{"id":246615,"date":"2025-07-07T09:44:25","date_gmt":"2025-07-07T09:44:25","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=246615"},"modified":"2025-07-07T09:44:27","modified_gmt":"2025-07-07T09:44:27","slug":"fill-in-the-table-below-for-each-molecule-to-determine-if-the-molecule-is-polar-or-nonpolar","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/07\/fill-in-the-table-below-for-each-molecule-to-determine-if-the-molecule-is-polar-or-nonpolar\/","title":{"rendered":"Fill in the table below for each molecule to determine if the molecule is polar or nonpolar."},"content":{"rendered":"\n
Fill in the table below for each molecule to determine if the molecule is polar or nonpolar. You may want to refer to a table of electronegativity values: Name Dichloromethane Carbon dioxide Ammonia Structure Cl-C-Cl O=C=O H-N-H Does the molecule have polar bonds? If yes, which ones? Dichloromethane: Yes, the C-Cl bonds are polar. Carbon dioxide: No, the C=O bonds are nonpolar. Ammonia: Yes, the N-H bonds are polar. Does the molecule have lone pairs on the center atom? If there are polar bonds and\/or lone pairs, are they symmetric? Is the molecule polar or nonpolar? Dichloromethane: No lone pairs, the molecule is polar. Carbon dioxide: No lone pairs, the molecule is nonpolar. Ammonia: Yes, there is one lone pair on the N atom. The molecule is polar. 18. Draw the three-dimensional structures for each molecule. Fill in the table for each molecule to determine if the molecule is polar or nonpolar: Methane (CH4) Formaldehyde (CH2O) Xenon tetrafluoride (XeF4) Name Methane Formaldehyde Xenon tetrafluoride Structure H | H-C-H | H H | H-C=O | H F | F-Xe-F | F Does the molecule have polar bonds? If yes, which ones? Does the molecule have lone pairs on the center atom? If there are polar bonds and\/or lone pairs, are they symmetric? Is the molecule polar or nonpolar? Methane: No polar bonds, no lone pairs, the molecule is nonpolar. Formaldehyde: Yes, the C=O bond is polar. No lone pairs, the molecule is polar. Xenon tetrafluoride: Yes, the Xe-F bonds are polar. No lone pairs, the molecule is polar. 19. Determine if the following molecules are polar or nonpolar: Carbon tetrafluoride (CF4), Phosphorous pentachloride (PCl5), Water (H2O), Hydrogen sulfide (H2S), Sulfur dioxide (SO2). Title_with_topic: Determining Polarity of Molecules<\/pre>\n\n\n\n
\"\"<\/figure>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
Of course. Here are the completed tables and answers, along with a detailed explanation of how to determine molecular polarity.<\/p>\n\n\n\n
Question 17: Completed Table<\/strong><\/h3>\n\n\n\n
Name<\/strong><\/td>Dichloromethane<\/strong><\/td>Carbon dioxide<\/strong><\/td>Ammonia<\/strong><\/td><\/tr>
Structure<\/strong><\/td>A tetrahedral structure with Carbon at the center.<\/td>O=C=O (Linear)<\/td>A trigonal pyramidal structure with Nitrogen at the apex.<\/td><\/tr>
Does the molecule have polar bonds? If yes, which ones?<\/strong><\/td>Yes, the C-Cl bonds are polar. The C-H bonds are considered nonpolar or very weakly polar.<\/td>Yes, the two C=O bonds are polar.<\/td>Yes, the three N-H bonds are polar.<\/td><\/tr>
Does the molecule have lone pairs on the center atom?<\/strong><\/td>No.<\/td>No.<\/td>Yes, one lone pair.<\/td><\/tr>
If there are polar bonds and\/or lone pairs, are they symmetric?<\/strong><\/td>No. The dipoles of the C-Cl and C-H bonds do not cancel out.<\/td>Yes. The two polar C=O bonds are 180\u00b0 apart and their dipoles cancel.<\/td>No. The three N-H bond dipoles and the lone pair create an asymmetric charge distribution.<\/td><\/tr>
Is the molecule polar or nonpolar?<\/strong><\/td>Polar.<\/td>Nonpolar.<\/td>Polar.<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n
\n\n\n\n
Question 18: Completed Table<\/strong><\/h3>\n\n\n\n
Name<\/strong><\/td>Methane (CH\u2084)<\/strong><\/td>Formaldehyde (CH\u2082O)<\/strong><\/td>Xenon tetrafluoride (XeF\u2084)<\/strong><\/td><\/tr>
Structure<\/strong><\/td>Tetrahedral<\/td>Trigonal planar<\/td>Square planar<\/td><\/tr>
Does the molecule have polar bonds? If yes, which ones?<\/strong><\/td>No. The C-H bonds are considered nonpolar.<\/td>Yes, the C=O bond is polar.<\/td>Yes, the four Xe-F bonds are polar.<\/td><\/tr>
Does the molecule have lone pairs on the center atom?<\/strong><\/td>No.<\/td>No.<\/td>Yes, two lone pairs.<\/td><\/tr>
If there are polar bonds and\/or lone pairs, are they symmetric?<\/strong><\/td>Yes. The four C-H bonds are arranged symmetrically.<\/td>No. The strong C=O dipole is not canceled by the other bonds.<\/td>Yes. The four Xe-F bond dipoles cancel, and the two lone pairs are opposite each other, also canceling their effect.<\/td><\/tr>
Is the molecule polar or nonpolar?<\/strong><\/td>Nonpolar.<\/td>Polar.<\/td>Nonpolar.<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n
\n\n\n\n
Question 19: Polarity of Molecules<\/strong><\/h3>\n\n\n\n
    \n
  • a. Carbon tetrafluoride (CF\u2084):<\/strong>\u00a0Nonpolar<\/li>\n\n\n\n
  • b. Water (H\u2082O):<\/strong>\u00a0Polar<\/li>\n\n\n\n
  • c. Sulfur dioxide (SO\u2082):<\/strong>\u00a0Polar<\/li>\n\n\n\n
  • d. Phosphorous pentachloride (PCl\u2085):<\/strong>\u00a0Nonpolar<\/li>\n\n\n\n
  • e. Hydrogen sulfide (H\u2082S):<\/strong>\u00a0Polar<\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n
    Explanation of Molecular Polarity<\/strong><\/h3>\n\n\n\n
    Determining if a molecule is polar or nonpolar involves two key steps: assessing bond polarity and analyzing the molecule’s three dimensional geometry.<\/p>\n\n\n\n
    First, a polar covalent bond forms between two atoms with a significant difference in electronegativity. The more electronegative atom pulls the shared electrons closer, creating a partial negative charge (\u03b4-) and leaving a partial positive charge (\u03b4+) on the other atom. This separation of charge is called a bond dipole. For example, the oxygen in carbon dioxide (CO\u2082) is more electronegative than carbon, so the C=O bonds are polar. In contrast, the C-H bonds in methane (CH\u2084) have a very small electronegativity difference and are considered nonpolar.<\/p>\n\n\n\n
    Second, the overall polarity of a molecule depends on its shape. If a molecule contains polar bonds, you must look at their arrangement. If the polar bonds are arranged symmetrically around the central atom, their individual dipoles cancel each other out, resulting in a nonpolar molecule. This is the case for carbon dioxide (CO\u2082), which has a linear shape. The two polar C=O bonds point in opposite directions and cancel, making the molecule nonpolar. Other symmetric shapes that lead to nonpolar molecules include tetrahedral (like CF\u2084), trigonal bipyramidal (like PCl\u2085), and square planar (like XeF\u2084), provided all surrounding atoms are identical.<\/p>\n\n\n\n
    A molecule is polar if its bond dipoles do not cancel out. This usually happens in molecules with an asymmetrical shape. The presence of lone pairs on the central atom often creates asymmetry, as seen in ammonia (NH\u2083) with its trigonal pyramidal shape and water (H\u2082O) with its bent shape. In both cases, the bond dipoles and the effect of the lone pairs combine to create a net dipole moment, making the molecules polar. Similarly, dichloromethane (CH\u2082Cl\u2082) is polar because its tetrahedral shape is made asymmetric by having two different types of atoms (H and Cl) attached to the central carbon<\/p>\n\n\n\n
    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
    Fill in the table below for each molecule to determine if the molecule is polar or nonpolar. You may want to refer to a table of electronegativity values: Name Dichloromethane Carbon dioxide Ammonia Structure Cl-C-Cl O=C=O H-N-H Does the molecule have polar bonds? If yes, which ones? Dichloromethane: Yes, the C-Cl bonds are polar. Carbon […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-246615","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246615","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=246615"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246615\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246615"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246615"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246615"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}