A special type of\u00a0ionic compound\u00a0is exemplified by\u00a0ammonium nitrate\u00a0(NH4<\/sub>NO3<\/sub>), which contains two polyatomic ions, NH4<\/sub>+<\/sup>\u00a0and NO3<\/sub>\u2212<\/sup>. As the name suggests, a polyatomic ion is a charged entity composed of several atoms bound together. Polyatomic ions have special names that are used in the nomenclature of the compounds containing them.<\/p>\n\n\n\n Several series of polyatomic anions exist that contain an atom of a given element in combination with different numbers of oxygen atoms. Such anions are called oxy anions. When the series contains only two members, the name of the ion with fewer oxygen atoms ends in\u00a0-ite<\/em>, and the name of the other ion ends in\u00a0-ate<\/em>. For example, SO3<\/sub>2\u2212<\/sup>\u00a0is called sulfite and SO4<\/sub>2\u2212<\/sup>\u00a0is called\u00a0sulfate. In those cases where more than two oxy anions\u00a0constitute\u00a0the series,\u00a0hypo-<\/em>\u00a0(less than) and\u00a0per-<\/em>\u00a0(more than) are used as prefixes to name the members of the series with the smallest and the largest number of oxygen atoms, respectively. The chlorine-containing oxy anions provide an example:<\/p>\n\n\n\n Naming ionic compounds that contain polyatomic ions is similar to naming binary ionic compounds. For example, the compound NaOH is called\u00a0sodium hydroxide, because it contains the Na+<\/sup>\u00a0(sodium) cation and the OH\u2212<\/sup>\u00a0(hydroxide) anion. As in binary ionic compounds, when a\u00a0metal\u00a0that can form multiple cations is present, a Roman numeral is required to specify the charge on the cation. For example, the compound FeSO4<\/sub>\u00a0is called iron(II) sulfate, because it contains Fe2+<\/sup>.<\/p>\n","protected":false},"excerpt":{"rendered":" Ionic compounds containing polyatomic ions A special type of\u00a0ionic compound\u00a0is exemplified by\u00a0ammonium nitrate\u00a0(NH4NO3), which contains two polyatomic ions, NH4+\u00a0and NO3\u2212. As the name suggests, a polyatomic ion is a charged entity composed of several atoms bound together. Polyatomic ions have special names that are used in the nomenclature of the compounds containing them. Common polyatomic […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[11],"tags":[],"class_list":["post-2071","post","type-post","status-publish","format-standard","hentry","category-inorganic-compounds"],"Cooking_time":"","jetpack_featured_media_url":"","_links":{"self":[{"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/posts\/2071","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/comments?post=2071"}],"version-history":[{"count":1,"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/posts\/2071\/revisions"}],"predecessor-version":[{"id":2072,"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/posts\/2071\/revisions\/2072"}],"wp:attachment":[{"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/media?parent=2071"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/categories?post=2071"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/tags?post=2071"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Common polyatomic ions<\/th><\/tr><\/thead> ion<\/th> name<\/th> <\/th> ion<\/th> name<\/th><\/tr> NH4<\/sub>+<\/sup><\/th> ammonium<\/td> <\/td> CO3<\/sub>2\u2212<\/sup><\/td> carbonate<\/td><\/tr> NO2<\/sub>\u2212<\/sup><\/th> nitrite<\/td> <\/td> HCO3<\/sub>\u2212<\/sup><\/td> hydrogen carbonate**<\/td><\/tr> NO3<\/sub>\u2212<\/sup><\/th> nitrate<\/td> <\/td> ClO\u2212<\/sup><\/td> hypochlorite<\/td><\/tr> SO3<\/sub>2\u2212<\/sup><\/th> sulfite<\/td> <\/td> ClO2<\/sub>\u2212<\/sup><\/td> chlorite<\/td><\/tr> SO4<\/sub>2\u2212<\/sup><\/th> sulfate<\/td> <\/td> ClO3<\/sub>\u2212<\/sup><\/td> chlorate<\/td><\/tr> HSO4<\/sub>\u2212<\/sup><\/th> hydrogen sulfate*<\/td> <\/td> ClO4<\/sub>\u2212<\/sup><\/td> perchlorate<\/td><\/tr> OH\u2212<\/sup><\/th> hydroxide<\/td> <\/td> C2<\/sub>H3<\/sub>O2<\/sub>\u2212<\/sup><\/td> acetate<\/td><\/tr> CN\u2212<\/sup><\/th> cyanide<\/td> <\/td> MnO4<\/sub>\u2212<\/sup><\/td> permanganate<\/td><\/tr> PO4<\/sub>3\u2212<\/sup><\/th> phosphate<\/td> <\/td> Cr2<\/sub>O7<\/sub>2\u2212<\/sup><\/td> dichromate<\/td><\/tr> HPO4<\/sub>2\u2212<\/sup><\/th> hydrogen phosphate<\/td> <\/td> CrO4<\/sub>2\u2212<\/sup><\/td> chromate<\/td><\/tr> H2<\/sub>PO4<\/sub>\u2212<\/sup><\/th> dihydrogen phosphate<\/td> <\/td> O2<\/sub>2\u2212<\/sup><\/td> peroxide<\/td><\/tr><\/tbody> *Bisulfate and **bicarbonate are widely used common names for hydrogen sulfate
and hydrogen carbonate, respectively.<\/td><\/tr><\/tfoot><\/table><\/figure>\n\n\n\nClO\u2212<\/sup><\/td> hypochlorite<\/td><\/tr> ClO2<\/sub>\u2212<\/sup><\/td> chlorite<\/td><\/tr> ClO3<\/sub>\u2212<\/sup><\/td> chlorate<\/td><\/tr> ClO4<\/sub>\u2212<\/sup><\/td> perchlorate<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n