Chemical Bonding and Molecular Structure

The Square Planar molecular geometry tells us about the stereochemistry of various molecular compounds. When there are four bonds and two lone pairs on the molecule’s central atom, this shape is Square Planar. Xenon tetrafluoride (XeF4) is a molecular compound with a square planar structure. The XeF4 molecule comprises six equally spaced sp3d2 (or d2sp3) […]

The Hybridisation of p orbitals is an important factor in understanding molecular structures and properties. Hybridisation involves electrons in the s and p orbitals interacting chemically to form bonding and nonbonding electron pairs. These orbital arrangements are further classified as sp, sp3, and sp2 Hybridisation. Hybridisation is the overlap of atomic orbitals around a nucleus

The hybridisation of orbitals was first introduced to explain the phenomenon of molecular structure. Before hybridisation, molecular structures were explained using the valence bond theory until they could not predict them correctly. The valence bond theory explained that the local bonds formed between two atoms due to losing electrons from each atom. The VSEPR theory

Solvate isomerism, also known as hydrate isomerism, refers to isomers that have the same composition but differ in whether a solvent molecule is directly linked to the metal ion or is only present on free solvent molecules in the crystal. This is a slightly unique case of the above ligand exchange using neutral solvate molecules.

A chemical bond is generally an attraction between different atoms, molecules or ions which helps in formation of the different types of chemical compound that enables the formation of chemical compounds.in oppositely charged ions, there is an electrostatic force of attraction existing between the two which might result into formation of various bonds. Or maybe

Introduction to Sigma and Pi bonds The Sigma and Pi bonds are distinguished by the overlapping of atomic orbitals. This overlapping ultimately forms the covalent bonds. The sigma bonds are formed by the head-to-head overlapping of the atomic orbitals, whereas; the pi bonds are formed by the lateral overlap of two atomic orbitals.  Both Sigma

Introduction Molecules have different forms. From their physical features to their chemical reactivity, there is a wealth of scientific evidence to support this claim. Small molecules, defined as those with a single core atom, have predictable structures. Valence shell electron pair repulsion is a fundamental concept in molecular structures (VSEPR). According to VSEPR, electron pairs

Molecules have different forms. From their physical features to their chemical reactivity, there is a wealth of scientific evidence to support this claim. Small molecules, defined as those with a single core atom, have predictable structures. Valence shell electron pair repulsion is a fundamental concept in molecular structures (VSEPR). According to VSEPR, electron pairs repel

Resonance effect is the polarity formed in a molecule as a result of contact between a lone pair of electrons and a pi bond, or the interaction of two pi bonds between two nearby atoms. In molecules with conjugated double bonds or at least one lone pair of electrons and one double bond, the effect

We describe the connection between each atom as a chemical bond when atoms are compatible with each other, They combine to form a molecule. The atoms in the molecule, ion, or crystal are held together by the bond. The bonds can often last endlessly until they are broken apart by external pressure or strength. Chemical