CHEM 1442 1st Edition Lecture 3Outline of Last Lecture I. Molecular GastronomyII. Vapor PressureIII. Chapter 16: Kinetics Outline of Current Lecture IV. PolarizabilityV. Aqueous SolutionVI. Concentration UnitsVII. Chapter 16Current LecturePolarizability- An atom is always non-polar- Polarizability occurs when non-polar becomes polar- This is also known as “induced” dipole o “Induced” dipole is not the same as “permanent” dipole- Polarizability refers to how easily the electron cloud can be distortedExample: Which element is more polarizable? Explain.Fluorine or BromineAnswer: Bromine is more polarizable because it is a larger molecule than Fluorine because the electron cloud is larger and the nucleus does not have that much attraction.Non-polar molecule is “induced” to be polar by the cation (“Induced” dipole force)Aqueous SolutionsThese 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.Solubility Rules for Ionic Compounds *NEED TO KNOW*Example: Soluble in water?a. NaClb. PbCl2c. CaSO4d. (NH4)2CO3e. Ca3(PO4)2Answer:a. Yesb. Noc. Yesd. Yese. NoDissolved ions turn into electrolytesDissolved molecules turn into non-electrolytesSolubility Rules for Covalent CompoundsRule: “like dissolves like”Substances with similar intermolecular forces tend to be soluble in one another:The more polar the molecule is, the better it dissolves in a polar solventThe more non-polar the molecule is, the better is dissolves in a non-polar solvent*Ionic is an extreme case of polarWhat affects solubility?- The tendency of substance to dissolve in another substance depends on:o Temperature  Most of the time as temperature increases, solubility increases *be careful with solids* With gases as temperature increases, solubility decreaseso Pressure (affects only gaseous substances) Negligible for liquids and solidsHenry’s LawSgas = kH x PgasSgasis the solubility in mol/L (M)kHis the Henry’s law constant (dependent on gas-solvent combination and a temperature) in (mol/L x atm)Pgas(in atm)Concentration UnitsMolarity (M) = mol of solute/ L of solutionMole fraction = mass of solute/ mass of solution x 100%Molality (m) = mol of solute/ kG of solventChapter 16Concept of Rate (Speed)= change of “whatever quantity” / time elapsedInitial Rate = instantaneous rate at time = 0Instantaneous speed = Slope of the tangent lineReactant: amount decreasesProduct: amount