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Atomic radii l Covalent radii l Vander Waals Radii l Metallic radii l Variation of atomic radius|

In the video, we will be disscussing about Atomic radii, Covalent radii, Vander waals radii, Metallic radii and then we will move on to Variation of atomic radius. Enhance your knowledge: Atomic Radii: Atomic radius refers to the size of an atom, defined as the distance from the center of the nucleus to the outermost shell of electrons. Atomic radii vary for different elements and can change depending on the chemical environment of the atom. There are two main types of atomic radii: The "ionic" radius, which refers to the size of an atom in a positive ion (cation). The "covalent" radius, which refers to the size of an atom in a neutral molecule or a bonded atom. The size of an atom can be influenced by several factors, including electron configuration, electron shielding, and the effective nuclear charge. In general, as one moves down a group (vertical column) in the periodic table, the atomic radius tends to increase due to the increasing number of electron shells. On the other hand, as one moves across a period (horizontal row), the atomic radius tends to decrease due to the increasing effective nuclear charge. Covalent Radii: The covalent radius of an element refers to the size of the atom when it is bonded covalently to another atom. Covalent bonding occurs when atoms share electrons to form a stable bond. The covalent radius is typically half of the distance between the nuclei of two bonded atoms. Covalent radii can vary depending on the element and the specific bond type. For example, the covalent radius of a carbon atom in a single bond is typically smaller than the covalent radius of a carbon atom in a triple bond. The periodic table of elements can be used to approximate the covalent radii of different elements. However, it is important to note that covalent radii are not a fixed property and can vary based on the specific chemical environment and bonding partners of an atom. Vander wall Radii: Van der Waals radius is a measure of the size of an atom or molecule that takes into account the non-bonded interactions between atoms. It is defined as the distance at which the interaction energy between two atoms or molecules is equal to the thermal energy of the system. Van der Waals interactions include forces such as London dispersion forces and dipole-dipole interactions, which occur between neutral atoms and molecules. These forces are much weaker than covalent or ionic bonds, but can still play a role in determining the size and behavior of molecules. Van der Waals radii are used in molecular modeling and computer simulations to help predict and understand molecular behavior, as well as in the design of synthetic materials and drugs. The value of a van der Waals radius can vary depending on the specific atom or molecule, and different sources may provide slightly different values. Metallic Radius: Metallic radius refers to the size of an atom in a metallic compound, where the electrons are not localized to specific atoms but are instead shared by all atoms in the metallic lattice. In metals, the valence electrons are free to move through the lattice, giving rise to the characteristic metallic properties of high electrical and thermal conductivity, malleability, and ductility. The size of a metal atom in a metallic compound is often referred to as the metallic radius and is typically larger than the covalent or ionic radius of the same atom. The metallic radius of an atom can depend on several factors, including crystal structure, coordination number, and the type of metallic bonding present. The metallic radius is an important consideration in materials science, as it can influence the properties and behavior of metallic compounds. Variation in Atomic Radius: The atomic radius varies in a periodic table as you move from left to right across a period (row) due to an increase in the number of protons and electrons, causing the positive pull of the nucleus to increase. This results in the electrons being drawn closer to the nucleus, thus reducing the atomic radius. Down a group (column), the atomic radius generally increases due to an increase in the number of electron shells. This results in the electrons being further away from the nucleus and causing an increase in the atomic radius. 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