{"id":2067,"date":"2024-03-04T17:28:41","date_gmt":"2024-03-04T17:28:41","guid":{"rendered":"https:\/\/cake.appscodestudio.com\/?p=2067"},"modified":"2024-03-04T17:28:42","modified_gmt":"2024-03-04T17:28:42","slug":"binary-compounds","status":"publish","type":"post","link":"https:\/\/cake.appscodestudio.com\/index.php\/2024\/03\/04\/binary-compounds\/","title":{"rendered":"Binary compounds"},"content":{"rendered":"\n

Binary ionic compounds<\/h2>\n\n\n\n

The nomenclature for\u00a0binary\u00a0ionic compounds simply entails naming the ions according to the following rules:<\/p>\n\n\n\n

    \n
  1. The\u00a0positive ion\u00a0(called a cation) is named first and the\u00a0negative ion\u00a0(anion) second.<\/li>\n\n\n\n
  2. A simple cation (obtained from a single atom) takes its name from its parent element. For example, Li+<\/sup> is called lithium in the names of compounds containing this ion. Similarly, Na+<\/sup> is called sodium, Mg2+<\/sup> is called magnesium, and so on.<\/li>\n\n\n\n
  3. A simple anion (obtained from a single atom) is named by taking the root of the parent element\u2019s name and adding the suffix\u00a0-ide<\/em>. Thus, the F\u2212<\/sup>\u00a0ion is called fluoride, Br\u2212<\/sup>\u00a0is called bromide, S2\u2212<\/sup>\u00a0is called\u00a0sulfide, and so on.<\/li>\n<\/ol>\n\n\n\n

    The following examples illustrate the nomenclature rules for binary ionic compounds:<\/p>\n\n\n\n

    sodium chloride(opens in a new tab)<\/p>\n\n\n\n

    compound<\/th>ions present<\/th>name<\/th><\/tr><\/thead>
    NaCl<\/td>Na+<\/sup>, Cl\u2212<\/sup><\/td>sodium chloride<\/td><\/tr>
    KI<\/td>K+<\/sup>, I\u2212<\/sup><\/td>potassium iodide<\/td><\/tr>
    CaS<\/td>Ca2+<\/sup>, S2\u2212<\/sup><\/td>calcium sulfide<\/td><\/tr>
    CsBr<\/td>Cs+<\/sup>, Br\u2212<\/sup><\/td>cesium bromide<\/td><\/tr>
    MgO<\/td>Mg2\u2212<\/sup>, O2\u2212<\/sup><\/td>magnesium\u00a0oxide<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

    In the formulas of ionic compounds, simple ions are represented by the\u00a0chemical symbol\u00a0for the element: Cl means Cl\u2212<\/sup>, Na means Na+<\/sup>, and so on. When individual ions are shown, however, the charge is always included. Thus, the formula of potassium bromide is given as KBr, but, when the potassium and bromide ions are shown individually, they are written K+<\/sup>\u00a0and Br\u2212<\/sup>.<\/p>\n\n\n\n

    When a given metal atom can form more than one type of cation, the charge on the particular cation present must be specified in the name of the compound. For example, lead (Pb) can exist as Pb2+<\/sup>\u00a0or Pb4+<\/sup>\u00a0ions in ionic compounds. Also, iron (Fe) can form Fe2+<\/sup>\u00a0or Fe3+<\/sup>\u00a0ions, tin (Sn) can form Sn2+<\/sup>\u00a0or Sn4+<\/sup>\u00a0ions, gold (Au) can form Au+<\/sup>\u00a0or Au3+<\/sup>\u00a0ions, and so on. Therefore, the names of binary compounds containing metals such as these must include a\u00a0Roman numeral\u00a0to specify the charge on the ion. For example, the compound FeCl3<\/sub>, which contains Fe3+<\/sup>, is named iron(III) chloride. On the other hand, the compound FeCl2<\/sub>, which contains Fe2+<\/sup>, is designated as iron(II) chloride. In each case, the Roman numeral in the name specifies the charge of the metal ion present.<\/p>\n\n\n\n

    Common simple cations and anions<\/th><\/tr><\/thead>
    cation<\/th>name<\/th>anion<\/th>name<\/th><\/tr>
    H+<\/sup><\/th>hydrogen<\/td>H\u2212<\/sup><\/td>hydride<\/td><\/tr>
    Li+<\/sup><\/th>lithium<\/td>F\u2212<\/sup><\/td>fluoride<\/td><\/tr>
    Na+<\/sup><\/th>sodium<\/td>Cl\u2212<\/sup><\/td>chloride<\/td><\/tr>
    K+<\/sup><\/th>potassium<\/td>Br\u2212<\/sup><\/td>bromide<\/td><\/tr>
    Cs+<\/sup><\/th>cesium<\/td>I\u2212<\/sup><\/td>iodide<\/td><\/tr>
    Be2+<\/sup><\/th>beryllium<\/td>O2\u2212<\/sup><\/td>oxide<\/td><\/tr>
    Mg2+<\/sup><\/th>magnesium<\/td>S2\u2212<\/sup><\/td>sulfide<\/td><\/tr>
    Ca2+<\/sup><\/th>calcium<\/td><\/td><\/td><\/tr>
    Ba2+<\/sup><\/th>barium<\/td><\/td><\/td><\/tr>
    Al3+<\/sup><\/th>aluminum<\/td><\/td><\/td><\/tr>
    Ag+<\/sup><\/th>silver<\/td><\/td><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

    An\u00a0alternative\u00a0system for naming compounds containing metals that form only two ions is sometimes seen, especially in older literature. The ion with the higher charge has a name ending in\u00a0-ic<\/em>, and the one with the lower charge has the suffix\u00a0-ous<\/em>. For example, Fe3+<\/sup>\u00a0is called the ferric ion, and Fe2+<\/sup>\u00a0is called the ferrous ion. The names for FeCl3<\/sub>\u00a0and FeCl2<\/sub>\u00a0are then ferric chloride and ferrous chloride, respectively.<\/p>\n\n\n\n

    Common ions that form multiple cations<\/th><\/tr><\/thead>
    ion<\/th>systematic name<\/th>alternate name<\/th><\/tr>
    Fe3+<\/sup><\/th>iron(III)<\/td>ferric<\/td><\/tr>
    Fe2+<\/sup><\/th>iron(II)<\/td>ferrous<\/td><\/tr>
    Cu2+<\/sup><\/th>copper(II)<\/td>cupric<\/td><\/tr>
    Cu+<\/sup><\/th>copper(I)<\/td>cuprous<\/td><\/tr>
    Co3+<\/sup><\/th>cobalt(III)<\/td>cobaltic<\/td><\/tr>
    Co2+<\/sup><\/th>cobalt(II)<\/td>cobaltous<\/td><\/tr>
    Sn4+<\/sup><\/th>tin(IV)<\/td>stannic<\/td><\/tr>
    Sn2+<\/sup><\/th>tin(II)<\/td>stannous<\/td><\/tr>
    Pb4+<\/sup><\/th>lead(IV)<\/td>plumbic<\/td><\/tr>
    Pb2+<\/sup><\/th>lead(II)<\/td>plumbous<\/td><\/tr>
    Hg2+<\/sup><\/th>mercury(II)<\/td>mercuric<\/td><\/tr>
    Hg2<\/sub>2+<\/sup>(*)<\/th>mercury(I)<\/td>mercurous<\/td><\/tr><\/tbody>
    *Mercury(I) ions always occur bound together to form Hg2<\/sub>2+<\/sup>.<\/td><\/tr><\/tfoot><\/table><\/figure>\n","protected":false},"excerpt":{"rendered":"

    Binary ionic compounds The nomenclature for\u00a0binary\u00a0ionic compounds simply entails naming the ions according to the following rules: The following examples illustrate the nomenclature rules for binary ionic compounds: sodium chloride(opens in a new tab) compound ions present name NaCl Na+, Cl\u2212 sodium chloride KI K+, I\u2212 potassium iodide CaS Ca2+, S2\u2212 calcium sulfide CsBr Cs+, […]<\/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-2067","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\/2067","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=2067"}],"version-history":[{"count":1,"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/posts\/2067\/revisions"}],"predecessor-version":[{"id":2068,"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/posts\/2067\/revisions\/2068"}],"wp:attachment":[{"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/media?parent=2067"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/categories?post=2067"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/cake.appscodestudio.com\/index.php\/wp-json\/wp\/v2\/tags?post=2067"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}