Name _____________________

CHEM 1406. Problem Session on Bonding

1. Write formulas for six ionic compounds where the ions are present in a 1:1 ratio.

2. Circle the formulas of the covalent substances in the following list:

K₂Cr₂O₇ K N₂O He O₂ C₂H₅OH Li₂O H₂O

3. Write correct formulas for:

4. potassium hydroxide

5. silver chromate

6. iron(III) sulfate

7. magnesium nitride

8. magnesium nitrate

9. zinc dihydrogen phosphate

10. calcium perchlorate

11. chromium(III) nitrate

12. strontium oxide

13. copper(I) sulfide

14. Write electron configurations for the following ions:

15. zinc

16. iron(III)

17. thallium(I)

18. thallium(III)

19. scandium(III)

20. nitride

21. oxide

22. silver

23. copper(I)

24. Draw Lewis electron-dot structures for the following:

25. water

26. H₂CO

27. CO₂

E. CH₃OH

28. HCO₃^1-

29. NH₄¹⁺

30. SO₃

31. NO₂

32. The substance NO₂, above, is rather unstable and reacts with its own kind of molecules to form O₂NNO₂ (or N₂O₄). Explain this chemical behavior of NO₂ in terms of the tendency of stable molecules to obey the “octet rule.”

33. What types of forces must be overcome to boil substances represented by the following formulas? Choose as many as appropriate from the following list:

ionic covalent dispersion dipolar H-bond metallic

34. H₂O

35. H₂S

36. CBr₄

37. CS₂

38. CO₂

39. BF₃

40. CaH₂

41. MgCl₂

42. Mg

43. C (diamond)

44. He

45.

46.

47.

48. Based on the expected relative strengths of intermolecular (or other interparticle) forces, rank the following in terms of increasing boiling points:

49. CH₄ NH₃ PH₃

50. CH₄ SiH₄ GeH₄

51. O₂ N₂ H₂

52. CH₃OH CH₃SH CH₃F

53.

54. CaS CaO NaCl