{"id":5955,"date":"2020-10-13T11:28:04","date_gmt":"2020-10-13T05:58:04","guid":{"rendered":"http:\/\/astan.lk\/al_virtualclassroom\/?p=5955"},"modified":"2020-10-13T11:58:58","modified_gmt":"2020-10-13T06:28:58","slug":"secondary-interactions","status":"publish","type":"post","link":"https:\/\/astan.lk\/al_virtualclassroom\/secondary-interactions\/","title":{"rendered":"Secondary interactions"},"content":{"rendered":"<p>Polarization &#8211; The asymmetrical distribution of electron clouds between two atoms involved in a chemical bond due to the difference in electronegativities of the two atoms concerned or due to another external influence is known as polarization.<\/p>\n<p><strong><span style=\"text-decoration: underline;\">Dipole moment<\/span><\/strong><\/p>\n<p>The product of the charge ( \u03b4 ) present on individual atoms in such a molecule and the length of the bond between the atoms is called the dipole moment ( \u00b5 = \u03b4 \u00d7 r ) of the bond. In polyatomic molecules, the dipole moment is considered for each bond. Their resultant is taken as the dipole moment of the molecule.<\/p>\n<p><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/dmm.jpg\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter size-full wp-image-8252\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/dmm.jpg\" alt=\"dmm\" width=\"292\" height=\"173\" \/><\/a><\/p>\n<p>The resultant of the dipole moments of all the N- H bonds gives the dipole moment of the NH3 molecule and the resultant of the dipole moments of all the N- F bonds gives the dipole moment of the NF3 molecule.<\/p>\n<p>\u2022 For some symmetric molecules the dipole moment is zero<\/p>\n<p><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/d0-1.png\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter size-full wp-image-8333\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/d0-1.png\" alt=\"d0\" width=\"330\" height=\"115\" \/><\/a><\/p>\n<h3><span style=\"text-decoration: underline;\">Secondary interactions<\/span><\/h3>\n<p>All types of intermolecular interactions exist among molecules are commonly referred as van der Waals interactions. \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0Those interactions can be categorized into five types. \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 Ion \u2013 dipole interactions \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 Dipole \u2013 dipole interactions and hydrogen bonds \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 Ion \u2013 induced dipole interactions \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 Dipole \u2013 induced dipole interactions \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 Dispersion (London) forces<\/p>\n<p><span style=\"text-decoration: underline;\"><strong>Ion \u2013 dipole interactions <\/strong><\/span><\/p>\n<p>These interactions are said to take place when polar molecules are attracted to a cation or an anion. The strength of these interactions depend on the charge and size of the ions and on the magnitude of the dipole.<\/p>\n<p><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/idi.png\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-8246\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/idi.png\" alt=\"idi\" width=\"190\" height=\"158\" \/><\/a><\/p>\n<p><span style=\"text-decoration: underline;\"><strong>Dipole \u2013 dipole interactions<\/strong><\/span><\/p>\n<p>These forces are found in polar molecules which have permanent dipole<\/p>\n<p><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/dpdp.png\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-8245\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/dpdp.png\" alt=\"dpdp\" width=\"238\" height=\"57\" \/><\/a><\/p>\n<p><strong><span style=\"text-decoration: underline;\">Hydrogen bonds<\/span><\/strong><\/p>\n<p>Hydrogen bond is a special type of electrostatic interaction between a hydrogen atom covalently bonded to an electronegative element (X) and another electronegative element (Y) such as fluorine or oxygen or nitrogen which has one or more lone pairs. This interaction can be represented by X<sup>\u03b4-<\/sup>\u2014H<sup>\u03b4+\u00a0<\/sup>&#8211; &#8211; &#8211; &#8211; Y<sup>\u03b4-<\/sup><\/p>\n<p><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/h.png\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter size-full wp-image-8244\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/h.png\" alt=\"h\" width=\"230\" height=\"132\" \/><\/a><\/p>\n<p>&nbsp;<\/p>\n<p>Existence of hydrogen bonding can be proved by referring to the variation of boiling temperatures of group 15, 16 and 17 hydrides.<\/p>\n<p><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/figure-1.jpg\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-8243\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/figure-1.jpg\" alt=\"figure 1\" width=\"495\" height=\"384\" \/><\/a><\/p>\n<p><span style=\"text-decoration: underline;\"><strong>Ion &#8211; induced dipole interactions<\/strong><\/span><\/p>\n<p><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/chemical-bonding-2-by-aditya-abeysinghe-11-638-1.jpg\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-8338\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/chemical-bonding-2-by-aditya-abeysinghe-11-638-1.jpg\" alt=\"chemical-bonding-2-by-aditya-abeysinghe-11-638\" width=\"470\" height=\"363\" \/><\/a><\/p>\n<p><strong><span style=\"text-decoration: underline;\">Dipole &#8211; induced dipole interactions <\/span><\/strong><\/p>\n<p>This type of attraction is found between an uncharged non-polar and a polar species. \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/idi.png\"><br \/>\n<\/a>eg. Dissolving non-polar species such as O2 , I2 , Xe, etc. in water.<\/p>\n<p><strong><span style=\"text-decoration: underline;\">Dispersion forces (London forces or London dispersion forces)<\/span><\/strong><\/p>\n<p><a href=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/ldf-1.jpg\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-8337\" src=\"http:\/\/astan.lk\/al_virtualclassroom\/wp-content\/uploads\/2017\/01\/ldf-1.jpg\" alt=\"ldf\" width=\"234\" height=\"128\" \/><\/a><\/p>\n<p>Interactions between non-polar molecules or atoms are referred as dispersion forces. Any non-polar molecule can be temporary polarized due to an instantaneous deformation of its electron cloud. Due to the polarity of a such molecule another non polar molecule can also be temporary polarized. Interactions between such molecules are referred as dispersion forces. Such forces exist between any molecules.<\/p>\n<p>Generally dispersion forces are the weakest among all types of van der Waals forces. However, there are instances where strength of dispersion forces exceeds dipole &#8211; dipole interactions. \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 eg &#8211; \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<span style=\"text-decoration: underline;\"> Compound<\/span> \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<span style=\"text-decoration: underline;\">Melting point \u00a0<\/span> \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 <span style=\"text-decoration: underline;\">Nature of secondary interaction<\/span> \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 CH3 F \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0-142 \u00b0C \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0Dipole-dipole interactions and dispersion forces \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 CCl4 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 -23 \u00b0C \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0Dispersion forces<\/p>\n<p>&nbsp;<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Polarization &#8211; The asymmetrical distribution of electron clouds between two atoms involved in a chemical bond due to the difference in electronegativities of the two atoms concerned or due to another external influence is known as polarization. Dipole moment The product of the charge ( \u03b4 ) present on individual atoms in such a molecule [&hellip;]<\/p>\n","protected":false},"author":842,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"_monsterinsights_skip_tracking":false,"_monsterinsights_sitenote_active":false,"_monsterinsights_sitenote_note":"","_monsterinsights_sitenote_category":0,"footnotes":""},"categories":[14,1654],"tags":[],"class_list":["post-5955","post","type-post","status-publish","format-standard","hentry","category-chemistry","category-unit-02"],"acf":[],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v26.9 - https:\/\/yoast.com\/product\/yoast-seo-wordpress\/ -->\n<title>Secondary interactions - Learning &amp; Education Portal<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/astan.lk\/al_virtualclassroom\/secondary-interactions\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Secondary interactions - Learning &amp; Education Portal\" \/>\n<meta property=\"og:description\" content=\"Polarization &#8211; The asymmetrical distribution of electron clouds between two atoms involved in a chemical bond due to the difference in electronegativities of the two atoms concerned or due to another external influence is known as polarization. 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