{"id":85824,"date":"2025-06-01T03:28:52","date_gmt":"2025-06-01T03:28:52","guid":{"rendered":"https:\/\/exam.pscnotes.com\/mcq\/?p=85824"},"modified":"2025-06-01T03:28:52","modified_gmt":"2025-06-01T03:28:52","slug":"which-one-of-the-following-is-not-true-for-the-form-of-carbon-know","status":"publish","type":"post","link":"https:\/\/exam.pscnotes.com\/mcq\/which-one-of-the-following-is-not-true-for-the-form-of-carbon-know\/","title":{"rendered":"Which one of the following is * not * true for the form of carbon know"},"content":{"rendered":"<p>Which one of the following is *<b>not<\/b>* true for the form of carbon known as diamond?<\/p>\n<p>[amp_mcq option1=&#8221;It is harder than graphite.&#8221; option2=&#8221;It contains the same percentage of carbon as graphite.&#8221; option3=&#8221;It is a better electric conductor than graphite.&#8221; option4=&#8221;It has different carbon to carbon distance in all directions.&#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; 2018<\/div>\n<\/div>\n<div class=\"pyq-exam-psc-buttons\"><a href=\"\/pyq\/pyq-upsc-cds-2-2018.pdf\" target=\"_blank\" class=\"psc-pdf-button\" rel=\"noopener\">Download PDF<\/a><a href=\"\/pyq-upsc-cds-2-2018\" target=\"_blank\" class=\"psc-attempt-button\" rel=\"noopener\">Attempt Online<\/a><\/div>\n<\/div>\n<section id=\"pyq-correct-answer\">\nOption C is the correct answer. Diamond is an electrical insulator, whereas graphite is a good electrical conductor.<br \/>\n<\/section>\n<section id=\"pyq-key-points\">\nDiamond and graphite are allotropes of carbon, meaning they are made solely of carbon atoms but arranged differently. This structural difference leads to vastly different properties. Diamond has a tetrahedral structure where each carbon is bonded to four others, with all valence electrons tightly held in covalent bonds, making it very hard and a poor conductor of electricity. Graphite has a layered structure where each carbon is bonded to three others, forming hexagonal rings within layers. One valence electron per carbon atom is delocalized and free to move across the layers, making graphite soft and a good conductor of electricity. Therefore, the statement that diamond is a better electric conductor than graphite is false. Options A and B are true: diamond is much harder than graphite, and both are pure carbon, hence containing the same percentage of carbon (100%). Option D is generally considered true in that the distances between non-bonded carbon atoms vary depending on their relative positions in the lattice, unlike the consistent bond length. However, the distinct electrical conductivity is the most prominent difference.<br \/>\n<\/section>\n<section id=\"pyq-additional-information\">\nDiamond is known for its extreme hardness, high refractive index, and high thermal conductivity (higher than most metals), but it is an electrical insulator. Graphite is soft, opaque, and a good electrical conductor, used in pencils and electrodes. This stark contrast in properties arises solely from the different arrangement of carbon atoms.<br \/>\n<\/section>\n","protected":false},"excerpt":{"rendered":"<p>Which one of the following is *not* true for the form of carbon known as diamond? [amp_mcq option1=&#8221;It is harder than graphite.&#8221; option2=&#8221;It contains the same percentage of carbon as graphite.&#8221; option3=&#8221;It is a better electric conductor than graphite.&#8221; option4=&#8221;It has different carbon to carbon distance in all directions.&#8221; correct=&#8221;option3&#8243;] This question was previously asked &#8230; <\/p>\n<p class=\"read-more-container\"><a title=\"Which one of the following is * not * true for the form of carbon know\" class=\"read-more button\" href=\"https:\/\/exam.pscnotes.com\/mcq\/which-one-of-the-following-is-not-true-for-the-form-of-carbon-know\/#more-85824\">Detailed Solution<span class=\"screen-reader-text\">Which one of the following is * not * true for the form of carbon know<\/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":[1114,1368,1096],"class_list":["post-85824","post","type-post","status-publish","format-standard","hentry","category-upsc-cds-2","tag-1114","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 one of the following is * not * true for the form of carbon know<\/title>\n<meta name=\"description\" content=\"Option C is the correct answer. Diamond is an electrical insulator, whereas graphite is a good electrical conductor. Diamond and graphite are allotropes of carbon, meaning they are made solely of carbon atoms but arranged differently. This structural difference leads to vastly different properties. Diamond has a tetrahedral structure where each carbon is bonded to four others, with all valence electrons tightly held in covalent bonds, making it very hard and a poor conductor of electricity. Graphite has a layered structure where each carbon is bonded to three others, forming hexagonal rings within layers. One valence electron per carbon atom is delocalized and free to move across the layers, making graphite soft and a good conductor of electricity. Therefore, the statement that diamond is a better electric conductor than graphite is false. Options A and B are true: diamond is much harder than graphite, and both are pure carbon, hence containing the same percentage of carbon (100%). Option D is generally considered true in that the distances between non-bonded carbon atoms vary depending on their relative positions in the lattice, unlike the consistent bond length. However, the distinct electrical conductivity is the most prominent difference.\" \/>\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-of-the-following-is-not-true-for-the-form-of-carbon-know\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Which one of the following is * not * true for the form of carbon know\" \/>\n<meta property=\"og:description\" content=\"Option C is the correct answer. Diamond is an electrical insulator, whereas graphite is a good electrical conductor. Diamond and graphite are allotropes of carbon, meaning they are made solely of carbon atoms but arranged differently. This structural difference leads to vastly different properties. Diamond has a tetrahedral structure where each carbon is bonded to four others, with all valence electrons tightly held in covalent bonds, making it very hard and a poor conductor of electricity. Graphite has a layered structure where each carbon is bonded to three others, forming hexagonal rings within layers. One valence electron per carbon atom is delocalized and free to move across the layers, making graphite soft and a good conductor of electricity. Therefore, the statement that diamond is a better electric conductor than graphite is false. Options A and B are true: diamond is much harder than graphite, and both are pure carbon, hence containing the same percentage of carbon (100%). Option D is generally considered true in that the distances between non-bonded carbon atoms vary depending on their relative positions in the lattice, unlike the consistent bond length. However, the distinct electrical conductivity is the most prominent difference.\" \/>\n<meta property=\"og:url\" content=\"https:\/\/exam.pscnotes.com\/mcq\/which-one-of-the-following-is-not-true-for-the-form-of-carbon-know\/\" \/>\n<meta property=\"og:site_name\" content=\"MCQ and Quiz for Exams\" \/>\n<meta property=\"article:published_time\" content=\"2025-06-01T03:28:52+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 of the following is * not * true for the form of carbon know","description":"Option C is the correct answer. Diamond is an electrical insulator, whereas graphite is a good electrical conductor. Diamond and graphite are allotropes of carbon, meaning they are made solely of carbon atoms but arranged differently. This structural difference leads to vastly different properties. Diamond has a tetrahedral structure where each carbon is bonded to four others, with all valence electrons tightly held in covalent bonds, making it very hard and a poor conductor of electricity. Graphite has a layered structure where each carbon is bonded to three others, forming hexagonal rings within layers. One valence electron per carbon atom is delocalized and free to move across the layers, making graphite soft and a good conductor of electricity. Therefore, the statement that diamond is a better electric conductor than graphite is false. Options A and B are true: diamond is much harder than graphite, and both are pure carbon, hence containing the same percentage of carbon (100%). Option D is generally considered true in that the distances between non-bonded carbon atoms vary depending on their relative positions in the lattice, unlike the consistent bond length. However, the distinct electrical conductivity is the most prominent difference.","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-of-the-following-is-not-true-for-the-form-of-carbon-know\/","og_locale":"en_US","og_type":"article","og_title":"Which one of the following is * not * true for the form of carbon know","og_description":"Option C is the correct answer. Diamond is an electrical insulator, whereas graphite is a good electrical conductor. Diamond and graphite are allotropes of carbon, meaning they are made solely of carbon atoms but arranged differently. This structural difference leads to vastly different properties. Diamond has a tetrahedral structure where each carbon is bonded to four others, with all valence electrons tightly held in covalent bonds, making it very hard and a poor conductor of electricity. Graphite has a layered structure where each carbon is bonded to three others, forming hexagonal rings within layers. One valence electron per carbon atom is delocalized and free to move across the layers, making graphite soft and a good conductor of electricity. Therefore, the statement that diamond is a better electric conductor than graphite is false. Options A and B are true: diamond is much harder than graphite, and both are pure carbon, hence containing the same percentage of carbon (100%). Option D is generally considered true in that the distances between non-bonded carbon atoms vary depending on their relative positions in the lattice, unlike the consistent bond length. However, the distinct electrical conductivity is the most prominent difference.","og_url":"https:\/\/exam.pscnotes.com\/mcq\/which-one-of-the-following-is-not-true-for-the-form-of-carbon-know\/","og_site_name":"MCQ and Quiz for Exams","article_published_time":"2025-06-01T03:28:52+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-of-the-following-is-not-true-for-the-form-of-carbon-know\/","url":"https:\/\/exam.pscnotes.com\/mcq\/which-one-of-the-following-is-not-true-for-the-form-of-carbon-know\/","name":"Which one of the following is * not * true for the form of carbon know","isPartOf":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#website"},"datePublished":"2025-06-01T03:28:52+00:00","dateModified":"2025-06-01T03:28:52+00:00","author":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/5807dafeb27d2ec82344d6cbd6c3d209"},"description":"Option C is the correct answer. Diamond is an electrical insulator, whereas graphite is a good electrical conductor. Diamond and graphite are allotropes of carbon, meaning they are made solely of carbon atoms but arranged differently. This structural difference leads to vastly different properties. Diamond has a tetrahedral structure where each carbon is bonded to four others, with all valence electrons tightly held in covalent bonds, making it very hard and a poor conductor of electricity. Graphite has a layered structure where each carbon is bonded to three others, forming hexagonal rings within layers. One valence electron per carbon atom is delocalized and free to move across the layers, making graphite soft and a good conductor of electricity. Therefore, the statement that diamond is a better electric conductor than graphite is false. Options A and B are true: diamond is much harder than graphite, and both are pure carbon, hence containing the same percentage of carbon (100%). Option D is generally considered true in that the distances between non-bonded carbon atoms vary depending on their relative positions in the lattice, unlike the consistent bond length. However, the distinct electrical conductivity is the most prominent difference.","breadcrumb":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/which-one-of-the-following-is-not-true-for-the-form-of-carbon-know\/#breadcrumb"},"inLanguage":"en-US","potentialAction":[{"@type":"ReadAction","target":["https:\/\/exam.pscnotes.com\/mcq\/which-one-of-the-following-is-not-true-for-the-form-of-carbon-know\/"]}]},{"@type":"BreadcrumbList","@id":"https:\/\/exam.pscnotes.com\/mcq\/which-one-of-the-following-is-not-true-for-the-form-of-carbon-know\/#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 one of the following is * not * true for the form of carbon know"}]},{"@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\/85824","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=85824"}],"version-history":[{"count":0,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts\/85824\/revisions"}],"wp:attachment":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/media?parent=85824"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/categories?post=85824"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/tags?post=85824"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}