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

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

6. Which of these elements would make an ionic bond with potassium. Mg. N
Which of these elements would make an ionic bond with potassium? Mg N Sr Cl
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. O. F
Which of these elements would make an ionic bond with chlorine? O F Li Xe
Li; metal with non-metal bond (also difference in electronegativities is relatively large)

8. What type of bond exists between chlorine (EN = 3
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
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 CH2O

11. Draw the correct Lewis dot structure for CH2O

12. Draw the correct Lewis dot structure for SCl2

13. Draw the correct Lewis dot structure for SCl2

14. Draw the correct Lewis Dot Structure for O2

15. Draw the correct Lewis Dot Structure for O2

16. Electron Configuration
Review Questions

17. Write the electron configuration for the element fluorine
1s22s22p5

18. Write the electron configuration for the element potassium
1s22s22p63s23p64s1

19. Write the electron configuration for the element silicon
1s22s22p63s23p2

20. Write the electron configuration for the element titanium
1s22s22p63s23p64s23d2

21. Write the noble gas configuration for the element rubidium
[Kr]5s1

22. Write the noble gas configuration for the element chlorine
[Ne]3s2 3p5

23. Which element has the following electron configuration: 1s22s22p63s23p64s23d6
Iron, Fe

24. Which element has the following electron configuration: 1s22s22p63s23p64s23d104p3
Arsenic, As

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

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

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

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)