HL Bonding

1. HL Bonding Hybridisation

2. Hybridization is a model which is used to explain the behavior of atomic orbitals during the formation of covalent bonds. • When an atom forms a covalent bond with another atom, the orbitals of the atom become rearranged. • This rearrangement results in the "mixing" of orbitals. From: http://www.bookrags.com/Orbital_hybridisation

3. Hybridisation • When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals

4. Hybridisation • When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals • This process is called hybridisation

5. Hybridisation • When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals • This process is called hybridisation • The orbitals formed in this process are of the same energy

6. Hybridisation • When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals • This process is called hybridisation • The orbitals formed in this process are of the same energy • The orbitals are symmetrically arranged

7. Hybridisation • When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals • This process is called hybridisation • The orbitals formed in this process are of the same energy • The orbitals are symmetrically arranged • 3 types - sp3, sp2 and sp

8. Hybridisation • When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals • This process is called hybridisation • The orbitals formed in this process are of the same energy • The orbitals are symmetrically arranged • 3 types - sp3, sp2 and sp • Hybridisation doesn’t just occur in carbon

9. sp3 hybridisation • E.g. methane, ammonia, water

10. sp3 hybridisation • E.g. methane, ammonia, water • Methane contains 4 equal C - H bonds, therefore the outer shell electrons (2s2 2p2) have merged to form 4 hybrid sp3 orbitals of equal energy

11. sp3 hybridisation • E.g. methane, ammonia, water • Methane contains 4 equal C - H bonds, therefore the outer shell electrons (2s2 2p2) have merged to form 4 hybrid sp3 orbitals of equal energy • One electron is in each of the hybrid orbitals and can form a sigma bond with a hydrogen atom

12. sp3 hybridisation in methane From http://ibchem.com/IB/ibnotes/full/bon_htm/14.2.htm

13. sp3 hybridisation • The four hybrid orbitals arrange themselves to be as far apart as possible because of the repulsion between the electrons • This produces the tetrahedral shape of methane and a bond angle of 109.5º

14. sp3 hybridisation in methane From http://www.mhhe.com/physsci/chemistry/carey5e/Ch02/ch4hybrid2.gif

15. sp3 hybridisation in water • A similar thing occurs in water - 4 sp3 hybridised orbitals are formed around the oxygen and spread out in a tetrahedral shape

16. sp3 hybridisation in water • A similar thing occurs in water - 4 sp3 hybridised orbitals are formed around the oxygen and spread out in a tetrahedral shape • Two of these orbitals contain lone/non-bonded pairs of electrons, and the other two form sigma bonds with the hydrogen atoms

17. sp3 hybridisation in water • A similar thing occurs in water - 4 sp3 hybridised orbitals are formed around the oxygen and spread out in a tetrahedral shape • Two of these orbitals contain lone/non-bonded pairs of electrons, and the other two form sigma bonds with the hydrogen atoms • As the non-bonded pairs are closer to the centre of the molecule, they force the two O-H bonds slightly closer together forming a bond angle of 105 º

18. sp3 hybridisation in water From: http://www.rjc.edu.sg/subjects/chemistry/resources/simulations-hybridisation/lecture28.html

19. sp3 hybridisation in water From: http://www.rjc.edu.sg/subjects/chemistry/resources/simulations-hybridisation/lecture28.html

20. sp2 hybridisation • E.g. ethene - C2H4, BF3

21. sp2 hybridisation • E.g. ethene - C2H4, BF3 • In ethene, one 2p orbital from each carbon atom forms a pi bond - this is not involved in hybridisation

22. sp2 hybridisation • E.g. ethene - C2H4, BF3 • In ethene, one 2p orbital from each carbon atom forms a pi bond - this is not involved in hybridisation • The remaining 2s orbital and two 2p orbitals hybridise to form three sp2 orbitals, which form sigma bonds - two with hydrogen atoms and one between the C atoms

23. sp2 hybridisation in ethene From: http://www.rsu.ac.th/science/chem/yupa/Arjarnyupa/1historyorganic/sp2.htm

24. Hybridisation in BF3 From: http://www.rjc.edu.sg/subjects/chemistry/resources/simulations-hybridisation/lecture28.html

25. sphybridisation • E.g. ethyne (C2H2), BeF2

26. sphybridisation • E.g. ethyne (C2H2), BeF2 • The 2s orbital hybridises with just one of the 2 p orbitals

27. sphybridisation • E.g. ethyne (C2H2), BeF2 • The 2s orbital hybridises with just one of the 2 p orbitals • In BeF2 this is because there are only 2 electrons in the 2nd shell (1s2 2s2)

28. sphybridisation • E.g. ethyne (C2H2), BeF2 • The 2s orbital hybridises with just one of the 2 p orbitals • In BeF2 this is because there are only 2 electrons in the 2nd shell (1s2 2s2) • In ethyne this is because two pi bonds are formed between the carbons leaving only 2 electrons on each carbon to form sigma bonds - one with a H atom and one with the other C atom

29. sp hybridisation in ethyne From: http://www.citycollegiate.com/hybridization2.htm

30. sp hybridisation in BeF2 From: http://www.rjc.edu.sg/subjects/chemistry/resources/simulations-hybridisation/lecture28.html

31. Question • Identify the type of hybridisation in each of the carbon atoms in propene From: http://www.neiu.edu/~ncaftori/eng/propene.GIF

32. Answer • Identify the type of hybridisation in each of the carbon atoms in propene sp2 sp3 sp2 From: http://www.neiu.edu/~ncaftori/eng/propene.GIF