{"id":187072,"date":"2025-01-31T10:30:49","date_gmt":"2025-01-31T10:30:49","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=187072"},"modified":"2025-01-31T10:30:53","modified_gmt":"2025-01-31T10:30:53","slug":"draw-the-lewis-structure-for-ch4-methane-nh3-ammonia-and-h20-water","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/31\/draw-the-lewis-structure-for-ch4-methane-nh3-ammonia-and-h20-water\/","title":{"rendered":"Draw the Lewis structure for CH4, (methane), NH3, (ammonia), and H20 (water)"},"content":{"rendered":"\n<p>Chemistry: Bonding 4a. Draw the Lewis structure for CH4, (methane), NH3, (ammonia), and H20 (water). b. Calculate the bond polarity for the C-H bond, N-H bond, and O-H bond. c. Classify these molecules as either polar or nonpolar. If the molecule is polar, label the partial negative and partial positive sides of the molecules you drew above.<br>Chemistry: Bonding<\/p>\n\n\n\n<p>4a. Draw the Lewis structure for CH4, (methane), NH3, (ammonia), and H20 (water).<\/p>\n\n\n\n<p>b. Calculate the bond polarity for the C-H bond, N-H bond, and O-H bond.<\/p>\n\n\n\n<p>c. Classify these molecules as either polar or nonpolar. If the molecule is polar, label the partial negative and partial positive sides of the molecules you drew above.<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">4a. Lewis Structures<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Methane (CH\u2084):<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) has 4 valence electrons, and each hydrogen (H) has 1 valence electron.<\/li>\n\n\n\n<li>Carbon shares its 4 valence electrons with 4 hydrogen atoms, forming 4 single bonds.<\/li>\n\n\n\n<li>The Lewis structure for CH\u2084 is: <code>H | H - C - H | H<\/code><\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Ammonia (NH\u2083):<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Nitrogen (N) has 5 valence electrons, and each hydrogen (H) has 1 valence electron.<\/li>\n\n\n\n<li>Nitrogen shares its 3 valence electrons with 3 hydrogen atoms, forming 3 single bonds.<\/li>\n\n\n\n<li>The Lewis structure for NH\u2083 is: <code>H | H - N - H<\/code><\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Water (H\u2082O):<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen (O) has 6 valence electrons, and each hydrogen (H) has 1 valence electron.<\/li>\n\n\n\n<li>Oxygen shares 2 of its valence electrons with 2 hydrogen atoms, forming 2 single bonds.<\/li>\n\n\n\n<li>The Lewis structure for H\u2082O is: <code>H - O - H<\/code><\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">4b. Bond Polarity<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>C-H bond in CH\u2084:<\/strong><\/li>\n\n\n\n<li>Carbon has an electronegativity of 2.55, and hydrogen has an electronegativity of 2.20.<\/li>\n\n\n\n<li>The difference in electronegativity is 0.35, which is small. This means the C-H bond is <strong>nonpolar<\/strong>.<\/li>\n\n\n\n<li><strong>N-H bond in NH\u2083:<\/strong><\/li>\n\n\n\n<li>Nitrogen has an electronegativity of 3.04, and hydrogen has an electronegativity of 2.20.<\/li>\n\n\n\n<li>The difference in electronegativity is 0.84, which indicates a <strong>polar covalent bond<\/strong>. The nitrogen atom pulls the electron density slightly toward itself, creating a partial negative charge (\u03b4-) on nitrogen and a partial positive charge (\u03b4+) on hydrogen.<\/li>\n\n\n\n<li><strong>O-H bond in H\u2082O:<\/strong><\/li>\n\n\n\n<li>Oxygen has an electronegativity of 3.44, and hydrogen has an electronegativity of 2.20.<\/li>\n\n\n\n<li>The difference in electronegativity is 1.24, which makes the O-H bond <strong>polar<\/strong>. Oxygen becomes partially negative (\u03b4-), and hydrogen becomes partially positive (\u03b4+).<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">4c. Molecular Polarity<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Methane (CH\u2084):<\/strong><\/li>\n\n\n\n<li>CH\u2084 is <strong>nonpolar<\/strong> because the C-H bonds are weakly polar and the symmetrical tetrahedral shape causes any dipoles to cancel out.<\/li>\n\n\n\n<li><strong>Ammonia (NH\u2083):<\/strong><\/li>\n\n\n\n<li>NH\u2083 is <strong>polar<\/strong> because the N-H bonds are polar, and the trigonal pyramidal shape means the dipoles do not cancel, creating a net dipole moment pointing toward nitrogen.<\/li>\n\n\n\n<li><strong>Water (H\u2082O):<\/strong><\/li>\n\n\n\n<li>H\u2082O is <strong>polar<\/strong> because the O-H bonds are polar, and the bent shape of the molecule results in an overall dipole with the partial negative charge on the oxygen and partial positive charges on the hydrogens.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>CH\u2084<\/strong> is nonpolar.<\/li>\n\n\n\n<li><strong>NH\u2083<\/strong> and <strong>H\u2082O<\/strong> are polar molecules. In NH\u2083, nitrogen carries a partial negative charge, and in H\u2082O, oxygen carries a partial negative charge. The hydrogen atoms in both are partially positive.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Chemistry: Bonding 4a. Draw the Lewis structure for CH4, (methane), NH3, (ammonia), and H20 (water). b. Calculate the bond polarity for the C-H bond, N-H bond, and O-H bond. c. Classify these molecules as either polar or nonpolar. If the molecule is polar, label the partial negative and partial positive sides of the molecules you [&hellip;]<\/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-187072","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187072","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=187072"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187072\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187072"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187072"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187072"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}