Here are the correct chemical formulas for the compounds formed between rubidium (Rb) and each of the polyatomic ions:<\/p>\n\n\n\n
Part A: Carbonate (CO\u2083\u00b2\u207b)<\/strong> Explanation: Part B: Phosphate (PO\u2084\u00b3\u207b)<\/strong> Explanation: Part C: Hydrogen phosphate (HPO\u2084\u00b2\u207b)<\/strong> Explanation: Part D: Acetate (C\u2082H\u2083O\u2082\u207b)<\/strong> Explanation: In all these compounds, the key principle is ensuring that the total positive and negative charges balance out to form a neutral compound. The number of rubidium ions needed depends on the charge of the polyatomic ion involved.<\/p>\n\n\n\n Write a formula for the compound that forms between rubidium and each polyatomic ion: Part A Carbonate. Express your answer as a chemical formula. Part B Phosphate. Express your answer as a chemical formula. Part C Hydrogen phosphate. Express your answer as a chemical formula. Part D Acetate. Express your answer as a chemical formula. […]<\/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-256085","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/256085","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=256085"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/256085\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=256085"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=256085"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=256085"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Rubidium (Rb) has a charge of +1, and the carbonate ion (CO\u2083\u00b2\u207b) has a charge of -2. To balance the charges, two rubidium ions are required for every carbonate ion. Therefore, the chemical formula is:
Rb\u2082CO\u2083<\/strong><\/p>\n\n\n\n
Rubidium is an alkali metal, so it forms a cation (Rb\u207a) with a charge of +1. Carbonate is a polyatomic ion with a charge of -2. To neutralize the charges, two rubidium cations are needed to balance the -2 charge from the carbonate ion. Hence, the formula is Rb\u2082CO\u2083.<\/p>\n\n\n\n
The phosphate ion (PO\u2084\u00b3\u207b) has a charge of -3, and rubidium (Rb) has a charge of +1. To balance the charges, three rubidium ions are required for every phosphate ion. Therefore, the chemical formula is:
Rb\u2083PO\u2084<\/strong><\/p>\n\n\n\n
Rubidium\u2019s +1 charge and phosphate\u2019s -3 charge need to be balanced. Since one Rb\u207a ion cannot balance the -3 charge of phosphate, we need three rubidium ions to neutralize the charge. Hence, the formula is Rb\u2083PO\u2084.<\/p>\n\n\n\n
The hydrogen phosphate ion (HPO\u2084\u00b2\u207b) has a charge of -2, and rubidium (Rb) has a charge of +1. To balance the charges, two rubidium ions are required for every hydrogen phosphate ion. Therefore, the chemical formula is:
Rb\u2082HPO\u2084<\/strong><\/p>\n\n\n\n
The hydrogen phosphate ion has a -2 charge, and rubidium forms +1 cations. To balance the overall charge, two rubidium ions are needed. Therefore, the formula is Rb\u2082HPO\u2084.<\/p>\n\n\n\n
The acetate ion (C\u2082H\u2083O\u2082\u207b) has a charge of -1, and rubidium (Rb) has a charge of +1. Since the charges are equal in magnitude, one rubidium ion will balance the charge of one acetate ion. Therefore, the chemical formula is:
RbC\u2082H\u2083O\u2082<\/strong><\/p>\n\n\n\n
Acetate is a negatively charged ion with a charge of -1, while rubidium forms a cation with a charge of +1. The charges are already balanced, so one rubidium ion combines with one acetate ion to form RbC\u2082H\u2083O\u2082.<\/p>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-564.jpeg\")
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