{"id":231086,"date":"2025-06-10T12:37:36","date_gmt":"2025-06-10T12:37:36","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=231086"},"modified":"2025-06-10T12:37:38","modified_gmt":"2025-06-10T12:37:38","slug":"write-the-lewis-structure-for-each-molecule-or-ion-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/10\/write-the-lewis-structure-for-each-molecule-or-ion-2\/","title":{"rendered":"Write the Lewis structure for each molecule or ion."},"content":{"rendered":"\n

Write the Lewis structure for each molecule or ion. MISSED THIS? Read Section 10.7; Watch KCV 10.7, IWE 10.4 a. Cl
b. N
O c. SiH
d. Cl
CO<\/p>\n\n\n\n

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

Here are the Lewis structures for the given molecules and ions:<\/p>\n\n\n\n

a. Cl (Chlorine atom)<\/strong> Cl is a single atom with 7 valence electrons, represented as: Cl: \u25cf\u25cf\u25cf\u25cf\u25cf\u25cf\u25cf<\/p>\n\n\n\n

b. NO (Nitric oxide)<\/strong> N has 5 valence electrons, and O has 6, totaling 11 valence electrons. NO contains a double bond between N and O, with an unpaired electron on N:<\/p>\n\n\n\n

.. N=O .<\/p>\n\n\n\n

c. SiH (Silicon monohydride)<\/strong> Si has 4 valence electrons, and H has 1. Since SiH is an unstable radical, its structure is:<\/p>\n\n\n\n

H-Si\u25cf\u25cf\u25cf<\/p>\n\n\n\n

d. ClCO (Chlorocarbonyl radical)<\/strong> This molecule consists of Cl, C, and O with a total of 18 valence electrons. Carbon forms a double bond with oxygen and a single bond with chlorine:<\/p>\n\n\n\n

Cl-C=O\u25cf\u25cf<\/p>\n\n\n\n

Explanation (300 words)<\/h3>\n\n\n\n

Lewis structures help visualize molecular bonding and electron distribution, following the octet rule where atoms prefer 8 valence electrons (except H, which follows the duet rule).<\/p>\n\n\n\n

Chlorine (Cl) exists as a single atom with 7 valence electrons, seeking one more to complete its octet. Nitric oxide (NO) is unique, having an odd number of electrons, making it a radical. This contributes to NO\u2019s reactivity, as radicals are highly unstable.<\/p>\n\n\n\n

Silicon monohydride (SiH) is another radical, as silicon has an incomplete octet with an unpaired electron. Due to this instability, SiH typically exists in highly reactive environments.<\/p>\n\n\n\n

Chlorocarbonyl (ClCO) features a carbonyl group (-CO), where carbon forms a double bond with oxygen to satisfy the octet rule. The lone electron remains on carbon, making it a radical. Such structures often appear in reactive intermediates in organic and atmospheric chemistry.<\/p>\n\n\n\n

Lewis structures are fundamental in predicting chemical behavior, reactivity, and molecular properties!<\/p>\n\n\n\n

\"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

Write the Lewis structure for each molecule or ion. MISSED THIS? Read Section 10.7; Watch KCV 10.7, IWE 10.4 a. Clb. NO c. SiHd. ClCO The correct Answer and Explanation is: Here are the Lewis structures for the given molecules and ions: a. Cl (Chlorine atom) Cl is a single atom with 7 valence electrons, […]<\/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-231086","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231086","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=231086"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231086\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=231086"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=231086"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=231086"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}