2. Chapter 14 Liquids and Solids

3. Chapter 14 Table of Contents Copyright © Cengage Learning. All rights reserved 2 14.1 Water and Its Phase Changes 14.2 Energy Requirements for the Changes of State 14.3 Intermolecular Forces 14.4 Evaporation and Vapor Pressure 14.5 The Solid State: Types of Solids 14.6Bonding in Solids

4. Chapter 14 Table of Contents Copyright © Cengage Learning. All rights reserved 3 Intermolecular Forces O δ- H δ+ H δ+ Dipole-Dipole Forces Solid LiquidGas + -

5. Section 14.1 Water and Its Phase Changes Return to TOC Copyright © Cengage Learning. All rights reserved 4 Reviewing What We Know Gases  Low density  Highly compressible  Fill container Solids  High density  Slightly compressible  Rigid (keeps its shape)

6. Section 14.1 Water and Its Phase Changes Return to TOC Copyright © Cengage Learning. All rights reserved 5 Heating/Cooling Curve

7. Section 14.1 Water and Its Phase Changes Return to TOC Copyright © Cengage Learning. All rights reserved 6 Heating/Cooling Curve Normal boiling point: at 1 atm = 100°C Normal freezing point: at 1 atm = 0°C Density  Liquid water = 1.00 g/mL  Ice = 0.917 g/mL

8. Section 14.1 Water and Its Phase Changes Return to TOC Copyright © Cengage Learning. All rights reserved 7 Concept Check During the process of melting ice by adding heat, the temperature of the ice/liquid water slurry a)stays constant. b)increases. c)decreases. d)cannot be predicted.

9. Energy Requirements for the Changes of State Section 14.2 Return to TOC Copyright © Cengage Learning. All rights reserved 8 Changes of state are physical changes.  No chemical bonds are broken.

10. Energy Requirements for the Changes of State Section 14.2 Return to TOC Copyright © Cengage Learning. All rights reserved 9 Phase Changes When a substance changes from solid to liquid to gas, the molecules remain intact. The changes in state are due to changes in the forces among molecules rather than in those within the molecules.

11. Energy Requirements for the Changes of State Section 14.2 Return to TOC Copyright © Cengage Learning. All rights reserved 10 Phase Changes Solid to Liquid  As energy is added, the motions of the molecules increase, and they eventually achieve the greater movement and disorder characteristic of a liquid. Liquid to Gas  As more energy is added, the gaseous state is eventually reached, with the individual molecules far apart and interacting relatively little.

12. Energy Requirements for the Changes of State Section 14.2 Return to TOC Copyright © Cengage Learning. All rights reserved 11 Intramolecular Forces “Within” the molecule. Molecules are formed by sharing electrons between the atoms. Hold the atoms of a molecule together.

13. Energy Requirements for the Changes of State Section 14.2 Return to TOC Copyright © Cengage Learning. All rights reserved 12 Intermolecular Forces Forces that occur between molecules. Intramolecular bonds are stronger than intermolecular forces.

14. Energy Requirements for the Changes of State Section 14.2 Return to TOC Copyright © Cengage Learning. All rights reserved 13 Molar heat of fusion – energy required to melt 1 mol of a substance. Molar heat of vaporization – energy required to change 1 mol of a liquid to its vapor.

15. Energy Requirements for the Changes of State Section 14.2 Return to TOC Copyright © Cengage Learning. All rights reserved 14 Concept Check Which are stronger, intramolecular bonds or intermolecular forces? How do you know?

16. Energy Requirements for the Changes of State Section 14.2 Return to TOC Copyright © Cengage Learning. All rights reserved 15 Concept Check Which would you predict to be larger for a given substance:  H vap or  H fus ? Explain why.

17. Energy Requirements for the Changes of State Section 14.2 Return to TOC Copyright © Cengage Learning. All rights reserved 16 Concept Check The unusually high value of the molar heat of vaporization of water (40.6 kJ/mole) is an important factor in moderating the temperature of the earth’s surface, and results in an enormous transfer of energy to the atmosphere as liquid water evaporates as part of the hydrologic cycle. Calculate the amount of heat in kJ needed to evaporate 10.5 kg of liquid water at 100. o C. a)4.27 × 10 5 kJ b)3.15 × 10 4 kJ c)2.37 × 10 4 kJ d)1.18 × 10 3 kJ

18. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 17 Forces that occur between molecules.  Dipole–dipole forces  Hydrogen bonding  London dispersion forces

19. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 18 Dipole–Dipole Attraction

20. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 19 Dipole-Dipole Forces Dipole moment – molecules with polar bonds often behave in an electric field as if they had a center of positive charge and a center of negative charge. Molecules with dipole moments can attract each other electrostatically. They line up so that the positive and negative ends are close to each other. Only about 1% as strong as covalent or ionic bonds.

21. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 20 Hydrogen Bonding Strong dipole-dipole forces. Hydrogen is bound to a highly electronegative atom – nitrogen, oxygen, or fluorine.

22. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 21 Hydrogen Bonding in Water Blue dotted lines are the intermolecular forces between the water molecules.

23. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 22 Hydrogen Bonding Affects physical properties  Boiling point

24. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 23 London Dispersion Forces Instantaneous dipole that occurs accidentally when a given atom induces a similar dipole in a neighboring atom. Significant in large atoms/molecules. Occurs in all molecules, including nonpolar ones.

25. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 24 London Dispersion Forces – Nonpolar Molecules

26. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 25 London Dispersion Forces Become stronger as the sizes of atoms or molecules increase.

27. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 26 Melting and Boiling Points In general, the stronger the intermolecular forces, the higher the melting and boiling points.

28. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 27 Concept Check Which molecule is capable of forming stronger intermolecular forces? N 2 H 2 O Explain.

29. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 28 Concept Check Draw two Lewis structures for the formula C 2 H 6 O and compare the boiling points of the two molecules.

30. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 29 Concept Check Which gas would behave more ideally at the same conditions of P and T? CO or N 2 Why?

31. Intermolecular Forces Section 14.3 Return to TOC Copyright © Cengage Learning. All rights reserved 30 Concept Check Consider the following compounds: NH 3 CH 4 H 2 How many of the compounds above exhibit London dispersion forces? a)0 b)1 c)2 d)3

32. Section 14.4 Evaporation and Vapor Pressure Return to TOC Copyright © Cengage Learning. All rights reserved 31 Vaporization or Evaporation Molecules of a liquid can escape the liquid’s surface and form a gas. Endothermic process – requires energy to overcome the relatively strong intermolecular forces in the liquid.

33. Section 14.4 Evaporation and Vapor Pressure Return to TOC Copyright © Cengage Learning. All rights reserved 32 Vapor Pressure Amount of liquid first decreases then becomes constant. Condensation - process by which vapor molecules convert to a liquid. When no further change is visible the opposing processes balance each other – equilibrium

34. Section 14.4 Evaporation and Vapor Pressure Return to TOC Copyright © Cengage Learning. All rights reserved 33 Vapor Pressure Pressure of the vapor present at equilibrium. The system is at equilibrium when no net change occurs in the amount of liquid or vapor because the two opposite processes exactly balance each other.

35. Section 14.4 Evaporation and Vapor Pressure Return to TOC Copyright © Cengage Learning. All rights reserved 34 Ilustration of Vapor Pressure Budda Water Budda (air pressure) will keep the liquid water down while the heat vaporizes the surface water. Who’s this?

36. Section 14.4 Evaporation and Vapor Pressure Return to TOC Copyright © Cengage Learning. All rights reserved 35 Ilustration of Vapor Pressure Water When the vapor pressure exceeds the air pressure, Budda cannot keep the liquid water down. Then Budda rises and vapor bubbles form throughout the liquid. And it boils!

37. Section 14.4 Evaporation and Vapor Pressure Return to TOC Copyright © Cengage Learning. All rights reserved 36 Concept Check What is the vapor pressure of water at 100°C? How do you know? 1 atm

38. Section 14.4 Evaporation and Vapor Pressure Return to TOC Copyright © Cengage Learning. All rights reserved 37 Vapor Pressure Liquids in which the intermolecular forces are strong have relatively low vapor pressures.

39. Section 14.4 Evaporation and Vapor Pressure Return to TOC Copyright © Cengage Learning. All rights reserved 38 Concept Check Which of the following would be expected to have the highest vapor pressure at room temperature? a)CH 3 CH 2 CH 2 OH b)CH 3 CH 2 CH 2 NH 2 c)CH 3 CH 2 CH 2 CH 3 d)CH 3 CH 2 CH 3

40. Section 14.5 The Solid State: Types of Solids Return to TOC Copyright © Cengage Learning. All rights reserved 39 Crystalline Solids Regular arrangement of their components.

41. Section 14.5 The Solid State: Types of Solids Return to TOC Copyright © Cengage Learning. All rights reserved 40 Types of Crystalline Solids Diamonds

42. Section 14.5 The Solid State: Types of Solids Return to TOC Copyright © Cengage Learning. All rights reserved 41 Types of Crystalline Solids Ionic Solids – ions at the points of the lattice that describes the structure of the solid. Molecular Solids – discrete covalently bonded molecules at each of its lattice points. Atomic Solids – atoms at the lattice points that describe the structure of the solid.

43. Section 14.5 The Solid State: Types of Solids Return to TOC Copyright © Cengage Learning. All rights reserved 42 Examples of Three Types of Crystalline Solids

44. Section 14.6 Bonding in Solids Return to TOC Copyright © Cengage Learning. All rights reserved 43 Examples of the Various Types of Solids

45. Section 14.6 Bonding in Solids Return to TOC Copyright © Cengage Learning. All rights reserved 44 Ionic Solids Stable substances with high melting points. Held together by strong forces between ions.

46. Section 14.6 Bonding in Solids Return to TOC Copyright © Cengage Learning. All rights reserved 45 Molecular Solids Fundamental particle is a molecule. Melt at relatively low temperatures. Held together by weak intermolecular forces.

47. Section 14.6 Bonding in Solids Return to TOC Copyright © Cengage Learning. All rights reserved 46 Atomic Solids Fundamental particle is the atom. Properties vary greatly.  Group 8 – low melting points  Diamond – very high melting point

48. Section 14.6 Bonding in Solids Return to TOC Copyright © Cengage Learning. All rights reserved 47 Dr. Tacy Hall’s Artificial Diamond Presses Pictures to the left and below are of diamonds made from graphite. Dr. Hall made diamonds from peanut butter as well.

49. Section 14.6 Bonding in Solids Return to TOC Copyright © Cengage Learning. All rights reserved 48 Bonding in Metals Metals are held together by nondirectional covalent bonds (called the electron sea model) among the closely packed atoms. The word ICE made from Nitinol wire, stretched, reforms in warm water.

50. Section 14.6 Bonding in Solids Return to TOC Copyright © Cengage Learning. All rights reserved 49 Bonding in Metals Metals form alloys of two types.  Substitutional – different atoms are substituted for the host metal atoms.

51. Section 14.6 Bonding in Solids Return to TOC Copyright © Cengage Learning. All rights reserved 50 Bonding in Metals Metals form alloys of two types.  Interstitial – small atoms are introduced into the “holes” in the metallic structure.