In what type of bond do atoms share electrons to achieve stable electronic configurations?

In a covalent bond, atoms share pairs of electrons, allowing them to achieve stable electronic configurations similar to those of the noble gases. This electron sharing facilitates a greater stability for the atoms involved, as they can fill their outermost electron shells through this interaction.

For instance, in a molecule like water (H₂O), each hydrogen atom shares one of its electrons with the oxygen atom, enabling all involved atoms to attain a full outer shell of electrons. This sharing of electrons is critical because it not only leads to stable molecules but also contributes to the diverse range of chemical properties observed in covalent compounds.

In contrast, other types of bonds behave differently with respect to electron interactions. Hydrogen bonds are weak attractions between polar molecules, ionic bonds involve the transfer of electrons leading to charged ions that attract each other, and dative bonds (or coordinate covalent bonds) involve one atom providing both electrons for the bond, rather than sharing equally as seen in covalent bonding.