Alkenes and Alkynes

1. Alkenes and Alkynes Alkene: A hydrocarbon that contains one or more carbon-carbon double bonds. • Ethylene is the simplest alkene. Alkyne: A hydrocarbon that contains one or more carbon-carbon triple bonds. • Acetylene is the simplest alkyne.

2. Alkenes Structure: • The VSEPR model predicts bond angles of 120° about each carbon of a double bond. • In ethylene, the actual angles are close to 120°. • In substituted alkenes, angles about each carbon of the double bond may be greater than 120° because of repulsion between groups bonded to the double bond.

3. Alkenes Cis-trans isomerism • Because of restricted rotation about a carbon-carbon double bond, an alkene with two different groups on each carbon of the double bond shows cis-trans isomerism.

4. Alkenes—IUPAC Names To name an alkene; • The parent name is that of the longest chain that contains the C=C. • Number the chain from the end that gives the lower numbers to the carbons of the C=C. • Locate the C=C by the number of its first carbon. • Use the ending -ene to show the presence of the C=C • Branched-chain alkenes are named in a manner similar to alkanes in which substituted groups are located and named.

5. Alkenes—IUPAC Names Examples

6. Alkynes—IUPAC Names Follow the same rules as for alkenes, but use the ending -yne to show the presence of the triple bond.

7. Cycloalkenes To name a cycloalkene: • Number the carbon atoms of the ring double bond 1 and 2 in the direction that gives the lower number to the substituent encountered first. • Note that it is not necessary to explicitly number the position of the double bond in a cycloalkene as in linear alkenes. • Number and list substituents in alphabetical order.

8. Cycloalkenes • Alkenes that contain more than one double bond are named as alkadienes, alkatrienes, and so forth. • Those that contain several double bonds are referred to more generally as polyenes (Greek: poly, many).

9. Physical Properties • Alkenes and alkynes are nonpolar compounds. • The only attractive forces between their molecules are London dispersion forces. • Their physical properties are similar to those of alkanes with the same carbon skeletons. • Alkenes and alkynes are insoluble in water but soluble in one another and in nonpolar organic liquids. • Alkenes and alkynes that are liquid or solid at room temperature have densities less than 1.0 g/mL; they float on water.

10. Reactions of Alkenes

11. Reactions of Alkenes Most alkene addition reactions are exothermic. • the products are more stable (lower in energy) than the reactants. • Just because they are exothermic doesn’t mean that alkene addition reactions occur rapidly. • Reaction rate depends on the activation energy. • Many alkene addition reactions require a catalyst.

12. Addition of HX Addition of HX (HCl, HBr, or HI) to an alkene gives a haloalkane. • H adds to one carbon of the C=C and X to the other. • Reaction is regioselective. One direction of bond forming (or bond breaking) occurs in preference to all other directions. • Markovnikov’s rule: H adds to the less substituted carbon and X to the more substituted carbon.

13. Addition of HX Chemists account for the addition of HX to an alkene by a two-step reaction mechanism. • We use curved arrows to show the repositioning of electron pairs during a chemical reaction. • The tail of an arrow shows the origin of the electron pair (either on an atom or in the double bond). • The head of the arrow shows its new position. • Curved arrows show us which bonds break and which new ones form.

14. Common Mechanism Steps Pattern 1: Add a proton An acid is a proton donor and a base is a proton acceptor. We can use curved arrows to show how a proton transfer occurs. Patterns 2: Take a proton away. If we run the above reaction, in reverse it corresponds to taking a proton away.

15. Common Mechanism Steps • Pattern 3: Reaction of an electrophile and a nucleophile to form a new covalent bond. • An electrophile is an electron-poor species that can accept a pair of electrons to form a new covalent bond. • A nucleophile is an electron-rich species that can donate a pair of electrons to form a new covalent bond.

16. Common Mechanism Steps • Pattern 4: Reaction of a proton donor with a carbon-carbon double bond to form a new covalent bond. The double bond provides both of the electrons that forms the new covalent bond. In the following reaction we show the hydronium ion as the proton donor. • While the above equation is the most accurate way to show the proton transfer, we will simplify the equation to just show the proton and formation of the new covalent bond.

17. Addition of HCl to 2-Butene Step 1: Add a proton • Reaction of the carbon-carbon double bond with H+ gives a secondary (2°) carbocation intermediate, a species containing a carbon atom with only three bonds to it and bearing a positive charge. Step 2: Reaction of an electrophile and a nucleophile to form a new carbon-carbon bond. • Reaction of the carbocation intermediate with chloride ion completes the addition.

18. Addition of H2O Addition of water is called hydration. • Hydration is acid catalyzed, most commonly by H2SO4. • Hydration follows Markovnikov’s rule; H adds to the less substituted carbon and OH adds to the more substituted carbon.

19. Addition of H2O • Step 1: Add a proton • Step 2: Reaction of an electrophile and a nucleophile to form a new covalent bond. Step 3; Take a proton away.

20. Addition of Cl2 and Br2 Addition takes place readily at room temperature. • Reaction is generally carried out using pure reagents, or mixing them in a nonreactive organic solvent. • Addition of Br2 is a useful qualitative test for the presence of a carbon-carbon double bond. • Br2 has a deep red color; dibromoalkanes are colorless.

21. Addition of H2—Reduction Virtually all alkenes add H2 in the presence of a transition metal catalyst, commonly Pd, Pt, or Ni.