Which type of bond is characterized as being shorter and stronger than single bonds?

Double bonds are characterized as being shorter and stronger than single bonds due to the presence of two shared pairs of electrons between two atoms. This increased sharing of electrons not only leads to a stronger attraction between the bonded nuclei and the shared electron pairs but also results in a shorter bond length compared to single bonds, where only one pair of electrons is shared.

When two atoms form a single bond, they share one pair of electrons, which results in a longer bond length and less strength relative to double bonds. With the increase in the number of shared electron pairs, as seen in double bonds, the electrostatic forces pulling the nuclei closer together are stronger, which translates to a shorter bond distance.

While covalent bonds encompass both single and multiple bonds, the specific characteristic of being shorter and stronger applies primarily to double bonds in this context. Triple bonds, while even stronger and shorter than double bonds, are not the focus of the question, which is why double bonds are noted in this scenario. Therefore, double bonds represent a significant increase in bond strength and reduction in bond length compared to single bonds.