<P> Ionic bonding is a kind of chemical bonding that arises from the mutual attraction of oppositely charged ions . Ions of like charge repel each other, and ions of opposite charge attract each other . Therefore, ions do not usually exist on their own, but will bind with ions of opposite charge to form a crystal lattice . The resulting compound is called an ionic compound, and is said to be held together by ionic bonding . In ionic compounds there arise characteristic distances between ion neighbours from which the spatial extension and the ionic radius of individual ions may be derived . </P> <P> The most common type of ionic bonding is seen in compounds of metals and nonmetals (except noble gases, which rarely form chemical compounds). Metals are characterized by having a small number of electrons in excess of a stable, closed - shell electronic configuration . As such, they have the tendency to lose these extra electrons in order to attain a stable configuration . This property is known as electropositivity . Non-metals, on the other hand, are characterized by having an electron configuration just a few electrons short of a stable configuration . As such, they have the tendency to gain more electrons in order to achieve a stable configuration . This tendency is known as electronegativity . When a highly electropositive metal is combined with a highly electronegative nonmetal, the extra electrons from the metal atoms are transferred to the electron - deficient nonmetal atoms . This reaction produces metal cations and nonmetal anions, which are attracted to each other to form a salt . </P> <Table> <Tr> <Td> <Table> Common cations <Tr> <Th> Common name </Th> <Th> Formula </Th> <Th> Historic name </Th> </Tr> <Tr> <Th_colspan="3"> Simple cations </Th> </Tr> <Tr> <Td> Aluminium </Td> <Td> Al </Td> <Td> </Td> </Tr> <Tr> <Td> Barium </Td> <Td> Ba </Td> <Td> </Td> </Tr> <Tr> <Td> Beryllium </Td> <Td> Be </Td> <Td> </Td> </Tr> <Tr> <Td> Calcium </Td> <Td> Ca </Td> <Td> </Td> </Tr> <Tr> <Td> Chromium (III) </Td> <Td> Cr </Td> <Td> </Td> </Tr> <Tr> <Td> Copper (I) </Td> <Td> Cu </Td> <Td> cuprous </Td> </Tr> <Tr> <Td> Copper (II) </Td> <Td> Cu </Td> <Td> cupric </Td> </Tr> <Tr> <Td> Hydrogen </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Td> Iron (II) </Td> <Td> Fe </Td> <Td> ferrous </Td> </Tr> <Tr> <Td> Iron (III) </Td> <Td> Fe </Td> <Td> ferric </Td> </Tr> <Tr> <Td> Lead (II) </Td> <Td> Pb </Td> <Td> plumbous </Td> </Tr> <Tr> <Td> Lead (IV) </Td> <Td> Pb </Td> <Td> plumbic </Td> </Tr> <Tr> <Td> Lithium </Td> <Td> Li </Td> <Td> </Td> </Tr> <Tr> <Td> Magnesium </Td> <Td> Mg </Td> <Td> </Td> </Tr> <Tr> <Td> Manganese (II) </Td> <Td> Mn </Td> <Td> </Td> </Tr> <Tr> <Td> Mercury (II) </Td> <Td> Hg </Td> <Td> mercuric </Td> </Tr> <Tr> <Td> Potassium </Td> <Td> </Td> <Td> kalic </Td> </Tr> <Tr> <Td> Silver </Td> <Td> Ag </Td> <Td> argentous </Td> </Tr> <Tr> <Td> Sodium </Td> <Td> Na </Td> <Td> natric </Td> </Tr> <Tr> <Td> Strontium </Td> <Td> Sr </Td> <Td> </Td> </Tr> <Tr> <Td> Tin (II) </Td> <Td> Sn </Td> <Td> stannous </Td> </Tr> <Tr> <Td> Tin (IV) </Td> <Td> Sn </Td> <Td> stannic </Td> </Tr> <Tr> <Td> Zinc </Td> <Td> Zn </Td> <Td> </Td> </Tr> <Tr> <Th_colspan="3"> Polyatomic cations </Th> </Tr> <Tr> <Td> Ammonium </Td> <Td> NH + </Td> <Td> </Td> </Tr> <Tr> <Td> Hydronium </Td> <Td> H O </Td> <Td> </Td> </Tr> <Tr> <Td> Mercury (I) </Td> <Td> Hg 2 + </Td> <Td> mercurous </Td> </Tr> </Table> </Td> <Td> <Table> Common anions <Tr> <Th> Formal name </Th> <Th> Formula </Th> <Th> Alt . name </Th> </Tr> <Tr> <Th_colspan="3"> Simple anions </Th> </Tr> <Tr> <Td> Azide </Td> <Td> N − </Td> <Td> </Td> </Tr> <Tr> <Td> Bromide </Td> <Td> Br </Td> <Td> </Td> </Tr> <Tr> <Td> Chloride </Td> <Td> Cl </Td> <Td> </Td> </Tr> <Tr> <Td> Fluoride </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Td> Hydride </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Td> Iodide </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Td> Nitride </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Td> Oxide </Td> <Td> O </Td> <Td> </Td> </Tr> <Tr> <Td> Sulfide </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Th_colspan="3"> Oxoanions </Th> </Tr> <Tr> <Td> Carbonate </Td> <Td> CO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Chlorate </Td> <Td> ClO − </Td> <Td> </Td> </Tr> <Tr> <Td> Chromate </Td> <Td> CrO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Dichromate </Td> <Td> Cr 2O2 − 7 </Td> <Td> </Td> </Tr> <Tr> <Td> Dihydrogen phosphate </Td> <Td> 2PO − </Td> <Td> </Td> </Tr> <Tr> <Td> Hydrogen carbonate </Td> <Td> HCO − </Td> <Td> bicarbonate </Td> </Tr> <Tr> <Td> Hydrogen sulfate </Td> <Td> HSO − </Td> <Td> bisulfate </Td> </Tr> <Tr> <Td> Hydrogen sulfite </Td> <Td> HSO − </Td> <Td> bisulfite </Td> </Tr> <Tr> <Td> Hydroxide </Td> <Td> OH </Td> <Td> </Td> </Tr> <Tr> <Td> Hypochlorite </Td> <Td> ClO </Td> <Td> </Td> </Tr> <Tr> <Td> Monohydrogen phosphate </Td> <Td> HPO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Nitrate </Td> <Td> NO − </Td> <Td> </Td> </Tr> <Tr> <Td> Nitrite </Td> <Td> NO − </Td> <Td> </Td> </Tr> <Tr> <Td> Perchlorate </Td> <Td> ClO − </Td> <Td> </Td> </Tr> <Tr> <Td> Permanganate </Td> <Td> MnO − </Td> <Td> </Td> </Tr> <Tr> <Td> Peroxide </Td> <Td> O2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Phosphate </Td> <Td> PO 3 − </Td> <Td> </Td> </Tr> <Tr> <Td> Sulfate </Td> <Td> SO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Sulfite </Td> <Td> SO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Superoxide </Td> <Td> O − </Td> <Td> </Td> </Tr> <Tr> <Td> Thiosulfate </Td> <Td> 2O2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Silicate </Td> <Td> SiO 4 − </Td> <Td> </Td> </Tr> <Tr> <Td> Metasilicate </Td> <Td> SiO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Aluminium silicate </Td> <Td> AlSiO − </Td> <Td> </Td> </Tr> <Tr> <Th_colspan="3"> Anions from organic acids </Th> </Tr> <Tr> <Td> Acetate </Td> <Td> CH 3COO − </Td> <Td> ethanoate </Td> </Tr> <Tr> <Td> Formate </Td> <Td> HCOO − </Td> <Td> methanoate </Td> </Tr> <Tr> <Td> Oxalate </Td> <Td> 2O2 − </Td> <Td> ethanedioate </Td> </Tr> <Tr> <Td> Cyanide </Td> <Td> CN </Td> <Td> </Td> </Tr> </Table> </Td> </Tr> </Table> <Tr> <Td> <Table> Common cations <Tr> <Th> Common name </Th> <Th> Formula </Th> <Th> Historic name </Th> </Tr> <Tr> <Th_colspan="3"> Simple cations </Th> </Tr> <Tr> <Td> Aluminium </Td> <Td> Al </Td> <Td> </Td> </Tr> <Tr> <Td> Barium </Td> <Td> Ba </Td> <Td> </Td> </Tr> <Tr> <Td> Beryllium </Td> <Td> Be </Td> <Td> </Td> </Tr> <Tr> <Td> Calcium </Td> <Td> Ca </Td> <Td> </Td> </Tr> <Tr> <Td> Chromium (III) </Td> <Td> Cr </Td> <Td> </Td> </Tr> <Tr> <Td> Copper (I) </Td> <Td> Cu </Td> <Td> cuprous </Td> </Tr> <Tr> <Td> Copper (II) </Td> <Td> Cu </Td> <Td> cupric </Td> </Tr> <Tr> <Td> Hydrogen </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Td> Iron (II) </Td> <Td> Fe </Td> <Td> ferrous </Td> </Tr> <Tr> <Td> Iron (III) </Td> <Td> Fe </Td> <Td> ferric </Td> </Tr> <Tr> <Td> Lead (II) </Td> <Td> Pb </Td> <Td> plumbous </Td> </Tr> <Tr> <Td> Lead (IV) </Td> <Td> Pb </Td> <Td> plumbic </Td> </Tr> <Tr> <Td> Lithium </Td> <Td> Li </Td> <Td> </Td> </Tr> <Tr> <Td> Magnesium </Td> <Td> Mg </Td> <Td> </Td> </Tr> <Tr> <Td> Manganese (II) </Td> <Td> Mn </Td> <Td> </Td> </Tr> <Tr> <Td> Mercury (II) </Td> <Td> Hg </Td> <Td> mercuric </Td> </Tr> <Tr> <Td> Potassium </Td> <Td> </Td> <Td> kalic </Td> </Tr> <Tr> <Td> Silver </Td> <Td> Ag </Td> <Td> argentous </Td> </Tr> <Tr> <Td> Sodium </Td> <Td> Na </Td> <Td> natric </Td> </Tr> <Tr> <Td> Strontium </Td> <Td> Sr </Td> <Td> </Td> </Tr> <Tr> <Td> Tin (II) </Td> <Td> Sn </Td> <Td> stannous </Td> </Tr> <Tr> <Td> Tin (IV) </Td> <Td> Sn </Td> <Td> stannic </Td> </Tr> <Tr> <Td> Zinc </Td> <Td> Zn </Td> <Td> </Td> </Tr> <Tr> <Th_colspan="3"> Polyatomic cations </Th> </Tr> <Tr> <Td> Ammonium </Td> <Td> NH + </Td> <Td> </Td> </Tr> <Tr> <Td> Hydronium </Td> <Td> H O </Td> <Td> </Td> </Tr> <Tr> <Td> Mercury (I) </Td> <Td> Hg 2 + </Td> <Td> mercurous </Td> </Tr> </Table> </Td> <Td> <Table> Common anions <Tr> <Th> Formal name </Th> <Th> Formula </Th> <Th> Alt . name </Th> </Tr> <Tr> <Th_colspan="3"> Simple anions </Th> </Tr> <Tr> <Td> Azide </Td> <Td> N − </Td> <Td> </Td> </Tr> <Tr> <Td> Bromide </Td> <Td> Br </Td> <Td> </Td> </Tr> <Tr> <Td> Chloride </Td> <Td> Cl </Td> <Td> </Td> </Tr> <Tr> <Td> Fluoride </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Td> Hydride </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Td> Iodide </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Td> Nitride </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Td> Oxide </Td> <Td> O </Td> <Td> </Td> </Tr> <Tr> <Td> Sulfide </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Th_colspan="3"> Oxoanions </Th> </Tr> <Tr> <Td> Carbonate </Td> <Td> CO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Chlorate </Td> <Td> ClO − </Td> <Td> </Td> </Tr> <Tr> <Td> Chromate </Td> <Td> CrO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Dichromate </Td> <Td> Cr 2O2 − 7 </Td> <Td> </Td> </Tr> <Tr> <Td> Dihydrogen phosphate </Td> <Td> 2PO − </Td> <Td> </Td> </Tr> <Tr> <Td> Hydrogen carbonate </Td> <Td> HCO − </Td> <Td> bicarbonate </Td> </Tr> <Tr> <Td> Hydrogen sulfate </Td> <Td> HSO − </Td> <Td> bisulfate </Td> </Tr> <Tr> <Td> Hydrogen sulfite </Td> <Td> HSO − </Td> <Td> bisulfite </Td> </Tr> <Tr> <Td> Hydroxide </Td> <Td> OH </Td> <Td> </Td> </Tr> <Tr> <Td> Hypochlorite </Td> <Td> ClO </Td> <Td> </Td> </Tr> <Tr> <Td> Monohydrogen phosphate </Td> <Td> HPO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Nitrate </Td> <Td> NO − </Td> <Td> </Td> </Tr> <Tr> <Td> Nitrite </Td> <Td> NO − </Td> <Td> </Td> </Tr> <Tr> <Td> Perchlorate </Td> <Td> ClO − </Td> <Td> </Td> </Tr> <Tr> <Td> Permanganate </Td> <Td> MnO − </Td> <Td> </Td> </Tr> <Tr> <Td> Peroxide </Td> <Td> O2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Phosphate </Td> <Td> PO 3 − </Td> <Td> </Td> </Tr> <Tr> <Td> Sulfate </Td> <Td> SO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Sulfite </Td> <Td> SO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Superoxide </Td> <Td> O − </Td> <Td> </Td> </Tr> <Tr> <Td> Thiosulfate </Td> <Td> 2O2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Silicate </Td> <Td> SiO 4 − </Td> <Td> </Td> </Tr> <Tr> <Td> Metasilicate </Td> <Td> SiO 2 − </Td> <Td> </Td> </Tr> <Tr> <Td> Aluminium silicate </Td> <Td> AlSiO − </Td> <Td> </Td> </Tr> <Tr> <Th_colspan="3"> Anions from organic acids </Th> </Tr> <Tr> <Td> Acetate </Td> <Td> CH 3COO − </Td> <Td> ethanoate </Td> </Tr> <Tr> <Td> Formate </Td> <Td> HCOO − </Td> <Td> methanoate </Td> </Tr> <Tr> <Td> Oxalate </Td> <Td> 2O2 − </Td> <Td> ethanedioate </Td> </Tr> <Tr> <Td> Cyanide </Td> <Td> CN </Td> <Td> </Td> </Tr> </Table> </Td> </Tr>

Some nonmetal atoms do not release energy when forming a 1- anion