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Week 1 Notes - CHM1046

by: Monika Stark

Week 1 Notes - CHM1046 CHM 1046

Monika Stark
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About this Document

Beginning of Chapter 11
General Chemistry II
B. DePrince
Class Notes
General Chemistry, Chemistry, Intermolecular Forces, CHM1046, Chapter 11, phase diagrams




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This 2 page Class Notes was uploaded by Monika Stark on Sunday September 4, 2016. The Class Notes belongs to CHM 1046 at Florida State University taught by B. DePrince in Summer 2016. Since its upload, it has received 38 views. For similar materials see General Chemistry II in Chemistry at Florida State University.


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Date Created: 09/04/16
General Chemistry II Chapter 11 Week 1 BRIEF OUTLINE  2 concepts to look at in chemistry o 1. Thermodynamics  Will a process happen?  Will it happen completely?  Where is equilibrium? o 2. Kinetics  How fast will it happen?  Chapters 11-12: physical equilibrium  Chapter 13: kinetics  Chapters 14-16, 18 chemical equilibrium CHAPTER 11: INTERMOLECULAR FORCES (IMFs) AMONGST PURE SUBSTANCES Physical Process Chemical process  w/o breaking or forming  Formation/destruction of chemical bonds chemical bonds  INTERmolecular forces  INTRAmolecular forces = bonds  Polarity o Unequal sharing of electrons due to differences in electronegativity o NON-POLAR RULES  Central element connected to same elements  Central element less electronegative than other elements  Dipole moments cancel out  Examples: CO2 SiCl4 XeF4 IF2 - PCl2F  Types of IMFs o Ion-dipole: ion and a polar compound  Ex: NaCl----H2O o Hydrogen bonding: H connects with F, O, N  Ex: NH3----H2O o Dipole-dipole: polar covalent compounds  Ex: PH3----SiBr2- o Dipole-induced dipole: polar connects with nonpolar compound  H2O----CCl4 General Chemistry II Chapter 11 Week 1 o Dispersion/van der Walls: 2 nonpolar compounds. Everything has this!  Physical Properties that depend on IMFs o Stronger IMF = harder to break bonds apart  Higher boiling/condensing point  Higher melting/freezing point  Higher enthalpy of transition  Higher viscosity  Higher surface tension  LOWER VAPOR PRESSURE  States of Matter: Phase Diagram  Clasius-Clapeyron Equation: relationship between vapor pressure and temperature P Δ H 1 1 ln 2= νap − P1 R (T 2 T 1)


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