Editing Covalent bond (section)

==Types of covalent bonds==
[[Atomic orbitals]] (except for s orbitals) have specific directional properties leading to different types of covalent bonds. [[Sigma bond|Sigma (σ) bond]]s are the strongest covalent bonds and are due to head-on overlapping of orbitals on two different atoms. A [[single bond]] is usually a σ bond. [[Pi bond|Pi (π) bonds]] are weaker and are due to lateral overlap between p (or d) orbitals. A [[double bond]] between two given atoms consists of one σ and one π bond, and a [[triple bond]] is one σ and two π bonds.<ref name=":0" />

Covalent bonds are also affected by the [[electronegativity]] of the connected atoms which determines the [[chemical polarity]] of the bond. Two atoms with equal electronegativity will make nonpolar covalent bonds such as H–H. An unequal relationship creates a polar covalent bond such as with H−Cl. However polarity also requires [[Geometry|geometric]] [[asymmetry]], or else [[dipole]]s may cancel out, resulting in a non-polar molecule.<ref name=":0" />