Einzelbindungen

Einzelbindungen, or single bonds, represent the most fundamental type of covalent chemical bond. A single bond occurs when two atoms share one pair of electrons, typically forming a sigma bond. This sigma bond is characterized by the direct, head-on overlap of atomic orbitals, such as s-s, s-p, or p-p orbitals, resulting in electron density concentrated along the internuclear axis.

These bonds are generally the longest and weakest type of covalent bond when comparing single, double, and triple bonds between the same two elements. For instance, the carbon-carbon single bond in an alkane is longer and requires less energy to break than the double bond in an alkene. Despite being weaker, single bonds allow for rotation around the bond axis, which is a crucial property for the three-dimensional shapes and flexibility of molecules like long-chain hydrocarbons.

The concept is most commonly illustrated using the alkane series of hydrocarbons, where carbon atoms are connected exclusively by single bonds, as in methane (CH4) or ethane (C2H6). In structural formulas, single bonds are denoted by a single line connecting the atomic symbols, for example, H-H or H3C-CH3. The study of single bonds is essential for understanding molecular structure, stability, and reactivity in organic and inorganic chemistry.