6_Chemical_bonding_2021_annotations.pptx

Chemical_bonding

1. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 1 of 50 11-7 The Shapes of Molecules H O H

2. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 2 of 50

3. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 3 of 50

4. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 4 of 50

5. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 5 of 50 13-8 Crystal Structures

6. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 6 of 50 Unit Cells in the Cubic Crystal System

7. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 7 of 50 Sodium Chloride

8. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 8 of 50

9. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 9 of 50 13-9 Energy Changes in the Formation of Ionic Crystals

10. אנרגיית הסריג למול Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 10 of 50

11. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 11 of 50 אנרגיה פוטנציאלית של זוג יונים

12. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 12 of 50 Interionic Forces

13. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 13 of 50 11-1 Lewis Theory: An Overview Valence e - play a fundamental role in chemical bonding. e - transfer leads to ionic bonds. Sharing of e - leads to covalent bonds. e - are transferred of shared to give each atom a noble gas configuration the octet. שלום  אני לומדת אצלך בקורס כימיה כללית ואנליטית  אני אשמח אם יהיה אפשרי שנתפגש היום בין השעות 17:00-18:00 או אחרי שבע וחצי , יש לי רעיון לגבי התנועה של האלקטרון אני רוצה לשתתף אותך בו ויש לי כמה שאלות לגבי התאוריות שלימדת בעיקר השאלות יתעסקו בגלים . האם נוכל להתפגש היום ?    נסרין נאטור    ‏‫ من الـ  iPhone الخاص بي

14. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 14 of 50

15. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 15 of 50 Multiple Covalent Bonds N • • •• • N N • •• • • •• • N • • •• • N N • •• •• • N N •• ••

16. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 16 of 50 Multiple Covalent Bonds C • • • • O • • • • • • O • • • • • • C O O • •• •• • • • •• •• • C O O •• •• • • • •• •• C O O •• •• •• ••

17. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 17 of 50 Coordinate Covalent Bonds H N •• H H H N H H H H + Cl •• Cl •• •• •• -

18. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 18 of 50 Writing Lewis Structures All the valence e - of atoms must appear. Usually, the e - are paired. Usually, each atom requires an octet. H only requires 2 e - . Multiple bonds may be needed. Readily formed by C, N, O, S, and P.

19. פחמימנים Hydrocarbons Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 19 of 50

20. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 20 of 50 11-6 Exceptions to the Octet Rule Odd e - species. N=O •• •• •• • H—C—H H • • O—H •• ••

21. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 21 of 50 •• •• •• Exceptions to the Octet Rule Expanded octets. P Cl Cl Cl •• •• •• •• •• •• •• P Cl Cl •• •• Cl •• •• •• •• •• •• •• •• •• Cl •• •• •• Cl •• S F F •• •• F •• •• •• •• •• •• •• •• •• F •• •• •• F •• F •• •• ••

22. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 22 of 50

23. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 23 of 50 Formal Charge FC = # valence e - - # lone pair e - - # bond pair e - 2 1

24. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 24 of 50 Example 11-6 Writing a lewis Structure for a Polyatomic Ion. Write the Lewis structure for the nitronium ion, NO 2 + . Step 1: Total valence e - = 5 + 6 + 6 – 1 = 16 e - Step 2: Plausible structure: O—N—O Step 3: Add e - to terminal atoms: O—N—O •• •• •• •• •• •• Step 4: Determine e - left over: 16 – 4 – 12 = 0

25. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 25 of 50 Example 11-6 Step 5: Use multiple bonds to satisfy octets. •• •• •• •• •• •• O—N—O •• •• •• •• O=N=O Step 6: Determine formal charges: FC(O) = 6 - 4 – (4) = 0 2 1 FC(N) = 5 - 0 – (8) = +1 2 1 +

26. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 26 of 50 Alternative Lewis Structure •• •• •• •• •• •• O—N—O + - + FC(O ≡ ) = 6 - 2 – (6) = +1 2 1 FC(N) = 5 - 0 – (8) = +1 2 1 FC(O — ) = 6 - 6 – (2) = -1 2 1 •• O N O •• •• ••

27. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 27 of 50 Alternative Lewis Structures Sum of FC is the overall charge. FC should be as small as possible. Negative FC usually on most electronegative elements. FC of same sign on adjacent atoms is unlikely. + •• O ≡ N—O •• •• •• - +

28. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 28 of 50 11-5 Resonance O O O O O O •• •• •• •• •• •• •• •• •• •• •• •• + + - - O O O •• •• •• •• •• + -½ -½

29. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 29 of 50 27-4 Aromatic Hydrocarbons

30. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 30 of 50 Expanded Valence Shell

31. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 31 of 50 Terminology Bond length – distance between nuclei. Bond angle – angle between adjacent bonds. VSEPR Theory Electron pairs repel each other whether they are in chemical bonds (bond pairs) or unshared (lone pairs). Electron pairs assume orientations about an atom to minimize repulsions. Electron group geometry – distribution of e - pairs. Molecular geometry – distribution of nuclei.

32. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 32 of 50 Molecular Geometry Symetric Shapes

33. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 33 of 50 Balloon Analogy

34. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 34 of 50 Methane, Ammonia and Water