{"id":155801,"date":"2024-10-16T12:58:07","date_gmt":"2024-10-16T12:58:07","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=155801"},"modified":"2024-10-16T12:58:10","modified_gmt":"2024-10-16T12:58:10","slug":"in-order-for-sodium-to-have-8-valence-electrons-it-would-need-to-either-gain-_____-electrons-or-lose-_____-electron","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/16\/in-order-for-sodium-to-have-8-valence-electrons-it-would-need-to-either-gain-_____-electrons-or-lose-_____-electron\/","title":{"rendered":"In order for sodium to have 8 valence electrons, it would need to either gain _____ electrons or lose _____ electron."},"content":{"rendered":"\n

In order for sodium to have 8 valence electrons, it would need to either gain _ electrons or lose _<\/em><\/strong> electron.<\/p>\n\n\n\n

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

In order for sodium (Na) to have 8 valence electrons, it would need to either gain 7 electrons<\/strong> or lose 1 electron<\/strong>.<\/p>\n\n\n\n

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

Sodium is an alkali metal located in group 1 of the periodic table. Its atomic number is 11, which means it has 11 electrons when neutral. The electron configuration of sodium is (1s^2 2s^2 2p^6 3s^1). This shows that sodium has a total of 11 electrons: 2 in the first shell, 8 in the second shell, and 1 in the third shell. The first two shells can hold a maximum of 2 and 8 electrons, respectively, while the third shell can hold more than 8 electrons.<\/p>\n\n\n\n

The octet rule<\/strong> states that atoms tend to gain, lose, or share electrons in order to achieve a full outer shell of 8 electrons, which is energetically favorable and leads to increased stability. For sodium, the outermost shell (the third shell) has only 1 electron. To reach an octet, sodium has two main options:<\/p>\n\n\n\n

    \n
  1. Gain 7 Electrons:<\/strong> If sodium were to gain 7 electrons, it would have a total of 8 electrons in its outer shell. However, this is energetically unfavorable for sodium due to its position on the periodic table and the high energy required to add such a large number of electrons. Gaining multiple electrons would also create a very negatively charged ion, which is less likely for an alkali metal.<\/li>\n\n\n\n
  2. Lose 1 Electron:<\/strong> The more favorable option for sodium is to lose its single valence electron. By losing this 1 electron, sodium achieves a stable electron configuration similar to that of neon (the nearest noble gas), which has a full outer shell of 8 electrons. This loss results in the formation of a positively charged ion, Na\u207a. This process is energetically favorable because it allows sodium to achieve a more stable electron configuration with less energy required than gaining multiple electrons.<\/li>\n<\/ol>\n\n\n\n

    In summary, while sodium could theoretically gain 7 electrons to achieve a full octet, the more practical and favorable path is for it to lose 1 electron, resulting in a stable Na\u207a ion with a complete octet in the previous electron shell.<\/p>\n","protected":false},"excerpt":{"rendered":"

    In order for sodium to have 8 valence electrons, it would need to either gain _ electrons or lose _ electron. The Correct Answer and Explanation is: In order for sodium (Na) to have 8 valence electrons, it would need to either gain 7 electrons or lose 1 electron. Explanation: Sodium is an alkali 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-155801","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/155801","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=155801"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/155801\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=155801"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=155801"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=155801"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}