Which bond is typically associated with metals losing electrons to form positive ions?

The bond typically associated with metals losing electrons to form positive ions is the ionic bond. Ionic bonds are formed when one atom donates an electron to another atom, resulting in the creation of positive and negative ions. In metallic elements, this often involves the metal atoms losing one or more electrons, thus becoming positively charged ions (cations).

As a result, these cations can attract negatively charged ions (anions), usually nonmetals, which accept the electrons. This transfer of electrons leads to a strong electrostatic force of attraction between the oppositely charged ions, which is characteristic of ionic compounds.

In contrast, the other types of bonds listed—hydrogen bonds, polar covalent bonds, and covalent bonds—do not involve the complete transfer of electrons from one atom to another and therefore do not lead to the formation of positive metal ions. Hydrogen bonds are weak attractions typically between molecules, polar covalent bonds involve unequal sharing of electrons, and covalent bonds feature equal sharing of electrons, usually forming molecular compounds rather than ionic compounds.