The Lewis structure for ammonia (NH\u2083) consists of a nitrogen (N) atom covalently bonded to three hydrogen (H) atoms, with a lone pair of electrons on the nitrogen. Here\u2019s the step-by-step process to determine the Lewis structure:<\/p>\n\n\n\n
- \n
- Count Valence Electrons<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- \n
- Nitrogen (N) has 5<\/strong> valence electrons.<\/li>\n\n\n\n
- Each hydrogen (H) has 1<\/strong> valence electron, and since there are three hydrogens, we have 3 \u00d7 1 = 3<\/strong> valence electrons.<\/li>\n\n\n\n
- Total valence electrons = 5 (from N) + 3 (from H) = 8<\/strong>.<\/li>\n<\/ul>\n\n\n\n
- \n
- Determine the Central Atom<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- \n
- Nitrogen is less electronegative than hydrogen, so it becomes the central atom.<\/li>\n<\/ul>\n\n\n\n
- \n
- Form Bonds<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- \n
- Each hydrogen forms a single bond with nitrogen, using up 6 electrons<\/strong> (3 bonds \u00d7 2 electrons per bond).<\/li>\n<\/ul>\n\n\n\n
- \n
- Distribute Remaining Electrons<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- \n
- The remaining 2 electrons<\/strong> form a lone pair on nitrogen.<\/li>\n<\/ul>\n\n\n\n
Thus, the final Lewis structure of NH\u2083 has nitrogen at the center, single bonds connecting to three hydrogen atoms, and a lone pair of electrons on nitrogen.<\/p>\n\n\n\n
Answer:<\/h3>\n\n\n\n
Total valence electrons counted in the Lewis structure for ammonia (NH\u2083) = 8.<\/strong><\/p>\n\n\n\n
Explanation:<\/h3>\n\n\n\n
The Lewis structure of NH\u2083 follows the octet rule<\/strong>, ensuring that nitrogen has eight electrons in its valence shell (including its lone pair and bonding electrons). The molecular shape of NH\u2083 is trigonal pyramidal<\/strong>, influenced by the lone pair, which repels the bonding pairs, making the bond angles slightly less than the ideal 109.5\u00b0<\/strong> (approximately 107\u00b0<\/strong> in NH\u2083). The lone pair contributes to the polarity<\/strong> of NH\u2083, making it a polar molecule<\/strong> with a partial negative charge on nitrogen and partial positive charges on hydrogen. This polarity allows NH\u2083 to form hydrogen bonds, making it highly soluble in water. The correct count of 8 valence electrons<\/strong> ensures that the structure is valid and follows the octet rule<\/strong> properly.<\/p>\n\n\n\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-712.png\")
<\/figure>\n\n\n\nHere is the Lewis structure for ammonia (NH\u2083). The nitrogen atom (N) is at the center, forming three single bonds with hydrogen (H) atoms. The lone pair on nitrogen is represented above it. This structure accounts for all 8 valence electrons<\/strong> in NH\u2083, ensuring that nitrogen follows the octet rule while hydrogen completes its duet rule<\/strong>.<\/p>\n\n\n\n
- <\/ol>\n","protected":false},"excerpt":{"rendered":"
Draw and reference the Lewis structure for ammonia, NH3, How many total valence electrons are counted in the Lewis structure for ammonia? The correct answer and explanation is : The Lewis structure for ammonia (NH\u2083) consists of a nitrogen (N) atom covalently bonded to three hydrogen (H) atoms, with a lone pair of electrons on […]<\/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-198522","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198522","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=198522"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198522\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198522"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198522"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198522"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
- The remaining 2 electrons<\/strong> form a lone pair on nitrogen.<\/li>\n<\/ul>\n\n\n\n
- Distribute Remaining Electrons<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- Each hydrogen forms a single bond with nitrogen, using up 6 electrons<\/strong> (3 bonds \u00d7 2 electrons per bond).<\/li>\n<\/ul>\n\n\n\n
- Form Bonds<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- Nitrogen is less electronegative than hydrogen, so it becomes the central atom.<\/li>\n<\/ul>\n\n\n\n
- Each hydrogen (H) has 1<\/strong> valence electron, and since there are three hydrogens, we have 3 \u00d7 1 = 3<\/strong> valence electrons.<\/li>\n\n\n\n
- Nitrogen (N) has 5<\/strong> valence electrons.<\/li>\n\n\n\n