{"id":236685,"date":"2025-06-16T12:21:04","date_gmt":"2025-06-16T12:21:04","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=236685"},"modified":"2025-06-16T12:21:06","modified_gmt":"2025-06-16T12:21:06","slug":"write-out-the-complete-electron-configuration-for-cu-cu","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/16\/write-out-the-complete-electron-configuration-for-cu-cu\/","title":{"rendered":"Write out the complete electron configuration for Cu, Cu"},"content":{"rendered":"\n<p>Write out the complete electron configuration for Cu, Cu<br>and Cu<br>according to the normal pattern of filling electrons. (3 points) (b) Rewrite the electron configurations for Cu and Cu<br>promoting one electron to get a more stable configuration. (2 points) 7. Element Q, in the fourth period, has the following ionization energies:<br>=590 kJ,<br>=1145 kJ,<br>=4912 kJ,<br>=6491 kJ,<br>=8140 kJ,<br>=10,500. What is element Q? Explain briefly. (2 points) 8. Nitrogen is a nonmetal that \\&#8221;likes\\&#8221; to gain electrons. However, its electron affinity is +7.0 kJ. Explain what the positive value indicates. Use the electron configuration to explain why it is it is positive for nitrogen. (2 points)<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p><strong>(a) Complete Electron Configurations (normal filling pattern):<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Cu (Copper):<\/strong><br>1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 4s\u00b2 3d\u2079<\/li>\n\n\n\n<li><strong>Cu\u207a (Copper I ion):<\/strong><br>1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 4s\u00b9 3d\u2079<\/li>\n\n\n\n<li><strong>Cu\u00b2\u207a (Copper II ion):<\/strong><br>1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 3d\u2079<\/li>\n<\/ul>\n\n\n\n<p><strong>(b) More Stable (Promoted) Configurations:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Cu:<\/strong><br>1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 4s\u00b9 3d\u00b9\u2070<br><em>One electron from 4s is promoted to 3d to make 3d a full sublevel, which is more stable.<\/em><\/li>\n\n\n\n<li><strong>Cu\u207a:<\/strong><br>1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 3d\u00b9\u2070<br><em>Loss of the single 4s electron from neutral copper results in a stable, fully filled 3d sublevel.<\/em><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>7. Element Q Identification:<\/strong><\/p>\n\n\n\n<p>The ionization energies are:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>IE\u2081 = 590 kJ\/mol<\/li>\n\n\n\n<li>IE\u2082 = 1145 kJ\/mol<\/li>\n\n\n\n<li>IE\u2083 = 4912 kJ\/mol<\/li>\n\n\n\n<li>IE\u2084 = 6491 kJ\/mol<\/li>\n\n\n\n<li>IE\u2085 = 8140 kJ\/mol<\/li>\n\n\n\n<li>IE\u2086 = 10,500 kJ\/mol<\/li>\n<\/ul>\n\n\n\n<p>There is a significant jump between IE\u2082 and IE\u2083, indicating the removal of a core electron after two valence electrons have been removed. This pattern is characteristic of <strong>magnesium (Mg)<\/strong>, which has two valence electrons in the 3s orbital. Therefore, <strong>element Q is magnesium<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>8. Positive Electron Affinity of Nitrogen:<\/strong><\/p>\n\n\n\n<p>Electron affinity refers to the energy change when an atom gains an electron. For nitrogen, the value is <strong>+7.0 kJ\/mol<\/strong>, which means <strong>energy must be added<\/strong> for nitrogen to accept an additional electron. This is unusual for a nonmetal.<\/p>\n\n\n\n<p>Nitrogen\u2019s electron configuration is:<br><strong>1s\u00b2 2s\u00b2 2p\u00b3<\/strong><\/p>\n\n\n\n<p>Its 2p sublevel is half-filled, which is relatively stable due to minimized electron repulsion. Adding another electron would increase repulsion in the already half-filled 2p orbital. As a result, nitrogen resists gaining an extra electron and requires energy input, explaining the positive electron affinity.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-706.jpeg\" alt=\"\" class=\"wp-image-236686\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Write out the complete electron configuration for Cu, Cuand Cuaccording to the normal pattern of filling electrons. (3 points) (b) Rewrite the electron configurations for Cu and Cupromoting one electron to get a more stable configuration. (2 points) 7. Element Q, in the fourth period, has the following ionization energies:=590 kJ,=1145 kJ,=4912 kJ,=6491 kJ,=8140 kJ,=10,500. [&hellip;]<\/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-236685","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/236685","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=236685"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/236685\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=236685"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=236685"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=236685"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}