{"id":1808,"date":"2012-09-26T02:14:00","date_gmt":"2012-09-26T02:14:00","guid":{"rendered":"http:\/\/testpreparations.com\/help\/?p=1808"},"modified":"2014-12-02T08:32:01","modified_gmt":"2014-12-02T08:32:01","slug":"molecules-intermolecular-forces","status":"publish","type":"post","link":"https:\/\/schooltutoring.com\/help\/molecules-intermolecular-forces\/","title":{"rendered":"Molecules: Intermolecular Forces"},"content":{"rendered":"

Intermolecular forces are the forces that exist between 2 individual molecules. This is different from\u00a0intra<\/em>molecular forces, which are the forces that exist\u00a0within\u00a0<\/em>a molecule (ie. ionic\/covalent bonds).<\/p>\n

Intermolecular forces are generally described by a general term, Van der Waals forces.<\/p>\n

Dipole-dipole Force<\/h4>\n

– the attraction of a dipole on one molecule for the dipole of another molecule<\/p>\n

– the strength of this force depends on the strength of the dipole<\/p>\n

Example: HCl molecules have dipole-dipole forces between them<\/p>\n

Ion-dipole Force<\/h4>\n

– the attraction of an ion (anion\/cation) for a dipole<\/p>\n

Example: NaCl dissolves in water because of ions in NaCl are attracted to the dipoles in the water molecule<\/p>\n

Induced Intermolecular Forces<\/h4>\n

1) Ion induced dipole<\/h5>\n

– when an ion comes near a non-polar molecule, the ion can induce a dipole in the non-polar molecule<\/p>\n

Example: In blood, Fe+2 carries oxygen<\/p>\n

2) Dipole induced dipole<\/h5>\n

– when a dipole comes near a non-polar molecule, the dipole can induce a dipole in the non-polar molecule<\/p>\n

Example: Oxygen dissolves slightly in water<\/p>\n

London Dispersion Forces<\/h4>\n

– the only force that exists between 2 non-polar molecules<\/p>\n

– ALL things have London forces<\/p>\n

– temporary attractive force between atoms\/molecules close to each other<\/p>\n

– strength of the force depends on the size (number of protons) of the molecule, larger molecules have a stronger London Dispersion Force<\/p>\n

Example: Methane (CH4) vs Octane (C8H18)<\/p>\n

Hydrogen Bonding<\/h4>\n

– stronger than dipole-dipole force<\/p>\n

– occurs when when a highly electronegative element (Ex. N, O, F) is bonded to hydrogen<\/p>\n

– since the element is highly electronegative, it ‘takes’ the electron from the hydrogen<\/p>\n

– another highly electronegative element from another molecule then binds to that hydrogen<\/p>\n

Example: Hydrogen bonding between water molecules<\/p>\n

Looking to do the PSAT? We can help with PSAT<\/a> Prep<\/p>\n

This article was written for you by Samantha<\/strong>, one of the tutors with SchoolTutoring Academy<\/span>.<\/p>\n","protected":false},"excerpt":{"rendered":"

Intermolecular forces are the forces that exist between 2 individual molecules. This is different from\u00a0intramolecular forces, which are the forces that exist\u00a0within\u00a0a molecule (ie. ionic\/covalent bonds). Intermolecular forces are generally described by a general term, Van der Waals forces. Dipole-dipole Force – the attraction of a dipole on one molecule for the dipole of another […]<\/p>\n","protected":false},"author":6,"featured_media":1811,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"inline_featured_image":false,"footnotes":""},"categories":[2841,16],"tags":[3351,3360,3416,3421],"class_list":["post-1808","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-act","category-science","tag-what-are-dipole-dipole-forces","tag-what-are-intermolecular-forces","tag-what-is-hydrogen-bonding","tag-what-is-london-dispersion"],"acf":[],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/posts\/1808","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/users\/6"}],"replies":[{"embeddable":true,"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/comments?post=1808"}],"version-history":[{"count":0,"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/posts\/1808\/revisions"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/media\/1811"}],"wp:attachment":[{"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/media?parent=1808"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/categories?post=1808"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/tags?post=1808"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}