Covalent Bond

Imagine a single atom responsible for every organic and a few inorganic elements you see on Earth! Diamonds, methane, and even the molecules in your body.

When atoms engage to form molecules, they do so by the overlap of atomic orbitals, creating a bigger molecular orbital that now encompasses more than one atom of a molecule. 

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 (oct

A bond angle is a geometrical angle between two bonds originating from the same central atom in a covalently bonded molecule, measured in degrees (^o).
 

Once the sigma bonds are formed, any additional electrons in the perpendicular unhybridized p-atomic orbitals engage in side-to-sid

The single covalent bond is referred to as a sigma bond, denoted by the symbol σ.

Heterolytic cleavage or heterolysis is a chemical reaction in which the bond between two atoms breaks unequally so that the two bond electrons reside wit

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 t

In molecules consisting of more than two atoms, the least electronegative atom (except Hydrogen) is the central atom.

In a regular trigonal planar molecular geometry, a central atom is surrounded by three equally spaced substituents in one plane, so joining the three cor

In a regular tetrahedral molecular geometry, a central atom is surrounded by four substituents that occupy the four corners of a tetrahedron.

When two atoms come closer by attraction and overcome their repulsive interactions until they find a balance, at which point, the atoms contribute one valence ele

A sp³ hybridized carbon is a tetravalent carbon that forms four single covalent bonds with itself or atoms of other p-block elements to its ri

If you look at the shape of s and p orbitals before hybridization, you will notice that - 

• The s orbital is spherical.

The very premise of a covalent bond is electron sharing.

In his landmark paper, 'The Atom and the Molecule,' G.N. Lewis attempted to describe linkages between the atoms to understand the nature of covalent bonds.

Dalton, in 1804, in his work on ‘Atomic Theory,’ proposed the law of chemical combination to explain how atoms form compounds.

The three common hybridization states are - sp³, sp², and sp.

The arrangement of groups around a central atom creates its three-

The molecule H₂N-NH₂, also known as hydrazine, each Nitrogen atom has 3 bond pairs (two N-H and one N-N bonds) and one lone pair.

If only valence shells participate in bonding reactions, then Carbon should only form two bonds using its two unpaired electrons. However, Carbon forms four bonds, as seen in CH4, CH3X, H2C=O, and O=C=O molecules. This discrepancy between the number of valence electrons of an atom and the number of bonds it forms (valency) is explained by the hybridization concept, an extension of the Valence Bond (VB) Theory.

The bond angle is the angle at which two adjacent bonds converge and meet at the central ato

Bond lengths are smaller when atoms form multiple bonds. Single overlap between two atoms forms a single covalent bond.

An easy way to identify organic compounds is to look for several atoms in a long chain. These long chains are covalent bonds.

Did you know that, back in the 1900s, it was believed that a hook and a loop type of closure was the covalent bond responsible for holding atoms in a molecule?

If a two-electron covalent bond breaks symmetrically, each of the two atoms receive one electron; it is a homolytic bond cleavage.

Pre-Requisite Reading: Electronegativity

A covalent bond holding two atoms is made of two electrons.