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UT Arlington - MANAGEMENT - 4325
Followership1A closer lookSo, what are the complexities?So, what are the complexities?2The wheel of culture.TheAn interdisciplinary analysisDisciplines involvedCultural anthropologyBehavioral psychologySociologyOrganization behaviorCommunica
UT Arlington - MANAGEMENT - 4325
LeadershipLeadershipCommunicationCommunication1PROBLEM IN COMMUNICATIONThe single biggest problem incommunication is the illusion it has takenplace. George Bernard Shaw2LACK OF SENDING ANDRECEIVING DIRECTIONS3CommunicationA process by which
UT Arlington - MANAGEMENT - 4325
Building andBuildingLeading TeamsLeading1"Coming together is a beginning. Keepingtogether is progress.Working together is success."Henry Ford2"Individualcommitmenttoagroupeffortthatiswhatmakesateamwork,acompanywork,asocietywork,acivilizationw
UT Arlington - MANAGEMENT - 4325
DevelopingDevelopingLeadershipDiversityDiversity1EthnocentrismThe belief that ones ownculture and subculture areinherently superior to othercultures2BiculturalismThe sociocultural skillsand attitudes used byracial minorities as theymove ba
UT Arlington - MANAGEMENT - 4325
Courage andCourageMoralLeadershipLeadership1Wrong is wrong, no mater whodoes it or says it.Malcolm X2Unethical Climate In U.S.UnethicalBusinessesBusinesses Consequences of unethical and illegalbehavior Difficulty in attracting good employe
UT Arlington - MANAGEMENT - 4325
Leading ChangeThe Final Chapter!1Learning from Lincoln2Ex. 15.1 Forces Driving the Need for Major OrganizationalChangeChangeGlobalization, technological change, e-business, increasedcompetition, changing marketsMore threatsMore domestic competi
Duke - CHEM - 43
Three-Dimensional Structures of ProteinsThe properties of a protein are largely determined by its three-dimensional structure.Denatured: unfolded proteinThe peptide group has a rigid, planar structure, which, Pauling pointed out, is a consequence ofre
Duke - CHEM - 43
11/19/09Amino AcidsAmino AcidsMonomeric Units of ProteinsAt physiological pH, Zwitterionic form: compound that carries a net charge of zero, butcarries formal charges on different atomsThe Peptide BondAA1 + AA2 AA1AA2 + H2OWhat is a protein?Protei
Duke - CHEM - 43
11/24/09Protein 3 StructureA) Proteins are enormously complexStructures are abstracted in some wayDisplayed to highlight structural elements of interesti)Polypeptide backboneii)Key side chains: metal ligands, catalytic4 StructureMost proteins cont
Duke - CHEM - 43
12/1/09BiochemsitryHydrophobic ForcesCH4 in H2O CH4 in benzeneH117-TS-22.6G-10.9What happens when we introduce a nonpolar substance in H2O?H2O CANNOT H-bond to hydrocarbonsH2O must rearrange to accommodate the hydrophobic intruder# of ways H2
Duke - CHEM - 43
Amino Acids ChapterAmino acids: monomeric units of proteins-amino acids: standard amino acids that all have, except for proline, a primary amino group and acarboxylic acid group substituent on the same carbon atomIn the physiological pH range, both th
Duke - CHEM - 43
Chemistry43LFall2009TR8:309:45,BioSci111Instructor:Professor MichaelJ.Therien,5330FFSCMichael.Therien@duke.eduOffice HoursforProfessorTherien :TR4:005:00.Recitation Teaching Assistants :Jonathan Burg ,jmb95@duke.edu ;Office:XXXXX;Officehours:TOBEAN
Duke - CHEM - 43
Figure 8-29The triple helix of collagen.Voet Biochemistry 3e Page 235 2004 John Wiley & Sons, Inc.Collagen FibrilsVoet Biochemistry 3e 2004 John Wiley & Sons, Inc.Figure 8-32Banded appearance of collagen fibrils.Voet Biochemistry 3e Page 237 200
Duke - CHEM - 43
Biochemistry PowerpointSlidesLecture byDr. Michael J. TherienPage 66Covalent Structures and Abbreviations of the Standard AminoAcids Proteins, Their Occurrence, and the pK Values of TheirIonizable Groups.Page 67Table 4-1: Covalent Structures and
Duke - CHEM - 43
C hapter 4A mino A cids1.2.See Table 4-1 for the n ames a nd a bbreviations o f t he s tandard a mino acids. Leua nd De a re isomers w hereas n eutral L ys a nd GIn h ave e ssentially t he s amem olecular masses.(a)H2NN Hi" C.,yS-CHII3NHC
Duke - CHEM - 43
C hapter4Amino Acids1 T he A mino Acids o f P roteinsA. G eneral PropertiesB. P eptide BondsC. C'lilssiJjcation and CharacteristicsD. Acid-I3a&e PropertiesE. A F ew Words on Nomt:nclature2 O ptical Activit),A. A n O perational ClassificationB.
Duke - CHEM - 43
Chapter 8Three- DimensionalStructures o f P roteins1.W ith 3.6 r esidues p er20 x 5 .4/3.6 = 3 0 A long.t urna nda p itch o f 5.4AIt hea-helixisT he e nd-to-end d istance b etween t wo f ully e xtended a mino a nd r esidues is:."'f-~"1.33
Duke - CHEM - 43
C hapter8ThreeDimensionalStructures o fProteinsSecondary StructureA. T he Peptide GroupB. Helical StructuresC. B eta StructuresD. N onrepetitive Structures2 Fibrous ProteinsA. 0 : K eratin-A Helix of HelicesB. C ullagcn-A Triple Helical C
Duke - CHEM - 43L
12/1/09Chapter 15: Kinetics- Rates of Chemical Reactions-Notion of activation barrier-Molecules react by undergoing collision. These collisions impart energy; if there isenough energy to result in a reaction, the process goes forward-That notion conf
Duke - CHEM - 43L
12/3/09Chapter 15- Molecularity number of molecules colliding together for a reaction- If the concentration of a reagent was so great that its concentration did not change overthe course of a reaction, then the reaction was zero order in that reagent
Duke - CHEM - 43L
Chapter 15 Study GuideSpontaneous does not mean fast.Chemical kinetics: the area of chemistry that concerns reaction ratesThe definition of reaction rate assumes that the volume remains constant. A more general definition ofreaction rate is the change
Duke - CHEM - 43L
Chapter 9Stephanie Dudzinski8/25/09How will system x respond to:i)a specific load?ii)a specific action?Practical ramifications of chemical insight impact:EngineeringMedicineMaterialsKnow the Appendix: A1-A17Will cover: Chapters 6-10, 12-15Ce
Duke - CHEM - 43L
Chapter 98/27/09Associated with each system is some internal Energy, E (Kinetic & potential E of the system)E = q + wE results from changes in the heat content and/or the work done on or by the systemq+ endothermicq- exothermicw+ work done on the s
Duke - CHEM - 43L
Chapter 99/1/09How do we measure these thermodynamic quantitities?Calorimeter: an insulated device that can be used to determine the heat changeassociated with a chemical or physical process1) Constant pressure calorimeter2) Constant volume calorime
Duke - CHEM - 43L
Chapter 99/3/09IF the previous reaction were carried out at Pconstant, the surroundings would have donework on the system-11 kJ = nRT = PVOnly very few reactions are suitable for calorimetryEx: What is the enthalpy change when diamond is converted t
Duke - CHEM - 43L
Chapter 9: Energy Enthalpy, and Thermochemistry Study GuideEnergy: the capacity to do work or to cause heat flowLaw of conservation of energy: energy can be converted from one form to another but can beneither created nor destroyedThe total energy con
Duke - CHEM - 43L
1sn = 1, l = 02sn = 2, l = 03sn = 3, l = 0
Duke - CHEM - 43L
Chem 43Therien F 091.2 The Periodic Table In the early 19th Century Johann Dobereiner observed several groupsof three elements (triads) with similar chemical properties.[Dobereiners definition of an element was that of Boyles: a puresubstance that c
Duke - CHEM - 43L
The spectra of the elements are arrangedon horizontal lines spaced at equaldistances. The order chosen for theelements is the order of the atomic weights,except in the cases of Ar, Co and Te, wherethis clashes with the order of the chemicalpropertie
Duke - CHEM - 43L
Chapter 129/8/09Blackbody radiation: radiation that originates exclusively from the thermal energy of an object.Heating solids produced certain colors of light. At temperature of heating increased, glowing color ofsolid would change: redblue/yellowwhi
Duke - CHEM - 43L
Chapter 129/10/09Dobereiner observed several groups of three elements (triads) and noted that the atomic mass of 1 ofthe elements in the triad was the average of the other two: Cl, Br, I; S, Se, Te; Ca, Sr, Ba; Li, Na, K\Newlands organized elements fr
Duke - CHEM - 43L
Chapter 12 Study GuideElectromagnetic radiation: radiant energy that exhibits wavelike behavior and travels through spaceat the speed of light in a vacuumWavelength: the distance between two consecutive peaks or troughs in a waveFrequency: the number
Duke - CHEM - 43L
Chapter 139/17/09Lattice Energy: The change in E that takes place when separated gaseous ions arepacked together to form an ionic solid; Energy of stabilization that derives fromCoulombic interactionsE= kQ1Q2rIonic + Covalent BondsBonds that share
Duke - CHEM - 43L
Chapter 13 Study GuideBond energy: the energy required to break a given chemical bondIonic bonding: the electrostatic attraction between oppositely charged ionsIonic compound (binary): a compound that results when a metal reacts with a nonmetal to form
Duke - CHEM - 43L
10/1/09Chapter 10Spontaneity, Entropy, & Free EnergyThe first law of thermodynamics does not tell us if a reaction is spontaneous.A spontaneous reaction is a reaction has the potential to proceed on its own accordExamples:1)Ice spontaneously melts a
Duke - CHEM - 43L
10/8/09Chapter 10Ssolid<Sliquid<SgasExamples:1) C(s) + CO2(g) 2CO (g)Ssystem = +Whenever the products contain more moles of gas than the reactants, the change in entropy is alwayspositive for the system2) 2SO2(g) + O2(g) 2SO3(g)3) N2(g) + O2(g) 2
Duke - CHEM - 43L
10/13/09Chapter 10For an isothermal process, reversible process, S=qrev/TPhase TransitionsFusion (melting): solidliquidVaporizationliquidgasqp=HSfusion=Hfusion/TfSvap=Hvap/TvliquidsolidgasliquidWe can determine the differences in the entropies
Duke - CHEM - 43L
10/15/09Chapter 10Standard Free Energies of FormationGf= the change in standard free energies when one mole of a compound is formed in itsstandard state from its constituent elements in their standard statesGf (element, standard state) = 0Grxn = Gf(
Duke - CHEM - 43L
Chapter 10 Study GuideThe first law of thermodynamics: The energy of the universe is constantA process is spontaneous if it occurs without outside intervention.Thermodynamics tells us the direction of a process but NOT the speed(rate).Spontaneous proc
Duke - CHEM - 43L
9/24/09Chapter 14Demonstration: Neodymium magnets (element 60) Neodymium embedded in ceramic platesGraphite reactivity with neodymium magnetallows graphite piece to levitate above neodymiummagnetsDepending on the direction of the electrons orbiting t
Duke - CHEM - 43L
9/29/09Chapter 14*Figure 14.35: Three Mutually Perpendicular 2p Orbitals on Boron*Figure 14.36: Sigma Bonding and Antibonding Orbitals on Boron*Figure 14.40: Correct MO Energy-Level Diagram for B2*Figure 14.41: MO Energy-Level Diagrams, Bond orders,
Duke - CHEM - 43L
Chapter 14 Study GuideHybridization: a mixing of the native orbitals on a given atom to form special atomicorbitals for bondingHybridization is a modification of the LE model to account for the observation that atomsoften seem to use special atomic or
Duke - CHEM - 43L
9/29/09Chapter 21Introduction to Organic ChemistryCarbon-Has a large number of accessible oxidation states-Valence shell of 2s22p24 bonds-hybridized sp3offers the potential for a wide variety of 3-D shape*Figure 21.1: C-H Bonds in MethaneAlkanes:
Duke - CHEM - 43L
10/1/09Chapter 21*Figure 21.8: Bonding in Ethane*Figure 21.7: Bonding in EthyleneC-C double bonds are known as alkenesAlkenes: 2 orientations of sustituentsAlkenes do not rotate about C=C double bondCyclic Alkanes:Cyclohexane exists in two forms:
Duke - CHEM - 43L
Chapter 21 Study GuideBiomolecule: molecules that maintain and reproduce lifeOrganic chemistry: the study of carbon-containing compounds (typically chains ofcarbon atoms) and their propertiesHydrocarbon: compounds composed of carbon and hydrogenSatur
Duke - CHEM - 43L
C hemistry 43Midterm ExaminationTuesday, 20 O ctober 2009Name:Ans~ k~A nswer all questions completely a nd concisely. Give a n e xplanation for all y ouranswers. There are 10 q uestions o n 15 p ages w orth a total of 100 points. You h ave 75minute
Duke - CHEM - 43L
10/22/09Chapter 6Thermodynamic Definition of the Equilibrium Constant:Involves the ratio of the equilibrium pressure or concentration of a substanceActivity(A)= Pi/PreferenceKp is ALWAYS unitlessWhen the equilibrium constant is expressed in units o
Duke - CHEM - 43L
10/27/09Chapter 6GRxn = Go + RTlnQ1) Use the above relationship to calculate G and determine if a reaction is at equilibriumG=0K=Q2) For a reaction equilibrium, calculate GoChemical Equilbrium Chapter 6Acids/Bases Chapter 7 Acids/BaseSolubility o
Duke - CHEM - 43L
10/29/09Chapter 6Consider 3 changes to conditions that impact equilibrium:1)Changes in concentration (Partial pressure for gases of a constituent)2)Change in total pressure3) Change in TemperatureLe Chateliers Principle: when a stress is applied to
Duke - CHEM - 43L
Chapter 6 Study GuideChemical equilibrium: a dynamic reaction system in which the concentrations of all reactants andproducts remain constant as a function of timeEquilibrium is a dynamic situationHaber process: the manufacture of ammonia from nitroge
Duke - CHEM - 43L
H2(g) + I2(g) 2HI(g)Kp = 1.00 x 102A container holds 0.0100 atm H2(g), 0.00500 atm I2(g), and 0.500 atm HI(g). Whatare all equilibrium pressures?First do a Q test to predict the direction of the reaction.p20.500 2HIQ=== 5000 > 1.00 x 102p H 2 p
Duke - CHEM - 43L
10/29/09Chapter 7Define: properties of acids & bases / acid & base strengthEarliest definition:Acids- sour taste, turn litmus paper redBases- bitter taste, slippery when touched, turn litmus paper blueArrhenius (1887)Acids- substances that furnishe
Duke - CHEM - 43L
11/3/09Chapter 7Bronsted-Lowry (1923)Acid: substance that acts as a proton donorBase: substance that acts as a proton acceptorNeutralization reaction: Transfer of a proton from an acid to a baseWe can say:i)The stronger the acid, the more readily i
Duke - CHEM - 43L
11/5/09Chapter 7All of the acids we have considered thus far are monoprotic acidsStrong acids: HCl, HNO3Weak acids: HCN, HF, CH3, CO2HPolyprotic acids:H2CO3carbonic acidH2C2O4oxalic acidH3PO4phosphoric acidH2SO4sulfuricH2A + H2O H3O+ + HAHA- + H
Duke - CHEM - 43L
11/10/09Chapter 7Metal cations & their acid propertiesMetal ions attract the e- pairs of H2O molecules[Zn(H2O)4]2+[Zn(H2O)4]2+ +[Mn(H2O)g]2+H2O H3O+ + [Zn(H2O)3(OH)]+Cation hydrolysisimportant for metals with high charge & small sizeHydrolysis w
Duke - CHEM - 43L
Chapter 7 Study GuideArrhenius concept: a concept postulating that acids produce hydrogen ions in aqueoussolution, whereas bases roduce hydroxide ionsBronsted-Lowry definition (model): a model proposing that an acid is a proton donor,and a base is a p
Duke - CHEM - 43L
11/10/09Chapter 8Buffers: using the common ion effect to control pHBuffer solution: solution that resists a change in pH when acids or bases are addedExamples:1) Weak acid and its corresponding conjugate base salt2) Weak base and its corresponding c
Duke - CHEM - 43L
11/12/09Chapter 8In vivo BufferingRegulating of acidCO2 is rapidly released at the lungsH2O + CO2 H2CO3Hydrogen carbonate is blood acidH2O + H2CO3 H3O+ + HCO3-Ka = 4.3 x 10-7If CO2 is present in its dissolved form, it can not be eliminated15-20