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Introduction of Reaction Characteristics

A. Reaction Rates: Some reactions continue very swiftly, and some reactions continue very slowly that they are not normally observed. Among variables that affects the reaction rates are temperature (reactions are generally faster at a higher temperature), solvent and reactant or reagent concentrations. Valuable information of the reaction mechanisms may be obtained by studying the manner in which the rate of a reaction changes as the concentrations of the reagents and reactant are varied. This field of study is called the kinetics.

B. Intermediates: Many reactions continue in a step by step fashion. It can be explained convincingly if an intermediate species can be isolated and shown to proceed to similar products under the reaction conditions. Several intermediates are the stable compounds in their own right; however some are so reactive so that isolation is not possible. However, the confirmation for their existence may be obtained by so many other means, including the spectroscopic inference or observation from kinetic results.

Factors that Influence Reactions

It is useful to known some common features of a reaction that have a significant effect on its facility. Some of the most significant of these are:

A. Energetics: A reacting system's potential energy changes as the reaction progresses. The entire modification may be exothermic (energy is released) or endothermic (energy must be added), and there is generally an activation energy requirement as well. The Standard Bond Energies' Tables are extensively used by chemists for estimating the energy change in a specific reaction. According to the rule, compounds that are constructed of strong covalent bonds are more stable than compounds incorporating one or more relatively weak bonds.

B. Electronic Effects: The electrons' distribution at sites of reaction (functional groups) is a specifically essential feature. The Electron deficient species or groups, which may be or may not be positively charged, are attracted to the electron rich species or groups, which may be or may not be negatively charged. We are referring to these species as electrophiles & nucleophiles respectively. Generally, opposites attract and like repel.

Charge distribution in a molecule is generally discussed with respect to two interacting effects: A function of the electronegativity differences that exist between atoms or group of atoms known as inductive effect; and the electrons move in a discontinuous fashion between parts of a molecule known as resonance effect.

C. Steric Effects: Atoms occupy space. When they crowded together van der Waals repulsions generate an unfavorable steric hindrance. The Steric hindrance may affect conformational equilibria, as well as destabilizing transition states of reactions.

D. Stereoelectronic Effects: In several reactions molecular or atomic orbitals interact with each other in a manner that has an optimal geometrical or configurational alignment. The Departure from this alignment inhibits the reaction.

E. Solvent Effects: various reactions are conducted in solution, not in a gaseous state. Solvent that is selected for a given reaction may exert a strong influence on its course. Remember, the solvents are chemicals and most undergo chemical reaction under the right conditions.

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