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

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

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

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

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

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

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

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

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

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)

Practice 1 Unit 5

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

Why do compounds with strong intermolecular attractive forces have higher boiling points than compounds with weak intermolecular forces? Day

1. Which noble gas has the highest boiling point? Explain! Day

Thursday 12-18

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)

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

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

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

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

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

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

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

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

Day 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.

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

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”)

Chapter 11 Homework # 1 – 10 correct wn_chemistry_9/2/660/ cw /index.html

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

Thursday day 2

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

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

Chapter 11 Homework # 1 – 10 correct wn_chemistry_9/2/660/ cw /index.html

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

Thursday day 2

BINDERS

Excused Late (1/2) Unexcused Late (1) Excused Absences (1) Unexcused Absences (2) Total Period Period Period Period Period