PowerPoint PresentationSlide 2Slide 3Slide 4Slide 5Slide 6Slide 7Slide 8Slide 9Slide 10Slide 11Slide 12Slide 13Slide 14Slide 15Slide 16Slide 17Slide 18Slide 19Slide 20Slide 21Slide 22Slide 23Slide 24Slide 25Slide 26Slide 27Slide 28Slide 29Slide 30Slide 31Slide 32Slide 33Slide 34Slide 35Slide 36Slide 37Slide 38Slide 39Slide 40Slide 41Slide 42Slide 43Slide 44Slide 45Slide 46Slide 47Draw the resonance structure indicated by the arrows.1)2)OO3)OOLabel each atom with the correct hybridization.4)HOOsp3sp3sp3sp3sp3sp3N5)sp3sp3sp2sp26)Osp3sp2sp2spsp7) Draw H2NCH2+ in its second best resonance structure.N CH2HHN CH2HHN CH2HH8) Draw the best Lewis structure for CH3CHO, a neutral molecule H3CCOH9) Draw the Lewis structure for CH3COOH, a neutral molecule. H3CCOOH10) Draw the Lewis structure for N2H2, a neutral molecule. HN NH11) Draw in the electron flow arrows in on the left hand structure that lead to the resonance structure on the right.OO12) In the empty box, draw the best resonance structure of the left-hand compound, and draw one or more electron-flow arrows on the preexisting structure that lead to the new structure. OOOO13)14)ClClClClClClClCl1234Label each of the following as an ionic or covalently bonded compound.a) NaFb) BrClc) NaOCHeioniccovalentionicCalculate the formal charge of nitrogen in each of the following compounds.a)b)NFC = 5 – (4 + (1/2(4))) = -1N NFC = 5 – (0 + (1/2(8))) = +1FC = 5 – (2 + (1/2(6))) = 0Draw the Lewis structure.a) (CH3(OH2))+b) CH3NO2C OHHHHHC NHHHOODraw all possible isomers of C2H4O.H3CCOHCH2CHHOH2C CH2OAre each of the following pairs isomers or resonance structures?a)b)H3CCH2CH3H3CCH2CH2Neither, different formulasOOIsomers, same formula but different arrangement of atoms.Draw a resonance structure of each, and identify which is the major contributor.a)b)ONH2HONH2HH3C COCHCH2H3C COCHCH2Draw all possible resonance structures of the compound below and it’s resonance hybrid.CH2CH2CH2CH2CH2CH2Predict the geometry around each indicated atom.a)b)H3CH2CCH2CH3tetrahderalCH2H3C OHTrigonal planarDraw the three dimensional structure of the following.a) CH3OHb) (CH3)2NHHCOHHHHCNHHHHHHConvert each molecule into a skeletal structure.a) (CH3)2CHCH2CH2CH(CH3)2b)C CH3CHHH HHHHCHCH3H3CHConvert into Lewis structures.a) (CH3)3COHb) CH3COCH2BrH3CCH3CH3O HOHHHHHBrWhat is the hybridizatio of th eindicated atom.a)b)sp2sp3CO2Hspsp2Which is the weakest of the indicated bonds?abcA is the weakest bond due to it being composed of a sp3 and sp2 hybridized orbital, thus having the least amount of S characterHONH2abB is the weakest, b/c bond strength increases across a row in the periodic table and N is to the left of O.Draw the products and label each part.OOH+OCH3OO+HOCH3ACBBCA+HNaNH2+NH3NaACBBCADraw the products and determine if the reaction occurs.F3COOH+O CH2CH3F3COO+HO CH2CH3pka=0.2pka=16Products favoredOOH+NaClOO+HClpka=5pka=-7reactants favoredWhich is the strongest base?HBr, HCl or HFHF, b/c it is the weakest acid.Identify the most acidic hydrogen.HHHHHabcC is the most acidic hydrogen b/c it’s bonded to an sp hybridized carbon.Draw the products of each reaction and label the starting materials as a Lewis acid and base.Cl+ClBCl ClClBCl ClClLBLAO+ClBCl ClOClBClClLBLA1) Complete the following acid-base reaction.O+OHOH+O2) Complete the following acid-base reaction. Draw only the organic products.OHKOHOOHHO+HOHK3)OHOHOH+OH4) Choose the strongest acid.H ClH BrSHHH BrBoth Cl and Br are further right than S. And Br is further down than Cl. So most acidic.5)OHPH2SHSHBoth O and S are further right than P. And S is further down than O. So most acidic.6) Choose the weakest acid.OHSHCH3CH3C is further left than O and S so weakest acid.7) The following compound has two stereoisomers. One has a dipole of 0 D, and the other has a dipole moment of 2.95 D. Draw the structure of the stereoisomer with dipole moment of 2.95 D. Cl ClClHHClClHClHClHHClClHClHOHSiH3CH38) Rank the three compounds from least acidic (rank 1) to most. 123We know Si is more acidic than C because it is below C in the same column. Although Si and O can’t be compared directly, O is much more acidic.9) Rank the following compounds from most acidic (rank 1) to least. H3CH2COOHClH3CH2COOHBrH3CH2COOHOHH3CH2CH2COOH1234Acidity is based on the electron withdrawing effect of the four different substituents. O is the most electronegative, furthest up and to the right, and thus gives the most acidic compd. And Cl is more electronegative than Br b/c electronegativity increases up the column.10) Draw the electron-flow arrows that lead from starting materials to products in this acid–base reaction. H HNHHHNHHH11)NOOHNHOO1) Draw an aldehyde.ROHRCHO2) Draw an ester.ROORRCOOR or RCO2R3) Draw a sulfide.RSRRSR4) Draw 1,1-dimethylcyclohexane.5) Draw 2,2,4-trimethylhexane. 6) Draw trans-1,3-dibromocyclobutane. BrBrBrHBrHHBrHBrBrBr7) Draw cis-1-chloro-3-isopropylcyclopentane. ClClClHHHClH8) Draw sec-butylcycloheptane9) Draw 2,2,4,4-tetramethylhexane 10) Draw the structural formula of an alkane that has eight carbons and only primary hydrogens. CH3CH3H3CCH3CH3CH3Primary hydrogens are attached to carbons attached to only one other carbon.11) Draw the conformation favored by 1,2-dichloroethane at equilibrium in the liquid phase by following this procedure. ClH HClHHHCl HClHHanitgaucheThe gauche conformer is favored in the liquid phase due to a polar effect. However, for this class I would accept the anit conformer as your answer, which would be correct if in the gas form.12) Draw cis-3-ethyl-1-isopropylcyclohexane in its lowest energy conformation HH13) Draw trans-1-bromo-3-methylcyclohexane in its lowest energy conformation CH3HHBr1) Draw the Lewis structure of HNO3. ONHO O2) What is the formal charge of the following compound? H CHHFC = 4 – (2 + (1/2)(6)) = -13) Draw all resonance structures OOOOO4) What are the hybridizations of the numbered carbons?12sp3sp25) Which of the following compounds has the largest net dipole? Draw the contributing dipoles of the compound you choose. CO2 H2O CHCl3 HOH6) Draw the product of the following reaction. (Label the Lewis Acid and Base) OHLALB 7) Which molecule plays the role of acid? HNO3 + H2SO4 → HSO4– + H2NO3+ acid8) Using pKa values from the table, determine if the following reaction will occur. pKa HA 3.7 HCOOH 4.2 C6H5COOH 4.75 CH3COOH 15.5 CH3OH OOH+NaOCH3HO CH3+OO4.7515.5pKa of
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