Ionic bonds are indeed real bonds, but they differ from covalent bonds in their nature. Ionic bonding occurs when there is a complete transfer of electrons from one atom to another, resulting in the formation of positively charged ions (cations) and negatively charged ions (anions). These oppositely charged ions are held together by electrostatic forces, creating an ionic bond.
The reason some might argue that ionic bonds are not "real" bonds is because they lack the characteristic sharing of electrons seen in covalent bonds. In covalent bonds, atoms share electron pairs, creating a more equal distribution of charge. In contrast, ionic bonds involve a transfer of electrons, resulting in a strong electrostatic attraction between ions but not the direct sharing of electrons.
However, it is important to note that ionic bonds are very real and play a significant role in the formation of many compounds and structures, such as ionic solids and salts. Ionic compounds have distinct properties, such as high melting and boiling points, crystalline structures, and the ability to conduct electricity when dissolved in water or molten state. These characteristics are a result of the strong attractions between ions within the ionic lattice.