{"id":86166,"date":"2025-06-01T03:39:17","date_gmt":"2025-06-01T03:39:17","guid":{"rendered":"https:\/\/exam.pscnotes.com\/mcq\/?p=86166"},"modified":"2025-06-01T03:39:17","modified_gmt":"2025-06-01T03:39:17","slug":"which-of-the-following-carbon-allotropes-is-are-good-conductors-of-e","status":"publish","type":"post","link":"https:\/\/exam.pscnotes.com\/mcq\/which-of-the-following-carbon-allotropes-is-are-good-conductors-of-e\/","title":{"rendered":"Which of the following carbon allotropes is\/are good conductor(s) of e"},"content":{"rendered":"<p>Which of the following carbon allotropes is\/are good conductor(s) of electricity ?<\/p>\n<ul>\n<li>1. Diamond<\/li>\n<li>2. Graphite<\/li>\n<li>3. Fullerene<\/li>\n<\/ul>\n<p>Select the correct answer using the code given below :<\/p>\n<p>[amp_mcq option1=&#8221;1 only&#8221; option2=&#8221;1 and 2 only&#8221; option3=&#8221;2 only&#8221; option4=&#8221;1 and 3 only&#8221; correct=&#8221;option3&#8243;]<\/p>\n<div class=\"psc-box-pyq-exam-year-detail\">\n<div class=\"pyq-exam\">\n<div class=\"psc-heading\">This question was previously asked in<\/div>\n<div class=\"psc-title line-ellipsis\">UPSC CDS-2 &#8211; 2021<\/div>\n<\/div>\n<div class=\"pyq-exam-psc-buttons\"><a href=\"\/pyq\/pyq-upsc-cds-2-2021.pdf\" target=\"_blank\" class=\"psc-pdf-button\" rel=\"noopener\">Download PDF<\/a><a href=\"\/pyq-upsc-cds-2-2021\" target=\"_blank\" class=\"psc-attempt-button\" rel=\"noopener\">Attempt Online<\/a><\/div>\n<\/div>\n<section id=\"pyq-correct-answer\">\n1. Diamond: In diamond, each carbon atom is covalently bonded to four other carbon atoms in a rigid tetrahedral structure. All valence electrons are involved in strong covalent bonds, and there are no free electrons. Hence, diamond is a very poor conductor of electricity (an insulator).<br \/>\n2. Graphite: In graphite, carbon atoms are arranged in layers of hexagonal rings. Within each layer, atoms are covalently bonded (sp2 hybridisation). Each carbon atom has one valence electron that is not involved in sigma bonding and is delocalized across the layers. These delocalized electrons are free to move, making graphite a good conductor of electricity.<br \/>\n3. Fullerene: Fullerenes, such as C60, have carbon atoms arranged in spherical or cage-like structures involving pentagons and hexagons. The bonding is predominantly sp2 hybridisation with some delocalized electrons. However, in their pure form, most fullerenes are semiconductors or insulators due to the localisation of the pi electrons compared to graphite. While some doped fullerenes can become conductors or even superconductors, pure fullerenes are not considered good conductors in the same way as graphite.<br \/>\nTherefore, among the listed common allotropes, only graphite is a good conductor of electricity.<br \/>\n<\/section>\n<section id=\"pyq-key-points\">\n&#8211; Electrical conductivity in carbon allotropes depends on the presence of delocalized or free electrons.<br \/>\n&#8211; Diamond has no free electrons.<br \/>\n&#8211; Graphite has delocalized pi electrons allowing it to conduct electricity.<br \/>\n&#8211; Pure fullerenes are typically semiconductors or insulators.<br \/>\n<\/section>\n<section id=\"pyq-additional-information\">\nThe differences in electrical conductivity (and other properties like hardness) among carbon allotropes arise from the different ways carbon atoms are bonded and arranged in their crystal structures. Graphite&#8217;s layered structure and delocalized electrons make it suitable for applications like electrodes and lubricants. Diamond&#8217;s strong 3D network makes it extremely hard.<br \/>\n<\/section>\n","protected":false},"excerpt":{"rendered":"<p>Which of the following carbon allotropes is\/are good conductor(s) of electricity ? 1. Diamond 2. Graphite 3. Fullerene Select the correct answer using the code given below : [amp_mcq option1=&#8221;1 only&#8221; option2=&#8221;1 and 2 only&#8221; option3=&#8221;2 only&#8221; option4=&#8221;1 and 3 only&#8221; correct=&#8221;option3&#8243;] This question was previously asked in UPSC CDS-2 &#8211; 2021 Download PDFAttempt Online &#8230; <\/p>\n<p class=\"read-more-container\"><a title=\"Which of the following carbon allotropes is\/are good conductor(s) of e\" class=\"read-more button\" href=\"https:\/\/exam.pscnotes.com\/mcq\/which-of-the-following-carbon-allotropes-is-are-good-conductors-of-e\/#more-86166\">Detailed Solution<span class=\"screen-reader-text\">Which of the following carbon allotropes is\/are good conductor(s) of e<\/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":[1088],"tags":[1110,1368,1096],"class_list":["post-86166","post","type-post","status-publish","format-standard","hentry","category-upsc-cds-2","tag-1110","tag-carbon-and-its-various-forms","tag-chemistry","no-featured-image-padding"],"yoast_head":"<!-- This site is optimized with the Yoast SEO Premium plugin v22.2 (Yoast SEO v23.3) - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>Which of the following carbon allotropes is\/are good conductor(s) of e<\/title>\n<meta name=\"description\" content=\"1. Diamond: In diamond, each carbon atom is covalently bonded to four other carbon atoms in a rigid tetrahedral structure. All valence electrons are involved in strong covalent bonds, and there are no free electrons. Hence, diamond is a very poor conductor of electricity (an insulator). 2. Graphite: In graphite, carbon atoms are arranged in layers of hexagonal rings. Within each layer, atoms are covalently bonded (sp2 hybridisation). Each carbon atom has one valence electron that is not involved in sigma bonding and is delocalized across the layers. These delocalized electrons are free to move, making graphite a good conductor of electricity. 3. Fullerene: Fullerenes, such as C60, have carbon atoms arranged in spherical or cage-like structures involving pentagons and hexagons. The bonding is predominantly sp2 hybridisation with some delocalized electrons. However, in their pure form, most fullerenes are semiconductors or insulators due to the localisation of the pi electrons compared to graphite. While some doped fullerenes can become conductors or even superconductors, pure fullerenes are not considered good conductors in the same way as graphite. Therefore, among the listed common allotropes, only graphite is a good conductor of electricity. - Electrical conductivity in carbon allotropes depends on the presence of delocalized or free electrons. - Diamond has no free electrons. - Graphite has delocalized pi electrons allowing it to conduct electricity. - Pure fullerenes are typically semiconductors or insulators.\" \/>\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-of-the-following-carbon-allotropes-is-are-good-conductors-of-e\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Which of the following carbon allotropes is\/are good conductor(s) of e\" \/>\n<meta property=\"og:description\" content=\"1. Diamond: In diamond, each carbon atom is covalently bonded to four other carbon atoms in a rigid tetrahedral structure. All valence electrons are involved in strong covalent bonds, and there are no free electrons. Hence, diamond is a very poor conductor of electricity (an insulator). 2. Graphite: In graphite, carbon atoms are arranged in layers of hexagonal rings. Within each layer, atoms are covalently bonded (sp2 hybridisation). Each carbon atom has one valence electron that is not involved in sigma bonding and is delocalized across the layers. These delocalized electrons are free to move, making graphite a good conductor of electricity. 3. Fullerene: Fullerenes, such as C60, have carbon atoms arranged in spherical or cage-like structures involving pentagons and hexagons. The bonding is predominantly sp2 hybridisation with some delocalized electrons. However, in their pure form, most fullerenes are semiconductors or insulators due to the localisation of the pi electrons compared to graphite. While some doped fullerenes can become conductors or even superconductors, pure fullerenes are not considered good conductors in the same way as graphite. Therefore, among the listed common allotropes, only graphite is a good conductor of electricity. - Electrical conductivity in carbon allotropes depends on the presence of delocalized or free electrons. - Diamond has no free electrons. - Graphite has delocalized pi electrons allowing it to conduct electricity. - Pure fullerenes are typically semiconductors or insulators.\" \/>\n<meta property=\"og:url\" content=\"https:\/\/exam.pscnotes.com\/mcq\/which-of-the-following-carbon-allotropes-is-are-good-conductors-of-e\/\" \/>\n<meta property=\"og:site_name\" content=\"MCQ and Quiz for Exams\" \/>\n<meta property=\"article:published_time\" content=\"2025-06-01T03:39:17+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 of the following carbon allotropes is\/are good conductor(s) of e","description":"1. Diamond: In diamond, each carbon atom is covalently bonded to four other carbon atoms in a rigid tetrahedral structure. All valence electrons are involved in strong covalent bonds, and there are no free electrons. Hence, diamond is a very poor conductor of electricity (an insulator). 2. Graphite: In graphite, carbon atoms are arranged in layers of hexagonal rings. Within each layer, atoms are covalently bonded (sp2 hybridisation). Each carbon atom has one valence electron that is not involved in sigma bonding and is delocalized across the layers. These delocalized electrons are free to move, making graphite a good conductor of electricity. 3. Fullerene: Fullerenes, such as C60, have carbon atoms arranged in spherical or cage-like structures involving pentagons and hexagons. The bonding is predominantly sp2 hybridisation with some delocalized electrons. However, in their pure form, most fullerenes are semiconductors or insulators due to the localisation of the pi electrons compared to graphite. While some doped fullerenes can become conductors or even superconductors, pure fullerenes are not considered good conductors in the same way as graphite. Therefore, among the listed common allotropes, only graphite is a good conductor of electricity. - Electrical conductivity in carbon allotropes depends on the presence of delocalized or free electrons. - Diamond has no free electrons. - Graphite has delocalized pi electrons allowing it to conduct electricity. - Pure fullerenes are typically semiconductors or insulators.","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-of-the-following-carbon-allotropes-is-are-good-conductors-of-e\/","og_locale":"en_US","og_type":"article","og_title":"Which of the following carbon allotropes is\/are good conductor(s) of e","og_description":"1. Diamond: In diamond, each carbon atom is covalently bonded to four other carbon atoms in a rigid tetrahedral structure. All valence electrons are involved in strong covalent bonds, and there are no free electrons. Hence, diamond is a very poor conductor of electricity (an insulator). 2. Graphite: In graphite, carbon atoms are arranged in layers of hexagonal rings. Within each layer, atoms are covalently bonded (sp2 hybridisation). Each carbon atom has one valence electron that is not involved in sigma bonding and is delocalized across the layers. These delocalized electrons are free to move, making graphite a good conductor of electricity. 3. Fullerene: Fullerenes, such as C60, have carbon atoms arranged in spherical or cage-like structures involving pentagons and hexagons. The bonding is predominantly sp2 hybridisation with some delocalized electrons. However, in their pure form, most fullerenes are semiconductors or insulators due to the localisation of the pi electrons compared to graphite. While some doped fullerenes can become conductors or even superconductors, pure fullerenes are not considered good conductors in the same way as graphite. Therefore, among the listed common allotropes, only graphite is a good conductor of electricity. - Electrical conductivity in carbon allotropes depends on the presence of delocalized or free electrons. - Diamond has no free electrons. - Graphite has delocalized pi electrons allowing it to conduct electricity. - Pure fullerenes are typically semiconductors or insulators.","og_url":"https:\/\/exam.pscnotes.com\/mcq\/which-of-the-following-carbon-allotropes-is-are-good-conductors-of-e\/","og_site_name":"MCQ and Quiz for Exams","article_published_time":"2025-06-01T03:39:17+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-of-the-following-carbon-allotropes-is-are-good-conductors-of-e\/","url":"https:\/\/exam.pscnotes.com\/mcq\/which-of-the-following-carbon-allotropes-is-are-good-conductors-of-e\/","name":"Which of the following carbon allotropes is\/are good conductor(s) of e","isPartOf":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#website"},"datePublished":"2025-06-01T03:39:17+00:00","dateModified":"2025-06-01T03:39:17+00:00","author":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/5807dafeb27d2ec82344d6cbd6c3d209"},"description":"1. Diamond: In diamond, each carbon atom is covalently bonded to four other carbon atoms in a rigid tetrahedral structure. All valence electrons are involved in strong covalent bonds, and there are no free electrons. Hence, diamond is a very poor conductor of electricity (an insulator). 2. Graphite: In graphite, carbon atoms are arranged in layers of hexagonal rings. Within each layer, atoms are covalently bonded (sp2 hybridisation). Each carbon atom has one valence electron that is not involved in sigma bonding and is delocalized across the layers. These delocalized electrons are free to move, making graphite a good conductor of electricity. 3. Fullerene: Fullerenes, such as C60, have carbon atoms arranged in spherical or cage-like structures involving pentagons and hexagons. The bonding is predominantly sp2 hybridisation with some delocalized electrons. However, in their pure form, most fullerenes are semiconductors or insulators due to the localisation of the pi electrons compared to graphite. While some doped fullerenes can become conductors or even superconductors, pure fullerenes are not considered good conductors in the same way as graphite. Therefore, among the listed common allotropes, only graphite is a good conductor of electricity. - Electrical conductivity in carbon allotropes depends on the presence of delocalized or free electrons. - Diamond has no free electrons. - Graphite has delocalized pi electrons allowing it to conduct electricity. - Pure fullerenes are typically semiconductors or insulators.","breadcrumb":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/which-of-the-following-carbon-allotropes-is-are-good-conductors-of-e\/#breadcrumb"},"inLanguage":"en-US","potentialAction":[{"@type":"ReadAction","target":["https:\/\/exam.pscnotes.com\/mcq\/which-of-the-following-carbon-allotropes-is-are-good-conductors-of-e\/"]}]},{"@type":"BreadcrumbList","@id":"https:\/\/exam.pscnotes.com\/mcq\/which-of-the-following-carbon-allotropes-is-are-good-conductors-of-e\/#breadcrumb","itemListElement":[{"@type":"ListItem","position":1,"name":"Home","item":"https:\/\/exam.pscnotes.com\/mcq\/"},{"@type":"ListItem","position":2,"name":"UPSC CDS-2","item":"https:\/\/exam.pscnotes.com\/mcq\/category\/upsc-cds-2\/"},{"@type":"ListItem","position":3,"name":"Which of the following carbon allotropes is\/are good conductor(s) of e"}]},{"@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\/86166","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=86166"}],"version-history":[{"count":0,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts\/86166\/revisions"}],"wp:attachment":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/media?parent=86166"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/categories?post=86166"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/tags?post=86166"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}