Final answer:
A double bond has a larger electron density than a single bond and it attracts single bonds more. The space occupied by electrons in bonds follows the order: lone pair > triple bond > double bond > single bond. Double bonds are also stronger and shorter than single bonds.
Step-by-step explanation:
A double bond has a larger electron density than a single bond, and attracts single bonds more than they attract each other. Electron density in a polar bond is distributed unevenly and is greater around the atom that attracts the electrons more significantly. For example, a carbon-to-oxygen double bond is more polar and has a greater electron density compared to a carbon-to-oxygen single bond.
The general order of sizes from largest to smallest is: lone pair > triple bond > double bond > single bond. This order reflects the amount of space occupied by different regions of electrons, with multiple bonds occupying more space around the central atom than single bonds. Furthermore, the strength of a bond between two atoms increases as the number of electron pairs in the bond increases, with double bonds being stronger and shorter than single bonds.