New version page

BU CHEM 108 - Overview

Type: Lecture Note
Pages: 5
Documents in this Course
Load more

This preview shows page 1-2 out of 5 pages.

View Full Document
View Full Document

End of preview. Want to read all 5 pages?

Upload your study docs or become a GradeBuddy member to access this document.

View Full Document
Unformatted text preview:

CHEM 108 1st Edition Lecture 1Notes for Lecture 1:Chem 108 is the second semester of the two-semester sequence in the fundamentals of chemistry; Chemistry 107 is the first semester of the sequence. Upon successful completion of the two-semester sequence, a student has sufficient chemistry background. This is a 4-credits course and comprises of topics from intermolecular forces to organic chemistry. Each week therewill be a lab for which a lab write up is due and a quiz during your discussion section. This will be the course objectives for the semester:CHEM 108 - Learning Objectives (Outcomes)Liquids, Solids and Intermolecular forces1. Phase diagramsa. identify liquid, solid, gaseous regions of phase diagramb. contrast and compare phase diagrams of water and carbon dioxidec. identify and comprehend triple point and critical pointd. interpret phase transitions when temperature or pressure is held constant2. Liquidse. comprehend van der Waals and hydrogen bonding interactions in liquidsf. predict liquid properties based on intermolecular interactions3. Solid stateg. contrast and compare different types of solidsh. comprehend crystal latticei. calculate density, unit cell dimensions, atomic radii, atomic mass for cubic unit cells4. X-ray diffractionj. comprehend diffraction in crystalline solid.k. use Bragg equation to calculate lattice spacingsSolutions1. Solutionsa. comprehend and interconvert between different concentration unitsb. comprehend energetic basis for solubilityc. predict probably effect of concentration, pressure, temperature, polarity on solubilityd. calculate gas solubility in solution with Henry’s lawe. comprehend deviations from ideal solution behavior2. Colligative propertiesa. comprehend thermodynamic and molecular basis for colligative propertiesb. calculate fp depression, bp elevation, vp lowering, osmotic pressure. Calculate molar mass from osmotic pressureKinetics1. Ratea. determine rate from reaction time courseb. contrast and compare instantaneous rate, average rate, IUPAC rate2. Rate lawa. determine rate law from experimental datab. computer reaction order from rate lawc. design experiment to determine reaction orderd. predict the effect of a concentration change on reaction rate3. Integrated rate lawsa. familiarity with 1st and 2nd order (self-association) rate lawsb. determine rate law and rate constants from reaction time course4. Reaction mechanismsa. familiarity with molecularity, elementary reactions, rate determining stepb. differentiate among rate law, reaction mechanism, overall reactionc. assess consistency between reaction mechanism and rate lawd. comprehend relationship between elementary reaction and molecular interpretation5. Theorya. comprehend correlation between rates and energy barriersb. familiarity with activation energy, catalyst, transition state, Arrhenius equationc. determine activation energy from temperature dependence of rate constantd. determine rate at one temperature from rate at another temperatureEquilibrium1. Conceptsa. comprehend, contrast, and compare definitions of equilibrium: dynamic, infinite timeb. comprehend law of mass actionc. differentiate between equilibrium and kinetics concepts2. Calculations with equilibrium constantsa. comprehend, contrast, and compare equilibrium constant and reaction quotientb. predict direction of reaction by comparison of equilibrium constant and reaction quotientc. calculate equilibrium constant given equilibrium concentrationsd. calculate equilibrium concentrations given equilibrium constant and some concentrations3. LeChatelier’s Principlea. comprehend LeChatelier’s Principleb. predict effect of concentration, temperature, pressure on direction of reactionAcids and Bases1. Conceptsa. familiarity with Arrhenius acids and bases (identify these in a proton transfer reaction andnamethe conjugate acid base pairs)b. familiarity with Bronsted-Lowry acids and basesc. familiarity with Lewis acids and basesd. evaluate direction of reaction based on the relative strengths of acids or bases involved2. Calculationsa. comprehend meaning of H3O+and OH–concentrations in aqueous solutions of strong acids,demonstrating proficiency in calculating either/both of these concentrations based onconcentrations of the strong acid or baseb. calculate concentrations of strong acids or bases given the value for either H3O+ and OH–ConcentrationsAcids-Base Equilibrium1. Conceptsa. comprehend weak acids and bases as partially-dissociated equilibrated species in solutionb. differentiate between Kc, Kw, Ka and Kb (and their p counterparts) for aqueous solutionsc. predict if a salt solution will be acidic, basic, or neutrald. familiarity with capacity and pH of bufferse. familiarity with preparation of a buffer, given a pK of weak acid or base, and desired pHf. interpret acid-base titration curves, noting equivalence point, buffering range, and pK2. Calculationsa. calculate Ka and Kb from solution pH and molarity of speciesb. calculate concentrations of species in solution given Ka or Kb, pH, and/or initialconcentrations of weak acid or basec. determine the influence of a common ion on the ionization of a weak acidd. calculate the pH of a buffer given initial weak acid or base concentratione. calculate the change in pH of a buffer when a strong acid or base is addedf. find the pH at the equivalence point for the titration of a weak acid or base with a strong baseor acidSolubility and Complex-Ion Equilibrium1. Conceptsa. understand the solubility product constant as the equilibrium constant for the solubilityequilibrium of a slightly soluble ionic compound.b. familiarity with writing expressions for the solubility product.c. comprehend the influence of a common ion on solubilityd. describe the qualitative effect of a pH change on solubilitye. comprehend the process of complexation and the meaning of the formation constant Kf2. Calculationsa. calculate Ksp from solubility or solubility from Kspb. calculate solubility of a slightly soluble salt in a solution containing a common ion.c. predict if/when precipitation will occur when two solutions are mixed given the volumes,molarities, and Ksp valuesd. perform calculations on complex ion equilibria using Kfe. predict whether a precipitate will form in the presence of a complex ion given Kf and Kspf. calculate solubility of a slightly soluble ionic compound in a solution of the complex ionEquilibrium and Thermodynamics1. Free Energy and Equilibriuma.


View Full Document
Loading Unlocking...
Login

Join to view Overview and access 3M+ class-specific study document.

or
We will never post anything without your permission.
Don't have an account?
Sign Up

Join to view Overview and access 3M+ class-specific study document.

or

By creating an account you agree to our Privacy Policy and Terms Of Use

Already a member?