Intermolecular Forces: Liquids, and Solids. Chapter 11
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1 Intermolecular Forces: Liquids, and Solids Chapter 11 1
2 Review Practice Excited Na atoms may emit radiation having a wavelength of 589 nm. a) What is the wavelength in meters? b) What is the frequency of this light? c) What region of the spectrum is this in? d) What is the energy of this light? A radio station has a frequency of 96.5 MHz. Find the wavelength and E. Microwaves have a frequency of around 2.5 GHz. What is the wavelength? (1 GHz = 10 9 Hz) 2
3 Review Practice What is the energy associated with 688 nm light? What color light is this? A certain photon of radiation has energy of 4.65 x J. What is the wavelength of this light, in nm? A certain light has an energy of 4.56 x J. What color is this light? (Hint: find wavelength in nm.) The density of NO 2 gas at STP is 3
4 Reading Strategies for Free Response questions The Five Analytical Moves 4
5 1. Suspend Your Judgment Try not to jump to conclusions and evaluate what is being asked without knowing all the parts. Ex. What is the molecular geometry of XeF 4? I hope you did not guess tetrahedral because you see four(4) atoms around the central 5
6 2. Define significant parts and how they are related Identify what is needed to find the solution to the questions. What are all of the pieces Are there any special rules of circumstances I should remember Ex. What is the molecular geometry of XeF 4? What are the pieces: 6 e - domains: 4 bonding and 2 none bonding Are there any special rules of circumstances I should remember: Violation of octet rule allowed because Xe is high than 3d 6
7 3. Look for patterns of repetition and contrast and for anomaly Are there any key words that might be a hint to go in a specific direction? Are the examples extremely familiar to you because they were used in your text or in class 7
8 4. Make the Implicit Explicit Explicit (overtly stated) Implicit (suggested but not directly stated) Process of converting suggestions into direct statements is ESSENTIAL to analysis. Looking for key words that will help you in decision making of how to solve a problem. Steps, justify, analyze, explain, etc. 8
9 5. Keep reformulating questions and explanations What details/ data seem significant? Why? What does the detail/data mean? What else might it mean? How do the details/ data fit together? What do they have in common? What details do not fit? How might they be connected with other details to form a different pattern? Fortunately most if not all free response questions will be strait forward a VERY clear. 9
10 Lets Try One Expectations: At each part of the questions you will go through steps 1-5 AND incorporate them with the problem solving method we use in here time should not be a factor right now. Remember keep your answers to the point and simple. 10
11 2008 AP Free Response Question: Part A question2 Answer the following questions relating to gravimetric analysis. In the first of two experiments, a student is assigned the task of determining the number of moles of water in one mole of MgCl 2 n H 2 O. The student collects the data shown in the following table. Mass of empty container g Initial mass of sample and container g Mass of sample and container after first heating g Mass of sample and container after second heating g Mass of sample and container after third heating g 11
12 2008 AP Free Response Question (a) Explain why the student can correctly conclude that the hydrate was heated a sufficient number of times in the experiment. (b) Use the data above to (i) calculate the total number of moles of water lost when the sample was heated, and (ii) determine the formula of the hydrated compound. 12
13 2008 AP Free Response Question (c) A different student heats the hydrate in an uncovered crucible, and some of the solid spatters out of the crucible. This spattering will have what effect on the calculated mass of the water lost by the hydrate? Justify your answer. 13
14 2008 AP Free Response Question In the second experiment, a student is given 2.94 g of a mixture containing anhydrous MgCl 2 and KNO 3. To determine the percentage by mass of MgCl 2 in the mixture, the student uses excess AgNO 3 (aq) to precipitate the chloride ion as AgCl(s). 14
15 2008 AP Free Response Question (d) Starting with the 2.94 g sample of the mixture dissolved in water, briefly describe the steps necessary to quantitatively determine the mass of the AgCl precipitate. 15
16 2008 AP Free Response Question (e) The student determines the mass of the AgCl precipitate to be 5.48 g. On the basis of this information, calculate each of the following. (i) The number of moles of MgCl 2 in the original mixture (ii) The percent by mass of MgCl 2 in the original mixture 16
17 A Molecular Comparison of Liquids and Solids 17
18 Intermolecular Forces 18
19 Intermolecular Forces Ion-Dipole Forces - Interaction between an ion (Na + ) and a dipole (water). - Strongest of all intermolecular forces 19
20 Intermolecular Forces 20
21 Na +, Cl - and H 2 O 21
22 Intermolecular Forces Dipole-Dipole Forces - Interaction between a on one molecule and a on an adjacent molecule. - forces exist between neutral polar molecules. - Weaker than ion-dipole forces 22
23 Intermolecular Forces 23
24 Intermolecular Forces London Dispersion Forces Induced Dipole Induced Dipole - of all intermolecular forces. - It is possible for two adjacent nonpolar molecules to affect each other. 24
25 Intermolecular Forces London Dispersion Forces Induced Dipole Induced Dipole - The nucleus of one molecule (or atom) of the adjacent molecule (or atom). - This attraction causes the electron clouds become distorted. - In that instant a polar molecule ( ) is formed (called an instantaneous dipole). 25
26 Intermolecular Forces London Dispersion Forces 26
27 Intermolecular Forces Hydrogen Bonding - A special case of dipole-dipole forces. - This intermolecular force is very strong. - of the three Van der Waal s forces (Hydrogen bonding, Dipole-dipole, London forces,) - H-bonding requires H bonded to an electronegative element (most important for compounds of F, O, and N). 27
28 Hydrogen Bonding Intermolecular Forces 28
29 29
30 30
31 31
32 Viscosity - Viscosity Some Properties of Liquids - A liquid flows by sliding molecules over each other. - The stronger the intermolecular forces, the the viscosity. 32
33 Some Properties of Liquids Surface Tension - The surface of a liquid behaves as a. - This is due to the unequal attractive forces on molecules at the surface. - Surface molecules are only attracted towards the bulk molecules. 33
34 Some Properties of Liquids Surface Tension - Cohesive forces - Adhesive forces 34
35 Surface Tension Some Properties of Liquids - Meniscus is the shape of the liquid surface. If adhesive forces are greater than cohesive forces, the liquid surface is to its container more than the bulk molecules. Therefore, the meniscus is U-shaped (e.g. water in glass). If cohesive forces are greater than adhesive forces, the meniscus is curved downwards. 35
36 Surface Tension Some Properties of Liquids - When a narrow glass tube is placed in water, the meniscus pulls the water up the tube. 36
37 Recall. 37
38 Properties of Liquids Vaporization Also called evaporation _ Standard molar enthalpy of vaporization (DH o vap) The resulting gas will exert a pressure on a system. 38
39 Properties of Liquids Vapor Pressure This is the pressure exerted by a substance in the gas phase. As a liquid s temperature increases, its vapor pressure increases. 39
40 Vapor Pressure Volatile Properties of Liquids Or 40
41 Properties of Liquids Vapor Pressure and Boiling Point - Liquids boil when the external pressure the vapor pressure. - Two ways to get a liquid to boil: temperature or pressure. - Normal boiling point is the boiling point at 760 mmhg (1 atm). 41
42 Properties of Liquids Vapor Pressure and Boiling Point Try to draw a picture representing the gas and liquid molecules and what they are doing during boiling of a liquid. 42
43 Properties of Liquids Vapor Pressure and Boiling Point - Vapor pressure, temperature and enthalpy of vaporization can be related to each other using: Clausius-Clapeyron equation: ln P = T = R = DH o vap = o P D H vap P1 R T T
44 Properties of Liquids Vapor Pressure and Boiling Point The Clausius-Clapeyron equation makes more sense when it is rearranged into the slope intercept form. ln P D H RT o vap C 44
45 Properties of Liquids Vapor Pressure and Boiling Point 45
46 Structures of Solids Unit Cells - Crystalline solid: well-ordered, definite arrangements of molecules, atoms or ions. - Crystals have an ordered, repeated structure. - The smallest repeating unit in a crystal is a. - Three-dimensional stacking of unit cells is the crystal lattice. 46
47 Review Name the intermolecular forces that must be overcome to convert each of the following from a liquid to a gas: a) Br 2 ; b) CH 3 OH; c) H 2 S 47
48 Unit Cells Structures of Solids 48
49 Unit Cells Structures of Solids 49
50 Cell Occupancy Structures of Solids 50
51 Cell Occupancy Structures of Solids 51
52 Cell Occupancy Structures of Solids Site Occupancy Corner 1/8 Edge 1/4 Face 1/2 Center 1 52
53 Structures of Solids Cell Occupancy Zn 4 S 4 ZnS Zinc (grey) 4 Center 4 atoms Sulfur (yellow) 8 corners 6 faces 1 atom 3 atoms 53
54 Structures of Solids Close Packing of Spheres - A crystal is built up by placing close packed layers of spheres on top of each other. - There is only one place for the second layer of spheres. 54
55 Structures of Solids Close Packing of Spheres - There are two choices for the third layer of spheres: - Third layer eclipses the first (ABAB arrangement). This is called hexagonal close packing (hcp). - Third layer is in a different position relative to the first (ABCABC arrangement). This is called cubic close packing (ccp). 55
56 Structures of Solids Close Packing of Spheres 56
57 Structures of Solids Close Packing of Spheres - Each sphere is surrounded by 12 other spheres (6 in one plane, 3 above and 3 below). - Coordination number: the number of spheres directly surrounding a central sphere. 57
58 Structures of Solids Other Kinds of Solid Materials Molecular Solids These are crystalline substances in which the building blocks are composed of molecules in place of ions. Example: Table Sugar 58
59 Structures of Solids Other Kinds of Solid Materials Network Solids These are crystalline substances in which the building blocks are atoms and all the atoms are connected by covalent bonds. Example: Diamond 59
60 Phase Diagrams Phase diagram: plot of pressure vs. temperature summarizing all equilibria between phases. 60
61 Phase Diagrams Triple point - Temperature and pressure at which all three phases are in equilibrium. Critical point Point above which the liquid and gas phases indistinguishable. are 61
62 Phase Diagrams Critical temperature - The minimum temperature for liquefaction of a gas using pressure Critical pressure - 62
63 Homework Ch. 11: 11, 13, 15, 19, 23, 27, 29, 33, 39, 47, 55, 69, 76 63
2. As gas P increases and/or T is lowered, intermolecular forces become significant, and deviations from ideal gas laws occur (van der Waal equation).
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