1. 1. What intermolecular forces have we covered so far (there are two)? 2. Briefly describe each. Day 2 12-10

2. D. Induced dipole - ___________________ ____________________________________ 1. Exists in a molecule that is normally _________. 2. Induced dipoles are ___________. temporary dipole in a nonpolar molecule usually caused by brining it near a polar molecule nonpolar temporary

3. D. Induced dipole - ___________________ ____________________________________ temporary dipole in a nonpolar molecule usually caused by brining it near a polar molecule Soluble O 2 Ex.– (+) pole of water temporarily attracts the elecs. of O 2 (+) OOO H H (-)(+)(-) electrons

4. C. London Dispersion Forces 1. London dispersion forces exist between _________ _________ and are found in ____ ___________ 2. Induced dipoles and instantaneous dipoles arise when the ________ clouds of atoms or molecules are _________ by an outside influence such as a collision. nonpolar particles All substances electron distorted

5. 3. Polarizability is the _____ in distorting or “squashing” the electron cloud. 4. The _________ of the dispersion forces depends upon several factors ________ of _________ - more electrons = more polarizable (easier to distort)  stronger dispersion forces ease strength numberelectrons He vs. Ne

6. 4. The _________ of the dispersion forces depends upon several factors _____ or ____ - more mass = more polarizable (easier to distort)  stronger dispersion forces strength masssize CH 4 vs. C 6 H 14

7. D. Hydrogen Bonding 1. Hydrogen bonding is the attraction of an atom of _________ from one molecule to an atom with a high ________________ in another molecule, especially __, __, & __. hydrogen electronegativity F O N

8. 2. Hydrogen bonds affect compound characteristics such as _____________ _________________________________ 3. Diagram an example: H 2 O mixed with NH 3 and HF (see also p 390) boiling point, phase at room temp., shape ( DNA ), density  see C and H p 391

9. 1. In the table above the boiling points increase with _________________ molecular weight because the London dispersion forces are _________________. 2. Which of the following substances is most likely to exist as a gas at room temperature and normal atmospheric pressure: P 4 O 10, Cl 2, AgCl, I 2 ? Noble GasBoiling Point (K) He4.6 Ne27.3 Ar87.5 Kr120.9 Xe166.1

10. E. van der Waals Forces is an umbrella term for the intermolecular forces _________________, ____________, and __________________. F. How do the intermolecular forces compare in strength? london dispersiondipole-dipole hydrogen bonding london < dip.-dip. < H-bond < ion-dip. < ion-ion (for solids)

11. Practice 1 Unit 5

12. page 257 #s 65, 66, 67 … page 181 = electronegative values Ammonia = NH 3

13. Why do compounds with strong intermolecular attractive forces have higher boiling points than compounds with weak intermolecular forces? Day 3 12-11

14. 1. Which noble gas has the highest boiling point? Explain! Day 4 12-12

15. Thursday 12-18

16. E. van der Waals Forces is an umbrella term for the intermolecular forces _________________, ____________, and __________________. F. How do the intermolecular forces compare in strength? london dispersiondipole-dipole hydrogen bonding london < dip.-dip. < H-bond < ion-dip. < ion-ion (for solids)

17. III. Properties of Liquids A. Viscosity is a liquid’s ____________ to _____. 1. Higher viscosity indicates _____________, ___________, & _______________ resistance flow “thickness”slow flow Strong bonds

18. 2. Lower viscosity indicates ____________, __________, & _____________ 3. Temperature affects viscosity. a. How? b. Why? “thinness”fast flow weak bonds - T up, KE up, movement/flow up - T up, viscosity down

19. B. Surface Tension 1. Surface tension = net ________ force on the particles at a _________ surface a. “Skin” is visible as molecules are ________ __________. b. Creates ___________ shape and less _________ ______ inward liquid’s packed together surfacearea spherical

20. 2. Capillary action is a liquid’s rising in a _________ ______ until cohesive and adhesive forces _________. Examples: narrow tube balance

21. 3. Meniscus shape depends on strengths of cohesion versus adhesion. a. H 2 O  shape indicates stronger ___________ and weaker __________ b. Hg  shape indicates stronger __________ and weaker ___________ cohesion  adhesion  adhesioncohesion adhesion water sticking to water water sticking to another polar substance

22. IV. Vapor Pressure A. Vapor pressure is the pressure just above the _________ of a _______ or ______ as the particles escape into the air. B. Volatility 1. Liquids that are volatile ___________ easily. surface liquid solid evaporate

23. 2. Volatility depends on _________________, ________________________, vapor pressure intermolecular forces Higher vapor pressure = MORE volatile Weaker intermolecular forces of attraction = MORE volatile

24. Page 257 #s 70 page 257 #s 65, 66, 67 … page 181 = electronegative values Ammonia = NH 3

25. Day 5 12-15 1. Which liquid should be more viscous at room temperature honey or rubbing alcohol? 2. What if the honey is cooled by 10 degrees and the rubbing alcohol is heated by 10 degrees? 3. What intermolecular forces exist for NH 3 ? Put them in increasing order of strength.

26. 2. Volatility depends on ______________, and ______________. C. Boiling 1. ______ ___________ = __________ __________ size / weight temperature vapor pressureexternal pressure

27. C. Boiling 2. What obstacles must a water molecule overcome in order to boil? Intermolecular forces, especially H bonds (love of neighbors & family) Surface tension (surface sentinels  who goes there?) Pressure from outside (kept down by “the Man”)

28. Chapter 11 Homework # 1 – 10 correct http://wps.prenhall.com/esm_bro wn_chemistry_9/2/660/169060.cw /index.html

29. 1. How could we get water to boil withOUT changing temperature? 2. Which is more volatile water or methane? Explain reasoning! methane = Day 6 12-16

30. Thursday 12-18 day 2

32. Critical temperature – the highest temp. at which a substance can exist as a liquid (greater intermolecular attractive forces = higher critical temp.  substance would rather be liquid) critical pressure – pressure necessary to achieve liquid at critical temp. Triple point – temp. at which solid, liquid, and gas phases coexist in equilibrium

36. * During a phase change, temperature does NOT change (slope = 0) AS WE HEAT A SOLID!

37. Chapter 11 Homework # 1 – 10 correct http://wps.prenhall.com/esm_bro wn_chemistry_9/2/660/169060.cw /index.html

38. 100 mL of 0.1M SrCl 2 100 mL of 0.1M NaCl 100 mL of 0.1M CaCl 2 100 mL of 0.1M Ba(NO 3 ) 2

39. Thursday 12-18 day 2

40. BINDERS

41. Excused Late (1/2) Unexcused Late (1) Excused Absences (1) Unexcused Absences (2) Total Period 1102716.5 Period 3100919 Period 61181641.5 Period 7035618 Period 9025211