1. Announcements To join clicker to class today: – Turn on the Clicker (the red LED comes on). – Push “Join” button followed by “20” followed by the “Send” button (switches to flashing green LED if successful). ● If you gave me an exam to double- check, last week, you can pick it up at the end of class. ● Will be starting chapter 8 Today. Reading and problems have been e-mailed to you and posted on class web site. ● Quiz Today will cover all of Chapter 7 except for section 7.5. ● Wear appropriate clothes to lab (no sandals, shorts, etc...)

2. 07_29.jpg ● Hybrid orbitals to explain molecular shape and bonding. ● Double bonds are made from 1  and 1 , giving a bond that cannot rotate. Leads to cis- and trans- isomers. Review Trans- Cis-

3. Quantitative Calculations with Dipoles µ = Qr –µ = dipole moment in Cm –Q = magnitude in Coulomb (C) of separated charge –r = distance in meters between the charges. Ex: Suppose dipole of a molecule is: 1.30 D and r = 112 pm, what is the partial charge in C and in fraction of an electron? (1 e- has a charge of 1.60 x 10 -19 C/e)

4. Chapter 8 – Gases Pressure Ideal Gas Law (PV = nRT, solutions for P, V, n, T, density and molar mass) Dalton’s Law of Partial Pressures Henry’s Law of gas solubility Kinetic Molecular Theory of Gases (molecular speeds, diffusion and effusion) Real Gases/Non-Ideal behavior (van der Waals equation)

5. PV=nRT Called Ideal Gas Law P = pressure, we will use unit of atm, but can also be in –mmHg=Torr (1 atm = 760 Torr) –Pa = Nm -2 (1 atm = 101325 Pa) –bar = 10 5 Pa (1 atm = 1.01325 bar) V = the volume occupied by the gas n = the number of moles of gas in the volume R = the gas constant = 0.082058 Latmmol –1 K –1 T = temperature in Kelvin Model works well for gases near room temperature and 1 atm.