The formation of a covalent bond always results in a net decrease in potential energy, leading to greater stability compared to isolated atoms.

Overlapping of atomic orbitals leads to increased electron density between the nuclei, contributing to bond formation.

The strength of a covalent bond is inversely proportional to the extent of orbital overlap.

The stability of a covalent bond arises from the balance between attractive forces between nuclei and electrons, and repulsive forces between nuclei and between electrons.

$s$

$p$

$d$

$f$

Photosynthesis

Atomic structure

Chemical bonding

Thermodynamics

Combining capacity of an element

Atomicity of an element

Oxidation number of an element

None of the above

${\rm{C}}{{\rm{l}}_2}{{\rm{O}}_6}$

${\rm{C}}{{\rm{l}}_2}{{\rm{O}}_7}$

${\rm{C}}{{\rm{l}}_2}{\rm{O}}$

${\rm{Cl}}{{\rm{O}}_2}$

They are formed by the sharing of electrons between atoms.

They can occur between two nonmetals.

They can result in polar or nonpolar molecules.

They involve the transfer of electrons to form ions.

Super oxide ion

Oxygen

Carbon molecule

Unipositive ion of ${{\rm{N}}_2}$ molecule

Naphthalene

Diamond

$NaCl$

$Mn$

${\rm{HF}}$

${\rm{N}}{{\rm{F}}_3}$

${\rm{B}}{{\rm{F}}_3}$

${\rm{Cl}}{{\rm{F}}_3}$

Ionic bond

Covalent bond

Coordinate

All of three

Nitrogen has no vacant 2$d$-orbitals

${\rm{NC}}{{\rm{l}}_5}$ is unstable

Nitrogen atom is much smaller than phosphorus

Nitrogen is highly mert