Lewis Dot Structures and Explanations<\/strong> Structure<\/strong>: Dot Structure Representation<\/strong>:<\/p>\n\n\n\n Each sulfur atom (S) has 6 valence electrons and gains 2 electrons to complete its octet (now having 8 electrons, shown as dots). Each iron atom loses 3 electrons (thus shown as Fe\u00b3\u207a), and three sulfur atoms balance the charge from two Fe\u00b3\u207a ions. The total charge remains neutral.<\/p>\n\n\n\n Structure<\/strong>: Dot Structure Representation<\/strong>:<\/p>\n\n\n\n Hydrogen atoms are represented with two electrons, forming a complete shell (1s\u00b2). This is an ionic compound<\/strong>, and the Ca\u00b2\u207a cation is electrostatically attracted to two H\u207b anions.<\/p>\n\n\n\n Structure<\/strong>: Dot Structure Representation<\/strong>:<\/p>\n\n\n\n Each fluorine ion has a full octet (8 valence electrons including the gained one), and aluminum is left as a 3+ ion. This results in a stable ionic structure.<\/p>\n\n\n\n Lewis dot structures are simplified diagrams that represent valence electrons around atoms. These are essential tools in visualizing the bonding in molecules and ionic compounds. In ionic compounds like Fe\u2082S\u2083, CaH\u2082, and AlF\u2083, atoms achieve full outer shells by transferring electrons rather than sharing them.<\/p>\n\n\n\n In Fe\u2082S\u2083<\/strong>, iron is a transition metal with a variable oxidation state. In this compound, it forms Fe\u00b3\u207a ions, meaning each iron atom loses three electrons. Sulfur, a nonmetal, gains electrons to become S\u00b2\u207b. Since the total positive charge from two Fe\u00b3\u207a ions is +6, three S\u00b2\u207b ions are needed to balance the charges, making the compound electrically neutral.<\/p>\n\n\n\n Calcium hydride (CaH\u2082)<\/strong> demonstrates a classic metal-to-nonmetal ionic bond. Calcium loses two electrons (forming Ca\u00b2\u207a), while each hydrogen atom gains one electron (forming two H\u207b hydride ions). The resulting structure shows strong electrostatic attraction between the Ca\u00b2\u207a and two H\u207b ions.<\/p>\n\n\n\n In aluminum fluoride (AlF\u2083)<\/strong>, aluminum donates its three valence electrons to three fluorine atoms, each of which needs one more electron to complete an octet. This forms Al\u00b3\u207a and three F\u207b ions. The ionic bonds result from electrostatic forces between oppositely charged ions.<\/p>\n\n\n\n Although Lewis structures are more detailed for covalent compounds, they still help illustrate the transfer of electrons in ionic compounds. The dot representations highlight which atoms lose or gain electrons and help us understand charge balance and the resulting stability of compounds.<\/p>\n\n\n\n Draw Lewis dot structures for the following chemical formulas. 1) Fe2S3 2) CaH2 3) AlF3 The Correct Answer and Explanation is: Lewis Dot Structures and ExplanationsLet us consider each compound and draw the correct Lewis dot structure based on their ionic nature and electron arrangements. 1) Fe\u2082S\u2083 (Iron(III) sulfide) Structure:Fe (Iron) is a transition metal […]<\/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-233427","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233427","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=233427"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233427\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=233427"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=233427"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=233427"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Let us consider each compound and draw the correct Lewis dot structure based on their ionic nature and electron arrangements.<\/p>\n\n\n\n
\n\n\n\n1) Fe\u2082S\u2083 (Iron(III) sulfide)<\/strong><\/h3>\n\n\n\n
Fe (Iron) is a transition metal and does not follow the typical octet rule in Lewis structures. However, in Fe\u2082S\u2083, each Fe loses 3 electrons to form Fe\u00b3\u207a, and each S gains 2 electrons to become S\u00b2\u207b.<\/p>\n\n\n\ncssCopyEdit
Fe\u00b3\u207a Fe\u00b3\u207a [ :S: ]\u00b2\u207b [ :S: ]\u00b2\u207b [ :S: ]\u00b2\u207b \n .. .. ..\n<\/code><\/pre>\n\n\n\n
\n\n\n\n2) CaH\u2082 (Calcium hydride)<\/strong><\/h3>\n\n\n\n
Calcium (Ca) is an alkaline earth metal and has two valence electrons. It donates both electrons, forming Ca\u00b2\u207a. Each hydrogen gains one electron to become H\u207b (hydride ion).<\/p>\n\n\n\ncssCopyEdit
Ca\u00b2\u207a [ H: ]\u207b [ :H ]\u207b\n<\/code><\/pre>\n\n\n\n
\n\n\n\n3) AlF\u2083 (Aluminum fluoride)<\/strong><\/h3>\n\n\n\n
Aluminum (Al) has three valence electrons and donates one to each fluorine (F) atom to form Al\u00b3\u207a. Each fluorine atom has 7 valence electrons and gains 1 electron to complete the octet, forming F\u207b.<\/p>\n\n\n\ncssCopyEdit
Al\u00b3\u207a [ :F: ]\u207b [ :F: ]\u207b [ :F: ]\u207b\n .. .. .. .. .. ..\n<\/code><\/pre>\n\n\n\n
\n\n\n\nExplanation (300 words)<\/strong><\/h3>\n\n\n\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-236.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"