1. Types of Bonding and Lewis Structures

2. Describe the structure of metallic bonding. Positive metallic ions surrounded by electrons.

3. Example of Metallic Bonding

4. Potassium bromide forms a crystal lattice structure. What type of bonding would you expect it have? Ionic

5. Which of these elements would make a covalent bond with nitrogen? AlMgBaC C; non-metal with non-metal bonding (also similar electronegativity)

6. Which of these elements would make an ionic bond with potassium? MgNSrCl N, Cl; metal with non-metal bond (also difference in electronegativities is relatively large)

7. Which of these elements would make an ionic bond with chlorine? OFLiXe Li; metal with non-metal bond (also difference in electronegativities is relatively large)

8. What type of bond exists between chlorine (EN = 3.0) and bromine (EN = 2.8) Non-polar covalent; both elements are non-metals with their difference in electronegativity being less than 0.5

9. What type of bond exists between nitrogen (EN = 3.0) and hydrogen (EN = 2.1) Polar covalent; both elements are non-metals with their difference in electronegativity being between 0.5 and 1.7

10. Draw the correct Lewis dot structure for CH 2 O

12. Draw the correct Lewis dot structure for SCl 2

14. Draw the correct Lewis Dot Structure for O 2

16. Electron Configuration Review Questions

17. Write the electron configuration for the element fluorine 1s 2 2s 2 2p 5

18. Write the electron configuration for the element potassium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1

19. Write the electron configuration for the element silicon 1s 2 2s 2 2p 6 3s 2 3p 2

20. Write the electron configuration for the element titanium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2

21. Write the noble gas configuration for the element rubidium [Kr]5s 1

22. Write the noble gas configuration for the element chlorine [Ne]3s 2 3p 5

23. Which element has the following electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 Iron, Fe

24. Which element has the following electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 3 Arsenic, As

25. Write the orbital notation for the element carbon ↑↓ ↑↓ ↑ ↑. 1s 2s 2p

26. Write the orbital notation for the element sulfur ↑↓ ↑↓ ↑↓ ↑↓ ↑↓. 1s 2s 2p ↑↓ ↑↓ ↑ ↑. 3s 3p

27. Write the orbital notation for the element selenium ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ 1s 2s 2p 3s3p4s 3d 4p

28. Write the Lewis Dot structure for the following atoms and their ions

29. Aluminum Al (group 13; 3 valence electrons) Al +3 (aluminum loses its 3 valence electrons to satisfy the octet rule)

30. Phosphorus P (group 15; 5 valence electrons) P -3 (phosphorus gains 3 electrons to satisfy the octet rule)

31. Helium He (group 18 but it has 2 valence electrons) No ionic form of helium. It already has a full valence shell so it already satisfies the octet rule

32. Strontium Sr (group 2; 2 valence electrons) Sr +2 (strontium loses its 2 valence electrons to satisfy the octet rule)