing hydrogen and can ignite, but this reaction is slightly less violent than the other alkali metals | + | Lithium, like all the alkali metals reacts violently with water, releasing hydrogen and can ignite, but this reaction is slightly less violent than the other alkali metals. |
| − | + | : Li + H<sub>2</sub>O → LiOH + ½ H<sub>2</sub> | |
| − | Contrary to popular belief, lithium, not cesium, is the most reactive element on the periodic table. It has the lowest reduction potential in aqueous solution, and gram-for-gram (as well as mole-for-mole) has a higher energy content than [[cesium]]. | + | In open air, it quickly forms a layer of oxide as well as nitride, and if the air also contains [[water]] vapors and [[carbon dioxide]], [[lithium hydroxide]] and [[lithium carbonate]]. |
| + | |||
| + | : 4 Li + O<sub>2</sub> → 2 Li<sub>2</sub>O | ||
| + | : 6 Li + 2 N<sub>2</sub> → 2 Li<sub>3</sub>N<sub>2</sub> | ||
| + | |||
| + | Lithium will burn in air, and it tends to burn with a red-crimson flame. As noted by NurdRage in his video where he extracted lithium from an energizer battery, this flame is incredibly bright, so welding goggles should be used if this reaction is attempted. Such fires are difficult to extinguish, requiring dry powder extinguishers (class D). | ||
| + | |||
| + | Lithium is also a strong reducing agent. It is also used in organometallic synthesis in the form of organolithium compounds such as [[n-butyllithium]] and [[tert-butyllithium]], although they are extremely rarely used by the amateur chemist, mainly because they're very dangerous (pyrophoric and caustic). Molten lithium is probably the most powerful reducing agent known, and will explode on contact with almost anything non-metallic, including wood, glass and concrete. It is the only alkali metal that cannot be safely melted in a glass container, as it reacts exothermically with glass almost immediately.<ref>https://www.youtube.com/watch?v=GE-NkVqUiHs</ref> | ||
| + | |||
| + | Contrary to popular belief, lithium, not cesium, is the most reactive element on the periodic table. It has the lowest reduction potential in aqueous solution, and gram-for-gram (as well as mole-for-mole) has a higher energy content than [[caesium|cesium]]. | ||
Lithium metal can dissolve in anhydrous [[ammonia]] and [[ethylenediamine]], forming its electride salt. | Lithium metal can dissolve in anhydrous [[ammonia]] and [[ethylenediamine]], forming its electride salt. | ||
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Lithium is a soft, silver-white metal. It is soft enough to be cut with a knife. | Lithium is a soft, silver-white metal. It is soft enough to be cut with a knife. | ||
| − | Lithium has the highest specific heat capacity of any solid element, 3.58 kJ/( | + | Lithium has the highest specific heat capacity of any solid element, 3.58 kJ/(kg·K), the highest of all solids. Because of this, lithium metal is often used in coolants for heat transfer applications.<ref>http://hilltop.bradley.edu/~spost/THERMO/solidcp.pdf</ref> |
Lithium has a density of only 534 kg/m<sup>3</sup>, making it the lightest metal and solid element at standard conditions. It is lighter than any hydrocarbon oil, which causes the metal to float in the oil is stored. The only organic hydrocarbons lighter than lithium are liquid methane (465 kg/m<sup>3</sup>), liquid propane (493.5 kg/m<sup>3</sup>), liquid propylene (514.4 kg/m<sup>3</sup>).<ref>http://www.engineeringtoolbox.com/liquids-densities-d_743.html</ref> Since these solvents are liquid only at very low temperatures or under high pressure, storing lithium in them is impractical. | Lithium has a density of only 534 kg/m<sup>3</sup>, making it the lightest metal and solid element at standard conditions. It is lighter than any hydrocarbon oil, which causes the metal to float in the oil is stored. The only organic hydrocarbons lighter than lithium are liquid methane (465 kg/m<sup>3</sup>), liquid propane (493.5 kg/m<sup>3</sup>), liquid propylene (514.4 kg/m<sup>3</sup>).<ref>http://www.engineeringtoolbox.com/liquids-densities-d_743.html</ref> Since these solvents are liquid only at very low temperatures or under high pressure, storing lithium in them is impractical. | ||
| − | In addition, lithium has the highest melting point of all alkali metals, at roughly 180 degrees Celsius. | + | In addition, lithium has the highest melting point of all alkali metals, at roughly 180 degrees Celsius. This makes it difficult to melt it under oil (a common tactic for removing tarnish from the other alkali metals). Molten lithium is extremely reactive and will react with almost all ceramic materials, therefore lithium is only melted in crucibles made of special metals, such as molybdenum. It also has a high boiling point, of 1330 °C. |
Lithium dissolves in liquid ammonia.<ref>http://pubs.acs.org/doi/abs/10.1021/j150343a013</ref> | Lithium dissolves in liquid ammonia.<ref>http://pubs.acs.org/doi/abs/10.1021/j150343a013</ref> | ||
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==Preparation== | ==Preparation== | ||
| − | Industrially, elemental lithium is produced electrolytically from a mixture of fused 55% [[lithium chloride]] and 45% [[potassium chloride]] at about 450 <sup>o</sup>C. As molten lithium is highly reactive, this process should be performed in installations made of corrosion resistant alloys. | + | Industrially, elemental lithium is produced electrolytically from a mixture of fused 55% [[lithium chloride]] and 45% [[potassium chloride]] at about 450 <sup>o</sup>C.<ref>https://www.youtube.com/watch?v=cIII542y0C8</ref> |
| + | |||
| + | As molten lithium is highly reactive, this process should be performed in installations made of corrosion resistant alloys and under inert atmosphere, such as argon. | ||
==Projects== | ==Projects== | ||
| − | * | + | *Butyllithium synthesis (pyrophoric) |
*Isolation of reactive metals, including lanthanides | *Isolation of reactive metals, including lanthanides | ||
*Lithium lubricating grease | *Lithium lubricating grease | ||
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<references /> | <references /> | ||
===Relevant Sciencemadness threads=== | ===Relevant Sciencemadness threads=== | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=156445 What are some interesting uses for lithium metal] | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=32593 Lithium electride in ethylenediamine] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=32593 Lithium electride in ethylenediamine] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=156454 Making Lithium Powder] | ||
[[Category:Elements]] | [[Category:Elements]] | ||
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[[Category:S-block]] | [[Category:S-block]] | ||
[[Category:DEA SS List]] | [[Category:DEA SS List]] | ||
| + | [[Category:Air-sensitive materials]] | ||
Latest revision as of 18:05, 23 November 2022
 Lithium metal from an Energizer battery | |||||
| General properties | |||||
|---|---|---|---|---|---|
| Name, symbol | Lithium, Li | ||||
| Appearance | White-silvery metal | ||||
| Lithium in the periodic table | |||||
| |||||
| Atomic number | 3 | ||||
| Standard atomic weight (Ar) | 6.94 | ||||
| Group, block | I; s-block | ||||
| Period | period 2 | ||||
| Electron configuration | [He] 2s1 | ||||
per shell | 2, 1 | ||||
| Physical properties | |||||
| Silvery-white | |||||
| Phase | Solid | ||||
| Melting point | 453.65 K (180.5 °C, 356.9 °F) | ||||
| Boiling point | 1603 K (1330 °C, 2426 °F) | ||||
| Density near r.t. | 0.534 g/cm3 | ||||
| when liquid, at | 0.512 g/cm3 | ||||
| Critical point | 3220 K, 67 MPa(extrapolated) | ||||
| Heat of fusion | 3.00 kJ/mol | ||||
| Heat of | 136 kJ/mol | ||||
| Molar heat capacity | 24.86 J/(mol·K) | ||||
| pressure | |||||
| Atomic properties | |||||
| Oxidation states | +1 (a strongly basic oxide) | ||||
| Electronegativity | Pauling scale: 0.98 | ||||
| energies |
1st: 520.2 kJ/mol 2nd: 7298.1 kJ/mol 3rd: 11815 kJ/mol | ||||
| Atomic radius | empirical: 152 pm | ||||
| Covalent radius | 128±7 pm | ||||
| Van der Waals radius | 182 pm | ||||
| Miscellanea | |||||
| Crystal structure | | ||||
| Speed of sound thin rod | 6000 m/s (at 20 °C) | ||||
| Thermal expansion | 46 µm/(m·K) (at 25 °C) | ||||
| Thermal conductivity | 84.8 W/(m·K) | ||||
| Electrical resistivity | 9.28·10-8 Ω·m | ||||
| Magnetic ordering | Paramagnetic | ||||
| Young's modulus | 4.9 GPa | ||||
| Shear modulus | 4.2 GPa | ||||
| Bulk modulus | 11 GPa | ||||
| Mohs hardness | 0.6 | ||||
| Brinell hardness | 5 MPa | ||||
| CAS Registry Number | 7439-93-2 | ||||
| History | |||||
| Discovery | Johan August Arfwedson (1817) | ||||
| First isolation | William Thomas Brande (1821) | ||||
Lithium is a an alkali metal, the lightest metal and least dense solid element at room temperature, with the atomic number 3 and symbol Li. It is soft, silvery-white metal, with a density of 534 kg/m3. It is highly reactive, and it is usually stored in [[[mineral oil]]. However, because of its extremely low density, it floats in mineral oil, storing the metal proves to be difficult.
Contents
Properties
Chemical
Lithium, like all the alkali metals reacts violently with water, releasing hydrogen and can ignite, but this reaction is slightly less violent than the other alkali metals.
- Li + H2O → LiOH + ½ H2
In open air, it quickly forms a layer of oxide as well as nitride, and if the air also contains water vapors and carbon dioxide, lithium hydroxide and lithium carbonate.
- 4 Li + O2 → 2 Li2O
- 6 Li + 2 N2 → 2 Li3N2
Lithium will burn in air, and it tends to burn with a red-crimson flame. As noted by NurdRage in his video where he extracted lithium from an energizer battery, this flame is incredibly bright, so welding goggles should be used if this reaction is attempted. Such fires are difficult to extinguish, requiring dry powder extinguishers (class D).
Lithium is also a strong reducing agent. It is also used in organometallic synthesis in the form of organolithium compounds such as n-butyllithium and tert-butyllithium, although they are extremely rarely used by the amateur chemist, mainly because they're very dangerous (pyrophoric and caustic). Molten lithium is probably the most powerful reducing agent known, and will explode on contact with almost anything non-metallic, including wood, glass and concrete. It is the only alkali metal that cannot be safely melted in a glass container, as it reacts exothermically with glass almost immediately.[1]
Contrary to popular belief, lithium, not cesium, is the most reactive element on the periodic table. It has the lowest reduction potential in aqueous solution, and gram-for-gram (as well as mole-for-mole) has a higher energy content than cesium.
Lithium metal can dissolve in anhydrous ammonia and ethylenediamine, forming its electride salt.
Physical
Lithium is a soft, silver-white metal. It is soft enough to be cut with a knife.
Lithium has the highest specific heat capacity of any solid element, 3.58 kJ/(kg·K), the highest of all solids. Because of this, lithium metal is often used in coolants for heat transfer applications.[2]
Lithium has a density of only 534 kg/m3, making it the lightest metal and solid element at standard conditions. It is lighter than any hydrocarbon oil, which causes the metal to float in the oil is stored. The only organic hydrocarbons lighter than lithium are liquid methane (465 kg/m3), liquid propane (493.5 kg/m3), liquid propylene (514.4 kg/m3).[3] Since these solvents are liquid only at very low temperatures or under high pressure, storing lithium in them is impractical.
In addition, lithium has the highest melting point of all alkali metals, at roughly 180 degrees Celsius. This makes it difficult to melt it under oil (a common tactic for removing tarnish from the other alkali metals). Molten lithium is extremely reactive and will react with almost all ceramic materials, therefore lithium is only melted in crucibles made of special metals, such as molybdenum. It also has a high boiling point, of 1330 °C.
Lithium dissolves in liquid ammonia.[4]
Availability
Lithium can be extracted from lithium batteries, as shown by NurdRage is his video. It comes as a long sheet of lithium metal, that quickly tarnishes in air. It's risky, as the battery can short and overheat. One safer method is to use a pipe cutter and split the battery case in the middle. Larger quantities of lithium can be bought from Galliumsource, though it's pretty expensive (150$/100g). Due to its low molar mass, one may get away with using much smaller amounts of lithium than expected.
In recent years, some jurisdictions in United States limit the sale of lithium batteries, as elemental lithium can be used to reduce pseudoephedrine and ephedrine to the illegal drug methamphetamine.
Preparation
Industrially, elemental lithium is produced electrolytically from a mixture of fused 55% lithium chloride and 45% potassium chloride at about 450 oC.[5]
As molten lithium is highly reactive, this process should be performed in installations made of corrosion resistant alloys and under inert atmosphere, such as argon.
Projects
- Butyllithium synthesis (pyrophoric)
- Isolation of reactive metals, including lanthanides
- Lithium lubricating grease
- Aluminium-lithium alloys
- Cesium synthesis by distillation (DANGER!)
Safety
Handling
Contrary to what one may think, NEVER HANDLE LITHIUM WITH GLOVES OF ANY KIND! You can easily tell if your hands are wet, but not if your gloves are wet, and if you get lithium wet (or it ignites) while handling it with gloves, it will burn through your gloves (and potentially explode) faster than you can remove them.[6] Pliers are another safe option. Glove boxes are also very good for work with lithium.
Toxicity
Breathing lithium dust or lithium compounds irritate the nose and throat, while higher exposure can cause a buildup of fluid in the lungs, leading to pulmonary edema. Acetic acid a good neutralizing agent.
Storage
Like every other alkali metal, it must be kept away from any fire source. Keeping lithium under mineral oil is difficult because lithium floats on mineral oil, though a small rock may be used to keep it down. The best solution is to keep it in an inert argon atmosphere (nitrogen will react to form lithium nitride). Sulfur hexafluoride can also be used, except when it's molten (it will react).
Disposal
Lithium compounds are not particularly dangerous to the environment, but it's recommended to recycle them when possible.
References
- ↑ https://www.youtube.com/watch?v=GE-NkVqUiHs
- ↑ http://hilltop.bradley.edu/~spost/THERMO/solidcp.pdf
- ↑ http://www.engineeringtoolbox.com/liquids-densities-d_743.html
- ↑ http://pubs.acs.org/doi/abs/10.1021/j150343a013
- ↑ https://www.youtube.com/watch?v=cIII542y0C8
- ↑ Thunderf00t knows what he's talking about. https://www.youtube.com/watch?v=Nn3M1hfjxMU
