Chapter 12 – Liquids and Solids

1. Chapter 12 – Liquids and Solids

2. Which one represents a liquid? Why?

3. Liquids have a definite volume, but not a definite shape. The particles are closer together than gases so the intermolecular forces are now a factor.

4. Liquids have a definite volume, but not a definite shape. The particles are closer together than gases so the intermolecular forces are now a factor. Hydrogen Bonding Dipole-Dipole London Forces

5. Due to the greater attraction of the intermolecular forces, the particles are more orderly than gases, and have a lower mobility.

6. Due to the greater attraction of the intermolecular forces, the particles are more orderly than gases, and have a lower mobility. Although there liquids have a lower mobility, they are still able to flow, thus classified as a fluid. They are, therefore, able to diffuse.

7. Due to the greater attraction of the intermolecular forces, the particles are more orderly than gases, and have a lower mobility. Although there liquids have a lower mobility, they are still able to flow, thus classified as a fluid. They are, therefore, able to diffuse. The more orderly arrangements causes liquids to be about 1000 times more dense than the gas form of the substance. The typical density of liquids makes them incompressible.

8. In addition, liquids will exhibit surface tension. The stronger the intermolecular forces, the more they can pull the surface molecules together.

9. In addition, liquids will exhibit surface tension. The stronger the intermolecular forces, the more they can pull the surface molecules together. The greater the strength of the intermolecular forces, the smaller the resulting surface area will be. (A sphere has the smallest surface area for it’s volume of any other geometric shape.)

10. Often liquids not only experience intermolecular forces within themselves, but can experience intermolecular forces with the walls of a container. The attraction of a liquid to the walls of a container results in capillary action – which forms the meniscus, and in a capillary tube can even pull the liquid up the tube.

11. Which one represents a Solid? Why?

12. Solids particles are more closely packed than even liquids (usually the most dense phase). Due to very large intermolecular forces, solids have definite volume and definite shape.

13. Solids particles are more closely packed than even liquids (usually the most dense phase). Due to very large intermolecular forces, solids have definite volume and definite shape. The only motion the particles are able to have is vibrational and rotational, there is no more ability to have translational motion (as with liquids).

14. Solids particles are more closely packed than even liquids (usually the most dense phase). Due to very large intermolecular forces, solids have definite volume and definite shape. The only motion the particles are able to have is vibrational and rotational, there is no more ability to have translational motion (as with liquids). Solids are also incompressible and have a low rate of diffusion.

15. There are two types of solids: Amorphous solids have particles that are randomly arranged.

16. There are two types of solids: Amorphous solids have particles that are randomly arranged. Amorphous solids do not have a definite melting point, but rather become more and more fluidic when more and more heat is added. Thus they are sometimes called supercooledliquids. Glass is an amorphous solid, and old windows are thicker at the bottom and thinner at the top, adding to the draftiness of old buildings.

17. Crystalline solids have particles arranged in an orderly, geometric, repeating pattern (a crystal). Crystalline solids will have a definite meltingpoint, which can often be useful in identifying a particular solid.

20. The total 3-dimensional arrangement of the particles in a crystal is referred to as the crystalstructure. The entire crystal structure in a sample is the crystallattice. The smallest portion of the crystal lattice that shows the 3-dimensional pattern (as in the previous graphics) is called the unitcell.

21. Solids can be categorized by shape based on the unit cell (as in the previous graphics) or on the bindingforce. When based on the binding force there are four types of crystals: Molecular, Ionic, Covalent Network, and Metallic.

22. Molecular Solids

23. Ionic Covalent Network Metallic

24. Phases are any part of a system that has uniformcomposition and properties. Phase changes occur as a substance changes from one phase to another. Melting / Freezing – solid to liquid / liquid to solid Vaporizing (Boiling) /Condensing – liquid to gas / gas to liquid Sublimation / Deposition – solid to gas / gas to solid Evaporation – vaporization occurring below boiling point (temperature) – only molecules with high energy at the surface become a vapor (a cooling process)

25. Equilibrium is a dynamic condition in which two opposing changes occur at equal rates in a closed system. (Like ice in water at 0°C.) For chemical reactions, this is shown with a double sided arrow.

26. Equilibrium is a dynamic condition in which two opposing changes occur at equal rates in a closed system. (Like ice in water at 0°C.) For chemical reactions, this is shown with a double sided arrow. LeChatelier’s Principle – when a system that was at equilibrium is subjected to some outside stress, the system reacts in such a way to relieve the stress and return to another equilibrium.

27. If the concentration of a chemical is increased / decreased, shift to use up more / make more of that chemical.

28. If the concentration of a chemical is increased / decreased, shift to use up more / make more of that chemical. If gases are involved, increasing / decreasing the pressure (or decreasing / increasing the volume) will shift the equilibrium to the side of the equation with the fewer / greater number of gaseous chemicals.

29. Le Chatelier’s Principle Review 1 Le Chatelier’s Principle Review 2

30. Equilibrium vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid at a given temperature. Volatile liquids evaporate easily due to weak intermolecular forces.

31. Boiling is the conversion of liquid to vapor, within the liquid as well as at its surface. It occurs when the equilibrium vapor pressure of the liquid equals the atmospheric pressure. The temperature at which the liquid must be heated to reach an equilibrium with the atmospheric pressure is called the boiling point. Pressure cookers increase the vapor pressure to increase the temperature at which the water must be heated before it will boil – thus cooking food faster.

32. Molar heat of vaporization is the amount of heat energy needed to vaporize one mole of liquid at the boiling point. (The stronger the intermolecular forces, the higher the heat of vaporization.)

33. Molar heat of vaporization is the amount of heat energy needed to vaporize one mole of liquid at the boiling point. (The stronger the intermolecular forces, the higher the heat of vaporization.) Normal freezing point is the temperature at which the solid and liquid are in equilibrium at 1 atm.

34. Molar heat of vaporization is the amount of heat energy needed to vaporize one mole of liquid at the boiling point. (The stronger the intermolecular forces, the higher the heat of vaporization.) Normal freezing point is the temperature at which the solid and liquid are in equilibrium at 1 atm. Molar heat of fusion is the amount of heat energy required to melt one mole of solid at its melting point.

35. Phase diagrams:

36. The triple point is the temperature at which all three states of matter are in equilibrium (solid, liquid and gas)

37. The critical temperature is the temperature above which the substance cannot exist in the liquid state.

38. The critical pressure is the pressure above which the substance cannot exist in the liquid state if above the critical temperature.

39. You must be able to label on a blank chart: • sublimation curve • melting curve • boiling curve • normal melting and boiling points (temperatures) • triple point • critical temperature • solid, liquid, and gas regions

40. Water is a very special compound! It is a polarcovalent compound with angular molecular geometry. Hydrogen bonding between water molecules accounts for water’s high melting point (for it’s mass), high heats of fusion and vaporization (more energy to pull the molecules apart), and high melting and boiling points. In the solid phase, water has a hexagonal arrangement with more empty space between the molecules than as a liquid. This gives ice a lowerdensity than the liquid.

41. Compare water’s phase diagram to carbon dioxide.

42. It should be obvious by now that heat has a large influence over the phases of matter. If it is desired to quantitize the amount of effect the heat can cause the following formula will be useful: Q = m × Cp × ∆T where Q = heat (in calories or joules) m = mass (in grams) Cp = specific heat ∆T = Tfinal – Tinitial (in °C)

43. The specific heat is different with every substance, and is also different for each phase of a substance. For example: Cpice = 2.06 J/g °C Cpwater = 4.18 J/g °C Cpsteam = 2.08 J/g °C CpAl = 0.903 J/g °C

44. During a phase change, the temperature is constant, therefore temperature cannot be a factor in the equation for heat during a phase change, thus: Q = m × Hf or Q = m × Hv where Hf = molar heat of fusion Hv = molar heat of vaporization

45. A great way to visualize what is occurring during a process that involves changing the heat of a substance is with a heating curve:

46. Each segment will require a different formula due to different values for Cp, Hf, or Hv! To solve the heat necessary to do the curve below, it would take 5 calculations and a sum!