CHEM 106 1nd EditionExam # 1 Study Guide Lectures: 1 - 10Exam1 Breakdown: Exam: February 13, 2014 @ 6:00 PMChapter 12 – 7 QuestionsChapter 13 – 10 QuestionsChapter 14 – 7 QuestionsExperiment 13 – 1 QuestionChapter 12: SolidsMetallic Bonds & Conduction Bonds: electrons from partially filled orbitals, and involves delocalized electrons that are sharedBand Theory: # atomic orbitals = # molecular orbitals-A filled band does not allow conductionUnit Cells: corner atom = 1/8 face atom = ½ edge atom = ¼ center atom = 1-unit cells represent stoichiometry, geometry, and density of the entire crystalAtomic radius from a unit cell: r = √24l (l is the edge length of the unit cell)Substitutional alloy: atoms of similar size replace others (have similar radii and crystal structure)Interstitial alloy: atoms are added in the holes in the pure metal crystalHoles: tetrahedral-4 atoms around the hole, smaller, 2 holes per host atomOctahedral-6 atoms around the hole, larger, 1 hole per host atomRadius ratio: r non−hostr hosttetrahedral hole: r = .22 - .41 octahedral hole: r = .41 - .73Notes: -for metals, the more electrons there are, the higher boiling point due to stronger forces-for metal crystals, a lower T means the atoms have lower kinetic energy, can get closer together-an alloy can be both substitutional and interstitial if voids are roughly same size-body centered = 2 atoms/unit cell face centered cubic = 4 atoms/unit cellSome Practice Questions for Chapter 12:Answer: BAnswer: CChapter 13: Organic ChemistryC forms strong bonds with C, H, N, and O-review lewis structures and VESPR Functional Groups: (review structures as well)Alkanes: single bond, only C or H ex: 3 carbon, propane rotation with single bondsAlkenes: at least one C=C ex: 3 carbon, propene no rotation with double bondsAlkynes: at least one C≡C ex: 3 carbon, propyneAromatic: at least one benzene ring (with alternating single and double bonds)Amines: any compound with C – N ex: methyl amine N makes 3 bonds + lone pairAlcohol: C compound with OH ex: 1 carbon, propanolEther: replace alcoholic H with a C ex: di ethyl ether Aldehyde: C without double bond at end of chain ex: butanal Ketone: C=O but not at the end of a chain ex: propanone Carboxylic Acid: ends with C=O,-OH (off C) group ex: ethanoic acid = acetic acidEster: structure includes C=O,-O-C (off C) ex: methyl propanoateAmide: structure includes C=O, -N- (off C) ex: methyl propanamideHydrocarbons (CxHy) with only C – C bondsUnsaturated hydrocarbons are converted to saturated by hydrogenationStructural Isomers: have the same molecular formula, but different structure and propertiesIsomers must have the same molecular formula, different orientations are not different isomersNaming Alkanes: 1-meth, 2-eth, 3-prop, 4-but, 5-pent, 6-hex, 7-hept, 8-oct, 9-non, 10-dec Simple unbranched chain: n-____ane ex: n-heptane (7 carbons) Naming Branched Chains: first name longest chain, then name branches by number of carbons with prefix + ___yl, indicate point of attachment by carbon number to main branch, multiple identical groups (di, tri, tetra), multiple substituents are alphabetically named.(Review pictures and examples in notes)Rings are indicated by cyclo____aneTrans: larger substituents are on opposite sides Cis: same side-molecules with free rotation do not have trans or cis isomersAromatic Compounds are named based off of location of attachments, and benzene.Amines: R- a group that bonds through a single bond (has N)Remember that like dissolves likeSynthesis Reaction: acid + alcohol → ester + H2O (condensation reaction)-be able to predict which alcohol + ester combine to make a particular esterPolymers: copolymer equal moles of 2 different monomers (alternating continuing)Chirality: optical isomers, not superimposable on their mirror image, is certain if there are 4 different substituents on a C, must be single bondSome practice questions from Chapter 13: Answer: EAnswer: CChapter 14: ThermodynamicsEnergy is not destroyed, only transferred between system and surroundings (1st law)Spontaneous Reaction: occurs without outside intervention, often exothermic (ΔH < 0) but not alwaysNon Spontaneous Reaction: occurs only with the continuous input of energyEntropy (S): measure of the distribution of energy, measure of order/disorderThe total entropy of the universe increases in any spontaneous reaction (2nd law)Forms of kinetic energy: translational, rotational, and vibrationalMicrostates: unique distribution of particles among energy levels (ex: # of possible outcomes)# of microstates ↑ entropy ↑S = k ln W S=entropy k=Boltzmann’s constant (1.38(10^23)) w=# microstatesSolids have the lowest entropy (least disorder), and entropy is a state functionΔSsystem = Sfinal – Sinitial ΔSsys = q rev / T q rev = heat entering or leavingΔSuniv = ΔSsys + ΔSsurr isothermal means constant TExothermic Reaction: q sys < 0 q surr > 0 ΔSsurr > 0S° values are absolute value, ΔH values are notQ = n Cp ΔTAs phase changes from more condense to less condense, S° ↑Entropy always ↑ with T (for given molecule)ΔS rxn = Σ n products S° products – Σ n reactants S° reactants (numbers provided)Gibbs Free Energy: ΔG the energy available to do work ΔG = ΔH – TΔS (check units)ΔG < 0 – spontaneous ΔS univ > 0 – spontaneousIf reaction is reversed, so is sign on ΔGIf ΔG = 0, then the system is at equilibriumLimitations of Thermodynamics: tells us nothing about rate of reaction or how it occurred Some questions from Chapter 14:Answer: DAnswer: