{"id":90209,"date":"2025-06-01T10:23:03","date_gmt":"2025-06-01T10:23:03","guid":{"rendered":"https:\/\/exam.pscnotes.com\/mcq\/?p=90209"},"modified":"2025-06-01T10:23:03","modified_gmt":"2025-06-01T10:23:03","slug":"the-number-of-angular-and-radial-nodes-for-4d-orbital-is-respectively-2","status":"publish","type":"post","link":"https:\/\/exam.pscnotes.com\/mcq\/the-number-of-angular-and-radial-nodes-for-4d-orbital-is-respectively-2\/","title":{"rendered":"The number of angular and radial nodes for 4d orbital is respectively"},"content":{"rendered":"

The number of angular and radial nodes for 4d orbital is respectively<\/p>\n

[amp_mcq option1=”2 and 1″ option2=”1 and 2″ option3=”3 and 1″ option4=”4 and 0″ correct=”option1″]<\/p>\n

\n
\n
This question was previously asked in<\/div>\n
UPSC CAPF – 2018<\/div>\n<\/div>\n
Download PDF<\/a>Attempt Online<\/a><\/div>\n<\/div>\n
\nThe correct answer is A) 2 and 1.
\n<\/section>\n
\nFor an atomic orbital described by the principal quantum number *n* and azimuthal (angular momentum) quantum number *l*:
\n– The number of angular nodes is equal to *l*.
\n– The total number of nodes is equal to *n* – 1.
\n– The number of radial nodes is the total number of nodes minus the number of angular nodes, i.e., (*n* – 1) – *l*.
\nFor a 4d orbital:
\n– Principal quantum number *n* = 4.
\n– For a d orbital, the azimuthal quantum number *l* = 2 (s=0, p=1, d=2, f=3).
\n– Number of angular nodes = *l* = 2.
\n– Number of radial nodes = (*n* – 1) – *l* = (4 – 1) – 2 = 3 – 2 = 1.
\nThe question asks for the number of angular and radial nodes *respectively*.
\n<\/section>\n
\nAngular nodes are surfaces where the probability of finding the electron is zero, and their shape depends on the value of *l* (e.g., for p orbitals, the angular node is a plane; for d orbitals, there are two angular nodes, often planes or conical surfaces). Radial nodes are spherical surfaces where the radial probability density (probability per unit volume) is zero. The number of radial nodes depends on both *n* and *l*.
\n<\/section>\n","protected":false},"excerpt":{"rendered":"

The number of angular and radial nodes for 4d orbital is respectively [amp_mcq option1=”2 and 1″ option2=”1 and 2″ option3=”3 and 1″ option4=”4 and 0″ correct=”option1″] This question was previously asked in UPSC CAPF – 2018 Download PDFAttempt Online The correct answer is A) 2 and 1. For an atomic orbital described by the principal … <\/p>\n

Detailed SolutionThe number of angular and radial nodes for 4d orbital is respectively<\/span><\/a><\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1085],"tags":[1114,1162,1096],"class_list":["post-90209","post","type-post","status-publish","format-standard","hentry","category-upsc-capf","tag-1114","tag-atomic-structure","tag-chemistry","no-featured-image-padding"],"yoast_head":"\nThe number of angular and radial nodes for 4d orbital is respectively<\/title>\n<meta name=\"description\" content=\"The correct answer is A) 2 and 1. For an atomic orbital described by the principal quantum number *n* and azimuthal (angular momentum) quantum number *l*: - The number of angular nodes is equal to *l*. - The total number of nodes is equal to *n* - 1. - The number of radial nodes is the total number of nodes minus the number of angular nodes, i.e., (*n* - 1) - *l*. For a 4d orbital: - Principal quantum number *n* = 4. - For a d orbital, the azimuthal quantum number *l* = 2 (s=0, p=1, d=2, f=3). - Number of angular nodes = *l* = 2. - Number of radial nodes = (*n* - 1) - *l* = (4 - 1) - 2 = 3 - 2 = 1. The question asks for the number of angular and radial nodes *respectively*.\" \/>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/exam.pscnotes.com\/mcq\/the-number-of-angular-and-radial-nodes-for-4d-orbital-is-respectively-2\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"The number of angular and radial nodes for 4d orbital is respectively\" \/>\n<meta property=\"og:description\" content=\"The correct answer is A) 2 and 1. For an atomic orbital described by the principal quantum number *n* and azimuthal (angular momentum) quantum number *l*: - The number of angular nodes is equal to *l*. - The total number of nodes is equal to *n* - 1. - The number of radial nodes is the total number of nodes minus the number of angular nodes, i.e., (*n* - 1) - *l*. For a 4d orbital: - Principal quantum number *n* = 4. - For a d orbital, the azimuthal quantum number *l* = 2 (s=0, p=1, d=2, f=3). - Number of angular nodes = *l* = 2. - Number of radial nodes = (*n* - 1) - *l* = (4 - 1) - 2 = 3 - 2 = 1. The question asks for the number of angular and radial nodes *respectively*.\" \/>\n<meta property=\"og:url\" content=\"https:\/\/exam.pscnotes.com\/mcq\/the-number-of-angular-and-radial-nodes-for-4d-orbital-is-respectively-2\/\" \/>\n<meta property=\"og:site_name\" content=\"MCQ and Quiz for Exams\" \/>\n<meta property=\"article:published_time\" content=\"2025-06-01T10:23:03+00:00\" \/>\n<meta name=\"author\" content=\"rawan239\" \/>\n<meta name=\"twitter:card\" content=\"summary_large_image\" \/>\n<meta name=\"twitter:label1\" content=\"Written by\" \/>\n\t<meta name=\"twitter:data1\" content=\"rawan239\" \/>\n\t<meta name=\"twitter:label2\" content=\"Est. reading time\" \/>\n\t<meta name=\"twitter:data2\" content=\"1 minute\" \/>\n<!-- \/ Yoast SEO Premium plugin. -->","yoast_head_json":{"title":"The number of angular and radial nodes for 4d orbital is respectively","description":"The correct answer is A) 2 and 1. For an atomic orbital described by the principal quantum number *n* and azimuthal (angular momentum) quantum number *l*: - The number of angular nodes is equal to *l*. - The total number of nodes is equal to *n* - 1. - The number of radial nodes is the total number of nodes minus the number of angular nodes, i.e., (*n* - 1) - *l*. For a 4d orbital: - Principal quantum number *n* = 4. - For a d orbital, the azimuthal quantum number *l* = 2 (s=0, p=1, d=2, f=3). - Number of angular nodes = *l* = 2. - Number of radial nodes = (*n* - 1) - *l* = (4 - 1) - 2 = 3 - 2 = 1. The question asks for the number of angular and radial nodes *respectively*.","robots":{"index":"index","follow":"follow","max-snippet":"max-snippet:-1","max-image-preview":"max-image-preview:large","max-video-preview":"max-video-preview:-1"},"canonical":"https:\/\/exam.pscnotes.com\/mcq\/the-number-of-angular-and-radial-nodes-for-4d-orbital-is-respectively-2\/","og_locale":"en_US","og_type":"article","og_title":"The number of angular and radial nodes for 4d orbital is respectively","og_description":"The correct answer is A) 2 and 1. For an atomic orbital described by the principal quantum number *n* and azimuthal (angular momentum) quantum number *l*: - The number of angular nodes is equal to *l*. - The total number of nodes is equal to *n* - 1. - The number of radial nodes is the total number of nodes minus the number of angular nodes, i.e., (*n* - 1) - *l*. For a 4d orbital: - Principal quantum number *n* = 4. - For a d orbital, the azimuthal quantum number *l* = 2 (s=0, p=1, d=2, f=3). - Number of angular nodes = *l* = 2. - Number of radial nodes = (*n* - 1) - *l* = (4 - 1) - 2 = 3 - 2 = 1. The question asks for the number of angular and radial nodes *respectively*.","og_url":"https:\/\/exam.pscnotes.com\/mcq\/the-number-of-angular-and-radial-nodes-for-4d-orbital-is-respectively-2\/","og_site_name":"MCQ and Quiz for Exams","article_published_time":"2025-06-01T10:23:03+00:00","author":"rawan239","twitter_card":"summary_large_image","twitter_misc":{"Written by":"rawan239","Est. reading time":"1 minute"},"schema":{"@context":"https:\/\/schema.org","@graph":[{"@type":"WebPage","@id":"https:\/\/exam.pscnotes.com\/mcq\/the-number-of-angular-and-radial-nodes-for-4d-orbital-is-respectively-2\/","url":"https:\/\/exam.pscnotes.com\/mcq\/the-number-of-angular-and-radial-nodes-for-4d-orbital-is-respectively-2\/","name":"The number of angular and radial nodes for 4d orbital is respectively","isPartOf":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#website"},"datePublished":"2025-06-01T10:23:03+00:00","dateModified":"2025-06-01T10:23:03+00:00","author":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/5807dafeb27d2ec82344d6cbd6c3d209"},"description":"The correct answer is A) 2 and 1. For an atomic orbital described by the principal quantum number *n* and azimuthal (angular momentum) quantum number *l*: - The number of angular nodes is equal to *l*. - The total number of nodes is equal to *n* - 1. - The number of radial nodes is the total number of nodes minus the number of angular nodes, i.e., (*n* - 1) - *l*. For a 4d orbital: - Principal quantum number *n* = 4. - For a d orbital, the azimuthal quantum number *l* = 2 (s=0, p=1, d=2, f=3). - Number of angular nodes = *l* = 2. - Number of radial nodes = (*n* - 1) - *l* = (4 - 1) - 2 = 3 - 2 = 1. The question asks for the number of angular and radial nodes *respectively*.","breadcrumb":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/the-number-of-angular-and-radial-nodes-for-4d-orbital-is-respectively-2\/#breadcrumb"},"inLanguage":"en-US","potentialAction":[{"@type":"ReadAction","target":["https:\/\/exam.pscnotes.com\/mcq\/the-number-of-angular-and-radial-nodes-for-4d-orbital-is-respectively-2\/"]}]},{"@type":"BreadcrumbList","@id":"https:\/\/exam.pscnotes.com\/mcq\/the-number-of-angular-and-radial-nodes-for-4d-orbital-is-respectively-2\/#breadcrumb","itemListElement":[{"@type":"ListItem","position":1,"name":"Home","item":"https:\/\/exam.pscnotes.com\/mcq\/"},{"@type":"ListItem","position":2,"name":"UPSC CAPF","item":"https:\/\/exam.pscnotes.com\/mcq\/category\/upsc-capf\/"},{"@type":"ListItem","position":3,"name":"The number of angular and radial nodes for 4d orbital is respectively"}]},{"@type":"WebSite","@id":"https:\/\/exam.pscnotes.com\/mcq\/#website","url":"https:\/\/exam.pscnotes.com\/mcq\/","name":"MCQ and Quiz for Exams","description":"","potentialAction":[{"@type":"SearchAction","target":{"@type":"EntryPoint","urlTemplate":"https:\/\/exam.pscnotes.com\/mcq\/?s={search_term_string}"},"query-input":"required name=search_term_string"}],"inLanguage":"en-US"},{"@type":"Person","@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/5807dafeb27d2ec82344d6cbd6c3d209","name":"rawan239","image":{"@type":"ImageObject","inLanguage":"en-US","@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/image\/","url":"https:\/\/secure.gravatar.com\/avatar\/761a7274f9cce048fa5b921221e7934820d74514df93ef195a9d22af0c1c9001?s=96&d=mm&r=g","contentUrl":"https:\/\/secure.gravatar.com\/avatar\/761a7274f9cce048fa5b921221e7934820d74514df93ef195a9d22af0c1c9001?s=96&d=mm&r=g","caption":"rawan239"},"sameAs":["https:\/\/exam.pscnotes.com"],"url":"https:\/\/exam.pscnotes.com\/mcq\/author\/rawan239\/"}]}},"amp_enabled":true,"_links":{"self":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts\/90209","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/comments?post=90209"}],"version-history":[{"count":0,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts\/90209\/revisions"}],"wp:attachment":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/media?parent=90209"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/categories?post=90209"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/tags?post=90209"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}