1 / 35

Types of Bonding and Lewis Structures

Types of Bonding and Lewis Structures. Quiz on Monday. Describe the structure of metallic bonding. Positive metallic ions surrounded by electrons. Example of Metallic Bonding. What type of bonding must exist if a substance can conduct electricity dry? Why?.

shel
Download Presentation

Types of Bonding and Lewis Structures

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Types of Bonding and Lewis Structures Quiz on Monday

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

  3. Example of Metallic Bonding

  4. What type of bonding must exist if a substance can conduct electricity dry? Why? • Metallic; the delocalized electrons are able to flow freely around the positive metal ions

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

  6. If a substance dissolves in water and makes a solution that conducts electricity, what types of bonds do you expect hold it together? Ionic; forms ions in solution to make it an electrolyte

  7. If a substance melts in your hands, what type of bonds do you expect to hold it together? • Covalent (polar and non-polar); covalently bonded substances have low melting points

  8. 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)

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

  10. 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)

  11. 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

  12. 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

  13. Draw the correct Lewis dot structure for CH2O

  14. Draw the correct Lewis dot structure for CH2O

  15. Draw the correct Lewis dot structure for SCl2

  16. Draw the correct Lewis dot structure for SCl2

  17. Draw the correct Lewis Dot Structure for O2

  18. Draw the correct Lewis Dot Structure for O2

  19. Electron Configuration Review Questions

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

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

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

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

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

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

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

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

  28. Write the orbital notation for the element carbon ↑↓↑↓↑ ↑ . 1s2s2p

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

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

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

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

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

  34. 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

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

More Related