{"id":234720,"date":"2025-06-14T11:56:04","date_gmt":"2025-06-14T11:56:04","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=234720"},"modified":"2025-06-14T11:56:06","modified_gmt":"2025-06-14T11:56:06","slug":"complete-this-table","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/14\/complete-this-table\/","title":{"rendered":"Complete this table"},"content":{"rendered":"\n

Complete this table. name empirical formula barium iodide rubidium fluoride<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

Of course. Here is the completed table with the correct empirical formulas, followed by a detailed explanation.<\/p>\n\n\n\n

name<\/td>empirical formula<\/td><\/tr>
barium iodide<\/td>BaI\u2082<\/strong><\/td><\/tr>
rubidium fluoride<\/td>RbF<\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

Explanation:<\/strong><\/h3>\n\n\n\n

An empirical formula represents the simplest whole-number ratio of atoms or ions within a chemical compound. For ionic compounds, which are typically formed between a metal and a nonmetal, the chemical formula is the empirical formula. The key to determining this formula is to balance the electrical charges of the ions to form a neutral compound.<\/p>\n\n\n\n

1. Barium Iodide (BaI\u2082)<\/strong><\/p>\n\n\n\n

To find the formula for barium iodide, the constituent ions and their charges must be identified.<\/p>\n\n\n\n

    \n
  • Barium (Ba)<\/strong>\u00a0is an alkaline earth metal, located in Group 2 of the periodic table. Elements in this group consistently lose two valence electrons to form a stable cation with a +2 charge. Thus, the barium ion is\u00a0Ba\u00b2\u207a<\/strong>.<\/li>\n\n\n\n
  • Iodine (I)<\/strong>\u00a0is a halogen, found in Group 17. Halogens tend to gain one electron to achieve a stable electron configuration, forming an anion with a -1 charge. The iodide ion is\u00a0I\u207b<\/strong>.<\/li>\n<\/ul>\n\n\n\n

    For the compound to be neutral, the sum of the positive and negative charges must be zero. One barium ion (Ba\u00b2\u207a) has a charge of +2. To balance this, two iodide ions (I\u207b) are needed, as each has a charge of -1. The calculation is: (1 \u00d7 +2) + (2 \u00d7 -1) = 0.<\/p>\n\n\n\n

    This results in a ratio of one barium ion to two iodide ions. The cation (Ba) is written first, and the number of ions is indicated by a subscript. Therefore, the empirical formula for barium iodide is BaI\u2082<\/strong>.<\/p>\n\n\n\n

    2. Rubidium Fluoride (RbF)<\/strong><\/p>\n\n\n\n

    A similar process is followed for rubidium fluoride.<\/p>\n\n\n\n

      \n
    • Rubidium (Rb)<\/strong>\u00a0is an alkali metal from Group 1. These metals lose one valence electron to form a cation with a +1 charge. The rubidium ion is\u00a0Rb\u207a<\/strong>.<\/li>\n\n\n\n
    • Fluorine (F)<\/strong>\u00a0is the most electronegative halogen in Group 17. It gains one electron, forming the fluoride anion with a -1 charge,\u00a0F\u207b<\/strong>.<\/li>\n<\/ul>\n\n\n\n

      In this case, the +1 charge of the rubidium ion perfectly balances the -1 charge of the fluoride ion. The ratio is one-to-one. The calculation is: (1 \u00d7 +1) + (1 \u00d7 -1) = 0.<\/p>\n\n\n\n

      Because the simplest whole-number ratio is 1:1, only one of each ion is needed for a neutral compound. When the subscript is 1, it is omitted from the formula. The empirical formula for rubidium fluoride is RbF<\/strong>.<\/p>\n\n\n\n

      \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

      Complete this table. name empirical formula barium iodide rubidium fluoride The Correct Answer and Explanation is: Of course. Here is the completed table with the correct empirical formulas, followed by a detailed explanation. name empirical formula barium iodide BaI\u2082 rubidium fluoride RbF Explanation: An empirical formula represents the simplest whole-number ratio of atoms or ions […]<\/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-234720","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234720","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=234720"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234720\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=234720"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=234720"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=234720"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}