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  Reaction Energetics Homework Help - K-12 Grade Level, College Level Chemistry

Introduction of Reaction Energetics

Chemical reactions involve the making and breaking some or even all of the bonds that hold together the atoms of reactant and product molecules. For breaking the bonds energy is required and because the force of different types of bonds is different from each other, there is a often major overall energy change in the course of a reaction. In combustion of methane, for an instance, in the reactant molecules all six bonds are broken and six new bonds are produced in product molecules (equation 1).

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Reactants                                          Product

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In this case sum of the product bond strengths, is greater than the sum of reactant bond strengths; subsequently, than reactants the products are energetically (or thermodynamically) more stable and in the form of heat energy is released. this types of reactions are called exothermic. It is usefull to think of the exothermic reactions as proceeding from a higher energy (less stable) reactant state to a lower energy (more stable) product state, as displayed in the picture. Endothermic are the Reactions in which the products are higher energy than the reactants require energy input to occur. An essential case of an endothermic process is the Photosynthesis in the equation no.2. Energy in form of photons (sunlight) drives reaction, as a catalyst which requires chlorophyll.

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Reactants                                                                 Products

Ordinary sense suggests that molecules in which bonds are weak will be not more stable than molecules having stronger bonds. Before we described the strengths of bond, as the energy required to break a bond into neutral fragments (radicals or atoms). So, Sum of all bond energies of a molecule can be considered its atomization energy that is the energy which is required to break the molecule completely into its component atoms. To the group of isomers if this concept is applied, it should be clear that all isomers will have a general atomization state and that total bond energy of each isomer is oppositely related to that isomer's potential energy. So, that isomer having the lowest total bond energy has the greatest potential energy & vice versa and is thermodynamically most stable. In short, the energy that must be introduced to break a bond and not component of a molecule's potential energy is known as bond energy.

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Three C6H12 isomers in the diagram demonstrate this relationship. The Cyclohexane is made up of six C-C sigma bonds and twelve C-H sigma bonds configured in a strain-free six-membered ring. Isomer having a double bond, 1-hexene, alternatively, has four C-C single bonds (all sigma) and one C-C double bond (one sigma and one pi bond). Since sigma bond is stronger than a pi bond, the cyclohexane has larger total bond energy (by nearly 20 kcal/mol) and is thermodynamically more stable than 1-hexene. Four-membered ring compound that is the ethylcyclobutane has the same kinds of bonds as cyclohexane but they are weakened by ring strain to such type of a degree that this isomer is even less stable (thermodynamically) than 1-hexene.

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