CHM 303 1st EditionExam # 1 Study Guide Lectures: 1 - 10Lecture 1 (September 3)Review of how structure determines propertyLewis dot structure, Molecular Geometry, Calculating formal charges, Resonance Forms (2 or more ways to draw LS, but remember, MG does NOT change), polarity/electronegativityCarbon are able to have chains with tens of thousands of carbons because they do not have any lone pairs!: Two main forms; diamond and graphiteLecture 2 (September 5)Structure of Ionic and Covalent BondsIonic bonds: moving electrons to satisfy octetsCovalent bonds: sharing of electronsCalculating Formal Charges: # of elements valence electrons - 1/2 (electrons from covalent bonds) - # of lone pairs on element = formal charge of elementResonance forms: least electronegative usually in middle of configura-tionDipole moments: measure of compound polarityLecture 3 (September 8)Structure, Structural Formulas, and Curved ArrowsAdding protons increase electronegativity*dipole moment (μ)= amount charge (e) x distance between charges (d)*First two rows (s and p) do not allow for octet expandingTo draw structures1. Draw Carbon skeleton2. Add Hydrogen and other elements3. Write condensed formConstitutional Isomers: 2 or more different compounds from same for-mulaWhen moving electrons, use a single-barbed arrow to depict one elec-tron and a double-barbed arrow to depict moving two electrons.Lecture 4 (September 10)Know differences between Bronsted and Lewis acid/basesBronsted acids are proton donors (donate H+) and bases accept pro-tons (H+).Lewis acids are electron pair acceptors and bases are electron pair donorsClassification of hydrocarbonsAliphatic (greasy/oily): Alkanes (saturated in H), Alkenes and AlkynesAromatic (pleasant smell): ArenesLecture 5 (September 12)Knowing types of bonds, hybridization, and nomenclatureMethane: 109.5 degrees, SP3 tetrahedralEthane: sigma bond, SP3-SP3 Ethylene: trigonal planar, pi bond, SP2-SP2Acetylene: linear carbons, perpendicular SP orbitalsMethyl: -CH3Ethyl: -CH2CH3Propyl: -CH2CH2CH34 carbon chain: butane5 carbon chain: pentane6 carbon chain: hexane7 carbon chain: heptane8 carbon chain: octane 4 carbon ring: cyclobutane5 carbon ring:cyclopentane6 carbon ring: cyclohexaneLecture 6 (September 15)More branching of compounds leads to a lower boiling point, less induced dipole, and less intermolecular forces.Lecture 7 (September 17)Less negative H value means higher stability.Decrease in change of H = Decrease in stabilityMore branching (when comparing isomers) = More stabilityOxidation: adding bonds to oxygen and/or removing hydrogenReduction: removing bonds to oxygen and/or adding hydrogenEclipsed Conformation: when front and back are in alignment: Torsion angle: 0 degStaggered Conformation: when front and back are not alignedEclipsed and Staggered are the two extremesNewman Projections: a form of drawing depicting one bond right behind an-otherStaggered conformations are much more stable than EclipsedTorsion Angles: Eclipsed: 0 deg, Gouche: 60 deg, Anti: 180 deg (most stable)Lecture 8 (September 19)Chair conformations: Certain angle strains can cause instability, so a confor-mation will twist bonds in order to get other conformations that are more sta-ble (based upon torsion angles)Lecture 9 (September 22)axial and equatorial compounds: more equatorial means more stabilitytrans: compound groups on opposite sides (one is eq., one is ax.)cis: compound groups on same side (both are eq., both are ax.) stereoisomers: same bond sequence, different representations, not the samecompoundLecture 10 (September 24)Polycyclic Rings: Spiro compounds: 2 rings share a common carbonFused-ring compounds: side by sideBridged compounds: found a lot in