12.E: Homework Chapter 12

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Chemical Species/Chemical Interactions:

1. State whether each solid is molecular, atomic, or ionic.

a.) Cu_(s)

b.) H₂O_(s)

c.) NaCl_(s)

d.) Fe_(s)

2. What is a molecular solid? What makes it different than an atomic or ionic solid?

3. If you were to mix CH₃CH₂OH with H₂O, would this mixture be miscible or immiscible? Why?

4. If you were to mix CH₃CH₂CH₂CH₃ with H₂O, would this mixture be miscible or immiscible? Why?

5. Define a homogeneous mixture.

6. Determine whether a homogeneous mixture will form when each pair of substances interacts:

a.) H₂O and CH₃CH₂CH₃

b.) CH₃OH and CH₃CH₂OH

c.) CH₃CH₂CH₃ and CH₃CH₂CH₂CH₃

Intermolecular Forces:

7. Identify the strongest intermolecular force present in each of the species:

a.) CH₄

b.) HF

c.) H₂O

d.) CHCl₃

8. What intermolecular force do ALL species have?

9. List ALL of the intermolecular forces present in the following molecules:

a.) CH₃CH₂OH

b.) CCl₄

c.) CHF₃

10. Identify the strongest intermolecular force in each molecule:

a.) NH₃

b.) HCl

11. Under what circumstances is a hydrogen-bond present?

12. Identify the strongest intermolecular force present in the following molecules:

a.) CO₂

b.) O₂

c.) Ni

d.) CH₃CHO₂

13. List the following molecules in order of increasing dominant intermolecular force:

HF, CH₄, CH₃CHO₂

14. List the following molecules in order of decreasing dominant intermolecular force:

NH₃ , CH₃CH₂CH₃ , HCl

15. List all of the intermolecular forces in the following substances:

a.) CO

b.) HBr

c.) CCl₄

d.) KCl

16. Identify the dominant intermolecular force in the following substances:

a.) N₂H₂

b.) SO

c.) CH₄O

d.) BH₃

17. Circle the correct dominant intermolecular force for: NH₂CH₃**Hint: Drawing the Lewis Structure may be helpful**

a.) Dispersion

b.) Dipole-Dipole

c.) H-Bond

18. Circle all intermolecular forces that silicon tetrabromide has:

a.) Dispersion

b.) Dipole-Dipole

c.) H-Bond

19. What is the dominant intermolecular force in each of the following molecules?

a.) ammonia

b.) silicon dioxide

c.) ethanol

d.) acetic acid

20. List all of the intermolecular forces present in each of the following substances:

a.) copper (s)

b.) phosphoric acid

c.) selenium difluoride

d.) butane

21. Circle the dominant intermolecular force for the compound: CH₃OCH₃

a.) Dispersion

b.) Dipole-Dipole

c.) H-Bond

22. All of the following molecules have hydrogen-bonding forces, EXCEPT…

a.) HF

b.) HCl

c.) H₂O

d.) NH₃

23. All of the following molecules have dipole-dipole forces, EXCEPT…

a.) CH₄

b.) CH₃OCH₂CH₃

c.) CH₃OCH₃

d.) HF

24. All of the following molecules have dispersion forces as their DOMINANT intermolecular force, EXCEPT…

a.) CF₄

b.) CCl₄

c.) CH₃CH₂CH₂CH₂CH₃

d.) CH₂Cl₂

25. List the dominant intermolecular forces for the following substances:

a.) I₂

b.) F₂

c.) SO₂

d.) HCH₃COO

Boiling/Melting Point:

26. By looking at the Lewis structures of different molecules, how would you know which molecule has the higher boiling point?

27. If you are given the formula of different molecules, how would you know which molecule has the higher boiling point?

28. Circle which molecule will has the higher boiling point:

a.) CH₄

b.) CH₃CH₃

29. Given the following substances, list them in order of decreasing boiling point:

NaCl, CH₃CH₂OH, Ar, CHCl₃

30. When given two molecules, how would you know which substance is a liquid at room temperature?

31. At room temperature, CO₂ is in its gas form, while CH₃OH is in its liquid form. Explain why.

32. List the following noble gases in order of increasing boiling point:

Kr, He, Ar, Xe, Rn, Ne

33. When comparing NaCl and CH₄, which molecule has the higher melting point?

34. When comparing solid CO₂ with solid SO₂, which one will have the higher melting point? Why?

35. Circle the molecule with the highest melting point:

a.) NH₄Cl

b.) CH₃OH

c.) HF

36. Circle the molecule with the highest boiling point:

a.) CH₃CH₂CH₂CH₂CH₃

b.) CH₃CH₂CH₂CH₂CH₂CH₂CH₃

c.) CH₃CH₃

37. Circle the molecule with the lowest boiling point:

a.) CH₃OCH₃

b.) CH₃CH₂CH₃

c.) CH₄

38. Determine which molecule has the higher boiling point.

a.) methanol

b.) carbon dioxide

39. Determine which molecule has the higher boiling point.

a.) H₂

b.) HCl

40. Which substance has the lowest boiling point?

a.) H₂O

b.) Ne

c.) NH₃

d.) NaF

41. Arrange the list of acids in order of highest to lowest melting point.

HCl, HI, HBr

42. Compare H₂O(s) and H₂S(s). Which molecule has the higher melting point? Why?

43. Arrange the molecules in order of decreasing boiling point:

Hexane (C₆H₁₄), Octane (C₈H₁₈), Butane (C₄H₁₀)

44. From the choices below, which one has the lowest boiling point?

a.) C₅H₁₂

b.) C₁₀H₂₂

c.) C₂H₂

45. Ethanol (CH₃CH₂OH) and propane (C₅H₁₂) have similar molar masses. Does that mean they have the same boiling point? Explain.

46. For each of the pairs below, circle the substance with the higher boiling point:

a.) I₂ and F₂

b.) HF and LiF

c.) CH₂O₂ and CCl₄

47. For each of the pairs below, circle the substance with the higher boiling point:

a.) propanol and methanol

b.) methane and pentane

c.) dihydrogen monoxide and dihydrogen monosulfide

48. Arrange the following substances in order of increasing boiling points:

acetic acid (CH₃COOH), acetone (C₃H₆O), water (H₂O)

49. Which substance would most likely be a liquid at room temperature, CH₃COOH or CCl₄?

50. From the following molecules, which one has the highest boiling point? Which one has the lowest boiling point?

a.) CH₃CH₂CH₂CH₃

b.) CH₃CH₂CH₂CH₂CH₂CH₂CH₂CH₃

c.) CH₃CH₂CH₃

d.) CH₃CH₂CH₂CH₂CH₂CH₃

51. For the pair below, which one has the higher boiling point? Explain.

CH₃CH₂COH or CH₃CH₃

52. From the following molecules, which one has the higher boiling point?

a.) CH₃CH₂CH₂COH

b.) CH₃CH₂CH₂CH₃

c.) CH₄

53. From the following molecules, which one has the lowest boiling point?

a.) CH₃CH₂CH₂CH₃

b.) CH₄

c.) CO₂

Cumulative/Challenge Problems:

54. Why are hydrogen-bonding forces unusually stronger than the average dipole-dipole force?

55. The Lewis structure for acetone is provided below. Can a hydrogen-bond form if two acetone molecules were allowed to bond together? Explain.

56. Could a water molecule form a hydrogen bond with an acetone molecule? Explain. (The Lewis structure provided in the previous problem may be helpful).

57. Circle the choice that is a homogeneous mixture:

a.) orange juice with pulp

b.) vinegar

c.) bowl of cereal

d.) vegetable soup

58. The Lewis structures for butane and iso-butane are provided below. Which molecule will have the higher boiling point? Do they have the same boiling point because each molecule has the same amount of carbons and hydrogens? Explain.

59. Determine the dominant intermolecular forces for each of the following molecules: **Hint: use the Lewis structures provided in the previous problems for extra help.**

a.) acetone

b.) butane

c.) iso-butane

60. Determine all of the intermolecular forces present in each of the following substances:

a.) nitric acid

b.) benzene

c.) ethanol