{"id":230895,"date":"2025-06-10T07:45:59","date_gmt":"2025-06-10T07:45:59","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=230895"},"modified":"2025-06-10T07:46:01","modified_gmt":"2025-06-10T07:46:01","slug":"write-electronic-configurations-for-the-following-ions-a-al3-z-13-b-o2-z-8-c-fe3-z-26-d-cu2-z-29-e-cu-z-29","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/10\/write-electronic-configurations-for-the-following-ions-a-al3-z-13-b-o2-z-8-c-fe3-z-26-d-cu2-z-29-e-cu-z-29\/","title":{"rendered":"Write electronic configurations for the following ions: a. Al3+ (Z = 13) b. O2- (Z = 8) c. Fe3+ (Z = 26) d. Cu2+ (Z = 29) e. Cu+ (Z = 29)"},"content":{"rendered":"\n

Write electronic configurations for the following ions: a. Al3+ (Z = 13) b. O2- (Z = 8) c. Fe3+ (Z = 26) d. Cu2+ (Z = 29) e. Cu+ (Z = 29)<\/p>\n\n\n\n

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

ChatGPT said:<\/h6>\n\n\n\n

Electronic Configurations of Ions<\/strong><\/h3>\n\n\n\n

a. Al\u00b3\u207a (Z = 13)<\/strong>
Neutral Al: 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u00b9
Al\u00b3\u207a: 1s\u00b2 2s\u00b2 2p\u2076<\/strong><\/p>\n\n\n\n

b. O\u00b2\u207b (Z = 8)<\/strong>
Neutral O: 1s\u00b2 2s\u00b2 2p\u2074
O\u00b2\u207b: 1s\u00b2 2s\u00b2 2p\u2076<\/strong><\/p>\n\n\n\n

c. Fe\u00b3\u207a (Z = 26)<\/strong>
Neutral Fe: [Ar] 4s\u00b2 3d\u2076
Fe\u00b3\u207a: [Ar] 3d\u2075<\/strong><\/p>\n\n\n\n

d. Cu\u00b2\u207a (Z = 29)<\/strong>
Neutral Cu: [Ar] 4s\u00b9 3d\u00b9\u2070
Cu\u00b2\u207a: [Ar] 3d\u2079<\/strong><\/p>\n\n\n\n

e. Cu\u207a (Z = 29)<\/strong>
Neutral Cu: [Ar] 4s\u00b9 3d\u00b9\u2070
Cu\u207a: [Ar] 3d\u00b9\u2070<\/strong><\/p>\n\n\n\n

\n\n\n\n

Explanation<\/strong><\/h3>\n\n\n\n

The electronic configuration of an ion depends on the number of electrons it possesses, which differs from its neutral atom depending on whether it loses or gains electrons.<\/p>\n\n\n\n

For Al\u00b3\u207a<\/strong>, aluminum has an atomic number of 13, with a neutral configuration of 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u00b9. It loses three electrons to become Al\u00b3\u207a. The electrons are lost from the outermost shell first (3p and 3s orbitals), leaving the stable noble gas configuration of neon (1s\u00b2 2s\u00b2 2p\u2076).<\/p>\n\n\n\n

In the case of O\u00b2\u207b<\/strong>, oxygen has 8 electrons in its neutral state (1s\u00b2 2s\u00b2 2p\u2074). Gaining two electrons gives it a full 2p orbital (2p\u2076), resulting in a noble gas configuration like neon. Negative ions (anions) gain electrons to achieve full outer shells.<\/p>\n\n\n\n

For Fe\u00b3\u207a<\/strong>, iron has 26 electrons, and its neutral configuration is [Ar] 4s\u00b2 3d\u2076. Electrons are removed first from the 4s orbital (higher energy in ions) and then from the 3d. Removing three electrons gives [Ar] 3d\u2075, which is a half-filled d-subshell and relatively stable.<\/p>\n\n\n\n

Cu\u00b2\u207a<\/strong> and Cu\u207a<\/strong> are exceptions due to copper’s unusual electron configuration. Neutral copper has a configuration of [Ar] 4s\u00b9 3d\u00b9\u2070, favoring a full d-subshell over a filled 4s. Cu\u207a loses the 4s\u00b9 electron, resulting in [Ar] 3d\u00b9\u2070. Cu\u00b2\u207a loses both the 4s\u00b9 and one 3d electron, resulting in [Ar] 3d\u2079.<\/p>\n\n\n\n

These examples illustrate the principles of electron configuration in ions, where stability and energy levels govern which electrons are lost or gained.<\/p>\n\n\n\n

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

Write electronic configurations for the following ions: a. Al3+ (Z = 13) b. O2- (Z = 8) c. Fe3+ (Z = 26) d. Cu2+ (Z = 29) e. Cu+ (Z = 29) The Correct Answer and Explanation is: ChatGPT said: Electronic Configurations of Ions a. Al\u00b3\u207a (Z = 13)Neutral Al: 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u00b9Al\u00b3\u207a: […]<\/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-230895","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230895","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=230895"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230895\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=230895"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=230895"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=230895"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}