[PDF] [PDF] Reactions of Alkenes

[PDF] Mechanisms – Answers a Addition of HCl or HBr to an alkene Answer

Addition of HCl or HBr to an alkene Answer: Step 1 The nucleophilic pi bond attacks the proton of H-Cl, forming a carbocation on the Markovnikov end (most 

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+ k[alkene][XY] 2 C=C X-Y X-Y Additions of HCl, HBr The ionic addition of HX produces the more stable carbocation which then reacts with the bromide ion

[PDF] Reactions of Alkenes

Markovnikov's rule: In the addition of HX or H2O to an alkene, H adds to the carbon of the double bond having the greater In addition of HCl to an alkene

[PDF] Reactions of Alkenes

The alkene abstracts a proton from the HBr, and a carbocation and bromide ion are (HCl and HI perform analogous electrophilic addition reactions)

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The most characteristic reaction of alkenes is addition to the carbon–carbon The addition of HCl to propene gives 2-chloropropane (isopropyl chloride); 

[PDF] Addition of Hydrogen Halides To Alkenes - Master Organic Chemistry

Acids (HX) include HCl, HBr, and HI • First step is protonation of alkene to give a carbocation, with the pi bond acting as a base • Rearrangements may occur to 

[PDF] Alkenes - Addition Reactions - BITS Pilani

3 Addition of hydrogen halides — C = C — + HX → — C — C — H X a) HX = HI, HBr, HCl b) Markovnikov orientation CH 3 CH=CH 2 + HI → CH

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6 4 Electrophilic Addition of Hydrogen Halides to Alkenes 0°C CH 3 Cl CH 3 (100 ) Markovnikov's Rule Example 3 Example 3 HCl 

[PDF] 46 ADDITION REACTIONS OF ALKENES 47 ADDITION OF

In an addition reaction, the carbon–carbon p bond of the alkene and the XLY bond of the reagent addition of HCl because additions of HBr and HI are faster

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1

Reactions

of Alkenes

Chapter 6

2 • A reaction mechanism describes how a reaction occurs and explains the following. Which bonds are broken and which new ones are formed. The order and relative rates of the various bond-breaking and bond-forming steps.

If in solution, the role of the solvent.

If there is a catalyst, the role of a catalyst.

The position of all atoms and energy of the entire system during the reaction.

Reactions Mechanisms

3 • Gibbs free energy change, ΔG0: - A thermodynamic function relating enthalpy, entropy, and temperature. - Exergonic reaction:A reaction in which the Gibbs free energy of the products is lower than that of the reactants; the position of equilibrium for an exergonic reaction favors products - Endergonic reaction:A reaction in which the Gibbs free energy of the products is higher than that of the reactants; the position of equilibrium for an endergonic reaction favors starting materials. ΔΔΔΔG0 = ΔΔΔΔH0 -TΔΔΔΔS0

Gibbs Free Energy

4 • Enthalpy change, ΔΗ0: The difference in total bond energy between reactants and products. - a measure of bond making (exothermic) and bond breaking (endothermic). • Heat of reaction, ΔΗ0:The difference in enthalpy between reactants and products. - Exothermic reaction:A reaction in which the enthalpy of the products is lower than that of the reactants; a reaction in which heat is released. - Endothermic reaction:A reaction in which the enthalpy of the products is higher than that of the reactants; a reaction in which heat is absorbed.

Energy Diagrams

5 • Energy diagram:A graph showing the changes in energy that occur during a chemical reaction. • Reaction coordinate:A measure in the change in positions of atoms during a reaction.

Reaction

coordinate

Energy

Energy Diagrams

6 • Transition state ‡: - An unstable species of maximum energy formed during the course of a reaction. - A maximum on an energy diagram. • Activation Energy, ΔG‡: The difference in Gibbs free energy between reactants and a transition state. - If ΔG‡is large, few collisions occur with sufficient energy to reach the transition state; reaction is slow. - If ΔG‡is small, many collisions occur with sufficient energy to reach the transition state; reaction is fast.

Activation Energy

7 - An energy diagram for a one-step reaction with no intermediate.quotesdbs_dbs3.pdfusesText_6