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  Alkenes Reduction Reactions Homework Help - K-12 Grade Level, College Level Chemistry

Introduction to Alkenes Reduction Reactions

Hydrogenation is Addition of hydrogen to a carbon-carbon double bond. The complete effect of this type of an addition is the reductive removal of the double bond functional group. Regioselectivity is not an issue, because similar group (a hydrogen atom) is bonded to each of the double bond carbons. The simple most sources of the two hydrogen atoms is molecular hydrogen (H2) but mixing alkenes with hydrogen does not product in any discernible reaction. Even though the entire hydrogenation reaction is exothermic, high activation energy stops it from taking place under usual conditions. This restriction can be circumvented by the make use of a catalyst, as displayed in the diagram.

1752_Functional Group Reactions Reduction Homework Help.jpg

Without being consumed or appearing as part of the product Catalysts are substances which changes the rate (velocity) of a chemical reaction. Catalysts act by lowering the activation energy of reactions, but they do not alter the relative potential energy of the products and reactants. Finely divided metals, like platinum, nickel and palladium, are in between the most extensively used hydrogenation catalysts. Catalytic hydrogenations come into existence in at least two stages, as represented in the picture. 1st, on the surface of the catalyst along with some of the hydrogen the alkene must be adsorbed. After that, two hydrogens move from the metal surface to the carbons of the double bond, and the resultant saturated hydrocarbon, which is more weakly adsorbed, remains the catalyst surface. The precise timing and nature of the last events is not well understood.

As displayed in the energy diagram, the alkenes' hydrogenation is exothermic and heat is released consequent to the ΔE (green in color) in the picture. This heat of reaction can be employed to evaluate the thermodynamic stability of alkenes that having distinct numbers of alkyl substituents on the double bond. For an instance, the table lists the heats of hydrogenation for three C5H10 alkenes which give similar alkane product (2-methylbutane). Because a large heat of reaction point out a high energy reactant, these heats are in reverse proportional to the stabilities of the alkene isomers. To a rough approximation, we observe that each alkyl substituent on a double bond stabilizes this functional group by a bit more than 1 kcal/mole.

Alkene Isomer

(CH3)2CHCH=CH2
3-methyl-1-butene

CH2=C(CH3)CH2CH3
2-methyl-1-butene

(CH3)2C=CHCH3
2-methyl-2-butene

Heat of Reaction
( ΔHº )

-30.3 kcal/mole

-28.5 kcal/mole

-26.9 kcal/mole

From the technique displayed here we would suppose the addition of hydrogen to occur with syn-stereoselectivity. This is frequently true, but the hydrogenation catalysts may also cause isomerization of the double bond prior to hydrogen addition, in which case stereoselectivity may be not certain. 
The formation of transition metal complexes with alkenes has been persuasively illustrated by the isolation of stable platinum complexes like Zeise's salt, K[PtCl3(C2H4)].H2O, and ethylenebis(triphenylphosphine)platinum, [(C6H5)3P]2Pt(H2C=CH2). In the later, platinum is three-coordinate and zero-valent, where Zeise's salt is a derivative of platinum (II). Identical complexes have been reported for palladium and nickel, metals which also function as catalysts for alkene hydrogenation.

A non-catalytic process for the syn-addition of hydrogen makes use of the unstable compound diimide, N2H2. This reagent should be newly generated in the reaction system, generally by oxidation of hydrazine and the strongly exothermic reaction is favored through the elimination of nitrogen gas (a very stable compound). Diimide may present as cis-trans isomers; only the cis-isomer serves like a reducing agent. Illustrations of alkene reductions by both procedures are displayed in the following diagram.

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