Final answer:
Oxygen's binding characteristics are most similar to other nonmetallic elements with high electronegativity, such as sulfur and nitrogen, which also form covalent bonds and oxyacids. Elements like phosphorus and sulfur exhibit similar bonding behaviors due to d-orbital interactions.
Step-by-step explanation:
The binding characteristics of oxygen are most similar to other elements that have similar electronegativity and the ability to form covalent bonds. Oxygen has six electrons in its valence shell and forms a stable molecule by sharing two pairs of electrons in a double covalent bond, as seen in oxygen gas (O=O).
Similar behavior is exhibited by other nonmetallic elements like sulfur and nitrogen, which have high electronegativity and the capacity to form multiple covalent bonds. For instance, sulfur and oxygen can form sulfurous or sulfuric acid by sharing two pairs of electrons between them, while nitrogen can create molecules like nitrogen dioxide (NO₂) or nitric acid (HNO₃).
Oxyacids are an example of compounds where oxygen shows its high electronegativity by attracting shared electrons and producing polar bonds. Such characteristics are common with nonmetals that have the ability to create molecules with acidic properties. Therefore, elements like phosphorus or sulfur in period 3, which tend to form strong multiple bonds as a result of d-orbital interactions, exhibit similar bonding characteristics to oxygen.