6 Organic Chemistry ll For Dummies
6 Organic Chemistry II For Dummies 03_178157-intro.indd 6 5/28/10 9:44 AM
PartI Brushing Up on Important Organic Chemistry I Concepts The 5th Wave By Rich Tennant JASON WAS ALWAYS LATE FOR CLASSES HELD IN THE ESCHER BUILDING RLHTENNANT
Part I Brushing Up on Important Organic Chemistry I Concepts 04_178157-pp01.indd 7 5/28/10 9:45 AM
In this part... emary and Organic Chemistry I topics you need a firm grounding in before moving on to Organic Chemistry Il.Different books and different instructors break Organic I and Organic lI material at different places.We use the most common break,but some Part I material may,in fact,be new to you.Even if you covered these concepts last semester,some of them have a high vapor pressure and may have escaped between semesters. e darrows.We jog your memory with a dise g you tomotneoosancineshaSerohei0dcec eview the stru coniugated unsaturated systems.finall we remind you of spectroscopic techniques.from the R fingerprints to NMR shifts.The review in this part moves at a pretty fast pace,but we're sure you can keep up
In this part . . . Part I is a review of some general chemistry and Organic Chemistry I topics you need a firm grounding in before moving on to Organic Chemistry II. Different books and different instructors break Organic I and Organic II material at different places. We use the most common break, but some Part I material may, in fact, be new to you. Even if you covered these concepts last semester, some of them have a high vapor pressure and may have escaped between semesters. We begin by bringing you up to speed on mechanisms and reminding you how to push electrons around with those curved arrows. We jog your memory with a discussion of substitution and elimination reactions and their mechanisms, in addition to free radical reactions. Next you review the structure, nomenclature, synthesis, and reactions of alcohols and ethers, and then you get to tackle conjugated unsaturated systems. Finally, we remind you of spectroscopic techniques, from the IR fingerprints to NMR shifts. The review in this part moves at a pretty fast pace, but we’re sure you can keep up. 04_178157-pp01.indd 8 5/28/10 9:45 AM
Chapter 1 Organic Chemistry ll: Here We Go Again! In This Chapter Reviewing the material you learned in Organic I Previewing what you find out in Organic ll Il.or you're trying to figure out what Organic ll covers in time to chang major from pre-med to art history.In any respect.you probably successfully completed Organic Chemistry I.Many of the study techniques(and coping mechanisms)you learned that helped you do well in Organic I are helpful in Organic lI.The two primary things to remember are Never get behind. Carbon has four bonds. In this book ens book wa ose lars weshese to do this because firstly that's the sty,tha Sec you will b 0 emistr at af ou do take bioch For Du b are really great guys.) To get you started,this chapter does a quick review of the topics commonly found in Organic I,and then gives an overview of what we cover in Organic lI
Chapter 1 Organic Chemistry II: Here We Go Again! In This Chapter ▶ Reviewing the material you learned in Organic I ▶ Previewing what you find out in Organic II If you’re looking at this chapter, it’s probably because you’re getting ready to take the second half of organic chemistry, are in the midst of Organic II, or you’re trying to figure out what Organic II covers in time to change your major from pre-med to art history. In any respect, you probably successfully completed Organic Chemistry I. Many of the study techniques (and coping mechanisms) you learned that helped you do well in Organic I are helpful in Organic II. The two primary things to remember are ✓ Never get behind. ✓ Carbon has four bonds. In this book we use larger, more complex molecules than you may have encountered in Organic I. We chose to do this because, firstly, that’s the nature of Organic II — larger and more complex molecules. Secondly, many of you will be taking biochemistry at some point, and to succeed in that subject you need to become comfortable with large, involved molecules. (If you do take biochemistry, be sure to check out Biochemistry For Dummies by John T. Moore and Richard H. Langley [Wiley]. We understand the authors are really great guys.) To get you started, this chapter does a quick review of the topics commonly found in Organic I, and then gives an overview of what we cover in Organic II. 05_178157-ch01.indd 9 5/28/10 9:45 AM
10 Part I:Brushing Up on Important Organic Chemistry I Concepts Recapping Organic Chemistry In Organic I you learned that organic chemistry is the study of carbon compounds.Until the mid-1800s,people believed that all carbon compounds were the result of biological processes requiring a living organism.This was called the vital force theory.The synthesis (or formation)of urea from inorganic aterials showed that other paths to the production of carbon compounds are poss s of organic compo nds ause rm sta e process of one om on er.The w 10 amnk chain ounds Carbon is also capable of forming stable bonds to a number of other elements including the biochemically important elements hydrogen,nitrogen,oxygen, and sulfur.The latter three elements form the foundation of many of the functional groups you studied in Organic I. Intermolecular forces orce or eten hemieeere em mprtan r explaining the interaction between molecules.Intermolecular forces that you saw in Organic I and see again in Organic ll include dipole-dipole interac- tions,London,hydrogen bonding,and sometimes ionic interactions. Dipole-dipole forces exist between polar regions of different molecules.The presence of a dipole means that the molecule has a partially positive (+)end epposite partlal charges attract each other. Hydroge n bonding.as the n name implies,involves hydr rogen.This hydroger bonds to a fluorine atom.)H en bonding is significantly stro rer than normal dipole-dipole force and is due to the fluctuations of the electron clouds of atoms or molecules.The hydro en bonded to either a nitrogen or oxygen atom is strongly attracted to a different nitrogen or oxygen atom. Hydrogen bonding may be either intramolecular or intermolecular
10 Part I: Brushing Up on Important Organic Chemistry I Concepts Recapping Organic Chemistry I In Organic I you learned that organic chemistry is the study of carbon compounds. Until the mid-1800s, people believed that all carbon compounds were the result of biological processes requiring a living organism. This was called the vital force theory. The synthesis (or formation) of urea from inorganic materials showed that other paths to the production of carbon compounds are possible. Many millions of organic compounds exist because carbon atoms form stable bonds to other carbon atoms. The process of one type of atom bonding to identical atoms is catenation. Many elements can catenate, but carbon is the most effective, with apparently no limit to how many carbon atoms can link together. These linkages may be in chains, branched chains, or rings, providing a vast combination of compounds. Carbon is also capable of forming stable bonds to a number of other elements, including the biochemically important elements hydrogen, nitrogen, oxygen, and sulfur. The latter three elements form the foundation of many of the functional groups you studied in Organic I. Intermolecular forces You also learned about intermolecular forces in Organic I. Intermolecular forces (forces between chemical species) are extremely important in explaining the interaction between molecules. Intermolecular forces that you saw in Organic I and see again in Organic II include dipole-dipole interactions, London, hydrogen bonding, and sometimes ionic interactions. Dipole-dipole forces exist between polar regions of different molecules. The presence of a dipole means that the molecule has a partially positive (δ+) end and a partially negative (δ–) end. Opposite partial charges attract each other, whereas like partial charges repel. Hydrogen bonding, as the name implies, involves hydrogen. This hydrogen atom must be bonded to either an oxygen atom or a nitrogen atom. (In nonbiological situations, hydrogen bonding also occurs when a hydrogen atom bonds to a fluorine atom.) Hydrogen bonding is significantly stronger than a normal dipole-dipole force, and is stronger than London dispersion forces, the forces between nonpolar molecules due to the fluctuations of the electron clouds of atoms or molecules. The hydrogen bonded to either a nitrogen or oxygen atom is strongly attracted to a different nitrogen or oxygen atom. Hydrogen bonding may be either intramolecular or intermolecular. 05_178157-ch01.indd 10 5/28/10 9:45 AM