Lanthanides || Electronic Configuration, Oxidation State & Lanthanoids Contraction || Chemistry скачать в хорошем качестве

Lanthanides || Electronic Configuration, Oxidation State & Lanthanoids Contraction || Chemistry

#lanthanides #electronicconfiguration #lanthanidescontraction #actinides #inorganicchemistry #chemistry #neet #chemistryclass12 #chemistryconcept #chemistryneet #neetpreparation #neet2024 #neetmotivation #studymotivation #studymaterials #studywithme #mindmentor23 #mindmentor #educationalvideo #contentcreator #exampreparation #viralcontent #viral Lanthanoids (Lanthanides): Lanthanides, also known as lanthanoids or rare earth elements, are a group of 15 chemical elements found in the f-block of the periodic table. These elements have atomic numbers ranging from 57 to 71, specifically from lanthanum (La) to lutetium (Lu). They are often referred to as "rare earth elements" because they were initially isolated from rare minerals, although they are not actually rare in terms of abundance in the Earth's crust. Lanthanides are typically shiny, silver-white, and have high melting points. They are known for their unique properties, including strong magnetism and a tendency to exhibit multiple oxidation states. 1) Electronic Configuration: The electronic configuration of an element describes the distribution of its electrons in various energy levels or atomic orbitals. For lanthanides, the electronic configuration is characterized by the filling of the 4f orbitals. The general form is [Xe] 4f^n 5s^2 5p^6, where 'n' varies from 0 to 14, depending on the specific lanthanide element. The "n" value corresponds to the number of electrons in the 4f orbitals. As you move across the lanthanide series from lanthanum to lutetium, electrons are successively added to the 4f orbitals. This gradual filling of the 4f orbitals is responsible for the similar chemical properties exhibited by the lanthanides. 2) Oxidation States: Lanthanides are known for their ability to exhibit various oxidation states, but the +3 oxidation state is the most common and stable for most of them. The +3 oxidation state results from the loss of three valence electrons, which are typically the two 5s and one 5p electrons. This leaves behind the stable electron configuration of the preceding noble gas (Xenon, Xe). Some lanthanides can also exhibit other oxidation states, such as +2, +4, or +5, depending on the specific element and the chemical conditions. However, the +3 state is the most prevalent and stable. 3) Lanthanide Contraction: Lanthanide contraction is a unique phenomenon observed as you move across the lanthanide series from lanthanum (La) to lutetium (Lu). It is characterized by a steady decrease in the size of the atoms and ions of the lanthanides as the atomic number increases. This is in contrast to the typical increase in atomic size seen in most elements as you move across a period of the periodic table. The lanthanide contraction occurs because the additional electrons added to the 4f orbitals do not effectively shield the increasing nuclear charge from the outer electrons. As a result, there is a greater attraction between the nucleus and the outer electrons, leading to a decrease in atomic and ionic radii. This contraction has significant implications in the chemistry of the lanthanides, affecting their chemical reactivity and properties. In summary, lanthanides are a fascinating group of elements with unique electronic configurations, the ability to exhibit multiple oxidation states, and a distinctive lanthanide contraction phenomenon that sets them apart from other elements on the periodic table. These characteristics make them crucial in various applications, from advanced materials to electronics and environmental science. Thanks for watching. If you like our videos please subscribe to our channel ‪@MindMentor23‬