1. 1 CH 1: Structure and Bonding Renee Y. Becker CHM 2210 Valencia Community College

2. 2 Organic Chemistry (present definition): –the chemistry of carbon compounds Organic Chemistry (Historical definition): –Study of compounds extracted from living organisms, study of compounds having the vital force Vitalism: –The belief that natural products needed a “vital force” to create them –In the 19th century experiments showed that organic compounds could be synthesized from inorganic compounds

3. 3 Friedrich Wohler In 1828, Wohler synthesized urea from ammonium cyanate Ammonium cyanate (inorganic)

4. 4 Natural Product or Synthesized Plant-derived compounds and synthesized compounds are identical (almost) –You can tell them apart by 14 C dating –Synthesized compounds have a lower content of radioactive 14 C, their 14 C has decayed over time –BUT, plant-derived compounds are recently synthesized from CO 2 in the air and therefore have a higher content of radioactive 14 C

5. 5 Not all carbon compounds are organic –Diamonds, graphite, CO 2, NH 4 + - OCN, Na 2 CO 3 Derived from minerals and have inorganic properties –Most of the millions of carbon compounds are classified as organic

6. 6 Structure of the Atom

7. 7 Atomic Orbitals

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9. 9 Aufbau principle: Place electrons in lowest energy orbital first. Hund’s rule: Equal energy orbitals are half-filled, then filled. Electronic Configurations

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12. 12 Example 1: Electron Configuration Draw electron configuration 1.Cl 2.Cl - 3.Mg 4.Mg 2+ 5.Fe 3+

13. 13 Ionic bonding: electrons are transferred. Covalent bonding: electron pair is shared. Bond Formation

14. 14 Lewis Structures Bonding electrons Nonbonding electrons or lone pairs Satisfy the octet rule!

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16. 16 Multiple Bonding

17. 17 Example 2: Lewis Dot Structures Draw Lewis structures for the following a) NH 3 b) CH 3 CH 2 F c) CH 3 OCH 3 d) BF 3 e) C 3 H 4

18. 18 Calculating Formal Charge Formal charge = (# own valence electrons in free atom)-(# own valence electrons in bonded atom) Put in formal charges

19. 19 Ionic Structures X

20. 20 Example 3: Lewis Dot Structures Draw the Lewis structure for the following compounds or ions, showing formal charges a) (CH 3 ) + b) (CH 3 ) - c) NH 4 Cl d) H 3 O + e) (CH 3 ) 2 NH 2 Cl

21. 21 Valence Bond Theory 1. Covalent bonds are formed by overlapping of atomic orbitals, each of which contains one electron of opposite spin. 2. Each of the bonded atoms maintains its own atomic orbitals, but the electron pair in the overlapping orbitals is shared by both atoms. 3. The greater the amount of orbital overlap, the stronger the bond.

22. 22 Valence Bond Theory Linus Pauling: Wave functions from s orbitals & p orbitals could be combined to form hybrid atomic orbitals.

23. 23 sp hybrid: acetylene Bond angle 180  Electron pair Geometry linear

24. 24 sp 2 hybrid: Ethylene Bond angle 120  (varies) Electron pair Geometry Trigonal Planar

25. 25 sp 2 hybrid (π bond):

26. 26 sp 3 hybrid: Ethane Bond angle 109.5  (varies) Electron pair Geometry Tetrahedral

27. 27 sp 3 d hybrid:

28. 28 sp 3 d 2 hybrid:

29. 29 Example 4: Hybridization What is the hybridization of the non-hydrogen atoms?

30. 30 Molecular Orbital Theory The molecular orbital (MO) model provides a better explanation of chemical and physical properties than the valence bond (VB) model. –Atomic Orbital: Probability of finding the electron within a given region of space in an atom. –Molecular Orbital: Probability of finding the electron within a given region of space in a molecule.

31. 31 Molecular Orbital Theory Additive combination of orbitals (  ) is lower in energy than two isolated 1s orbitals and is called a bonding molecular orbital.

32. 32 Molecular Orbital Theory Subtractive combination of orbitals (   ) is higher in energy than two isolated 1s orbitals and is called an antibonding molecular orbital.

33. 33 Molecular Orbital Theory Molecular Orbital Diagram for H 2 :

34. 34 Molecular Orbital Theory Molecular Orbital Diagrams for H 2 – and He 2 :

35. 35 Chemical Formulas Full structural formula (no lone pairs shown) Line-angle formula Skeletal Condensed structural formula Molecular formula Empirical formula CH 3 COOH C 2 H 4 O 2 CH 2 O

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38. 38 Example 5: Chemical Formulas Draw the condensed structural formula for the following 1.2. 3. 4.

39. 39 Example 6: Chemical Formulas Draw the skeletal structure 1.CH 3 (CH 2 ) 4 CH 3 2.CH 3 CH(CH 3 ) 2 3.CH 3 CH(CH 3 )CH(CH 2 CH 3 )CH 2 CH 3 4.C(CH 3 ) 4