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Elimination reaction of cyclohexanol to cyclohexene with sulfuric acid and heat [1] An elimination reaction is a type of organic reaction in which two substituents are removed from a molecule in either a one- or two-step mechanism. [2] The one-step mechanism is known as the E2 reaction, and the two-step mechanism is known as the E1 reaction ...
The rate law depends on the first order concentration of two reactants, making it a 2nd order (bimolecular) elimination reaction. Factors that affect the rate determining step are stereochemistry, leaving groups, and base strength. A theory, for an E2 reaction, by Joseph Bunnett suggests the lowest pass through the energy barrier between ...
In theoretical chemistry, Marcus theory is a theory originally developed by Rudolph A. Marcus, starting in 1956, to explain the rates of electron transfer reactions – the rate at which an electron can move or jump from one chemical species (called the electron donor) to another (called the electron acceptor). [1]
The electron sink which ultimately accepts the electron density is the nucleofuge (leaving group), with bond forming and bond breaking occurring simultaneously at the transition state (marked with a double-dagger). The rates of S N 2 reactions are dependent on the concentration of the haloalkane and the nucleophile.
The order of reactivity, as shown by the vigour of the reaction with water or the speed at which the metal surface tarnishes in air, appears to be Cs > K > Na > Li > alkaline earth metals, i.e., alkali metals > alkaline earth metals, the same as the reverse order of the (gas-phase) ionization energies.
The rate for a bimolecular gas-phase reaction, A + B → product, predicted by collision theory is [6] = = ()where: k is the rate constant in units of (number of molecules) −1 ⋅s −1 ⋅m 3.
Written as a reduction, cathodic current is positive. The net current density is the difference between the cathodic and anodic current density. Exchange current densities reflect intrinsic rates of electron transfer between an analyte and the electrode. Such rates provide insights into the structure and bonding in the analyte and the electrode.
As an example, self-exchange describes the degenerate reaction between permanganate and its one-electron reduced relative manganate: [MnO 4] − + [Mn*O 4] 2− → [MnO 4] 2− + [Mn*O 4] −. In general, if electron transfer is faster than ligand substitution, the reaction will follow the outer-sphere electron transfer route.