{"id":87111,"date":"2025-06-01T04:29:14","date_gmt":"2025-06-01T04:29:14","guid":{"rendered":"https:\/\/exam.pscnotes.com\/mcq\/?p=87111"},"modified":"2025-06-01T04:29:14","modified_gmt":"2025-06-01T04:29:14","slug":"which-one-among-the-following-is-the-correct-arrangement-of-molecules","status":"publish","type":"post","link":"https:\/\/exam.pscnotes.com\/mcq\/which-one-among-the-following-is-the-correct-arrangement-of-molecules\/","title":{"rendered":"Which one among the following is the correct arrangement of molecules"},"content":{"rendered":"

Which one among the following is the correct arrangement of molecules in increasing order of their dipole moment ?<\/p>\n

[amp_mcq option1=”NF\u2083 < NH\u2083 < BF\u2083\" option2=\"BF\u2083 < NH\u2083 < NF\u2083\" option3=\"BF\u2083 < NF\u2083 < NH\u2083\" option4=\"NF\u2083 < BF\u2083 < NH\u2083\" correct=\"option3\"]\n\n\n\n

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This question was previously asked in<\/div>\n
UPSC Geoscientist – 2024<\/div>\n<\/div>\n
Download PDF<\/a>Attempt Online<\/a><\/div>\n<\/div>\n
\nThe correct arrangement of molecules in increasing order of their dipole moment is BF\u2083 < NF\u2083 < NH\u2083.\n<\/section>\n
\nDipole moment is a measure of the net polarity of a molecule, resulting from the vector sum of individual bond dipoles and contributions from lone pairs.
\n– **BF\u2083**: Boron trifluoride has a central Boron atom bonded to three Fluorine atoms. Boron is sp\u00b2 hybridized, and the molecule is trigonal planar. The B-F bonds are polar, but the three bond dipoles are symmetrically arranged at 120\u00b0 to each other in a plane. Their vector sum is zero, so BF\u2083 has a zero net dipole moment.
\n– **NF\u2083**: Nitrogen trifluoride has a central Nitrogen atom bonded to three Fluorine atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-F bonds are polar (F is more electronegative). The bond dipoles point towards the F atoms, away from N. The lone pair contributes a dipole moment pointing away from N. The N-F bond dipoles and the lone pair dipole are in opposite directions along the molecular axis, partially canceling each other. This results in a small net dipole moment for NF\u2083.
\n– **NH\u2083**: Ammonia has a central Nitrogen atom bonded to three Hydrogen atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-H bonds are polar (N is more electronegative). The bond dipoles point towards the N atom. The lone pair contributes a dipole moment pointing away from N. Both the N-H bond dipoles and the lone pair dipole point in the same general direction (upwards along the molecular axis), reinforcing each other. This results in a significant net dipole moment for NH\u2083.
\nComparing NF\u2083 and NH\u2083, the dipole moment of NH\u2083 is significantly larger than that of NF\u2083.
\nTherefore, the order of increasing dipole moment is BF\u2083 (0) < NF\u2083 < NH\u2083.\n<\/section>\n
\nTypical dipole moment values (in Debye): BF\u2083 \u2248 0 D, NF\u2083 \u2248 0.23 D, NH\u2083 \u2248 1.47 D. The difference between NH\u2083 and NF\u2083 highlights the importance of the direction of bond dipoles relative to the lone pair dipole in determining the net molecular dipole moment.
\n<\/section>\n","protected":false},"excerpt":{"rendered":"

Which one among the following is the correct arrangement of molecules in increasing order of their dipole moment ? [amp_mcq option1=”NF\u2083 < NH\u2083 < BF\u2083\" option2=\"BF\u2083 < NH\u2083 < NF\u2083\" option3=\"BF\u2083 < NF\u2083 < NH\u2083\" option4=\"NF\u2083 < BF\u2083 < NH\u2083\" correct=\"option3\"] This question was previously asked in UPSC Geoscientist – 2024 Download PDFAttempt Online The ... \n\n

Detailed SolutionWhich one among the following is the correct arrangement of molecules<\/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":[1091],"tags":[1103,1162,1096],"class_list":["post-87111","post","type-post","status-publish","format-standard","hentry","category-upsc-geoscientist","tag-1103","tag-atomic-structure","tag-chemistry","no-featured-image-padding"],"yoast_head":"\nWhich one among the following is the correct arrangement of molecules<\/title>\n<meta name=\"description\" content=\"The correct arrangement of molecules in increasing order of their dipole moment is BF\u2083 < NF\u2083 < NH\u2083. Dipole moment is a measure of the net polarity of a molecule, resulting from the vector sum of individual bond dipoles and contributions from lone pairs. - **BF\u2083**: Boron trifluoride has a central Boron atom bonded to three Fluorine atoms. Boron is sp\u00b2 hybridized, and the molecule is trigonal planar. The B-F bonds are polar, but the three bond dipoles are symmetrically arranged at 120\u00b0 to each other in a plane. Their vector sum is zero, so BF\u2083 has a zero net dipole moment. - **NF\u2083**: Nitrogen trifluoride has a central Nitrogen atom bonded to three Fluorine atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-F bonds are polar (F is more electronegative). The bond dipoles point towards the F atoms, away from N. The lone pair contributes a dipole moment pointing away from N. The N-F bond dipoles and the lone pair dipole are in opposite directions along the molecular axis, partially canceling each other. This results in a small net dipole moment for NF\u2083. - **NH\u2083**: Ammonia has a central Nitrogen atom bonded to three Hydrogen atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-H bonds are polar (N is more electronegative). The bond dipoles point towards the N atom. The lone pair contributes a dipole moment pointing away from N. Both the N-H bond dipoles and the lone pair dipole point in the same general direction (upwards along the molecular axis), reinforcing each other. This results in a significant net dipole moment for NH\u2083. Comparing NF\u2083 and NH\u2083, the dipole moment of NH\u2083 is significantly larger than that of NF\u2083. Therefore, the order of increasing dipole moment is BF\u2083 (0) < NF\u2083 < NH\u2083.\" \/>\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\/which-one-among-the-following-is-the-correct-arrangement-of-molecules\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Which one among the following is the correct arrangement of molecules\" \/>\n<meta property=\"og:description\" content=\"The correct arrangement of molecules in increasing order of their dipole moment is BF\u2083 < NF\u2083 < NH\u2083. Dipole moment is a measure of the net polarity of a molecule, resulting from the vector sum of individual bond dipoles and contributions from lone pairs. - **BF\u2083**: Boron trifluoride has a central Boron atom bonded to three Fluorine atoms. Boron is sp\u00b2 hybridized, and the molecule is trigonal planar. The B-F bonds are polar, but the three bond dipoles are symmetrically arranged at 120\u00b0 to each other in a plane. Their vector sum is zero, so BF\u2083 has a zero net dipole moment. - **NF\u2083**: Nitrogen trifluoride has a central Nitrogen atom bonded to three Fluorine atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-F bonds are polar (F is more electronegative). The bond dipoles point towards the F atoms, away from N. The lone pair contributes a dipole moment pointing away from N. The N-F bond dipoles and the lone pair dipole are in opposite directions along the molecular axis, partially canceling each other. This results in a small net dipole moment for NF\u2083. - **NH\u2083**: Ammonia has a central Nitrogen atom bonded to three Hydrogen atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-H bonds are polar (N is more electronegative). The bond dipoles point towards the N atom. The lone pair contributes a dipole moment pointing away from N. Both the N-H bond dipoles and the lone pair dipole point in the same general direction (upwards along the molecular axis), reinforcing each other. This results in a significant net dipole moment for NH\u2083. Comparing NF\u2083 and NH\u2083, the dipole moment of NH\u2083 is significantly larger than that of NF\u2083. Therefore, the order of increasing dipole moment is BF\u2083 (0) < NF\u2083 < NH\u2083.\" \/>\n<meta property=\"og:url\" content=\"https:\/\/exam.pscnotes.com\/mcq\/which-one-among-the-following-is-the-correct-arrangement-of-molecules\/\" \/>\n<meta property=\"og:site_name\" content=\"MCQ and Quiz for Exams\" \/>\n<meta property=\"article:published_time\" content=\"2025-06-01T04:29:14+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=\"2 minutes\" \/>\n<!-- \/ Yoast SEO Premium plugin. -->","yoast_head_json":{"title":"Which one among the following is the correct arrangement of molecules","description":"The correct arrangement of molecules in increasing order of their dipole moment is BF\u2083 < NF\u2083 < NH\u2083. Dipole moment is a measure of the net polarity of a molecule, resulting from the vector sum of individual bond dipoles and contributions from lone pairs. - **BF\u2083**: Boron trifluoride has a central Boron atom bonded to three Fluorine atoms. Boron is sp\u00b2 hybridized, and the molecule is trigonal planar. The B-F bonds are polar, but the three bond dipoles are symmetrically arranged at 120\u00b0 to each other in a plane. Their vector sum is zero, so BF\u2083 has a zero net dipole moment. - **NF\u2083**: Nitrogen trifluoride has a central Nitrogen atom bonded to three Fluorine atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-F bonds are polar (F is more electronegative). The bond dipoles point towards the F atoms, away from N. The lone pair contributes a dipole moment pointing away from N. The N-F bond dipoles and the lone pair dipole are in opposite directions along the molecular axis, partially canceling each other. This results in a small net dipole moment for NF\u2083. - **NH\u2083**: Ammonia has a central Nitrogen atom bonded to three Hydrogen atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-H bonds are polar (N is more electronegative). The bond dipoles point towards the N atom. The lone pair contributes a dipole moment pointing away from N. Both the N-H bond dipoles and the lone pair dipole point in the same general direction (upwards along the molecular axis), reinforcing each other. This results in a significant net dipole moment for NH\u2083. Comparing NF\u2083 and NH\u2083, the dipole moment of NH\u2083 is significantly larger than that of NF\u2083. Therefore, the order of increasing dipole moment is BF\u2083 (0) < NF\u2083 < NH\u2083.","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\/which-one-among-the-following-is-the-correct-arrangement-of-molecules\/","og_locale":"en_US","og_type":"article","og_title":"Which one among the following is the correct arrangement of molecules","og_description":"The correct arrangement of molecules in increasing order of their dipole moment is BF\u2083 < NF\u2083 < NH\u2083. Dipole moment is a measure of the net polarity of a molecule, resulting from the vector sum of individual bond dipoles and contributions from lone pairs. - **BF\u2083**: Boron trifluoride has a central Boron atom bonded to three Fluorine atoms. Boron is sp\u00b2 hybridized, and the molecule is trigonal planar. The B-F bonds are polar, but the three bond dipoles are symmetrically arranged at 120\u00b0 to each other in a plane. Their vector sum is zero, so BF\u2083 has a zero net dipole moment. - **NF\u2083**: Nitrogen trifluoride has a central Nitrogen atom bonded to three Fluorine atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-F bonds are polar (F is more electronegative). The bond dipoles point towards the F atoms, away from N. The lone pair contributes a dipole moment pointing away from N. The N-F bond dipoles and the lone pair dipole are in opposite directions along the molecular axis, partially canceling each other. This results in a small net dipole moment for NF\u2083. - **NH\u2083**: Ammonia has a central Nitrogen atom bonded to three Hydrogen atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-H bonds are polar (N is more electronegative). The bond dipoles point towards the N atom. The lone pair contributes a dipole moment pointing away from N. Both the N-H bond dipoles and the lone pair dipole point in the same general direction (upwards along the molecular axis), reinforcing each other. This results in a significant net dipole moment for NH\u2083. Comparing NF\u2083 and NH\u2083, the dipole moment of NH\u2083 is significantly larger than that of NF\u2083. Therefore, the order of increasing dipole moment is BF\u2083 (0) < NF\u2083 < NH\u2083.","og_url":"https:\/\/exam.pscnotes.com\/mcq\/which-one-among-the-following-is-the-correct-arrangement-of-molecules\/","og_site_name":"MCQ and Quiz for Exams","article_published_time":"2025-06-01T04:29:14+00:00","author":"rawan239","twitter_card":"summary_large_image","twitter_misc":{"Written by":"rawan239","Est. reading time":"2 minutes"},"schema":{"@context":"https:\/\/schema.org","@graph":[{"@type":"WebPage","@id":"https:\/\/exam.pscnotes.com\/mcq\/which-one-among-the-following-is-the-correct-arrangement-of-molecules\/","url":"https:\/\/exam.pscnotes.com\/mcq\/which-one-among-the-following-is-the-correct-arrangement-of-molecules\/","name":"Which one among the following is the correct arrangement of molecules","isPartOf":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#website"},"datePublished":"2025-06-01T04:29:14+00:00","dateModified":"2025-06-01T04:29:14+00:00","author":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/5807dafeb27d2ec82344d6cbd6c3d209"},"description":"The correct arrangement of molecules in increasing order of their dipole moment is BF\u2083 < NF\u2083 < NH\u2083. Dipole moment is a measure of the net polarity of a molecule, resulting from the vector sum of individual bond dipoles and contributions from lone pairs. - **BF\u2083**: Boron trifluoride has a central Boron atom bonded to three Fluorine atoms. Boron is sp\u00b2 hybridized, and the molecule is trigonal planar. The B-F bonds are polar, but the three bond dipoles are symmetrically arranged at 120\u00b0 to each other in a plane. Their vector sum is zero, so BF\u2083 has a zero net dipole moment. - **NF\u2083**: Nitrogen trifluoride has a central Nitrogen atom bonded to three Fluorine atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-F bonds are polar (F is more electronegative). The bond dipoles point towards the F atoms, away from N. The lone pair contributes a dipole moment pointing away from N. The N-F bond dipoles and the lone pair dipole are in opposite directions along the molecular axis, partially canceling each other. This results in a small net dipole moment for NF\u2083. - **NH\u2083**: Ammonia has a central Nitrogen atom bonded to three Hydrogen atoms and one lone pair. Nitrogen is sp\u00b3 hybridized, and the molecule is trigonal pyramidal. N-H bonds are polar (N is more electronegative). The bond dipoles point towards the N atom. The lone pair contributes a dipole moment pointing away from N. Both the N-H bond dipoles and the lone pair dipole point in the same general direction (upwards along the molecular axis), reinforcing each other. This results in a significant net dipole moment for NH\u2083. Comparing NF\u2083 and NH\u2083, the dipole moment of NH\u2083 is significantly larger than that of NF\u2083. Therefore, the order of increasing dipole moment is BF\u2083 (0) < NF\u2083 < NH\u2083.","breadcrumb":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/which-one-among-the-following-is-the-correct-arrangement-of-molecules\/#breadcrumb"},"inLanguage":"en-US","potentialAction":[{"@type":"ReadAction","target":["https:\/\/exam.pscnotes.com\/mcq\/which-one-among-the-following-is-the-correct-arrangement-of-molecules\/"]}]},{"@type":"BreadcrumbList","@id":"https:\/\/exam.pscnotes.com\/mcq\/which-one-among-the-following-is-the-correct-arrangement-of-molecules\/#breadcrumb","itemListElement":[{"@type":"ListItem","position":1,"name":"Home","item":"https:\/\/exam.pscnotes.com\/mcq\/"},{"@type":"ListItem","position":2,"name":"UPSC Geoscientist","item":"https:\/\/exam.pscnotes.com\/mcq\/category\/upsc-geoscientist\/"},{"@type":"ListItem","position":3,"name":"Which one among the following is the correct arrangement of molecules"}]},{"@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\/87111","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=87111"}],"version-history":[{"count":0,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts\/87111\/revisions"}],"wp:attachment":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/media?parent=87111"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/categories?post=87111"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/tags?post=87111"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}