if all options ace nonpola checkMW CHM 1046 EXAM 1 REVIEW AND CONCEPT SHEET LECTURE 1 Be able to Identify the type of intermolecular forces IMFs experienced by molecules based on their structures Which are the strongest Which are the weakest o London Dispersion Forces the force of attraction that arise as a result of temporary dipoles induced in the atoms of molecules Experienced by ALL molecules increases w of e o Dipole Dipole Forces forces that occur between polar molecules A permanent dipole exists when one end of a molecule is electron deficient partially positive and the other end of a molecule is electron rich partially negative o Hydrogen Bonding a type of dipole dipole interaction between the hydrogen atom in a polar bond and an unshared electron pair of an element that is very electronegative Electronegative atom must be N O or F o Ion Dipole Forces experienced by ions interacting with polar molecules in solution o Dipole Induced Dipole Forces exists when a polar molecule induces a dipole on a Think NaCl in H2O nonpolar molecule due to proximity strongest Draw Lewis structures VSEPR theory and determine if the molecule is polar or nonpolar o VSEPR Theory electron pairs in a molecule will repel one another therefore electrons will distribute themselves in positions around the central atom that are as far away from each other as possible Understand the concept of polarizability o Polarizability measure of ease with which electron charge density is distorted by an external electric field reflects the ability for which a dipole can be induced Greater the polarizability of molecules stronger the IMFs Larger molecules have greater polarizability Distinguish between adhesive and cohesive forces the ngPIE ime Define viscosity surface tension and capillary rise Fill out and give reasoning for the trends seen in the table below resist gsgIncef o Adhesion the ability to stick to things like glass other than itself o Cohesion the ability to stick to itself o Viscosity resistance to flow exhibited by all liquids and gases o Surface Tension resistance of a liquid to increase in its surface area o Capillary Rise Action spontaneous rising of a liquid up a narrow tube o o Refer to videos Increase decrease or stay the same Boiling Point Melting Point Surface Tension MFnsgheianip EsisstongEaafact siYamse lyEEpEscmghf 1 891 higher higher higher higher higher lower higher lower lower lower lower lower higher lower lower higher higher higher higher higher higher lower lower lower higher Vapor Pressure lower lower Viscosity Freezing Heat of Point Vaporization Stronger IMFs Weaker IMFs increase lower Greater Electrons Lesser Electrons IMF Strongestbonding dispersion MW note e present so or ni Increase in MW Decrease in MW Increase in Temp Decrease in Temp higher higher higher higher higher lowel higher lower lower lower lower lower lower higher nochangeEnange Enangelower lower highes Focceration dependson renangeEnangeEnangehigher higher lower Tocceration substance LECTURE 2 Be able to Define phase transitions matter o Phase Transitions describe the conversion between solid liquid and gaseous states of o A specific temperature is required to induce a phase transition in a certain substance The stronger the IMFs the higher the phase transition temperatures will be t iengint Use phase diagrams to identify stable phases at given temperatures and pressures Describe the transitions resulting from changes in temperature and pressure Explain what the triple point and critical point are are in equilibrium o Triple Point the point on the phase diagram at which all three states of matter exist and o Critical Point the point on the phase diagram where the liquid and gaseous states are o Be able to identify these on any phase diagram indistinguishable Identify all the phase transitions fusion melting vaporization condensation sublimation deposition diagram Explain what a supercritical fluid is Where does a supercritical fluid exist in terms of the phase o Supercritical Fluid any substance at a temperature and pressure above its critical point Determine if phase changes are a physical or chemical change Why Understand the difference between endothermic and exothermic reactions is energy absorbed or released Is energy going into or out of the system Teaningbondsformationofbonds Draw heating cooling curves and determine the associated heat needed to perform the transition s o q mc T diagonal line and q n H horizontal line Be cautious of units WATCHUNITS doesitchangethechemicalformulaof thesubstan LECTURE 3 Be able to Explain the difference between crystalline and amorphous solids Explain the different types of crystalline solids stuptured ransom Ionic Solids ionic bonds hold the solid in a regular three dimensional arrangement o Mpakittle ionicbonds o Molecular Solids solids like ice that are held together by IMFs o Covalent Network a solid consists of atoms held together in large networks or chains by Properties low melting point nonconducting Properties high melting point brittle hard IMFS umpired mphard gaggedonas nconductor 1998 vauleneage covalent bonding Properties high melting point hard nonconducting o Metallic Solid similar to a covalent network but with metals Properties variable hardness and melting point high conductivity o Allotrope some solid substances can exist in more than one form diamond coal Explain what an allotrope is graphite Identify causes of crystal defects o Crystal defects are imperfections in the geometric shape of atoms within a crystalline o Deformation of the solid rapid cooling from a high temperature high energy radiation solid that can affect behavior striking solid Determine if a crystal is SC BCC or FCC based on the schematic drawing Memorize the following equations and use them in calculations o 2r a SC 4r 3a BCC 4r 2a FCC o Z M Na a3 mass volume o V a3 where a edge length o Vsphere 4 3 r3 Identify the number of atoms in the unit cell for SC BCC and FCC they are needed in calculations o SC 1 BCC 2 FCC 4 is iiii LECTURE 4 Be able to Ts d MW atoms a3 avogadros u Describe the basic properties of solutions and how they form what is the solute and what is the o The solvation process is thermodynamically favorable through the increase in entropy solvent and decrease in energy Understand like dissolves like and how to use this to answer conceptual questions Define solubility a saturated solution a supersaturated solution and a dilute solution temperature o Solubility the
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