{"id":225279,"date":"2025-06-04T06:26:11","date_gmt":"2025-06-04T06:26:11","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=225279"},"modified":"2025-06-04T06:26:13","modified_gmt":"2025-06-04T06:26:13","slug":"the-lewis-dot-symbol-for-the-chloride-cl-ion-is-oam-clm-cl-a","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/04\/the-lewis-dot-symbol-for-the-chloride-cl-ion-is-oam-clm-cl-a\/","title":{"rendered":"The Lewis dot symbol for the chloride (Cl-) ion is: O:am Cl:m Cl: a"},"content":{"rendered":"\n

The Lewis dot symbol for the chloride (Cl-) ion is: O:am Cl:m Cl: a<\/p>\n\n\n\n

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

Correct Lewis Dot Symbol for the Chloride Ion (Cl\u207b):<\/h3>\n\n\n\n

The correct Lewis dot symbol<\/strong> for the chloride ion (Cl\u207b)<\/strong> is:<\/p>\n\n\n\n

  ..\n: Cl :\n  ..\n[ Cl\u207b ]\n<\/code><\/pre>\n\n\n\n
This shows a chlorine atom<\/strong> with a full octet<\/strong> (8 valence electrons) and a negative charge<\/strong> enclosed in brackets.<\/p>\n\n\n\n
\n\n\n\n
Explanation<\/h3>\n\n\n\n
The Lewis dot symbol<\/strong> is a simple way to represent the valence electrons of an atom or ion. Each dot<\/strong> around the element\u2019s symbol represents one valence electron<\/strong>.<\/p>\n\n\n\n
Chlorine (Cl) is a group 17<\/strong> element (halogen) on the periodic table. As a neutral atom, it has 7 valence electrons<\/strong> (since group 17 elements have 7 electrons in their outer shell). In its neutral state<\/strong>, the Lewis symbol for chlorine is:<\/p>\n\n\n\n
: Cl .\n<\/code><\/pre>\n\n\n\n
(7 dots arranged around the symbol).<\/p>\n\n\n\n
However, chlorine readily gains one electron<\/strong> to form the chloride ion (Cl\u207b<\/strong>) to achieve a stable octet (8 electrons in the outer shell), like the nearest noble gas, argon (Ar).<\/p>\n\n\n\n
When Cl gains an electron, it becomes Cl\u207b<\/strong>, a negatively charged ion (anion). Now, instead of 7, it has 8 valence electrons<\/strong>. In the Lewis dot symbol, this is shown by surrounding the symbol with 8 dots<\/strong> and placing the ion inside square brackets<\/strong> with a superscript minus sign:<\/p>\n\n\n\n
  ..\n: Cl :\n  ..\n[ Cl\u207b ]\n<\/code><\/pre>\n\n\n\n
This format emphasizes two important features:<\/p>\n\n\n\n
    \n
  1. The full octet<\/strong> (8 dots around Cl) showing chemical stability.<\/li>\n\n\n\n
  2. The negative charge<\/strong> ([Cl\u207b]) resulting from the gained electron.<\/li>\n<\/ol>\n\n\n\n
    This representation is especially important in ionic bonding<\/strong>, such as in sodium chloride (NaCl)<\/strong>, where a Na\u207a ion<\/strong> (which loses one electron) and a Cl\u207b ion<\/strong> (which gains one) form an electrostatic attraction.<\/p>\n\n\n\n
    In summary, the correct Lewis dot structure of the chloride ion shows a Cl atom with eight electrons<\/strong> and a negative charge<\/strong>, enclosed in brackets to indicate it is an ion.<\/p>\n\n\n\n
    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
    The Lewis dot symbol for the chloride (Cl-) ion is: O:am Cl:m Cl: a The Correct Answer and Explanation is: Correct Lewis Dot Symbol for the Chloride Ion (Cl\u207b): The correct Lewis dot symbol for the chloride ion (Cl\u207b) is: This shows a chlorine atom with a full octet (8 valence electrons) and a negative […]<\/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-225279","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/225279","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=225279"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/225279\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=225279"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=225279"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=225279"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}