How many orbitals are in the following sublevels? <\/p>\n\n\n\n
a. ls <\/p>\n\n\n\n
b. 5s <\/p>\n\n\n\n
c. 4d <\/p>\n\n\n\n
d. 4f <\/p>\n\n\n\n
e. 7s <\/p>\n\n\n\n
f. 3p<\/p>\n\n\n\n
The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n Here is the number of orbitals in each of the sublevels:<\/p>\n\n\n\n a. 1s<\/strong>: There is 1 orbital<\/strong>. The “s” sublevel can only hold one orbital, which can accommodate two electrons.<\/p>\n\n\n\n b. 5s<\/strong>: There is 1 orbital<\/strong>. Like all “s” sublevels, the 5s can hold only one orbital, with a maximum of two electrons.<\/p>\n\n\n\n c. 4d<\/strong>: There are 5 orbitals<\/strong>. The “d” sublevel consists of five orbitals, each of which can hold two electrons, so it can hold up to ten electrons in total.<\/p>\n\n\n\n d. 4f<\/strong>: There are 7 orbitals<\/strong>. The “f” sublevel has seven orbitals, and each orbital can hold two electrons. Therefore, the 4f sublevel can hold up to 14 electrons.<\/p>\n\n\n\n e. 7s<\/strong>: There is 1 orbital<\/strong>. The “s” sublevel, regardless of the principal energy level, only has one orbital, so 7s contains just one orbital that can hold two electrons.<\/p>\n\n\n\n f. 3p<\/strong>: There are 3 orbitals<\/strong>. The “p” sublevel always contains three orbitals, and each orbital can hold up to two electrons. Hence, the 3p sublevel can hold up to six electrons.<\/p>\n\n\n\n The number of orbitals in a sublevel is determined by the type of orbital (s, p, d, or f) and the principal quantum number (n). The number of orbitals in each type of sublevel is fixed:<\/p>\n\n\n\n These orbitals are regions around the nucleus where there is a high probability of finding an electron. The sublevel is named according to the angular momentum quantum number (l):<\/p>\n\n\n\n Each orbital can hold two electrons with opposite spins, and the total number of electrons in a sublevel depends on the number of orbitals present.<\/p>\n","protected":false},"excerpt":{"rendered":" How many orbitals are in the following sublevels? a. ls b. 5s c. 4d d. 4f e. 7s f. 3p The correct answer and explanation is: Here is the number of orbitals in each of the sublevels: a. 1s: There is 1 orbital. The “s” sublevel can only hold one orbital, which can accommodate two […]<\/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-267570","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267570","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=267570"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267570\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=267570"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=267570"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=267570"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Explanation:<\/h3>\n\n\n\n
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