{"id":36097,"date":"2025-06-25T02:54:24","date_gmt":"2025-06-25T02:54:24","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=36097"},"modified":"2025-06-25T02:54:26","modified_gmt":"2025-06-25T02:54:26","slug":"identify-all-of-the-compounds-that-contain-polar-bonds-but-which-are-non-polar-overall","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/identify-all-of-the-compounds-that-contain-polar-bonds-but-which-are-non-polar-overall\/","title":{"rendered":"Identify all of the compounds that contain polar bonds but which are non-polar overall"},"content":{"rendered":"\n<p>Identify all of the compounds that contain polar bonds but which are non-polar overall: Group of answer choices a: SO2 b: SO3 c:SCl4 d: HCN e: CH4 f: NF3 g: PBr5 h: BF3 i: H2S<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To identify the compounds that contain <strong>polar bonds<\/strong> but are <strong>non-polar overall<\/strong>, we need to consider both <strong>bond polarity<\/strong> and <strong>molecular geometry<\/strong>.<\/p>\n\n\n\n<p>A <strong>polar bond<\/strong> forms between atoms with different electronegativities. However, a molecule can still be <strong>non-polar overall<\/strong> if its molecular geometry causes the bond dipoles to cancel out.<\/p>\n\n\n\n<p>Let\u2019s evaluate each compound:<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>a: SO\u2082 (Sulfur dioxide)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Contains polar bonds (S\u2013O)<\/li>\n\n\n\n<li>Bent shape<\/li>\n\n\n\n<li>Dipoles do not cancel<br>\u27a1\ufe0f <strong>Polar overall<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>b: SO\u2083 (Sulfur trioxide)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Contains polar bonds (S\u2013O)<\/li>\n\n\n\n<li>Trigonal planar shape<\/li>\n\n\n\n<li>Dipoles cancel out<br>\u27a1\ufe0f <strong>Non-polar overall<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>c: SCl\u2084 (Sulfur tetrachloride)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Contains polar bonds (S\u2013Cl)<\/li>\n\n\n\n<li>Seesaw shape due to one lone pair<\/li>\n\n\n\n<li>Dipoles do not cancel<br>\u27a1\ufe0f <strong>Polar overall<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>d: HCN (Hydrogen cyanide)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Contains polar bonds (H\u2013C, C\u2261N)<\/li>\n\n\n\n<li>Linear shape<\/li>\n\n\n\n<li>Dipoles do not cancel<br>\u27a1\ufe0f <strong>Polar overall<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>e: CH\u2084 (Methane)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Contains weakly polar bonds (C\u2013H)<\/li>\n\n\n\n<li>Tetrahedral symmetry<\/li>\n\n\n\n<li>Dipoles cancel out<br>\u27a1\ufe0f <strong>Non-polar overall<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>f: NF\u2083 (Nitrogen trifluoride)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Contains polar bonds (N\u2013F)<\/li>\n\n\n\n<li>Trigonal pyramidal shape<\/li>\n\n\n\n<li>Dipoles do not fully cancel<br>\u27a1\ufe0f <strong>Polar overall<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>g: PBr\u2085 (Phosphorus pentabromide)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Contains polar bonds (P\u2013Br)<\/li>\n\n\n\n<li>Trigonal bipyramidal shape<\/li>\n\n\n\n<li>Dipoles cancel out due to symmetry<br>\u27a1\ufe0f <strong>Non-polar overall<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>h: BF\u2083 (Boron trifluoride)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Contains polar bonds (B\u2013F)<\/li>\n\n\n\n<li>Trigonal planar shape<\/li>\n\n\n\n<li>Dipoles cancel out<br>\u27a1\ufe0f <strong>Non-polar overall<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>i: H\u2082S (Hydrogen sulfide)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Contains polar bonds (H\u2013S)<\/li>\n\n\n\n<li>Bent shape<\/li>\n\n\n\n<li>Dipoles do not cancel<br>\u27a1\ufe0f <strong>Polar overall<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">\u2705 Correct Answer:<\/h3>\n\n\n\n<p><strong>b: SO\u2083<\/strong>, <strong>e: CH\u2084<\/strong>, <strong>g: PBr\u2085<\/strong>, <strong>h: BF\u2083<\/strong><\/p>\n\n\n\n<p>These compounds contain polar bonds but are non-polar overall due to their symmetrical geometries that cancel out the dipole moments.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"852\" height=\"1024\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-750.jpeg\" alt=\"\" class=\"wp-image-36098\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-750.jpeg 852w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-750-250x300.jpeg 250w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-750-768x923.jpeg 768w\" sizes=\"auto, (max-width: 852px) 100vw, 852px\" \/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Identify all of the compounds that contain polar bonds but which are non-polar overall: Group of answer choices a: SO2 b: SO3 c:SCl4 d: HCN e: CH4 f: NF3 g: PBr5 h: BF3 i: H2S The Correct Answer and Explanation is: To identify the compounds that contain polar bonds but are non-polar overall, we need [&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-36097","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36097","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=36097"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36097\/revisions"}],"predecessor-version":[{"id":36099,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36097\/revisions\/36099"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=36097"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=36097"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=36097"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}