{"id":230658,"date":"2025-06-09T19:15:27","date_gmt":"2025-06-09T19:15:27","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=230658"},"modified":"2025-06-09T19:15:29","modified_gmt":"2025-06-09T19:15:29","slug":"draw-a-lewis-structure-that-represents-a-hydrogen-molecule-h2-and-show-the-relative-polarities-of-the-atoms-with-partial-charges-i-and-iae-if-any","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/09\/draw-a-lewis-structure-that-represents-a-hydrogen-molecule-h2-and-show-the-relative-polarities-of-the-atoms-with-partial-charges-i-and-iae-if-any\/","title":{"rendered":"Draw a Lewis structure that represents a hydrogen molecule (H2) and show the relative polarities of the atoms (with partial charges \u00ce\u00b4+ and \u00ce\u00b4\u00e2\u20ac\u201c), if any."},"content":{"rendered":"\n


Draw a Lewis structure that represents a hydrogen molecule (H2) and show the relative polarities of the atoms (with partial charges \u00ce\u00b4+ and \u00ce\u00b4\u00e2\u20ac\u201c), if any.<\/p>\n\n\n\n

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

Correct Answer:<\/strong><\/h3>\n\n\n\n

Lewis Structure of Hydrogen Molecule (H\u2082):<\/strong><\/p>\n\n\n\n

CopyEditH\u2014H\n<\/code><\/pre>\n\n\n\n
Each hydrogen atom shares one electron, forming a single covalent bond<\/strong>. There are no lone pairs in this molecule.<\/p>\n\n\n\n
Polarity (Partial Charges):<\/strong><\/p>\n\n\n\n
Since both atoms are identical hydrogen atoms<\/strong>, the electrons in the bond are shared equally<\/strong>. Therefore, there are no partial charges<\/strong> (\u03b4+ or \u03b4\u2212) on either hydrogen atom.<\/p>\n\n\n\n
\n
Polarity: Nonpolar molecule<\/strong>
Partial Charges: None (No \u03b4+ or \u03b4\u2212)<\/strong><\/p>\n<\/blockquote>\n\n\n\n
\n\n\n\n
 Explanation:<\/strong><\/h3>\n\n\n\n
A hydrogen molecule (H\u2082)<\/strong> is the simplest diatomic molecule, composed of two hydrogen atoms. Each hydrogen atom has one electron<\/strong> in its 1s orbital. When two hydrogen atoms come close enough, they can share<\/strong> their single electrons to form a covalent bond<\/strong>, resulting in a more stable configuration\u2014akin to a helium atom, which has two electrons.<\/p>\n\n\n\n
In the Lewis structure<\/strong> of H\u2082, this bond is depicted as a single line (H\u2014H<\/strong>) between the two hydrogen atoms. Each hydrogen atom “feels” as if it has two electrons around it, satisfying the duet rule (the equivalent of the octet rule for hydrogen).<\/p>\n\n\n\n
When evaluating polarity<\/strong>, we consider the electronegativity<\/strong> of the atoms involved. Electronegativity is a measure of how strongly an atom attracts electrons in a bond. If two atoms have different electronegativities<\/strong>, the shared electrons are pulled more toward the more electronegative atom, creating partial charges<\/strong> (\u03b4+ and \u03b4\u2212), and the molecule is said to be polar<\/strong>.<\/p>\n\n\n\n
However, in the case of H\u2082, both atoms are hydrogen<\/strong>\u2014they have the same electronegativity<\/strong> (2.1 on the Pauling scale). As a result, the shared electrons are equally attracted<\/strong> to both nuclei. There is no unequal distribution of electron density<\/strong>, meaning no partial charges<\/strong> form.<\/p>\n\n\n\n
Therefore, the hydrogen molecule is nonpolar<\/strong>, and neither atom carries a \u03b4+ or \u03b4\u2212 partial charge. It is a symmetrical, nonpolar covalent molecule<\/strong>, and one of the most basic examples used in chemistry to illustrate covalent bonding and molecular symmetry.<\/p>\n\n\n\n
\"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
Draw a Lewis structure that represents a hydrogen molecule (H2) and show the relative polarities of the atoms (with partial charges \u00ce\u00b4+ and \u00ce\u00b4\u00e2\u20ac\u201c), if any. The Correct Answer and Explanation is: Correct Answer: Lewis Structure of Hydrogen Molecule (H\u2082): CopyEditH\u2014H Each hydrogen atom shares one electron, forming a single covalent bond. There are no […]<\/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-230658","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230658","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=230658"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230658\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=230658"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=230658"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=230658"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}