{"id":3655,"date":"2023-01-09T10:11:03","date_gmt":"2023-01-09T10:11:03","guid":{"rendered":"https:\/\/9thclass.deltapublications.in\/?page_id=3655"},"modified":"2025-01-06T17:19:28","modified_gmt":"2025-01-06T17:19:28","slug":"s-4-c-how-are-electrons-distributed-in-different-orbits","status":"publish","type":"page","link":"https:\/\/9thclass.deltapublications.in\/index.php\/s-4-c-how-are-electrons-distributed-in-different-orbits\/","title":{"rendered":"S-4.c How Are Electrons Distributed In Different Orbits?"},"content":{"rendered":"\n<h2 class=\"wp-block-heading has-text-align-center has-text-color\" style=\"color:#00056d;text-transform:uppercase\"><strong>How Are Electrons Distributed In Different Orbits?<\/strong><\/h2>\n\n\n\n<p class=\"has-text-color has-huge-font-size\" style=\"color:#74008b\"><strong>Key Notes:<\/strong><\/p>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-2e1e90b29a6492d1e4896444bc613c2a\" style=\"color:#000060;background-color:#dfc816\"><strong>Structure of the Atom<\/strong>:<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"300\" height=\"250\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-13.png\" alt=\"\" class=\"wp-image-15859\"\/><\/figure><\/div>\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>Atoms consist of a central nucleus surrounded by electrons.<\/li>\n\n\n\n<li>The electrons revolve around the nucleus in specific paths called <em>orbits<\/em> or <em>shells<\/em>.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-75f43ba6aeb334513f751aeac3e55c52\" style=\"color:#000060;background-color:#dfc816\"><strong>Energy Levels (Shells)<\/strong>:<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full is-resized\"><img loading=\"lazy\" decoding=\"async\" width=\"800\" height=\"433\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/Untitled-design-45.png\" alt=\"\" class=\"wp-image-15861\" style=\"width:436px;height:auto\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/Untitled-design-45.png 800w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/Untitled-design-45-300x162.png 300w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/Untitled-design-45-768x416.png 768w\" sizes=\"auto, (max-width: 800px) 100vw, 800px\" \/><\/figure><\/div>\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>Electrons occupy <em>fixed energy levels<\/em> around the nucleus, designated as K, L, M, N, etc.<\/li>\n\n\n\n<li>These energy levels are numbered as n = 1, 2, 3, 4, and so on.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-160764ce8e6e4aad0cb6e6c6de2d9128\" style=\"color:#000060;background-color:#dfc816\"><strong>Bohr&#8217;s Model of the Atom<\/strong>:<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full is-resized\"><img loading=\"lazy\" decoding=\"async\" width=\"800\" height=\"433\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/Untitled-design-47.png\" alt=\"\" class=\"wp-image-15863\" style=\"width:421px;height:auto\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/Untitled-design-47.png 800w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/Untitled-design-47-300x162.png 300w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/Untitled-design-47-768x416.png 768w\" sizes=\"auto, (max-width: 800px) 100vw, 800px\" \/><\/figure><\/div>\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>Proposed by Niels Bohr, it suggests that electrons move in specific orbits with fixed energy.<\/li>\n\n\n\n<li>Electrons in lower orbits have less energy, while those in higher orbits have more energy.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-69e72ae82febd3bcbae66337bd62ef93\" style=\"color:#000060;background-color:#dfc816\"><strong>Maximum Number of Electrons in a Shell<\/strong>:<\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>The number of electrons each shell can hold is determined by the formula <strong>2n\u00b2<\/strong>, where &#8216;n&#8217; is the orbit number.\n<ul class=\"wp-block-list\">\n<li>K shell (n=1): 2 electrons<\/li>\n\n\n\n<li>L shell (n=2): 8 electrons<\/li>\n\n\n\n<li>M shell (n=3): 18 electrons<\/li>\n\n\n\n<li>N shell (n=4): 32 electrons<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-a28b6af2835a3fb8e1a711616579524d\" style=\"color:#000060;background-color:#dfc816\"><strong>Filling of Electrons in Shells<\/strong>:<\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>Electrons fill the shells in order of increasing energy (from K to N).<\/li>\n\n\n\n<li>Lower energy levels are filled first before moving to higher levels.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-d599aa1826b864aec327016c961caa9e\" style=\"color:#000060;background-color:#dfc816\"><strong>Octet Rule<\/strong>:<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full is-resized\"><img loading=\"lazy\" decoding=\"async\" width=\"800\" height=\"358\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-14.png\" alt=\"\" class=\"wp-image-15864\" style=\"width:476px;height:auto\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-14.png 800w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-14-300x134.png 300w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-14-768x344.png 768w\" sizes=\"auto, (max-width: 800px) 100vw, 800px\" \/><\/figure><\/div>\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>Atoms tend to fill their outermost shell to achieve a stable configuration with 8 electrons, similar to noble gases.<\/li>\n\n\n\n<li>Elements with less than 8 electrons in their outer shell are reactive.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-e069c8843754314304166b813f5cdb45\" style=\"color:#000060;background-color:#dfc816\"><strong>Valence Electrons<\/strong>:<\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>Electrons in the outermost shell are called <em>valence electrons<\/em>.<\/li>\n\n\n\n<li>These determine the chemical properties of an element.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-2e9bcf7d47b7a291017c325941d0ab6d\" style=\"color:#000060;background-color:#dfc816\"><strong>Example of Electron Distribution<\/strong>:<\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Carbon (Atomic number = 6)<\/strong>: 2 electrons in K shell, 4 electrons in L shell (2, 4)<\/li>\n\n\n\n<li><strong>Sodium (Atomic number = 11)<\/strong>: 2 electrons in K shell, 8 in L shell, 1 in M shell (2, 8, 1)<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-f69cd7a7dc79955e5edb55d44248182d\" style=\"color:#000060;background-color:#dfc816\"><strong>Stability and Reactivity<\/strong>:<\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>Atoms are most stable when their outermost shell is completely filled.<\/li>\n\n\n\n<li>Atoms with incomplete outer shells will gain, lose, or share electrons to achieve stability.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-color has-large-font-size\" style=\"color:#d90000\">Let&#8217;s practice!<\/p>\n\n\n\n<div class=\"wp-block-columns is-layout-flex wp-container-core-columns-is-layout-9d6595d7 wp-block-columns-is-layout-flex\">\n<div class=\"wp-block-column is-layout-flow wp-block-column-is-layout-flow\">\n<figure class=\"wp-block-image size-full\"><a href=\"https:\/\/wordwall.net\/play\/76016\/927\/500\"><img loading=\"lazy\" decoding=\"async\" width=\"500\" height=\"500\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/05\/Worksheet-1-2.png\" alt=\"\" class=\"wp-image-6765\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/05\/Worksheet-1-2.png 500w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/05\/Worksheet-1-2-300x300.png 300w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/05\/Worksheet-1-2-150x150.png 150w\" sizes=\"auto, (max-width: 500px) 100vw, 500px\" \/><\/a><\/figure>\n<\/div>\n\n\n\n<div class=\"wp-block-column is-layout-flow wp-block-column-is-layout-flow\">\n<figure class=\"wp-block-image size-full\"><a href=\"https:\/\/wordwall.net\/play\/76021\/604\/987\"><img loading=\"lazy\" decoding=\"async\" width=\"500\" height=\"500\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/05\/Worksheet-1-1-1.png\" alt=\"\" class=\"wp-image-6767\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/05\/Worksheet-1-1-1.png 500w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/05\/Worksheet-1-1-1-300x300.png 300w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/05\/Worksheet-1-1-1-150x150.png 150w\" sizes=\"auto, (max-width: 500px) 100vw, 500px\" \/><\/a><\/figure>\n<\/div>\n<\/div>\n","protected":false},"excerpt":{"rendered":"<p>How Are Electrons Distributed In Different Orbits? Key Notes: Structure of the Atom: Energy Levels (Shells): Bohr&#8217;s Model of the Atom: Maximum Number of Electrons in a Shell: Filling of Electrons in Shells: Octet Rule: Valence Electrons: Example of Electron Distribution: Stability and Reactivity: Let&#8217;s practice!<\/p>\n","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"om_disable_all_campaigns":false,"_monsterinsights_skip_tracking":false,"_monsterinsights_sitenote_active":false,"_monsterinsights_sitenote_note":"","_monsterinsights_sitenote_category":0,"footnotes":""},"class_list":["post-3655","page","type-page","status-publish","hentry","entry"],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages\/3655","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/comments?post=3655"}],"version-history":[{"count":19,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages\/3655\/revisions"}],"predecessor-version":[{"id":16347,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages\/3655\/revisions\/16347"}],"wp:attachment":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/media?parent=3655"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}