Lewis Dot Structure of Sodium Sulfite (Na\u2082SO\u2083)<\/strong><\/p>\n\n\n\n To draw the Lewis structure of sodium sulfite (Na\u2082SO\u2083)<\/strong>, we first recognize that this compound is an ionic compound<\/em> composed of two sodium ions (Na\u207a) and one sulfite ion (SO\u2083\u00b2\u207b)<\/strong>. Sodium, as an alkali metal, donates one electron to become Na\u207a and does not contribute to the covalent bonding in the sulfite ion. Therefore, the focus is on the structure of the SO\u2083\u00b2\u207b<\/strong> ion.<\/p>\n\n\n\n Steps to Draw the Lewis Structure of SO\u2083\u00b2\u207b:<\/strong><\/p>\n\n\n\n Total: Final Structure Summary:<\/strong><\/p>\n\n\n\n This structure reflects the delocalized nature of the sulfite ion with resonance among the oxygen atoms.<\/p>\n\n\n\n What is the Lewis dot structure of sodium hyposulfite (Na2SO3)? The Correct Answer and Explanation is: Lewis Dot Structure of Sodium Sulfite (Na\u2082SO\u2083) To draw the Lewis structure of sodium sulfite (Na\u2082SO\u2083), we first recognize that this compound is an ionic compound composed of two sodium ions (Na\u207a) and one sulfite ion (SO\u2083\u00b2\u207b). Sodium, as […]<\/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-232391","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/232391","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=232391"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/232391\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=232391"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=232391"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=232391"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\n\n
\n
= 6 (from S) + 3 \u00d7 6 (from O) + 2 (extra)
= 6 + 18 + 2
= 26 valence electrons<\/strong><\/p>\n\n\n\n\n
Place sulfur (central atom) connected to three oxygen atoms with single bonds.<\/li>\n\n\n\n
After placing 3 single bonds (6 electrons), 20 electrons remain. Distribute these electrons to complete octets of the oxygen atoms. Each of the three oxygens gets 6 electrons (3 lone pairs), using 18 electrons. The remaining 2 electrons go on sulfur as a lone pair.<\/li>\n\n\n\n
This structure results in high formal charges. To reduce them, form one double bond between sulfur and one oxygen atom. The result: one S=O and two S\u2013O\u207b bonds.<\/li>\n\n\n\n
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