Nature of chemical bonds for oxygen in its compounds

Molecules Arrays of atoms connected by covalent bonds 

The bonding for oxygen atoms in heteratomic molecules is viewed as essentially covalent [e.g., MeOH, Me2C=O, MeCH(O), and MeC(O)OOH] and similar to that for carbon, nitrogen, and chlorine atoms. In contrast, a Lewis acid-base formalism often is used for metal-oxygen compounds with ionic interactions by dianionic oxo groups (e.g., [Ba +O -], [Fe (O2-)4]2-, [Mn2+(O2-)4], and [(Cu+)2O2-]). This results from the thermodynamic relations for ionic solution equilibria, and the inference to some that the combination of ions results in molecules and complexes held together by electrostatic interactions, for example. 

the bonding in metal compounds and complexes has traditionally been viewed as ionic (positive metal center interacting with negative ions HO, O2-, Cl , AcO ) and coordinate donor [Lewis acid-base interactions positive metal center interacting with negative ions and electron-pair Lewis bases ( NH3, PPh3, HOH)]. Examples of ionic versus covalent bonding illustrate the tradition H+Cl-versus H-Cl (ls-3p), C4+(C1-)4 versus C(-C1)4 [Tsp -lSpU], Fe3+(C1 )3 versus Fe(-Cl)3 [3d sp -(3p)3 ], H+ OH versus H-OH (ls-2p), C4+(O2-)2 versus O=C=O 

---

Nature of Chemical Bonds for Oxygen in its Compounds Table 3-4 Examples of Oxygen Covalent Bonding with Nonmetals... 

---