1. Chapter 9 Alkynes

2. 9.1 Sources of Alkynes

3. Industrial preparation of acetylene is by dehydrogenation of ethylene CH 3 CH 3 800°C 1150°C cost of energy makes acetylene a more expensive industrial chemical than ethylene H2CH2CH2CH2C CH 2 H2CH2CH2CH2C HCCH H2H2H2H2+ H2H2H2H2+Acetylene

4. 9.2 Nomenclature

5. HC CH Acetylene and ethyne are both acceptable IUPAC names for Higher alkynes are named in much the same way as alkenes except using an -yne suffix instead of -ene. HC CCH 3 Propyne HC CCH 2 CH 3 1-Butyne (CH 3 ) 3 CC CCH 3 4,4-Dimethyl-2-pentyne Nomenclature

6. The physical properties of alkynes are similar to those of alkanes and alkenes. 9.3 Physical Properties of Alkynes

7. 9.4 Structure and Bonding in Alkynes: sp Hybridization

8. linear geometry for acetylene C C H H 120 pm 106 pm C C CH 3 H 121 pm 146 pm 106 pm Structure

9. Cyclononyne is the smallest cycloalkyne stable enough to be stored at room temperature for a reasonable length of time. Cyclooctyne polymerizes on standing. Cycloalkynes

10. 2s2s2s2s 2p2p2p2p 2sp 2sp Mix together (hybridize) the 2s orbital and one of the three 2p orbitals 2p2p2p2p sp Hybridization in Acetylene

11. 2sp 2sp Mix together (hybridize) the 2s orbital and one of the three 2p orbitals 2p2p2p2p Each carbon has two half-filled sp orbitals available to form  bonds. sp Hybridization in Acetylene

12. Each carbon is connected to a hydrogen by a  bond. The two carbons are connected to each other by a  bond and two  bonds. Figure 9.2 (a)  Bonds in Acetylene

13. One of the two  bonds in acetylene is shown here. The second  bond is at right angles to the first. Figure 9.2 (b)  Bonds in Acetylene

14. This is the second of the two  bonds in acetylene. Figure 9.2 (c)  Bonds in Acetylene

15. The region of highest negative charge lies above and below the molecular plane in ethylene. The region of highest negative charge encircles the molecule around its center in acetylene. Figure 9.3 Electrostatic Potential in Acetylene

16. C—C distance C—H distance H—C—C angles C—C BDE C—H BDE % s character pKapKapKapKa pKapKapKapKa 153 pm 111 pm 111.0°111.0° 368 kJ/mol 410 kJ/mol sp 3 25%25% 6262 134 pm 110 pm 121.4°121.4° 611 kJ/mol 452 kJ/mol sp 2 33%33% 4545 120 pm 106 pm 180°180° 820 kJ/mol 536 kJ/mol spsp 50%50% 2626 hybridization of C Ethane Ethylene Acetylene Table 9.1 Comparison of Ethane, Ethylene, and Acetylene