1. Chemistry 112 Sections 5-9 Please don’t sit in the last four rows. And, thanks.

2. Chemistry 112 Sections 5-9 Bill Vining 232 PSCI 436-2698 viningwj@oneonta.edu

3. You should have had: General Chemistry I – Up through drawing Lewis Structures and Determining Molecular Structure and Polarity

4. General Chemistry I Basics of Atomic Structure Chemical Reactions and Equations Stoichiometry Solution Chemistry, mainly in water Thermochemistry Electronic Structure of Atoms Properties of Atoms Ionic Bonding Covalent Bonding of p-Block Elements Properties of Gases

5. General Chemistry II IMFs and Properties of Liquids, Solids, and Solutions Control of Chemical Reactions and Stability – Thermodynamics – Kinetics

6. General Chemistry II Special Types of Chemical Systems: – Organic – Equilibrium – Acid-Base – Dissolution – Complexation – Electrochemical

7. Business

8. Class Rules Syllabus

9. Business I Class meetings: – Lecture MWF here – Lab once a week in Physical Sciences Bldg. – Recitation once a week in Physical Sci. Room 122. NO LABS or RECITATIONS this week- they start Monday

10. Business II Be here every single day Be here on time Don’t sit in back Don’t talk when I’m talking Don’t let me talk when you’re talking It’s ok to get up and wander Pick up handouts, generally in back You are responsible Be nice Trust me Classroom Rules

11. Business III 3 Hour Exams OWL Homework Labs Final Exam Grades

12. Business IV If I fail the lab, Recite After Me: I fail the course.

13. Review: Bonding When atoms stick together, that’s bonding.

14. Why do Covalent Bonds Form? Electrons on one atom attracted to nucleus of other atom Nucleus on each atom repels other nucleus Electron on each atom repels other electron If new attractions > new repulsions, then a bond forms

15. Determining Molecular Geometry Valence Lewis Electron-Pair Molecular Electrons Structure Geometry Geometry

16. Chapter 11 Properties of Liquids and Solids Formula  Lewis Structure  Electron Geometry  Molecular Geometry  Polarity  Intermolecular Forces  Properties

17. What happens when water boils. Draw pictures. Bonding vs. Intermolecular Forces (IMFs): Where do IMFs come from?

18. Types of forces between molecules: Intermolecular Forces (IMFs)

19. Enthalpy of hydration: Trends: Ion-Dipole Forces: Between dissolved ions and polar molecules

20. Dipole-Dipole Forces: Between polar molecules Trends:

21. Dipole-Induced Dipole Forces: Between polar and nonpolar molecules Trends:

22. Induced Dipole-Induced Dipole Forces: Between nonpolar molecules Trends:

23. Hydrogen Bonding: Molecules with F-H, O-H, or N-H bonds

25. Hydrogen Bonding: Properties of water

27. More on Boiling Points and Hydrogen Bonding

28. Identifying IMFs

29. Relative Contributions of Different IMFs

30. Properties of Liquids Vapor Pressure (volatility) Boiling Point Enthalpy of Vaporization Viscosity Surface Tension

31. Molecular interpretation of vapor pressure and boiling. Enthalpy of vaporization:

34. Clausius-Clapyron Equation: Vapor Pressure,  H vap, and T

35. Graphical Method of Determining Enthalpy of Vaporization

38. Example 2. What is the mass of water in the air in this lecture hall? 14 m x 5 m x 17 m T = 22 o C Humidity = 43%

39. Example 3. A 1-L flask of air is at 30 o C and relative humidity of 68%. The flask is put in a freezer and the temperature decreases to 5 o C. What happens?

40. Surface Tension