page_title: Inorganic chemistry
section_title: Key concepts
hierarchical_section_title: Inorganic chemistry / Key concepts
context_page_description: Inorganic chemistry deals with synthesis and behavior of inorganic and organometallic compounds. This field covers all chemical compounds except the myriad of organic compounds, which are the subjects of organic chemistry. The distinction between the two disciplines is far from absolute, as there is much overlap in the subdiscipline of organometallic chemistry. It has applications in every aspect of the chemical industry, including catalysis, materials science, pigments, surfactants, coatings, medications, fuels, and agriculture.
context_section_description: Many inorganic compounds are ionic compounds, consisting of cations and anions joined by ionic bonding.  Examples of salts (which are ionic compounds) are magnesium chloride MgCl₂, which consists of magnesium cations Mg²⁺ and chloride anions Cl⁻; or sodium oxide Na₂O, which consists of sodium cations Na⁺ and oxide anions O²⁻.  In any salt, the proportions of the ions are such that the electric charges cancel out, so that the bulk compound is electrically neutral. The ions are described by their oxidation state and their ease of formation can be inferred from the ionization potential (for cations) or from the electron affinity (anions) of the parent elements.
  Important classes of inorganic compounds are the oxides, the carbonates, the sulfates, and the halides.  Many inorganic compounds are characterized by high melting points.  Inorganic salts typically are poor conductors in the solid state.  Other important features include their high melting point and ease of crystallization.  Where some salts (e.g., NaCl) are very soluble in water, others (e.g., FeS) are not.
  The simplest inorganic reaction is double displacement when in mixing of two salts the ions are swapped without a change in oxidation state. In redox reactions one reactant, the oxidant, lowers its oxidation state and another reactant, the reductant, has its oxidation state increased. The net result is an exchange of electrons. Electron exchange can occur indirectly as well, e.g., in batteries, a key concept in electrochemistry.
  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.
  Inorganic compounds are found in nature as minerals. Soil may contain iron sulfide as pyrite or calcium sulfate as gypsum. Inorganic compounds are also found multitasking as biomolecules: as electrolytes (sodium chloride), in energy storage (ATP) or in construction (the polyphosphate backbone in DNA).
  The first important man-made inorganic compound was ammonium nitrate for soil fertilization through the Haber process. Inorganic compounds are synthesized for use as catalysts such as vanadium(V) oxide and titanium(III) chloride, or as reagents in organic chemistry such as lithium aluminium hydride.
  Subdivisions of inorganic chemistry are organometallic chemistry, cluster chemistry and bioinorganic chemistry. These fields are active areas of research in inorganic chemistry, aimed toward new catalysts, superconductors, and therapies.
caption: The structure of the ionic framework in potassium oxide, K2O
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