Inorganic compounds exhibit a range of bonding properties.  Some are ionic compounds, consisting of very simple cations and anions joined by ionic bonding. Examples of salts (which are ionic compounds) are magnesium chloride MgCl, which consists of magnesium cations Mg and chloride anions Cl; or sodium hydroxide NaOH, which consists of sodium cations Na and hydroxide anions OH.  Some inorganic compounds are highly covalent, such as sulfur dioxide and iron pentacarbonyl.  Many inorganic compounds feature polar covalent bonding, which is a form of bonding intermediate between covalent and ionic bonding.  This description applies to many oxides, carbonates, and halides.  Many inorganic compounds are characterized by high melting points.  Some salts (e.g., NaCl) are very soluble in water.
When one reactant contains hydrogen atoms, a reaction can take place by exchanging protons in acid-base chemistry. In a more general definition, any chemical species capable of binding to electron pairs is called a Lewis acid; conversely any molecule that tends to donate an electron pair is referred to as a Lewis base. As a refinement of acid-base interactions, the HSAB theory takes into account polarizability and size of ions.