{"id":225638,"date":"2025-06-04T11:03:21","date_gmt":"2025-06-04T11:03:21","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=225638"},"modified":"2025-06-04T11:03:23","modified_gmt":"2025-06-04T11:03:23","slug":"write-the-lewis-structure-for-the-nh4-ion","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/04\/write-the-lewis-structure-for-the-nh4-ion\/","title":{"rendered":"Write the Lewis structure for the NH4 + ion"},"content":{"rendered":"\n

Write the Lewis structure for the NH4 + ion.<\/p>\n\n\n\n

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

Lewis Structure for NH\u2084\u207a (Ammonium Ion):<\/h3>\n\n\n\n

Correct Lewis Structure:<\/h4>\n\n\n\n
      H\n      |\nH \u2013 N\u207a \u2013 H\n      |\n      H\n<\/code><\/pre>\n\n\n\n
Each hydrogen (H) forms a single bond with the central nitrogen (N) atom. Nitrogen has a formal positive charge in this structure.<\/p>\n\n\n\n
\n\n\n\n
 Explanation:<\/h3>\n\n\n\n
The ammonium ion (NH\u2084\u207a) is a polyatomic ion formed when ammonia (NH\u2083) accepts a proton (H\u207a). To understand its structure, we use Lewis dot structures, which show how valence electrons are distributed in a molecule or ion.<\/p>\n\n\n\n
Nitrogen (N) has 5 valence electrons, and each hydrogen (H) has 1. In total, we begin with:<\/p>\n\n\n\n
    \n
  • Nitrogen: 5 electrons<\/li>\n\n\n\n
  • Hydrogen (4 \u00d7 1): 4 electrons<\/li>\n\n\n\n
  • Total: 9 electrons<\/li>\n<\/ul>\n\n\n\n
    But NH\u2084\u207a has a +1 charge<\/strong>, meaning it has lost one electron<\/strong>. So we adjust the total number of electrons:<\/p>\n\n\n\n
    9 \u2013 1 = 8 valence electrons<\/strong> to distribute.<\/p>\n\n\n\n
    To satisfy the octet rule, nitrogen forms four single bonds<\/strong> with four hydrogen atoms. Each N\u2013H bond uses two electrons, and 4 bonds \u00d7 2 electrons = 8 electrons, which matches our available count.<\/p>\n\n\n\n
    After forming four single bonds, nitrogen has 8 electrons around it (2 per bond), achieving a complete octet. Each hydrogen has only 2 electrons (a single bond), which is sufficient because hydrogen follows the duet rule.<\/p>\n\n\n\n
    Since nitrogen normally forms three bonds (like in NH\u2083), forming four bonds gives it a formal positive charge<\/strong>, because it is effectively \u201csharing\u201d one more electron than usual. The ion\u2019s positive charge is indicated on nitrogen in the Lewis structure.<\/p>\n\n\n\n
    Also, because this is a charged ion, the entire Lewis structure should be placed inside brackets with the charge outside:<\/p>\n\n\n\n
         [      H\n           |\n    H \u2013 N\u207a \u2013 H   ]\u207a\n           |\n           H\n<\/code><\/pre>\n\n\n\n
    In summary, NH\u2084\u207a has a central nitrogen atom bonded to four hydrogen atoms, uses 8 electrons total, satisfies all atoms\u2019 valence needs, and carries a positive charge due to the extra proton accepted by NH\u2083.<\/p>\n\n\n\n
    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
    Write the Lewis structure for the NH4 + ion. The Correct Answer and Explanation is: Lewis Structure for NH\u2084\u207a (Ammonium Ion): Correct Lewis Structure: Each hydrogen (H) forms a single bond with the central nitrogen (N) atom. Nitrogen has a formal positive charge in this structure. Explanation: The ammonium ion (NH\u2084\u207a) is a polyatomic ion […]<\/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-225638","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/225638","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=225638"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/225638\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=225638"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=225638"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=225638"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}