{"id":16249,"date":"2025-06-11T08:15:32","date_gmt":"2025-06-11T08:15:32","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=16249"},"modified":"2025-06-11T08:15:34","modified_gmt":"2025-06-11T08:15:34","slug":"which-one-of-the-following-molecules-is-nonpolar","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/which-one-of-the-following-molecules-is-nonpolar\/","title":{"rendered":"Which one of the following molecules is nonpolar"},"content":{"rendered":"\n<p>Which one of the following molecules is nonpolar? SOF2 AsF3 NO2Br SF6 SO<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\"><strong>The correct answer and explanation is:<\/strong><\/mark><\/p>\n\n\n\n<p>The correct answer is: <strong>SF\u2086 (sulfur hexafluoride)<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation (Approximately 300 words):<\/h3>\n\n\n\n<p>To determine which molecule is <strong>nonpolar<\/strong>, we must analyze both the <strong>electronegativity<\/strong> of the atoms and the <strong>molecular geometry<\/strong> (shape).<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">1. <strong>Polarity Basics<\/strong>:<\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>A <strong>polar molecule<\/strong> has an uneven distribution of electrons, leading to a dipole moment (one end slightly positive, the other slightly negative).<\/li>\n\n\n\n<li>A <strong>nonpolar molecule<\/strong> either has <strong>no dipole moment<\/strong> or has dipoles that <strong>cancel out<\/strong> due to molecular symmetry.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\">2. <strong>Analysis of the Molecules<\/strong>:<\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>SOF\u2082 (Thionyl fluoride)<\/strong>: This molecule has a <strong>bent or trigonal pyramidal<\/strong> shape because of the lone pairs on sulfur. The F and O atoms have different electronegativities and are positioned asymmetrically, making the molecule <strong>polar<\/strong>.<\/li>\n\n\n\n<li><strong>AsF\u2083 (Arsenic trifluoride)<\/strong>: Has a <strong>trigonal pyramidal<\/strong> shape due to a lone pair on arsenic. The bond dipoles do not cancel, so the molecule is <strong>polar<\/strong>.<\/li>\n\n\n\n<li><strong>NO\u2082Br (Nitrogen dioxide bromide)<\/strong>: This molecule is <strong>asymmetrical<\/strong> with different atoms (O and Br) bonded to nitrogen. It has an uneven distribution of charge and is therefore <strong>polar<\/strong>.<\/li>\n\n\n\n<li><strong>SF\u2086 (Sulfur hexafluoride)<\/strong>: Sulfur is surrounded by six fluorine atoms in an <strong>octahedral<\/strong> geometry. Even though the S\u2013F bonds are polar, the molecule is <strong>highly symmetrical<\/strong>, so all the dipoles <strong>cancel out<\/strong>. This makes <strong>SF\u2086 a nonpolar molecule<\/strong> despite having polar bonds.<\/li>\n\n\n\n<li><strong>SO (Sulfur monoxide)<\/strong>: This is a <strong>diatomic molecule<\/strong> with polar bonds (oxygen is more electronegative), and there is no symmetry to cancel out the dipole. Thus, <strong>SO is polar<\/strong>.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\">3. <strong>Conclusion<\/strong>:<\/h4>\n\n\n\n<p><strong>SF\u2086 is nonpolar<\/strong> because of its <strong>perfectly symmetrical octahedral structure<\/strong>, which causes the bond dipoles to cancel out, resulting in no overall molecular dipole moment. All other choices have either asymmetrical structures or different electronegativities in positions that don&#8217;t cancel dipoles, making them polar.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Which one of the following molecules is nonpolar? SOF2 AsF3 NO2Br SF6 SO The correct answer and explanation is: The correct answer is: SF\u2086 (sulfur hexafluoride) Explanation (Approximately 300 words): To determine which molecule is nonpolar, we must analyze both the electronegativity of the atoms and the molecular geometry (shape). 1. Polarity Basics: 2. Analysis [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-16249","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16249","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=16249"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16249\/revisions"}],"predecessor-version":[{"id":16251,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16249\/revisions\/16251"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=16249"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=16249"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=16249"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}