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  F Block Elements

Introduction to F-block Elements

The f-block of the elements in the periodic table comprises of those elements whose atoms or ions have valence electrons in f-orbitals. Actual electronic configuration might be somewhat different from what is given by the Aufbau principle. Elements are also called as inner transition elements, though that term is generally taken to contain lutetium and lawrencium also, which are also part of d-block.

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Lanthanide

The lanthanide or lanthanoid (IUPAC nomenclature) series includes the fifteen metallic chemical elements with atomic numbers 57 to 71, from lanthanum till lutetium.

These 15 lanthanide elements, also with the chemically similar elements yttrium and scandium, are often together called as the rare earth elements.

Electron configuration

In quantum chemistry and atomic physics, the electron configuration is allocation of electrons of an atom or molecule (or other physical structure) in molecular or atomic orbitals. For example, the electron configuration of the neon atom founds to be 1s2 2s2 2p6. As per the Quantum's law, an energy is related with each electron configuration and upon particular conditions; the electrons are capable to shift from one orbital to another through emission or absorption of a quantum of energy in the form of photon.

Actinide

The actinide or actinoid (IUPAC nomenclature) series includes the 15 metallic chemical elements with atomic numbers ranging from 89 -103 i.e. actinium through lawrencium.

The actinide series get its name by the group 3 element actinium. All the elements except one of the actinides are f-block elements, corresponding to the filling of 5f electron shell; lawrencium, a d-block element, is generally considered an actinide as well. In comparison to the lanthanide also mostly f-block elements, actinides exhibit additional variable valence.

Electron shell

An electron shell can be thought of as an orbit followed by electrons round an atom's nucleus. Nearest shell to the nucleus is known as the "1 shell" (also known as "K shell"), followed by the "2 shell" (or "L shell"), "3 shell" and so on away from nucleus. The shell letters that are K, L, M, ... so on are alphabetically set.

Every shell can include only fixed number of electrons: The 1st shell can take up to two electrons only, 2nd shell can up to eight electrons, 3rd shell can take up to 18, and the 4th shell can take up to 32 so on and so forth. As the electrons are electrically attracted towards the nucleus, an atom's electrons will generally occupies outer shells only if the more inner shells have already been entirely filled by the electrons. However, this is not a strict requisite: Atoms can have two or even three outer shells that are partially filled with electrons.

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