{"id":261508,"date":"2025-07-20T06:45:51","date_gmt":"2025-07-20T06:45:51","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=261508"},"modified":"2025-07-20T06:45:53","modified_gmt":"2025-07-20T06:45:53","slug":"predict-the-formula-of-the-ionic-compound-formed-from-the-reaction-of-rubidium-and-oxygen-atoms","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/20\/predict-the-formula-of-the-ionic-compound-formed-from-the-reaction-of-rubidium-and-oxygen-atoms\/","title":{"rendered":"Predict the formula of the ionic compound formed from the reaction of rubidium and oxygen atoms"},"content":{"rendered":"\n<pre id=\"preorder-ask-header-text\" class=\"wp-block-preformatted\">Predict the formula of the ionic compound formed from the reaction of rubidium and oxygen atoms.<\/pre>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>When rubidium (Rb) reacts with oxygen (O), an ionic compound is formed. Rubidium is an alkali metal found in Group 1 of the periodic table. Alkali metals like rubidium have one electron in their outermost shell, which they tend to lose easily to achieve a stable electron configuration. In contrast, oxygen is a nonmetal located in Group 16 of the periodic table and has six electrons in its outer shell. To achieve a full octet (eight electrons), oxygen atoms need two additional electrons.<\/p>\n\n\n\n<p>During the reaction, rubidium atoms lose one electron each to form Rb+\\text{Rb}^+ ions. Oxygen, needing two electrons, gains two electrons to form an O2\u2212\\text{O}^{2-} ion. The resulting ionic compound is formed by the electrostatic attraction between the positively charged rubidium ions and the negatively charged oxide ions.<\/p>\n\n\n\n<p>To balance the charges, two rubidium ions are required for each oxide ion. This is because the Rb+\\text{Rb}^+ ion has a charge of +1, while the O2\u2212\\text{O}^{2-} ion has a charge of -2. Therefore, two Rb+\\text{Rb}^+ ions will balance out the -2 charge of one O2\u2212\\text{O}^{2-} ion, leading to the empirical formula Rb2O\\text{Rb}_2\\text{O}.<\/p>\n\n\n\n<p>In summary, the formula of the ionic compound formed from the reaction of rubidium and oxygen is Rb2O\\text{Rb}_2\\text{O}. This compound is known as rubidium oxide. The reaction involves the transfer of electrons from rubidium to oxygen, resulting in the formation of Rb+\\text{Rb}^+ and O2\u2212\\text{O}^{2-} ions that combine in a 2:1 ratio to form the ionic compound.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Predict the formula of the ionic compound formed from the reaction of rubidium and oxygen atoms. The correct answer and explanation is: When rubidium (Rb) reacts with oxygen (O), an ionic compound is formed. Rubidium is an alkali metal found in Group 1 of the periodic table. Alkali metals like rubidium have one electron in [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-261508","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261508","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=261508"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261508\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=261508"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=261508"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=261508"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}