Formation of Ionic Compounds and Their Lewis Structures: MgCl\u2082, Na\u2082O, MgO<\/strong><\/p>\n\n\n\n Ionic compounds are formed through the transfer of electrons between metals and nonmetals. Metals, which have few valence electrons, tend to lose electrons and form positively charged ions called cations<\/em>. Nonmetals, with more valence electrons and a high affinity for electrons, tend to gain electrons and form negatively charged ions called anions<\/em>. This transfer creates ions with opposite charges, which are held together by strong electrostatic forces known as ionic bonds<\/em>.<\/p>\n\n\n\n Magnesium (Mg) has two valence electrons (electron configuration: [Ne] 3s\u00b2), and each chlorine (Cl) atom has seven valence electrons (electron configuration: [Ne] 3s\u00b23p\u2075). Magnesium loses its two electrons to become Mg\u00b2\u207a, and each chlorine atom gains one electron to become Cl\u207b. Since magnesium donates two electrons, two chlorine atoms are needed:<\/p>\n\n\n\n Mg \u2192 Mg\u00b2\u207a + 2e\u207b<\/strong> Lewis Structure:<\/strong> Structure:<\/strong> [Mg]\u00b2\u207a [Cl]\u207b [Cl]\u207b<\/p>\n\n\n\n Sodium (Na) has one valence electron ([Ne] 3s\u00b9), and oxygen has six valence electrons ([He] 2s\u00b22p\u2074). Each sodium atom loses one electron to form Na\u207a, and oxygen gains two electrons to form O\u00b2\u207b. Two sodium atoms are required to provide two electrons:<\/p>\n\n\n\n 2Na \u2192 2Na\u207a + 2e\u207b<\/strong> Lewis Structure:<\/strong> Structure:<\/strong> [Na]\u207a [O]\u00b2\u207b [Na]\u207a<\/p>\n\n\n\n Magnesium loses two electrons to form Mg\u00b2\u207a, and oxygen gains two electrons to form O\u00b2\u207b. One magnesium atom bonds with one oxygen atom:<\/p>\n\n\n\n Mg \u2192 Mg\u00b2\u207a + 2e\u207b<\/strong> Lewis Structure:<\/strong> Structure:<\/strong> [Mg]\u00b2\u207a [O]\u00b2\u207b<\/p>\n\n\n\n In summary, ionic compounds form when metals transfer electrons to nonmetals, resulting in stable electron configurations for both ions. Their Lewis structures show complete octets for the anions and indicate the charge of each ion.<\/p>\n\n\n\n Explain the process of formation of ionic compounds and their Lewis structures. MgCl2, Na2O, MgO The Correct Answer and Explanation is: Formation of Ionic Compounds and Their Lewis Structures: MgCl\u2082, Na\u2082O, MgO Ionic compounds are formed through the transfer of electrons between metals and nonmetals. Metals, which have few valence electrons, tend to lose electrons […]<\/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-234128","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234128","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=234128"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234128\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=234128"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=234128"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=234128"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Formation of MgCl\u2082 (Magnesium Chloride)<\/strong><\/h3>\n\n\n\n
2Cl + e\u207b \u2192 2Cl\u207b<\/strong><\/p>\n\n\n\n
Mg\u00b2\u207a is shown as [Mg]\u00b2\u207a (no dots).
Each Cl\u207b is shown as [Cl]\u207b with a complete octet (8 dots).<\/p>\n\n\n\n
\n\n\n\nFormation of Na\u2082O (Sodium Oxide)<\/strong><\/h3>\n\n\n\n
O + 2e\u207b \u2192 O\u00b2\u207b<\/strong><\/p>\n\n\n\n
Each Na\u207a is [Na]\u207a (no dots), O\u00b2\u207b is [O]\u00b2\u207b with 8 electrons (dots).<\/p>\n\n\n\n
\n\n\n\nFormation of MgO (Magnesium Oxide)<\/strong><\/h3>\n\n\n\n
O + 2e\u207b \u2192 O\u00b2\u207b<\/strong><\/p>\n\n\n\n
[Mg]\u00b2\u207a (no dots), [O]\u00b2\u207b with full octet.<\/p>\n\n\n\n
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