Chapter 13:CHE-102 Lecture Outline Chapter 13Syllabus Info: (Please read entire syllabus located on UB Learns)Lecture UB Learns:Lecture MaterialAnnouncements: made at start of lectureRecording: Posted in Class Recording linkSkeleton Outlines: to help take notes, if you wishAnswers to Additional Problems: extra problems are located at end of each outlineAdditional Videos: YouTube videos I have found pertaining to the more difficult material Please bring to EVERY class Outlines (UB Learns) Calculator Periodic table & Equation pg (UB Learns)Mastering chemistry: Technical Issues: Contact Mastering Chemistry Pop-up Blocker disabled? OR Flash player updated? 6 attempts at each submit button Hints: Some questions have them If answer correctly, earns extra pts, but if answer incorrectly, can lose points,• But if help you answer overall question then you usually earn more points than you would lose if you didn’t answer the question• No points lost if look at them HIGHLY recommend using when available Suggestions: Each assignment ~1-3 hrs  Work the problems pertaining to material learned in that day’s lecture If can’t answer in 10 minutes or 3-4 tries?• Move on and seek helpGetting Help Go to Instructor office hrs: Starts 8/28/17 See pg 1 of syllabus: First 2 weeks of classes ALL Dr. Gulde’s office hrs are in NSC325 Go to NSC110 for TA help: Starts Mon. 9/11/17 1st come, 1st serve basis1CHE-102 Lecture Outline Chapter 13Chapter 13:Properties of SolutionsSolutions Solutions – are homogeneous (uniform) mixtures Solute – usually present in smaller amounts, it’s dissolving Solvent – usually present in larger amounts, causes dissolving• We are familiar w/ water but doesn’t have to beSolution Equilibrium Dissolution (dissolves) – solute breaks apart ( into ions or molecules ) Crystallize - when dissolved solute comes out of soln (forms a solid) Solution Equilibrium – when the rates of these processes are equaldissolvescrystalizeTypes of Solutions2CHE-102 Lecture Outline Chapter 131. Saturated solutions – contains max amount of solute for a solvent, at a specific tempSugar: 25C = 211g/100g H2O50 C = 260g/100g H2O  If add more solute it won’t dissolve Solubility – amount of solute needed to form a saturated solution2. Unsaturated solutions – contains less than max amount of solute, at a specific temp If add more solute it will dissolve, until reach saturation3. Supersaturated solutions – contains more than the max amount of solute, at a specific temp To make: heat saturated solution, add solute then cool to original temp• Not stable If add more solute, excess crystallizes, until saturation reached (Alum exp. From CHE101)3CHE-102 Lecture Outline Chapter 13WHY do Solutions form?1. Entropy (S) – an increase in disorder(randomness)2. Similar forces dissolve within each other“Like dissolves like”!!• Polar solvents dissolve: polar or ionic solutes• Nonpolar solvents dissolve: nonpolar solutes Liquid solubility terminology:• Miscible – mixes completely• Immiscible – doesn’t mix significantly- Ex: Oil & Water 4no solution b/c forcesnot similarCHE-102 Lecture Outline Chapter 13Type of Forces:A. Intramolecular forces: is b/t atoms within a molecule (aka BONDS! Solid lines) Chap. 8: Ionic, Covalent, Metallic B. Intermolecular forces (IMF): is b/t atoms of separate molecules (dashed lines) Chap. 11: London dispersion, Dipole-Dipole, H-bonding, Ion-dipoleIntermolecular Forces (IMF)1. London Dispersion– the movement of electrons in the electron cloud creating an instantaneousdipole (temporary partial charge) • All molecules have these2. Dipole-Dipole– attraction between neutral polar molecules• Permanent dipole ( + )5Intramolecular forceIntermolecular forceCHE-102 Lecture Outline Chapter 133. Hydrogen bonding – Extra strong Dipole-Dipole force  Required:a) H atom bonded to N, O, or F b) Attracted to lone pair of another N, O, or F atomIon-dipole  between ions & partial charges (dipoles, δ) of polar molecules • Exist when ionic compounds (ex. NaCl) dissolve in polar substance (ex. water)Sample Problems:1. List all the intermolecular forces associated with:a) CH3Cl:• Dispersion? Yes• Dipole-dipole? Yes• H-bonding? No• Ion-dipole? No2. Will a solution of CH3Cl and H2O form, are they miscible? Yes (Like Dissolves Like) CH3Cl: Polar H2O: Polar6b) H2O:• Dispersion? Yes• Dipole-dipole? Yes• H-bonding? Yes• Ion-dipole? NoCHE-102 Lecture Outline Chapter 13HOW do Solutions form?« Forces & bonds are broken & new forces created! Solvation – when solute (ions or molecules) is surrounded by solvent in a specific way Hydration – special case of solvation b/c water = solvent There are 3 interactions involved in solution formation & each has anenthalpy (H) changeA. SoluteSolute interaction (Hsolute): must be broken Requires energy, endothermic (+)B. SolventSolvent interaction (Hsolvent): must be broken Requires energy, endothermic (+)C. SoluteSolvent interaction (Hmix): must be formed Gives off energy, exothermic (-) All 3 processes occur at the same time 7NaCl(s) in waterWater _____________NaCl apartWater _________________to NaclEx: NaCl(s)  Na+(aq) + Cl(aq)CHE-102 Lecture Outline Chapter 13 OVERALL enthalpy of Solution (Hsoln): add all 3 processes Hsoln can be endothermic (+) or exothermic (-) Depends on size of IMF Soln formation is favored when Hsoln is exothermic! Solute-Solvent particles are highly attracted to each other(they want to be together, so  Hmix is large) Why does this disfavored endothermic solution form? (NH4NO3 HSoln = +26kJ) Entropy, S (disorder) counteracts small HSoln value• If Hsoln is very positive, no soln forms8CHE-102 Lecture Outline Chapter 13Solution Formation Review Solute-Solvent Interactions:1. Enthalpy (Hsoln): heat Solutions usually form when Hsoln < 0 (exo) Strong solvent-solute interactions2. Entropy (S): disorder Solutions usually form when S increasesi. Helps compensate for Hsoln > 0 (endo)Sample Problems1. What forces are associated with each process involved when CH3Cl dissolves in water?Solute= CH3Cl Solvent= H2ODiploe-Dipole H-bonding Dipole-DipoleQuestion:13.2: Label the following processes as exothermic or endothermic:(a)