When an atom is surrounded by six substituents, arranged in a manner that four are in one plane, one above and below, and their vertices join to give eight faces (octa-hedrons), such a molecular geometry is octahedral.
Since it looks like two pyramids projecting out from a square base, the geometry is also called square bipyramidal.
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A bond angle is a geometrical angle between two bonds originating from the same atom in a covalently bonded molecule, measured in degrees (o).
In other words, it is the angle between three atoms placed sequentially and held by covalent bonds.
Once the sigma bonds are formed, any additional electrons in the perpendicular unhybridized p-atomic orbitals engage in side-to-side or lateral overlap to form an additional bond known as the pie bond. The symbol π denotes the pie bond, drawn as an additional line over the sigma bond in the molecular structure.
The single covalent bond is referred to as a sigma bond, denoted by the symbol σ.
The sigma bonds are usually mentioned in valence bond theory to visualize the bond formation between atoms to form polyatomic molecules like H2, CH4, etc., by overlapping their atomic orbitals.
Benzynes, also known as Arynes, are highly reactive intermediates formed in organic chemistry aromatic reactions.
Heterolytic cleavage or heterolysis is a chemical reaction in which the bond between two atoms breaks unequally so that the two bond electrons reside with only one atom.
The atom that receives both electrons become an electron-rich negatively charged ion (anion, denoted with a negative sign), and the atom that lost the electrons forms a positively charged ion (cation, denoted with a positive sign).
Homolytic cleavage, or homolysis, is a chemical reaction in which a covalent bond between two atoms is broken equally, and each atom retains one of the two electrons that form the bond. This creates two species (similar or dissimilar), each with an unpaired electron, known as the radicals. The radical electron is denoted with a dot (.) over the atoms’ symbol.
London Dispersion, a type of Vander Waal Force, is the weakest of the three types, yet, it is the only one universally present in all the atoms and molecules.
In most cases, it is present in addition to the other forces; however, it is exclusively observed in nonpolar atoms and molecules devoid of any functional groups and, therefore, possess no other overpowering interactions. Examples are He, CH4, I2, C(CH3)4, etc.
Vander Waals is an attractive universal force that operates when the atoms and molecules are within a distance range of 0.4- 0.6 nm.
The attractive force closely gathers the atoms and molecules, so their collective strength can affect the state and other physical properties like melting and boiling points, viscosity, etc.
A permanent dipole is an inherent feature of the molecule due to the nature of the participating atoms forming the two-electron covalent bond.
Some atoms withdraw more of the bond electrons towards themselves, increasing their electron density and leaving the other end electron deficient. This unequal electron charge distribution creates positive and negative poles (denoted with δ+, δ- signs), causing the molecule to have permanent poles or a dipole.