False. While some redox reactions can result in the formation of ionic bonds, not all of them do.
Here's why:
**Redox reactions:** These involve the transfer of electrons between atoms, changing their oxidation states. This electron transfer can lead to several types of bond formation, not just ionic bonds. Here are some examples:
* **Ionic bond formation:** In some cases, when a metal loses electrons due to oxidation, it becomes a positively charged cation. This cation can then attract nearby non-metal anions with opposite charges, forming an ionic bond. For example, when sodium metal reacts with chlorine gas, sodium ions (Na⁺) and chloride ions (Cl⁻) form, giving sodium chloride (NaCl) - an ionic compound.
* **Covalent bond formation:** When atoms share electrons due to redox reactions, covalent bonds can form. For example, the combustion of hydrogen gas with oxygen gas results in the formation of water (H₂O). In this case, hydrogen atoms share electrons with oxygen atoms, forming covalent bonds and not ionic bonds.
* **Metallic bond formation:** In some redox reactions involving metals, the transferred electrons form a "sea" of delocalized electrons shared by all metal atoms. This "delocalized electron sea" is responsible for the characteristic properties of metals like high electrical conductivity and malleability. This type of bond is called a metallic bond, not an ionic bond.
Therefore, while redox reactions can certainly facilitate ionic bond formation through electron transfer and charge attraction, they are not limited to this outcome. The type of bond formed depends on various factors like the participating atoms, their electronegativities, and the reaction conditions.