To evaluate the intermolecular forces of each molecule, we need to consider the types of interactions that occur between the molecules and the factors that influence their strengths.<\/p>\n\n\n\n
1. Intermolecular Forces<\/strong>:<\/h3>\n\n\n\n\n- CH4 (Methane)<\/strong>: CH4 is a nonpolar molecule. The only intermolecular force present here is London dispersion forces<\/strong> (induced dipole-induced dipole), which are the weakest of all intermolecular forces. These forces arise from temporary shifts in electron density in the molecules.<\/li>\n\n\n\n
- NH3 (Ammonia)<\/strong>: NH3 is a polar molecule due to the difference in electronegativity between nitrogen and hydrogen. It has London dispersion forces<\/strong> and hydrogen bonding<\/strong>. The nitrogen-hydrogen bond allows for hydrogen bonding, a strong intermolecular force, where the hydrogen atoms are attracted to lone pairs of electrons on nitrogen atoms of neighboring molecules.<\/li>\n\n\n\n
- CH3OCH3 (Dimethyl Ether)<\/strong>: This molecule is polar because the oxygen atom is more electronegative than the carbon atoms. It exhibits London dispersion forces<\/strong> and dipole-dipole forces<\/strong>. The dipole-dipole interactions are stronger than the London forces but not as strong as hydrogen bonding.<\/li>\n\n\n\n
- NH4Cl (Ammonium Chloride)<\/strong>: NH4Cl is an ionic compound, so it has London dispersion forces<\/strong>, dipole-dipole forces<\/strong>, and ion-dipole forces<\/strong>. The ion-dipole forces (between the NH4+ and Cl-) are much stronger than the other forces in the molecule, giving NH4Cl significantly stronger intermolecular forces.<\/li>\n<\/ul>\n\n\n\n
2. Ranking by Strength of Intermolecular Forces<\/strong>:<\/h3>\n\n\n\nThe strength of the intermolecular forces follows the order from weakest to strongest:<\/p>\n\n\n\n
\n- Weakest<\/strong>: CH4 (only London dispersion forces)<\/li>\n\n\n\n
- Next<\/strong>: CH3OCH3 (London dispersion forces + dipole-dipole)<\/li>\n\n\n\n
- Next<\/strong>: NH3 (London dispersion forces + hydrogen bonding)<\/li>\n\n\n\n
- Strongest<\/strong>: NH4Cl (London dispersion forces + dipole-dipole + ion-dipole)<\/li>\n<\/ul>\n\n\n\n
3. Ranking by Boiling Point<\/strong>:<\/h3>\n\n\n\nThe boiling point of a substance is influenced by the strength of the intermolecular forces. Stronger forces require more energy to overcome, leading to higher boiling points.<\/p>\n\n\n\n
\n- Highest boiling point<\/strong>: NH4Cl (strong ion-dipole forces)<\/li>\n\n\n\n
- Next<\/strong>: NH3 (strong hydrogen bonding)<\/li>\n\n\n\n
- Next<\/strong>: CH3OCH3 (dipole-dipole forces)<\/li>\n\n\n\n
- Lowest boiling point<\/strong>: CH4 (weak London dispersion forces)<\/li>\n<\/ul>\n\n\n\n
4. Solubility in Water<\/strong>:<\/h3>\n\n\n\nWater is a highly polar solvent, so it will dissolve substances that can interact with it through hydrogen bonding or other polar interactions.<\/p>\n\n\n\n
\n- CH4<\/strong>: CH4 is nonpolar and does not have the capability to form hydrogen bonds or interact with water’s dipoles. It is insoluble<\/strong> in water.<\/li>\n\n\n\n
- CH3OCH3<\/strong>: Although CH3OCH3 is polar, it does not form hydrogen bonds with water, and thus it is only slightly soluble<\/strong> in water but generally considered insoluble<\/strong>.<\/li>\n\n\n\n
- NH3<\/strong>: NH3 can form hydrogen bonds with water molecules due to its polarity, making it soluble<\/strong> in water.<\/li>\n\n\n\n
- NH4Cl<\/strong>: NH4Cl dissociates into NH4+ and Cl-, and the NH4+ ion can form strong ion-dipole interactions with water molecules. Thus, NH4Cl is highly soluble<\/strong> in water.<\/li>\n<\/ul>\n\n\n\n
Conclusion:<\/h3>\n\n\n\n\n- NH4Cl<\/strong> has the strongest intermolecular forces and the highest boiling point.<\/li>\n\n\n\n
- CH4<\/strong> has the weakest intermolecular forces and the lowest boiling point.<\/li>\n\n\n\n
- NH4Cl<\/strong> and NH3<\/strong> are soluble in water, while CH4<\/strong> is insoluble. CH3OCH3<\/strong> is only slightly soluble, or considered insoluble<\/strong>.<\/li>\n<\/ul>\n\n\n\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-939.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"Take-home Practice Problems: Intermolecular Forces Consider the following molecules: CH4, NH3, CH3OCH3, and NH4Cl. What type of intermolecular forces do these substances have? CH4: London dispersion forces NH3: London dispersion forces and hydrogen bonding CH3OCH3: London dispersion forces and dipole-dipole forces NH4Cl: London dispersion forces, dipole-dipole forces, and ion-dipole forces Rank these substances by the […]<\/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-259328","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328","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=259328"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=259328"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=259328"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=259328"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
2. Ranking by Strength of Intermolecular Forces<\/strong>:<\/h3>\n\n\n\nThe strength of the intermolecular forces follows the order from weakest to strongest:<\/p>\n\n\n\n
\n- Weakest<\/strong>: CH4 (only London dispersion forces)<\/li>\n\n\n\n
- Next<\/strong>: CH3OCH3 (London dispersion forces + dipole-dipole)<\/li>\n\n\n\n
- Next<\/strong>: NH3 (London dispersion forces + hydrogen bonding)<\/li>\n\n\n\n
- Strongest<\/strong>: NH4Cl (London dispersion forces + dipole-dipole + ion-dipole)<\/li>\n<\/ul>\n\n\n\n
3. Ranking by Boiling Point<\/strong>:<\/h3>\n\n\n\nThe boiling point of a substance is influenced by the strength of the intermolecular forces. Stronger forces require more energy to overcome, leading to higher boiling points.<\/p>\n\n\n\n
\n- Highest boiling point<\/strong>: NH4Cl (strong ion-dipole forces)<\/li>\n\n\n\n
- Next<\/strong>: NH3 (strong hydrogen bonding)<\/li>\n\n\n\n
- Next<\/strong>: CH3OCH3 (dipole-dipole forces)<\/li>\n\n\n\n
- Lowest boiling point<\/strong>: CH4 (weak London dispersion forces)<\/li>\n<\/ul>\n\n\n\n
4. Solubility in Water<\/strong>:<\/h3>\n\n\n\nWater is a highly polar solvent, so it will dissolve substances that can interact with it through hydrogen bonding or other polar interactions.<\/p>\n\n\n\n
\n- CH4<\/strong>: CH4 is nonpolar and does not have the capability to form hydrogen bonds or interact with water’s dipoles. It is insoluble<\/strong> in water.<\/li>\n\n\n\n
- CH3OCH3<\/strong>: Although CH3OCH3 is polar, it does not form hydrogen bonds with water, and thus it is only slightly soluble<\/strong> in water but generally considered insoluble<\/strong>.<\/li>\n\n\n\n
- NH3<\/strong>: NH3 can form hydrogen bonds with water molecules due to its polarity, making it soluble<\/strong> in water.<\/li>\n\n\n\n
- NH4Cl<\/strong>: NH4Cl dissociates into NH4+ and Cl-, and the NH4+ ion can form strong ion-dipole interactions with water molecules. Thus, NH4Cl is highly soluble<\/strong> in water.<\/li>\n<\/ul>\n\n\n\n
Conclusion:<\/h3>\n\n\n\n\n- NH4Cl<\/strong> has the strongest intermolecular forces and the highest boiling point.<\/li>\n\n\n\n
- CH4<\/strong> has the weakest intermolecular forces and the lowest boiling point.<\/li>\n\n\n\n
- NH4Cl<\/strong> and NH3<\/strong> are soluble in water, while CH4<\/strong> is insoluble. CH3OCH3<\/strong> is only slightly soluble, or considered insoluble<\/strong>.<\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Take-home Practice Problems: Intermolecular Forces Consider the following molecules: CH4, NH3, CH3OCH3, and NH4Cl. What type of intermolecular forces do these substances have? CH4: London dispersion forces NH3: London dispersion forces and hydrogen bonding CH3OCH3: London dispersion forces and dipole-dipole forces NH4Cl: London dispersion forces, dipole-dipole forces, and ion-dipole forces Rank these substances by the […]<\/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-259328","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328","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=259328"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=259328"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=259328"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=259328"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
3. Ranking by Boiling Point<\/strong>:<\/h3>\n\n\n\nThe boiling point of a substance is influenced by the strength of the intermolecular forces. Stronger forces require more energy to overcome, leading to higher boiling points.<\/p>\n\n\n\n
\n- Highest boiling point<\/strong>: NH4Cl (strong ion-dipole forces)<\/li>\n\n\n\n
- Next<\/strong>: NH3 (strong hydrogen bonding)<\/li>\n\n\n\n
- Next<\/strong>: CH3OCH3 (dipole-dipole forces)<\/li>\n\n\n\n
- Lowest boiling point<\/strong>: CH4 (weak London dispersion forces)<\/li>\n<\/ul>\n\n\n\n
4. Solubility in Water<\/strong>:<\/h3>\n\n\n\nWater is a highly polar solvent, so it will dissolve substances that can interact with it through hydrogen bonding or other polar interactions.<\/p>\n\n\n\n
\n- CH4<\/strong>: CH4 is nonpolar and does not have the capability to form hydrogen bonds or interact with water’s dipoles. It is insoluble<\/strong> in water.<\/li>\n\n\n\n
- CH3OCH3<\/strong>: Although CH3OCH3 is polar, it does not form hydrogen bonds with water, and thus it is only slightly soluble<\/strong> in water but generally considered insoluble<\/strong>.<\/li>\n\n\n\n
- NH3<\/strong>: NH3 can form hydrogen bonds with water molecules due to its polarity, making it soluble<\/strong> in water.<\/li>\n\n\n\n
- NH4Cl<\/strong>: NH4Cl dissociates into NH4+ and Cl-, and the NH4+ ion can form strong ion-dipole interactions with water molecules. Thus, NH4Cl is highly soluble<\/strong> in water.<\/li>\n<\/ul>\n\n\n\n
Conclusion:<\/h3>\n\n\n\n\n- NH4Cl<\/strong> has the strongest intermolecular forces and the highest boiling point.<\/li>\n\n\n\n
- CH4<\/strong> has the weakest intermolecular forces and the lowest boiling point.<\/li>\n\n\n\n
- NH4Cl<\/strong> and NH3<\/strong> are soluble in water, while CH4<\/strong> is insoluble. CH3OCH3<\/strong> is only slightly soluble, or considered insoluble<\/strong>.<\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Take-home Practice Problems: Intermolecular Forces Consider the following molecules: CH4, NH3, CH3OCH3, and NH4Cl. What type of intermolecular forces do these substances have? CH4: London dispersion forces NH3: London dispersion forces and hydrogen bonding CH3OCH3: London dispersion forces and dipole-dipole forces NH4Cl: London dispersion forces, dipole-dipole forces, and ion-dipole forces Rank these substances by the […]<\/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-259328","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328","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=259328"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=259328"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=259328"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=259328"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
4. Solubility in Water<\/strong>:<\/h3>\n\n\n\nWater is a highly polar solvent, so it will dissolve substances that can interact with it through hydrogen bonding or other polar interactions.<\/p>\n\n\n\n
\n- CH4<\/strong>: CH4 is nonpolar and does not have the capability to form hydrogen bonds or interact with water’s dipoles. It is insoluble<\/strong> in water.<\/li>\n\n\n\n
- CH3OCH3<\/strong>: Although CH3OCH3 is polar, it does not form hydrogen bonds with water, and thus it is only slightly soluble<\/strong> in water but generally considered insoluble<\/strong>.<\/li>\n\n\n\n
- NH3<\/strong>: NH3 can form hydrogen bonds with water molecules due to its polarity, making it soluble<\/strong> in water.<\/li>\n\n\n\n
- NH4Cl<\/strong>: NH4Cl dissociates into NH4+ and Cl-, and the NH4+ ion can form strong ion-dipole interactions with water molecules. Thus, NH4Cl is highly soluble<\/strong> in water.<\/li>\n<\/ul>\n\n\n\n
Conclusion:<\/h3>\n\n\n\n\n- NH4Cl<\/strong> has the strongest intermolecular forces and the highest boiling point.<\/li>\n\n\n\n
- CH4<\/strong> has the weakest intermolecular forces and the lowest boiling point.<\/li>\n\n\n\n
- NH4Cl<\/strong> and NH3<\/strong> are soluble in water, while CH4<\/strong> is insoluble. CH3OCH3<\/strong> is only slightly soluble, or considered insoluble<\/strong>.<\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Take-home Practice Problems: Intermolecular Forces Consider the following molecules: CH4, NH3, CH3OCH3, and NH4Cl. What type of intermolecular forces do these substances have? CH4: London dispersion forces NH3: London dispersion forces and hydrogen bonding CH3OCH3: London dispersion forces and dipole-dipole forces NH4Cl: London dispersion forces, dipole-dipole forces, and ion-dipole forces Rank these substances by the […]<\/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-259328","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328","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=259328"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=259328"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=259328"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=259328"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Conclusion:<\/h3>\n\n\n\n\n- NH4Cl<\/strong> has the strongest intermolecular forces and the highest boiling point.<\/li>\n\n\n\n
- CH4<\/strong> has the weakest intermolecular forces and the lowest boiling point.<\/li>\n\n\n\n
- NH4Cl<\/strong> and NH3<\/strong> are soluble in water, while CH4<\/strong> is insoluble. CH3OCH3<\/strong> is only slightly soluble, or considered insoluble<\/strong>.<\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Take-home Practice Problems: Intermolecular Forces Consider the following molecules: CH4, NH3, CH3OCH3, and NH4Cl. What type of intermolecular forces do these substances have? CH4: London dispersion forces NH3: London dispersion forces and hydrogen bonding CH3OCH3: London dispersion forces and dipole-dipole forces NH4Cl: London dispersion forces, dipole-dipole forces, and ion-dipole forces Rank these substances by the […]<\/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-259328","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328","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=259328"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=259328"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=259328"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=259328"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
<\/figure>\n","protected":false},"excerpt":{"rendered":"Take-home Practice Problems: Intermolecular Forces Consider the following molecules: CH4, NH3, CH3OCH3, and NH4Cl. What type of intermolecular forces do these substances have? CH4: London dispersion forces NH3: London dispersion forces and hydrogen bonding CH3OCH3: London dispersion forces and dipole-dipole forces NH4Cl: London dispersion forces, dipole-dipole forces, and ion-dipole forces Rank these substances by the […]<\/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-259328","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328","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=259328"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259328\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=259328"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=259328"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=259328"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}