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UI CHEM 1120 - Solutions
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CHEM 1120 1st Edition Lecture 1Outline of Last LectureI. (No previous lecture) Outline of Current Lecture II. Intermolecular ForcesA. 6 Types of Intermolecular Forces (IMFs)III. Introduction to Chapter 13, The Solution ProcessA. Solution Terms: Homogeneous, Solute vs Solvent, etcB. Intermolecular Interactions Involved in Solution FormationIV. Dissolution processV. SolubilityCurrent LectureII. A. Before we can talk about chapter 13 and forming solutions, we mustremember the different types of IMFs, forces acting between molecules, because the ability to form solutions depends on the IMFs involved in the process. These IMFs, in order from strongest to weakest, are:1. Ion Dipole = force between an ion and a polar molecule possessing a permanent dipole moment2. Hydrogen Bonding = force resulting from attractions between molecules with a hydrogen bonded to an electronegative element (most common = OH, HF, NH)3. Dipole Dipole = force when polar molecules interact or become close (positive end of one approaches negative end of another)4. Ion Induced Dipole = weak attraction resulting from an ion influencing a dipole in an atom or nonpolar molecule by disturbing their electron arrangement These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.5. Dipole Induced Dipole = weak attraction resulting from a polar molecule influencing a dipole in an atom or nonpolar molecule by disturbingtheir electron arrangement6. Dispersion Forces = forces resulting from induced dipoles attracting each otherIII. A. Homogeneous = the same content throughout the solution or mixture Solution = homogeneous mixture of two or more substances Solute = the dissolved material (usually least abundant in solution) Solvent = the dissolving agent (usually most abundant in solution) Solvation = when solvent molecules array around a solute particle Hydration = when water solvent molecules array around a solute particle (solvation where water is the solvent)B. In solution formation, certain intermolecular interactions are involved, depending on whether they happen between a solute and another solute, a solute and a solvent, or a solvent and another solvent:1. Solute-Solute —> these interactions must be overcome to allow the solute to spread through the solvent2. Solute-Solvent —> interactions that happen as these different particles mix together3. Solvent-Solvent —> these interactions must be overcome to allow room or holes for the solute to spread throughFor Gas and Solid Solutions:1. Gas-Gas —> all gases are infinitely soluble in each other2. Gas-Solid —> Gases dissolve in solids by occupying “holes” in the crystalline structures 3. Solid-solid —> Atoms may replace atoms or fill in “holes” in the crystalline structuresIV. The process of dissolution, or dissolving a solute into a solvent, can be viewed as a three step process:Example- Dissolving NaCl in WaterStep 1 = The NaCl crystals are separated into ions (endothermic, requires work, change in HSOLUTE is positive)Step 2 = The water molecules separate to create “holes” that can accommodate the Na+ and the Cl- ions (endothermic, requires work, changein HSOLVENT is positive)Step 3 = The Na+ and Cl- ions enter and fill the “holes” created by the water molecules (exothermic, work is done by system, change in HMIX is negative)*Heat of Solution = HSOLUTE + HSOLVENT + HMIX*Processes in which entropy increases tend to be spontaneous and vice versa*Things will try to be as disordered as they can be with the energy they haveV. Solubility = the maximum amount of solute that dissolves in a given amount of solvent at a certain temperature when at equilibriumUnsaturated = solution where there is less solute than can dissolve in the solventSaturated = solution where the solvent holds as much solute as is possible at a certain temperature; dissolved solute is in dynamic equilibrium with solid solute particles Supersaturated = solution where the solvent holds more solute than an equivalent saturated solutionOverall, the general trend shows that “the stronger the attractions between solute and solvent molecules, the greater the solubility of the solute in that solvent”. Additionally, polarity comes into play when talking about the attractions and solubility because polar solutes tend to dissolve in polar solvents and nonpolar solutes tend to dissolve in nonpolar solvents. These tendencies bring us to the conclusion that polar solutes tend not to dissolve,or tend to be insoluble, in nonpolar solvents, and nonpolar solutes tend to beinsoluble in polar


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UI CHEM 1120 - Solutions

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