|Group||Lanthanides||Melting point||822°C, 1512°F, 1095 K|
|Period||6||Boiling point||1529°C, 2784°F, 1802 K|
|Block||f||Density (g cm−3)||5.24|
|Atomic number||63||Relative atomic mass||151.964|
|State at 20°C||Solid||Key isotopes||153Eu|
|Electron configuration||[Xe] 4f76s2||CAS number||7440-53-1|
|ChemSpider ID||22417||ChemSpider is a free chemical structure database|
- Europium is not found freely in nature. Most of the minerals comprise of europium with the vital sources being monazite and bastnasite.
- It is a soft white-silvery metal. The enrichment or depletion of europium in minerals related to other rare earth elements is termed as europium anomaly.
- It is used as control rods in nuclear reactors due to its effectiveness in absorbing neutrons.
- Europium oxide has its application as phosphor activator.
- Europium-doped plastics are used as laser materials and for making thin superconducting alloys.
- It is used in the euro currency as an anti-forgery measure.
- Europium is a member of the lanthanides group of elements. It is the most active element among the lanthanides.
- It reacts very quickly with water and gives off hydrogen. It reacts strongly with oxygen in the air and spontaneously catches fire.
- There are two stable isotopes of Europium that exist in nature, europium-151 and europium-153.
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