inorganic chemistry periodic table related short definitions

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. The first important man-made inorganic compound was ammonium nitrate for soil fertilization through the Haber process. Inorganic compounds are also found multitasking as biomolecules: as electrolytes ( sodium chloride), in energy storage ( ATP) or in construction (the polyphosphate backbone in DNA). Soil may contain iron sulfide as pyrite or calcium sulfate as gypsum. Inorganic compounds are found in nature as minerals. As a refinement of acid-base interactions, the HSAB theory takes into account polarizability and size of ions. 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. When one reactant contains hydrogen atoms, a reaction can take place by exchanging protons in acid-base chemistry. Electron exchange can occur indirectly as well, e.g., in batteries, a key concept in electrochemistry. The net result is an exchange of electrons. In redox reactions one reactant, the oxidant, lowers its oxidation state and another reactant, the reductant, has its oxidation state increased. The simplest inorganic reaction is double displacement when in mixing of two salts the ions are swapped without a change in oxidation state.

Some salts (e.g., NaCl) are very soluble in water, others (e.g., FeS) are not. Many inorganic compounds have high melting point and ease of crystallization. Many inorganic compounds are characterized by high melting points. Important classes of inorganic compounds are the oxides, the carbonates, the sulfates, and the halides. 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. In any salt, the proportions of the ions are such that the electric charges cancel out, so that the bulk compound is electrically neutral. Examples of salts (which are ionic compounds) are magnesium chloride MgCl 2, which consists of magnesium cations Mg 2+ and chloride anions Cl − or sodium oxide Na 2O, which consists of sodium cations Na + and oxide anions O 2−. Many inorganic compounds are ionic compounds, consisting of cations and anions joined by ionic bonding. It has applications in every aspect of the chemical industry, including catalysis, materials science, pigments, surfactants, coatings, medications, fuels, and agriculture. The distinction between the two disciplines is far from absolute, as there is much overlap in the subdiscipline of organometallic chemistry. This field covers chemical compounds that are not carbon-based, which are the subjects of organic chemistry.

Inorganic chemistry deals with synthesis and behavior of inorganic and organometallic compounds. The structure of the ionic framework in potassium oxide, K 2O For the journal, see Inorganic Chemistry (journal).

Inorganic chemistry periodic table related short definitions