Presentation on theme: "Intermolecular Forces (l) & (s) phases: 1.Molecule-molecule 2.Molecule-ion."— Presentation transcript:
Intermolecular Forces (l) & (s) phases: 1.Molecule-molecule 2.Molecule-ion
Suggested Reading: 1) Page 380, I suggest you read the first paragraph in section 8.8 if not the entire section. 2) Review Example 8.12 on pg 384 to make sense of why NH 3 is more polar than NF 3, which at first seems odd. 3) Read the bottom of pg 558 beginning with, “When a polar…” to “…dipole-dipole attraction.” 4) Read three paragraphs on pg 562, starting with “There is an unusually strong…” to “…(Figure 12.7).” 5) On pg 565-567, read the two sections: “Dipole/Induced Dipole Forces” and “London Dispersion Forces: Induced Dipole/Induced Dipole”.
12.1 Know the level of intermolecular forces for each state of matter, s, l, g. Which has the most and which has none?
Boiling Liquids Liquid boils when its vapor pressure equals atmospheric pressure. PLAY MOVIE
4. If external P = 760 mm Hg, T of boiling is the NORMAL BOILING POINT 5. VP of a given molecule at a given T depends on IM forces. Here the VP’s are in the order C 2 H 5 H 5 C 2 H H 5 C 2 H H wateralcoholether increasing strength of IM interactions extensive H-bonds dipole- dipole O O O Liquids See Figure 12.17: VP versus T
From Chapter 13.6 Know how to interpret phase diagrams
TRANSITIONS BETWEEN PHASES See Section 13.6 Lines connect all conditions of T and P where EQUILIBRIUM exists between the phases on either side of the line. (At equilibrium particles move from liquid to gas as fast as they move from gas to liquid, for example.)