{"id":3749,"date":"2018-07-16T20:30:41","date_gmt":"2018-07-16T20:30:41","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-potsdam-organicchemistry\/?post_type=chapter&p=3749"},"modified":"2018-07-31T03:37:17","modified_gmt":"2018-07-31T03:37:17","slug":"5-1-introduction-to-physical-organic-chemistry","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-potsdam-organicchemistry\/chapter\/5-1-introduction-to-physical-organic-chemistry\/","title":{"raw":"5.1. Introduction to physical organic chemistry","rendered":"5.1. Introduction to physical organic chemistry"},"content":{"raw":"Physical organic chemistry is mainly centered on two main components: Kinetics and thermodynamics.\u00a0 These should normally have been covered in your general chemistry class, but here we will apply these quantitative tools to help us understand what is happening in an organic reaction.\r\n\r\nIn this context, thermodynamics<\/strong> deals with energy and entropy changes that take place during a chemical reaction.\u00a0 It also deals with equilibrium constants for reversible reactions.\r\n\r\nIn contrast, kinetics deals with rates of reactions and energy barriers\/activation energies,\u00a0 It is less useful for reversible reactions, but can be very useful for understanding irreversible reactions.\r\n\r\n\r\n\r\n\r\n\r\n
Field<\/td>\r\nQuestions<\/td>\r\nUsual parameters<\/td>\r\n<\/tr>\r\n
Thermodynamics<\/td>\r\nWill a reaction occur?\u00a0 If so, how far will the reaction go?<\/td>\r\n\u0394G, \u0394H, \u0394S, Keq<\/sub><\/td>\r\n<\/tr>\r\n
Kinetics<\/td>\r\nHow quickly wiil the reaction go?<\/td>\r\n[X] (concn. of X), k (rate constant),\u00a0Ea<\/sub>, \u0394G\u2021<\/sup>.<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nIn some cases, the course of a reaction may be determined by the stability of the favored product.\u00a0 This is referred to as thermodynamic control<\/strong>, and it implies that the reaction can happen easily as most reactant molecules have enough energy to cross the energy barrier (free energy of activation, \u0394G\u2021<\/sup>).\u00a0 In other cases we have kinetic control<\/strong>, where the course of a reaction may be determined by which product has the lowest energy barrier, which implies that the molecules barely have enough energy to cross even the lowest barrier.\u00a0 Both of these scenarios can be seen in the diagram below:\r\n\r\n","rendered":"

Physical organic chemistry is mainly centered on two main components: Kinetics and thermodynamics.\u00a0 These should normally have been covered in your general chemistry class, but here we will apply these quantitative tools to help us understand what is happening in an organic reaction.<\/p>\n

In this context, thermodynamics<\/strong> deals with energy and entropy changes that take place during a chemical reaction.\u00a0 It also deals with equilibrium constants for reversible reactions.<\/p>\n

In contrast, kinetics deals with rates of reactions and energy barriers\/activation energies,\u00a0 It is less useful for reversible reactions, but can be very useful for understanding irreversible reactions.<\/p>\n\n\n\n\n\n
Field<\/td>\nQuestions<\/td>\nUsual parameters<\/td>\n<\/tr>\n
Thermodynamics<\/td>\nWill a reaction occur?\u00a0 If so, how far will the reaction go?<\/td>\n\u0394G, \u0394H, \u0394S, Keq<\/sub><\/td>\n<\/tr>\n
Kinetics<\/td>\nHow quickly wiil the reaction go?<\/td>\n[X] (concn. of X), k (rate constant),\u00a0Ea<\/sub>, \u0394G\u2021<\/sup>.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

In some cases, the course of a reaction may be determined by the stability of the favored product.\u00a0 This is referred to as thermodynamic control<\/strong>, and it implies that the reaction can happen easily as most reactant molecules have enough energy to cross the energy barrier (free energy of activation, \u0394G\u2021<\/sup>).\u00a0 In other cases we have kinetic control<\/strong>, where the course of a reaction may be determined by which product has the lowest energy barrier, which implies that the molecules barely have enough energy to cross even the lowest barrier.\u00a0 Both of these scenarios can be seen in the diagram below:<\/p>\n

\"image\"<\/p>\n\n\t\t\t

\n\t\t\t

Candela Citations<\/h3>\n\t\t\t\t\t
\n\t\t\t\t\t\t
\n\t\t\t\t\t\t\t
CC licensed content, Original<\/div>