Difference between revisions of "Yttrium"
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'''Yttrium''' is a transition metal with the symbol Y and the atomic number 39. It is chemically similar to the lanthanides, and is often grouped with them, as well as [[scandium]], as a rare earth metal. Yttrium is a powerful reducing agent, but is not a necessary addition to the amateur chemistry lab when cheaper agents, such as magnesium, are readily available. | '''Yttrium''' is a transition metal with the symbol Y and the atomic number 39. It is chemically similar to the lanthanides, and is often grouped with them, as well as [[scandium]], as a rare earth metal. Yttrium is a powerful reducing agent, but is not a necessary addition to the amateur chemistry lab when cheaper agents, such as magnesium, are readily available. | ||
| − | |||
| − | === Physical | + | ==Properties== |
| + | ===Physical=== | ||
Yttrium is a silvery metal that is not very dense (comparable to [[titanium]]). It tends to form crystals which are hexagonally close-packed. | Yttrium is a silvery metal that is not very dense (comparable to [[titanium]]). It tends to form crystals which are hexagonally close-packed. | ||
| − | ===Chemical | + | |
| + | ===Chemical=== | ||
Yttrium is a typical rare-earth metal, with similar chemistry to [[aluminium]]. It does not corrode in air, yet it has the highest thermodynamic affinity for oxygen of any element. Finely divided yttrium is prone to ignition. In solution, yttrium compounds do not exhibit any color due to the lack of free d or f electrons. Its standard reduction potential is almost exactly the same as that of [[magnesium]]. It reacts with [[Acid|acids]] to form salts, most of which are soluble except for [[yttrium fluoride]] and [[yttrium oxalate]]. [[Yttrium sulfate]] is only slightly soluble. The metal reacts with the halogens to produce trihalides. | Yttrium is a typical rare-earth metal, with similar chemistry to [[aluminium]]. It does not corrode in air, yet it has the highest thermodynamic affinity for oxygen of any element. Finely divided yttrium is prone to ignition. In solution, yttrium compounds do not exhibit any color due to the lack of free d or f electrons. Its standard reduction potential is almost exactly the same as that of [[magnesium]]. It reacts with [[Acid|acids]] to form salts, most of which are soluble except for [[yttrium fluoride]] and [[yttrium oxalate]]. [[Yttrium sulfate]] is only slightly soluble. The metal reacts with the halogens to produce trihalides. | ||
Its primary oxidation state is +3. Yttrium(II) compounds exist, but are not accessible to the amateur. | Its primary oxidation state is +3. Yttrium(II) compounds exist, but are not accessible to the amateur. | ||
| + | |||
==Availability== | ==Availability== | ||
| − | Yttrium is more common than tin on Earth, but it is very hard to find and expensive (though relatively cheap for a rare-earth element). One source for yttrium, as well as other rare earth metals, is [http://www.elementsales.com/pl_element.htm#yy Metallium]. It is sold in 5 gram and 50 gram sizes, as well as rods, ampoules, 100 gram ingots, and coins. Yttrium and its compounds occasionally sold on eBay as well. | + | Yttrium is more common than [[tin]] on Earth, but it is very hard to find and expensive (though relatively cheap for a rare-earth element). One source for yttrium, as well as other rare earth metals, is [http://www.elementsales.com/pl_element.htm#yy Metallium]. It is sold in 5 gram and 50 gram sizes, as well as rods, ampoules, 100 gram ingots, and coins. Yttrium and its compounds occasionally sold on eBay as well. |
| + | |||
==Projects== | ==Projects== | ||
*Yttrium thermite? | *Yttrium thermite? | ||
*Alloys with [[aluminium]]? | *Alloys with [[aluminium]]? | ||
| − | ==Safety== | + | ==Handling== |
| − | + | ===Safety=== | |
| − | + | ====Toxicity==== | |
Toxicity data of yttrium compounds is scarce, but they appear to be of low to moderate danger. Yttrium plays no biological role, but acts similarly to calcium within the body. Some yttrium compounds, notably the halides, will hydrolyze when heated and will give off acidic vapors. | Toxicity data of yttrium compounds is scarce, but they appear to be of low to moderate danger. Yttrium plays no biological role, but acts similarly to calcium within the body. Some yttrium compounds, notably the halides, will hydrolyze when heated and will give off acidic vapors. | ||
| − | ===Flammability=== | + | |
| + | ====Flammability==== | ||
Small pieces of yttrium metal or powder are flammable. Class D fire extinguishers should be readily available when working with yttrium near an open flame. Water should never be used to extinguish burning yttrium, as it will aggravate the flame. | Small pieces of yttrium metal or powder are flammable. Class D fire extinguishers should be readily available when working with yttrium near an open flame. Water should never be used to extinguish burning yttrium, as it will aggravate the flame. | ||
| + | ===Storage=== | ||
| + | Yttrium should be stored away from any corrosive reagents and flame source. | ||
| + | |||
| + | ===Disposal=== | ||
| + | Due to its rarity and price, it's best to try to recycle it. | ||
| + | |||
| + | ==References== | ||
| + | <references/> | ||
| + | ===Relevant Sciencemadness threads=== | ||
[[Category:Elements]] | [[Category:Elements]] | ||
[[Category:Metals]] | [[Category:Metals]] | ||
| + | [[Category:Transition metals]] | ||
| + | [[Category:Rare earth metals]] | ||
| + | [[Category:D-block]] | ||
| + | [[Category:Materials that react with water]] | ||
| + | [[Category:Materials unstable in acidic solution]] | ||
Revision as of 20:42, 24 August 2015
Yttrium is a transition metal with the symbol Y and the atomic number 39. It is chemically similar to the lanthanides, and is often grouped with them, as well as scandium, as a rare earth metal. Yttrium is a powerful reducing agent, but is not a necessary addition to the amateur chemistry lab when cheaper agents, such as magnesium, are readily available.
Contents
Properties
Physical
Yttrium is a silvery metal that is not very dense (comparable to titanium). It tends to form crystals which are hexagonally close-packed.
Chemical
Yttrium is a typical rare-earth metal, with similar chemistry to aluminium. It does not corrode in air, yet it has the highest thermodynamic affinity for oxygen of any element. Finely divided yttrium is prone to ignition. In solution, yttrium compounds do not exhibit any color due to the lack of free d or f electrons. Its standard reduction potential is almost exactly the same as that of magnesium. It reacts with acids to form salts, most of which are soluble except for yttrium fluoride and yttrium oxalate. Yttrium sulfate is only slightly soluble. The metal reacts with the halogens to produce trihalides.
Its primary oxidation state is +3. Yttrium(II) compounds exist, but are not accessible to the amateur.
Availability
Yttrium is more common than tin on Earth, but it is very hard to find and expensive (though relatively cheap for a rare-earth element). One source for yttrium, as well as other rare earth metals, is Metallium. It is sold in 5 gram and 50 gram sizes, as well as rods, ampoules, 100 gram ingots, and coins. Yttrium and its compounds occasionally sold on eBay as well.
Projects
- Yttrium thermite?
- Alloys with aluminium?
Handling
Safety
Toxicity
Toxicity data of yttrium compounds is scarce, but they appear to be of low to moderate danger. Yttrium plays no biological role, but acts similarly to calcium within the body. Some yttrium compounds, notably the halides, will hydrolyze when heated and will give off acidic vapors.
Flammability
Small pieces of yttrium metal or powder are flammable. Class D fire extinguishers should be readily available when working with yttrium near an open flame. Water should never be used to extinguish burning yttrium, as it will aggravate the flame.
Storage
Yttrium should be stored away from any corrosive reagents and flame source.
Disposal
Due to its rarity and price, it's best to try to recycle it.
