What is Lutetium?
All the elements discovered so far are arranged in the Modern periodic table according to their atomic number (Z). The element with atomic number 71 is known as Lutetium. Its symbol is Lu. It belongs to the Lanthanide series of the f-block of the periodic table which consists of elements from atomic number 57 to 71. The electronic configuration of lutetium is 4f145d16s2 . It is not found in a pure state in nature but is obtained from its chloride through a reduction process by alkaline metals. Lutetium 177 is a radioactive isotope of Lutetium. Lutetium is a rare earth metal.
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Chemical Properties of Lutetium
The general chemical properties of Lanthanides are as follows-
The earlier members are quite reactive but with increasing, atomic number elements become less reactive.
Lanthanides react with hydrogen when slightly heated.
Carbides are formed when metals are heated with carbon.
They release hydrogen gas in reaction with acids.
They react with halogens to form halides. Lutetium forms trihalides.
They react with oxygen to give oxides. Lutetium can burn up to 150-degree Celcius to yield its oxide.
The oxidation states of Lu are +2 and +3.
Their hydroxides are alkaline just like alkaline earth metals.
Physical Properties of Lutetium
The general physical properties of Lanthanide elements are -
Lanthanides are silvery-white soft metals. Lutetium is also shiny white but is a solid and a hard metal.
The hardness of the metals in the lanthanide series increases with an increase in atomic number thus Lutetium is a very hard metal.
The melting point and boiling point of lanthanides are generally very high. Lutetium also has a very high melting point. Its reaction with oxygen takes place at a very high temperature.
The density of Lutetium is also very high and thus it is a dense metal. The density of lanthanoids changes smoothly except for Yb and Eu.
Colour is shown by many lanthanide ions. The colour is due to the unpaired electrons in their f orbitals. However, Lu+3 does not show any colour.
Paramagnetism is observed in lanthanide ions. However, Lu+3 does not show paramagnetism as it has 14 electrons in its f orbital (f14).
Lutetium has a very low value of third ionization enthalpy. It's due to the stability of empty/half-filled orbitals.
The atomic mass of Lutetium is 175.
Lutetium is a stable metal.
Lutetium is also malleable and ductile.
Certain Facts About Lutetium
Lutetium was discovered by George Ubain in 1907.
Lutetium is a toxic metal.
It explodes on heating so special care is taken when Lutetium is heated to carry out any reaction.
It causes various skin disorders if come in contact with the skin.
Lutetium 177 is radioactive and has a half-life of 6.7 days. It emits beta rays.
Lutetium was the earlier name of Lutetium. Its name was derived from the old name of Paris(France) which is Lutetia.
The atoms of Lu are the smallest of all the Lanthanides.
A major use of lanthanide elements is to produce alloy steels which are used for plates and pipe making.
Mischmetal is a well-known alloy of lanthanoid metal with iron. The major portion in the alloy is lanthanoid metal and the rest is iron (5%), traces of aluminium, calcium, carbon, etc.
FAQs on Lutetium
1. What is Lutetium and where is it located in the Periodic Table?
Lutetium is a chemical element with the atomic number 71 and the symbol Lu. It is a hard, dense, silvery-white metal. In the Periodic Table, Lutetium is the final element of the lanthanide series and is therefore classified as an f-block element. It is placed in period 6 and group 3 of the table.
2. What is the electronic configuration of Lutetium?
The electronic configuration of Lutetium (Lu) helps explain its chemical properties. As per the Aufbau principle, its configuration is [Xe] 4f¹⁴ 5d¹ 6s². This shows a completely filled 4f orbital, which is a key characteristic that places it at the end of the lanthanide series.
3. What are the common oxidation states of Lutetium and which is more stable?
Lutetium primarily exhibits a +3 oxidation state. While a +2 state can exist, the +3 state is significantly more stable. This is because losing the two 6s electrons and the single 5d electron results in a stable, completely filled 4f orbital (4f¹⁴), which is an energetically favourable configuration.
4. What are some important real-world applications of Lutetium?
Despite being rare and expensive, Lutetium has several specialised applications. Its main uses include:
- Catalysts: It is used as a catalyst in various chemical processes such as hydrogenation, polymerisation, and in petroleum cracking industries.
- Medical Isotopes: The radioactive isotope Lutetium-177 is used in nuclear medicine for targeted radiotherapy to treat certain types of cancers, like neuroendocrine tumours.
- Electronics: Lutetium compounds are used in detectors in positron emission tomography (PET) scans and as phosphors in LED light bulbs.
5. How does lanthanoid contraction influence the properties of Lutetium?
Lanthanoid contraction is the steady decrease in atomic and ionic radii across the lanthanide series. As Lutetium is the last element in this series, it experiences the maximum effect of this contraction. This makes Lutetium atoms the smallest among all lanthanides. Consequently, it has the highest density and is one of the hardest metals in the series.
6. Why is the Lutetium ion (Lu³⁺) colourless and diamagnetic?
The colour and magnetic properties of lanthanoid ions depend on the presence of unpaired electrons in their f-orbitals. The Lutetium ion (Lu³⁺) has an electronic configuration of [Xe] 4f¹⁴. Since its 4f orbital is completely filled, there are no unpaired electrons. The absence of unpaired electrons means it cannot absorb light for f-f electronic transitions, making it colourless. It also causes the ion to be repelled by magnetic fields, making it diamagnetic.
7. Is Lutetium considered a toxic or hazardous element?
Yes, Lutetium is considered a toxic metal and requires careful handling. It is known to be a skin and eye irritant. Furthermore, as a fine powder, it poses a fire and explosion hazard, especially when heated. Its radioactive isotope, Lutetium-177, while medically useful, also presents radiation hazards that must be managed with appropriate safety protocols.
