CHEM 301 1nd EditionExam # 1 Study Guide Lectures: 1 - 7Lecture 1 (August 21)Introduction to Organic ChemistryIonic bonds: When ions have separate charges and they attract each other. (Na+ and Cl-)Covalent bonding: Electrons are shared rather than transferred. Formal charges: provide a method for keeping track of electrons.-Formal charge = [group number] – [nonbonding electrons] – ½[shared electrons]Resonance structures: when two or more valence-bond structures are possible, differing only in the placement of electrons, molecule will show characteristic of both structures.Condensed structural formulas: written without showing all the individual bondsLine-angle formula: often used for cyclic compounds and bonds are represented by lines, and carbon atoms are assumed to be present wherever two lines meet or a line begins or ends. Isomers: same formula, different arrangement.-Constitutional: connected differently-Stereoisomers: same connectivity, different spatial order-Conformational: rotation around single bonds-Configurational: no rotationLecture 2 (August 26) Resonance Structures-The net charge must remain the same.-Double bond (pi) and lone pair electrons can be moved-Curved arrows show electron movement*The number of electrons CANNOT be different*Single bonds CANNOT be broken. Lecture 3 (August 28)A Bronsted-Lowry acid is any species that can donate a protonA Bronsted-Lowry base is any species that can accept a proton.Ka is called the acid-dissociation constant and its value indicates the relative strength of the acid.-A large Ka means the acid is a strong acid.-A small pKa means the acid is a strong acid.-A large pKa means the base is a strong base.Lewis bases are species with available electrons that can be donated to form new bonds.Lewis acids are species that can accept these electron pairs to form new bonds.Lecture 4 (September 2)The strength of an acid is inversely related to the strength of its conjugate base. For an acid to be strong, its conjugate base must be stable. If an acid is weak, its conjugate base is a strong base. A more electronegative element bears a negative charge more easily, giving a more stable conjugate base and a stronger acid. The negative charge of an anion is more stable if it is spread over a larger region of space.Resonance delocalization is often the dominant effect helping to stabilize an anion. Lecture 5 (September 4)Rules for Naming Alkanes1. Find the longest C chain; this is the parent (circle it) (ends in –ane)2. Groups outside the circle are substituents (ends in –yl)3. Number C of parent so subs get the lowest numbers.4. Alphabetize substituents in front of parents.Lecture 6 (September 9)Alcohols are organic compounds that contain the hydroxyl group (-OH)Ethers are composed of two alkyl groups bonded to an oxygen atom.The carbonyl group is the functional group for both aldehydes and ketons.A ketone has two alkyl groups bonded to the carbonyl group. An aldehyde has one alkyl group and a hydrogen atom bonded to the carbonyl group.Carboxylic acids contain the carboxyl group