1. IMF’s, Solids, and Liquids Ch. 11 in Textbook msconti.blogspot.com

2. I. Intermolecular Forces (IMF’s) attractions between separate molecules, not bonds attractions between separate molecules, not bonds relatively weak relatively weak occur based on molecular polarity and/or charge occur based on molecular polarity and/or charge the strength determines substance’s phase, b.p., m.p., vapor pressure, etc. the strength determines substance’s phase, b.p., m.p., vapor pressure, etc. itl.chem.ufl.edu HW: 11.4, 11.6

3. science.uwaterloo.ca

4. 1. Ion-Dipole Forces (AKA Molecule-Ion Attractions) between an ion (full charge) and the δ+ or δ- of a polar molecule between an ion (full charge) and the δ+ or δ- of a polar molecule usually the polar molecule is water acting as a solvent usually the polar molecule is water acting as a solvent the greater the magnitude of the ionic charge and/or the partial charges, the stronger the IMF’s the greater the magnitude of the ionic charge and/or the partial charges, the stronger the IMF’s chem.purdue.edu

5. chemprofessor.com

6. 2.van der Waals Forces A) Dipole-Dipole Forces a dipole (2 poles) is a polar molecule a dipole (2 poles) is a polar molecule attractions between polar molecules attractions between polar molecules relatively strong, but technically weaker than ion- dipole forces relatively strong, but technically weaker than ion- dipole forces the higher the value of μ (dipole moment), the higher the IMF’s (for similar mass/size molecules) the higher the value of μ (dipole moment), the higher the IMF’s (for similar mass/size molecules) chemtext.blogspot.com

7. chem.unsw.edu.au

8. B) Hydrogen Bonding NOT a bond NOT a bond when H is bonded to very EN elements (N,O,F, ONLY) a “super dipole” is formed when H is bonded to very EN elements (N,O,F, ONLY) a “super dipole” is formed usually NH 3, H 2 O, and HF usually NH 3, H 2 O, and HF this leads to unusually high dipole-dipole attractions and thus, unusually high b.p.’s this leads to unusually high dipole-dipole attractions and thus, unusually high b.p.’s also results in ice being less dense than water also results in ice being less dense than water weren’t you listening, I said it’s “NOT a bond!” weren’t you listening, I said it’s “NOT a bond!” chemed.chem.wisc.edu

9. yellowtang.org

10. C) London Dispersion Forces (AKA Weak Forces) occurs between nonpolar molecules occurs between nonpolar molecules helps when molecules are close to one another helps when molecules are close to one another results from momentary/temporary/ induced dipoles results from momentary/temporary/ induced dipoles itl.chem.ufl.edu

11. the more you can distort an atom or molecule’s electron cloud distribution, the more polarizable it is the more you can distort an atom or molecule’s electron cloud distribution, the more polarizable it is larger/massive atoms/molecules are more polarizable larger/massive atoms/molecules are more polarizable thus, larger atoms/molecules have stronger IMF’s thus, larger atoms/molecules have stronger IMF’s ex) halogens ex) halogens elmhurst.edu

12. cactus.dixie.edu C

13. NOTE: all molecules have London dispersion forces! NOTE: all molecules have London dispersion forces! when molecules are of similar size, polarity determines the strength of IMF’s when molecules are of similar size, polarity determines the strength of IMF’s when molecules differ greatly in size, then polarizability determines the strength of IMF’s when molecules differ greatly in size, then polarizability determines the strength of IMF’s phys.bspu.unibel.by HW: 11.8, 11.10, 11.12 (a)-(c), 11.18, 11.22

14. IMF flow chart do activity in lab area as a group of 4 do activity in lab area as a group of 4 have chart “Schu approved” have chart “Schu approved” copy as notes copy as notes adroll.com

15. II.Properties of Liquids 1. Viscosity resistance to flow resistance to flow high viscosity- molasses, syrup high viscosity- molasses, syrup low viscosity- ethanol, water low viscosity- ethanol, water based not only on the strength of the IMF’s, but also structural features that may cause entanglement of molecules based not only on the strength of the IMF’s, but also structural features that may cause entanglement of molecules as temp. inc., viscosity dec. due to the breaking of IMF’s as temp. inc., viscosity dec. due to the breaking of IMF’s syntheticperformanceoil.com

16. 2. Surface Tension due to the imbalance of IMF’s within a liquid due to the imbalance of IMF’s within a liquid there is a net downward pull of surface molecules there is a net downward pull of surface molecules results in close packing of molecules at the surface, forming a “skin” results in close packing of molecules at the surface, forming a “skin” fizyka.phys.put.poznan.pl

17. technically, surface tension is defined as the energy required to increase the surface area of a liquid by a unit amount technically, surface tension is defined as the energy required to increase the surface area of a liquid by a unit amount units: J/m 2 units: J/m 2 quest.nasa.gov

18. water has a high surface tension due to high IMF’s water has a high surface tension due to high IMF’s mercury has an even higher surface tension due to metallic bonding mercury has an even higher surface tension due to metallic bonding ramehart.com HW: 11.23

19. 3. Cohesion and Adhesion cohesion = IMF’s between molecules of the same substance cohesion = IMF’s between molecules of the same substance adhesion = IMF’s between molecules and other surface adhesion = IMF’s between molecules and other surface although both types of forces are present, mercury has greater cohesive forces than water whereas water has greater adhesive forces than mercury although both types of forces are present, mercury has greater cohesive forces than water whereas water has greater adhesive forces than mercury cr4.globalspec.com

20. 4. Capillary Action molecules of liquid rising up a narrow tube molecules of liquid rising up a narrow tube mechanism = adhesion causes water to stick to tube which increases the surface area; in order to reduce surface area, surface tension pushes water up tube against gravity mechanism = adhesion causes water to stick to tube which increases the surface area; in order to reduce surface area, surface tension pushes water up tube against gravity ex) chromatography; water in plant roots ex) chromatography; water in plant roots cc.gatech.edu HW: 11.24

21. III. Phase Changes chemistry.wustl.edu HW: 11.28

22. 1. Heating/Cooling Curves physicalweeding.com

23. heat is ALWAYS being added! heat is ALWAYS being added! when temperature increases, the KE (energy of motion) of the particles must be increasing (PE remains the same) when temperature increases, the KE (energy of motion) of the particles must be increasing (PE remains the same) when temperature remains the same, the KE of the particles must remain the same; thus, PE (energy of position) increases as the phase change occurs when temperature remains the same, the KE of the particles must remain the same; thus, PE (energy of position) increases as the phase change occurs funsci.com

24. ΔH vap > ΔH fus ΔH vap > ΔH fus q = mCΔT used for calculating heat during temp. changes q = mCΔT used for calculating heat during temp. changes where q = heat change in J m = mass in g C = specific heat in J/g·K or J/g·ºC ΔT = temp change (T f – T i ) in K or ºC where q = heat change in J m = mass in g C = specific heat in J/g·K or J/g·ºC ΔT = temp change (T f – T i ) in K or ºC mrbigler.com HW: 11.34

25. 2. Vapor and Vapor Pressure vapor = gaseous form of a substance normally found as a liquid vapor = gaseous form of a substance normally found as a liquid vapor pressure = pressure due to vapor vapor pressure = pressure due to vapor evaporation = vaporization of surface molecules of liquid evaporation = vaporization of surface molecules of liquid boiling = vaporization throughout liquid, occurs when the vapor pressure = atmospheric pressure boiling = vaporization throughout liquid, occurs when the vapor pressure = atmospheric pressure kidsgeo.com

26. STORYTIME! cityoflawton.ok.us

27. #1 Water in a Beaker @ room temp and standard pressure @ room temp and standard pressure what happens to it? what happens to it? goldcoast.qld.gov.au

28. #2 Stoppered Flask of Water @ room temp and standard pressure @ room temp and standard pressure what happens to it? what happens to it? daigger.com

29. #3 Ethanol Vs. Water @ room temp and standard pressure @ room temp and standard pressure what happens? what happens? volatility = the ability to evaporate easily volatility = the ability to evaporate easily outboardmotoroilblog.com images.veer.com

30. #4 Heated flask of Water constant heating @ standard pressure constant heating @ standard pressure what happens to it? what happens to it? normal boiling point = temperature at which the v.p. of water equals 1 atm (standard pressure) normal boiling point = temperature at which the v.p. of water equals 1 atm (standard pressure) demo.physics.uiuc.edu HW: 11.39, 11.42

31. 3. Vapor Pressure Curves kentchemistry.com HW: 11.43

32. 4.Phase Diagrams from textbook

33. triple point = temp. and pressure at which all 3 phases exist in equilibrium triple point = temp. and pressure at which all 3 phases exist in equilibrium critical point = the highest temp. and pressure at which a liquid can exist critical point = the highest temp. and pressure at which a liquid can exist supercritical fluid = liquid and gas phases are indistinguishable supercritical fluid = liquid and gas phases are indistinguishable definitiontees.com HW: 11.36, 11.47, 11.48, 11.50, 11.52

34. IV.Structures of Solids 1. Crystalline vs. Amorphous crystalline = well-defined arrangement of atoms or molecules (def. attractions = def. m.p.) crystalline = well-defined arrangement of atoms or molecules (def. attractions = def. m.p.) ex) quartz, diamond, ionic solids ex) quartz, diamond, ionic solids amorphous = no well-defined arrangement of atoms or molecules (indef. attractions = softens over temp. range, no distinct m.p.) amorphous = no well-defined arrangement of atoms or molecules (indef. attractions = softens over temp. range, no distinct m.p.) ex) glass, rubber ex) glass, rubber ndt-ed.org HW: 11.53

35. 2. Unit Cells unit cell = the “bricks” that make up a crystalline solid; the smallest repeating unit in a crystal lattice unit cell = the “bricks” that make up a crystalline solid; the smallest repeating unit in a crystal lattice fkp.jku.at

36. A) Primitive Cubic the lattice points are at the corners and are actually shared by 8 atoms! the lattice points are at the corners and are actually shared by 8 atoms! 1/8 of an atom x 8 corners = 1 atom 1/8 of an atom x 8 corners = 1 atom ece-www.colorado.edu mrsec.wisc.edu

37. B) Body-Centered Cubic lattice points are at the corners and at the center lattice points are at the corners and at the center 1/8 of an atom x 8 corners + 1 atom = 2 atoms 1/8 of an atom x 8 corners + 1 atom = 2 atoms ece-www.colorado.edu mrsec.wisc.edu

38. C) Face-Centered Cubic lattice points are at the corners and each face/side lattice points are at the corners and each face/side ½ of an atom x 6 sides + 1/8 atom x 8 corners = 4 atoms ½ of an atom x 6 sides + 1/8 atom x 8 corners = 4 atoms ece-www.colorado.edu mrsec.wisc.edu HW: 11.56, 11.58

39. 3. Bonding in Solids molecular solids molecular solids ionic solids ionic solids metallic solids metallic solids covalent-network solids = continuous lattice structure of covalent bonds (no molecules); rigid and dense with high m.p.’s (FYI, must break bonds to melt!) covalent-network solids = continuous lattice structure of covalent bonds (no molecules); rigid and dense with high m.p.’s (FYI, must break bonds to melt!) ex) SiO 2, C (diamond), C (graphite), C (buckyballs) ex) SiO 2, C (diamond), C (graphite), C (buckyballs) chem.ufl.edu HW: 11.69, 11.70

40. legacy.co.mohave.az.us