A textbook of inorganic chemistry vol.X The metal-amines

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18 shows the energy profile of the propagation steps of this reaction. CH4 (large excess) + Cl2 Initiation step: Propagation steps: Cl Cl + H CH3 + Cl Starting materials TS1 I1 Cl CH3 Cl TS2 400 °C Δ CH3Cl + HCl 2 Cl Cl CH3 H + CH3 Cl + Cl Fig. 17. Mechanism for monochlorination of methane with Cl2. Products E +1 Cl2 + CH4 + Cl • Cl2 + • CH3 + HCl –26 Cl • + CH3Cl + HCl Reaction coordinate Fig. 18. Energy profile of the propagation steps of the monochlorination of methane with Cl2 (enthalpies in kcal/mol).

For example, a carbon-iodine bond results from the overlap of an spn hybrid (2p-like) orbital of the carbon and a 5p or (“5p-like”) orbital of the iodine. The overlap is inherently poorer than that which would be found in the overlap of orbitals of similar size and shape. Overall, however, the homolytic bond dissociation energy of every Cspn-element bond increases in the order n = 3, 2, and 1. e. n = 3, 2, and 1, which, in turn, is due to the fact that the s character of the Cspn-element bond increases in the same order.

10—is this not true. Accordingly, except for this one reaction DH‡ and DHr are proportional for this series of radical-producing thermolyses. 3. DH‡ = const. 3) The thermolyses presented in this chapter are one example of a series of analogous reactions. 3 also holds for many other series of analogous reactions. 3 is that, at least for a reaction series, the more exothermic the enthalpy of reaction, the faster it will be. But this doesn’t mean that all reactions that are exothermic are fast, so be careful.

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