Let’s break down the Lewis structures, polarity, and intermolecular forces for each molecule:<\/p>\n\n\n\n
a) BH3 (Borane)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Boron (B) is in the center with three single bonds to three hydrogen atoms. Boron only has six valence electrons (3 from H atoms and 3 from its own electrons), so it is electron-deficient.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Boron (3) + Hydrogen (3 \u00d7 1) = 6 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Non-polar<\/strong>. The molecule has a trigonal planar shape due to the sp2 hybridization of boron. Since all the bonds are identical and there is no lone pair on boron, the dipoles cancel out.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: London Dispersion Forces (LDF)<\/strong> are the only intermolecular force present here, as there are no significant dipoles or hydrogen bonds.<\/li>\n<\/ul>\n\n\n\n
b) SO2 (Sulfur Dioxide)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Sulfur (S) is the central atom with two double bonds to two oxygen (O) atoms. Sulfur has a lone pair of electrons.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Sulfur (6) + Oxygen (2 \u00d7 6) = 18 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar<\/strong>. The molecule has a bent shape due to the lone pair on sulfur. The two oxygen atoms pull electron density away from sulfur, creating a net dipole pointing toward the more electronegative oxygens.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: Dipole-Dipole Interactions<\/strong> are the strongest intermolecular force due to the permanent dipole of the molecule. LDF also plays a role.<\/li>\n<\/ul>\n\n\n\n
c) H2CO3 (Carbonic Acid)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Carbon (C) is at the center with two single bonds to oxygen atoms and one double bond to another oxygen. One of the oxygen atoms is attached to a hydrogen atom (OH group).<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Carbon (4) + Oxygen (3 \u00d7 6) + Hydrogen (2 \u00d7 1) = 18 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar<\/strong>. The molecule has a trigonal planar shape with polar bonds. The dipole moments do not cancel, resulting in a net dipole.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: Hydrogen Bonding<\/strong> is the strongest force, in addition to dipole-dipole interactions and LDF.<\/li>\n<\/ul>\n\n\n\n
d) XeF2 (Xenon Difluoride)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Xenon (Xe) is at the center with two single bonds to fluorine (F) atoms. Xenon also has three lone pairs of electrons.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Xenon (8) + Fluorine (2 \u00d7 7) = 22 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Non-polar<\/strong>. Even though the bonds are polar, the molecule has a linear shape, and the dipoles cancel out because of symmetry.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: London Dispersion Forces<\/strong> are the primary intermolecular forces.<\/li>\n<\/ul>\n\n\n\n
e) C2H4 (Ethene or Ethylene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Two carbon atoms double-bonded to each other, each bonded to two hydrogen atoms.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Carbon (2 \u00d7 4) + Hydrogen (4 \u00d7 1) = 12 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Non-polar<\/strong>. The molecule is symmetrical, with equal sharing of electrons between the carbon atoms and hydrogens. The dipoles cancel out.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: London Dispersion Forces<\/strong> are the strongest force due to the relatively simple structure.<\/li>\n<\/ul>\n\n\n\n
Summary:<\/h3>\n\n\n\n\n- BH3<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- SO2<\/strong>: Polar, Dipole-Dipole.<\/li>\n\n\n\n
- H2CO3<\/strong>: Polar, Hydrogen Bonding.<\/li>\n\n\n\n
- XeF2<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- C2H4<\/strong>: Non-polar, LDF.<\/li>\n<\/ul>\n\n\n\n
The strongest intermolecular forces vary, but hydrogen bonding in H2CO3<\/strong> is the strongest among these examples.<\/p>\n\n\n\n![\"\"](\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1551.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"Given the following molecules: – Draw the lewis structure (don’t forget to show the number of valance electrons) – Determine the polarity (polar vs. non-polar). Show directions of dipole moments\/arrows to support your answers. – List all intermolecular forces. Indicate strongest force. a) BH3 b) SO2 c) H2CO3 d) XeF2 e) C2H4 The Correct Answer […]<\/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-44856","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856","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=44856"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions"}],"predecessor-version":[{"id":44865,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions\/44865"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=44856"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=44856"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=44856"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
b) SO2 (Sulfur Dioxide)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Sulfur (S) is the central atom with two double bonds to two oxygen (O) atoms. Sulfur has a lone pair of electrons.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Sulfur (6) + Oxygen (2 \u00d7 6) = 18 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar<\/strong>. The molecule has a bent shape due to the lone pair on sulfur. The two oxygen atoms pull electron density away from sulfur, creating a net dipole pointing toward the more electronegative oxygens.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: Dipole-Dipole Interactions<\/strong> are the strongest intermolecular force due to the permanent dipole of the molecule. LDF also plays a role.<\/li>\n<\/ul>\n\n\n\n
c) H2CO3 (Carbonic Acid)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Carbon (C) is at the center with two single bonds to oxygen atoms and one double bond to another oxygen. One of the oxygen atoms is attached to a hydrogen atom (OH group).<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Carbon (4) + Oxygen (3 \u00d7 6) + Hydrogen (2 \u00d7 1) = 18 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar<\/strong>. The molecule has a trigonal planar shape with polar bonds. The dipole moments do not cancel, resulting in a net dipole.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: Hydrogen Bonding<\/strong> is the strongest force, in addition to dipole-dipole interactions and LDF.<\/li>\n<\/ul>\n\n\n\n
d) XeF2 (Xenon Difluoride)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Xenon (Xe) is at the center with two single bonds to fluorine (F) atoms. Xenon also has three lone pairs of electrons.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Xenon (8) + Fluorine (2 \u00d7 7) = 22 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Non-polar<\/strong>. Even though the bonds are polar, the molecule has a linear shape, and the dipoles cancel out because of symmetry.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: London Dispersion Forces<\/strong> are the primary intermolecular forces.<\/li>\n<\/ul>\n\n\n\n
e) C2H4 (Ethene or Ethylene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Two carbon atoms double-bonded to each other, each bonded to two hydrogen atoms.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Carbon (2 \u00d7 4) + Hydrogen (4 \u00d7 1) = 12 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Non-polar<\/strong>. The molecule is symmetrical, with equal sharing of electrons between the carbon atoms and hydrogens. The dipoles cancel out.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: London Dispersion Forces<\/strong> are the strongest force due to the relatively simple structure.<\/li>\n<\/ul>\n\n\n\n
Summary:<\/h3>\n\n\n\n\n- BH3<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- SO2<\/strong>: Polar, Dipole-Dipole.<\/li>\n\n\n\n
- H2CO3<\/strong>: Polar, Hydrogen Bonding.<\/li>\n\n\n\n
- XeF2<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- C2H4<\/strong>: Non-polar, LDF.<\/li>\n<\/ul>\n\n\n\n
The strongest intermolecular forces vary, but hydrogen bonding in H2CO3<\/strong> is the strongest among these examples.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Given the following molecules: – Draw the lewis structure (don’t forget to show the number of valance electrons) – Determine the polarity (polar vs. non-polar). Show directions of dipole moments\/arrows to support your answers. – List all intermolecular forces. Indicate strongest force. a) BH3 b) SO2 c) H2CO3 d) XeF2 e) C2H4 The Correct Answer […]<\/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-44856","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856","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=44856"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions"}],"predecessor-version":[{"id":44865,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions\/44865"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=44856"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=44856"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=44856"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
c) H2CO3 (Carbonic Acid)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Carbon (C) is at the center with two single bonds to oxygen atoms and one double bond to another oxygen. One of the oxygen atoms is attached to a hydrogen atom (OH group).<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Carbon (4) + Oxygen (3 \u00d7 6) + Hydrogen (2 \u00d7 1) = 18 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar<\/strong>. The molecule has a trigonal planar shape with polar bonds. The dipole moments do not cancel, resulting in a net dipole.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: Hydrogen Bonding<\/strong> is the strongest force, in addition to dipole-dipole interactions and LDF.<\/li>\n<\/ul>\n\n\n\n
d) XeF2 (Xenon Difluoride)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Xenon (Xe) is at the center with two single bonds to fluorine (F) atoms. Xenon also has three lone pairs of electrons.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Xenon (8) + Fluorine (2 \u00d7 7) = 22 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Non-polar<\/strong>. Even though the bonds are polar, the molecule has a linear shape, and the dipoles cancel out because of symmetry.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: London Dispersion Forces<\/strong> are the primary intermolecular forces.<\/li>\n<\/ul>\n\n\n\n
e) C2H4 (Ethene or Ethylene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Two carbon atoms double-bonded to each other, each bonded to two hydrogen atoms.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Carbon (2 \u00d7 4) + Hydrogen (4 \u00d7 1) = 12 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Non-polar<\/strong>. The molecule is symmetrical, with equal sharing of electrons between the carbon atoms and hydrogens. The dipoles cancel out.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: London Dispersion Forces<\/strong> are the strongest force due to the relatively simple structure.<\/li>\n<\/ul>\n\n\n\n
Summary:<\/h3>\n\n\n\n\n- BH3<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- SO2<\/strong>: Polar, Dipole-Dipole.<\/li>\n\n\n\n
- H2CO3<\/strong>: Polar, Hydrogen Bonding.<\/li>\n\n\n\n
- XeF2<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- C2H4<\/strong>: Non-polar, LDF.<\/li>\n<\/ul>\n\n\n\n
The strongest intermolecular forces vary, but hydrogen bonding in H2CO3<\/strong> is the strongest among these examples.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Given the following molecules: – Draw the lewis structure (don’t forget to show the number of valance electrons) – Determine the polarity (polar vs. non-polar). Show directions of dipole moments\/arrows to support your answers. – List all intermolecular forces. Indicate strongest force. a) BH3 b) SO2 c) H2CO3 d) XeF2 e) C2H4 The Correct Answer […]<\/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-44856","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856","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=44856"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions"}],"predecessor-version":[{"id":44865,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions\/44865"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=44856"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=44856"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=44856"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
d) XeF2 (Xenon Difluoride)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Xenon (Xe) is at the center with two single bonds to fluorine (F) atoms. Xenon also has three lone pairs of electrons.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Xenon (8) + Fluorine (2 \u00d7 7) = 22 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Non-polar<\/strong>. Even though the bonds are polar, the molecule has a linear shape, and the dipoles cancel out because of symmetry.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: London Dispersion Forces<\/strong> are the primary intermolecular forces.<\/li>\n<\/ul>\n\n\n\n
e) C2H4 (Ethene or Ethylene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Two carbon atoms double-bonded to each other, each bonded to two hydrogen atoms.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Carbon (2 \u00d7 4) + Hydrogen (4 \u00d7 1) = 12 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Non-polar<\/strong>. The molecule is symmetrical, with equal sharing of electrons between the carbon atoms and hydrogens. The dipoles cancel out.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: London Dispersion Forces<\/strong> are the strongest force due to the relatively simple structure.<\/li>\n<\/ul>\n\n\n\n
Summary:<\/h3>\n\n\n\n\n- BH3<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- SO2<\/strong>: Polar, Dipole-Dipole.<\/li>\n\n\n\n
- H2CO3<\/strong>: Polar, Hydrogen Bonding.<\/li>\n\n\n\n
- XeF2<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- C2H4<\/strong>: Non-polar, LDF.<\/li>\n<\/ul>\n\n\n\n
The strongest intermolecular forces vary, but hydrogen bonding in H2CO3<\/strong> is the strongest among these examples.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Given the following molecules: – Draw the lewis structure (don’t forget to show the number of valance electrons) – Determine the polarity (polar vs. non-polar). Show directions of dipole moments\/arrows to support your answers. – List all intermolecular forces. Indicate strongest force. a) BH3 b) SO2 c) H2CO3 d) XeF2 e) C2H4 The Correct Answer […]<\/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-44856","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856","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=44856"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions"}],"predecessor-version":[{"id":44865,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions\/44865"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=44856"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=44856"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=44856"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
e) C2H4 (Ethene or Ethylene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Two carbon atoms double-bonded to each other, each bonded to two hydrogen atoms.<\/li>\n\n\n\n
- Valence Electrons<\/strong>: Carbon (2 \u00d7 4) + Hydrogen (4 \u00d7 1) = 12 electrons.<\/li>\n\n\n\n
- Polarity<\/strong>: Non-polar<\/strong>. The molecule is symmetrical, with equal sharing of electrons between the carbon atoms and hydrogens. The dipoles cancel out.<\/li>\n\n\n\n
- Intermolecular Forces<\/strong>: London Dispersion Forces<\/strong> are the strongest force due to the relatively simple structure.<\/li>\n<\/ul>\n\n\n\n
Summary:<\/h3>\n\n\n\n\n- BH3<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- SO2<\/strong>: Polar, Dipole-Dipole.<\/li>\n\n\n\n
- H2CO3<\/strong>: Polar, Hydrogen Bonding.<\/li>\n\n\n\n
- XeF2<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- C2H4<\/strong>: Non-polar, LDF.<\/li>\n<\/ul>\n\n\n\n
The strongest intermolecular forces vary, but hydrogen bonding in H2CO3<\/strong> is the strongest among these examples.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Given the following molecules: – Draw the lewis structure (don’t forget to show the number of valance electrons) – Determine the polarity (polar vs. non-polar). Show directions of dipole moments\/arrows to support your answers. – List all intermolecular forces. Indicate strongest force. a) BH3 b) SO2 c) H2CO3 d) XeF2 e) C2H4 The Correct Answer […]<\/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-44856","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856","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=44856"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions"}],"predecessor-version":[{"id":44865,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions\/44865"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=44856"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=44856"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=44856"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Summary:<\/h3>\n\n\n\n\n- BH3<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- SO2<\/strong>: Polar, Dipole-Dipole.<\/li>\n\n\n\n
- H2CO3<\/strong>: Polar, Hydrogen Bonding.<\/li>\n\n\n\n
- XeF2<\/strong>: Non-polar, LDF.<\/li>\n\n\n\n
- C2H4<\/strong>: Non-polar, LDF.<\/li>\n<\/ul>\n\n\n\n
The strongest intermolecular forces vary, but hydrogen bonding in H2CO3<\/strong> is the strongest among these examples.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Given the following molecules: – Draw the lewis structure (don’t forget to show the number of valance electrons) – Determine the polarity (polar vs. non-polar). Show directions of dipole moments\/arrows to support your answers. – List all intermolecular forces. Indicate strongest force. a) BH3 b) SO2 c) H2CO3 d) XeF2 e) C2H4 The Correct Answer […]<\/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-44856","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856","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=44856"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions"}],"predecessor-version":[{"id":44865,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions\/44865"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=44856"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=44856"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=44856"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
The strongest intermolecular forces vary, but hydrogen bonding in H2CO3<\/strong> is the strongest among these examples.<\/p>\n\n\n\n Given the following molecules: – Draw the lewis structure (don’t forget to show the number of valance electrons) – Determine the polarity (polar vs. non-polar). Show directions of dipole moments\/arrows to support your answers. – List all intermolecular forces. Indicate strongest force. a) BH3 b) SO2 c) H2CO3 d) XeF2 e) C2H4 The Correct Answer […]<\/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-44856","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856","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=44856"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions"}],"predecessor-version":[{"id":44865,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/44856\/revisions\/44865"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=44856"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=44856"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=44856"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}<\/figure>\n","protected":false},"excerpt":{"rendered":"