{"id":245114,"date":"2025-07-05T17:04:39","date_gmt":"2025-07-05T17:04:39","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=245114"},"modified":"2025-07-05T17:04:42","modified_gmt":"2025-07-05T17:04:42","slug":"what-is-the-ionic-compound-formula-sodium-nitride","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/05\/what-is-the-ionic-compound-formula-sodium-nitride\/","title":{"rendered":"what is the ionic compound formula sodium nitride"},"content":{"rendered":"\n

what is the ionic compound formula sodium nitride?<\/p>\n\n\n\n

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

The ionic compound formula for sodium nitride is Na\u2083N<\/strong>.<\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n
    \n
  1. Ionic Bond Formation<\/strong>: Sodium (Na) is a metal from Group 1 of the periodic table, and nitrogen (N) is a non-metal from Group 15. When forming an ionic compound, metals like sodium tend to lose electrons, and non-metals like nitrogen tend to gain electrons. This electron transfer forms positively charged ions (cations) and negatively charged ions (anions).<\/li>\n\n\n\n
  2. Sodium Ion (Na\u207a)<\/strong>: Sodium atoms have an atomic number of 11, meaning they have 11 electrons in total. The electron configuration of sodium is 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b9. To achieve a stable electron configuration (like the noble gas Ne), sodium loses its one valence electron, resulting in a Na\u207a ion.<\/li>\n\n\n\n
  3. Nitride Ion (N\u00b3\u207b)<\/strong>: Nitrogen has an atomic number of 7, so its electron configuration is 1s\u00b2 2s\u00b2 2p\u00b3. It needs three more electrons to fill its outer shell (2p\u2076), forming a nitride ion (N\u00b3\u207b).<\/li>\n\n\n\n
  4. Balancing Charges<\/strong>: The sodium ion has a charge of +1 (Na\u207a), and the nitride ion has a charge of -3 (N\u00b3\u207b). To balance the charges, three sodium ions (each with a +1 charge) are required to combine with one nitride ion (with a -3 charge). Therefore, the formula for sodium nitride becomes Na\u2083N<\/strong>.<\/li>\n\n\n\n
  5. Ionic Compound Characteristics<\/strong>: In Na\u2083N, the sodium ions are electrostatically attracted to the nitride ion, forming a stable ionic bond. This ionic structure leads to a solid lattice structure that is characteristic of many ionic compounds.<\/li>\n<\/ol>\n\n\n\n

    In conclusion, the formula for sodium nitride is Na\u2083N, where three sodium ions balance the charge of one nitride ion, resulting in a neutral ionic compound.<\/p>\n\n\n\n

    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

    what is the ionic compound formula sodium nitride? The Correct Answer and Explanation is: The ionic compound formula for sodium nitride is Na\u2083N. Explanation: In conclusion, the formula for sodium nitride is Na\u2083N, where three sodium ions balance the charge of one nitride ion, resulting in a neutral ionic compound.<\/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-245114","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/245114","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=245114"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/245114\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=245114"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=245114"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=245114"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}