{"id":240887,"date":"2025-07-03T13:09:24","date_gmt":"2025-07-03T13:09:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=240887"},"modified":"2025-07-03T13:09:27","modified_gmt":"2025-07-03T13:09:27","slug":"draw-the-lewis-structure-for-the-ch2o-molecule","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/03\/draw-the-lewis-structure-for-the-ch2o-molecule\/","title":{"rendered":"Draw the Lewis structure for the CH2O molecule"},"content":{"rendered":"\n
Draw the Lewis structure for the CH2O molecule: Based on this structure_ the number of polar bonds and non-polar bonds is 01) 3 polar bonds and no non-polar bonds 2) 2 polar bonds and non ~polar bond polar bonds and 2 non-polar bonds no polar bonds and 3 non-polar bonds 2 polar bonds and 2 non- polar bonds<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
To determine the number of polar and non-polar bonds in the CH2O molecule (formaldehyde), we must first look at its Lewis structure and analyze the bonds.<\/p>\n\n\n\n
Step 1: Draw the Lewis Structure of CH2O<\/h3>\n\n\n\n\n
Carbon is the central atom because it is less electronegative than oxygen and can form multiple bonds.<\/li>\n\n\n\n
Oxygen is double-bonded to carbon, and each hydrogen is single-bonded to carbon.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
Distribute Electrons<\/strong>:
Carbon will form two single bonds with two hydrogens and one double bond with oxygen.<\/li>
Oxygen will use 4 of its valence electrons to form the double bond with carbon and will have two lone pairs.<\/li><\/ul>The structure looks like this: mathematicaCopyEdit H | H-C=O<\/code> In this structure:\n
\n
Carbon (C) has 4 electrons: two single bonds to hydrogen and one double bond to oxygen.<\/li>\n\n\n\n
Oxygen (O) has 6 electrons: 4 are involved in the double bond with carbon, and the remaining 2 are lone pairs.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n
Step 2: Analyze the Bond Polarity<\/h3>\n\n\n\n
Now, let’s look at the polarity of the bonds:<\/p>\n\n\n\n
\n
Carbon-Hydrogen Bonds (C-H)<\/strong>:\n
\n
The C-H bond is non-polar<\/strong> because carbon and hydrogen have very similar electronegativities.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
Carbon-Oxygen Bond (C=O)<\/strong>:\n
\n
The C=O bond is polar<\/strong> because oxygen is more electronegative than carbon, creating a dipole where oxygen has a partial negative charge (\u03b4-) and carbon has a partial positive charge (\u03b4+).<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n
Step 3: Conclusion<\/h3>\n\n\n\n
In the CH2O molecule:<\/p>\n\n\n\n
\n
There are 2 non-polar bonds<\/strong> (C-H).<\/li>\n\n\n\n
There is 1 polar bond<\/strong> (C=O).<\/li>\n<\/ul>\n\n\n\n
Thus, the correct answer is:<\/p>\n\n\n\n
\n
2 polar bonds and 1 non-polar bond<\/strong>.<\/li>\n<\/ul>\n\n\n\n
This means the molecule contains both polar and non-polar bonds, and the number of polar bonds is greater than the non-polar ones.<\/p>\n\n\n\n
The overall polarity of the molecule is determined by the fact that the C=O bond introduces a dipole, making the CH2O molecule polar overall. However, this question only focuses on the individual bond types.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
Draw the Lewis structure for the CH2O molecule: Based on this structure_ the number of polar bonds and non-polar bonds is 01) 3 polar bonds and no non-polar bonds 2) 2 polar bonds and non ~polar bond polar bonds and 2 non-polar bonds no polar bonds and 3 non-polar bonds 2 polar bonds and 2 […]<\/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-240887","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240887","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=240887"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240887\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=240887"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=240887"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=240887"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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