CHEM 333 1stEditionLecture 4Outline of Last Lecture II. Combining resonance and hybridizationIII. Trends in hybridizationa. Strength b. LengthIV. Bond angles and bond polarity Outline of Current Lecture V. Writing compoundsa. Dash formulab. Condensed formulac. (bond) line angle formula VI. Hydrocarbons (start of chapter 2)a. Alkanesb. Alkenesc. Alkynesd. AromaticVII. Functional groupsa. Alkyl halidesb. Alcoholsc. Ethersd. Aminese. Aldehydes and ketonesf. Carboxylic acidsg. Estersh. Amidesi. NitritesVIII. Physical propertiesIX. Intermolecular forcesCurrent LectureI. Writing compoundsa. Dash formulab. Condensed formula c. Line angle formulai. Everywhere a line ends or there is a bend is a Cii. Assume there is the number of hydrogen’s to fill the octet of Ciii. Hydrogen’s on all other atoms are drawniv.II. Hydrocarbons (Chapter 2)a. Only contain C or Hb. Alkanesi. Saturated hydrocarbonsii. Every Carbon has the max number of Hydrogensiii. Only single bondsiv. Suffix “-ane”v. Ex.) methane, propane, and pentanec. Alkenesi. Unsaturated hydrocarbonsii. Less than the max number of hydrogensiii. Have 1 or more double bondsiv. Suffix “-ene”v. Ex.) d. Alkynesi. Unsaturated with 1 or more triple bondsii. Suffix “-yne”iii.e. Aromatic i. Special ringii. Double bonds alternating around a ringIII. Functional groupsa. Carbon plus other atomsb. Used for naming/classifying sites of reactivityc. Alkyl halidesi. Alkane with a halide (I, Br, Cl, F) in place of a Hydrogenii. Ex.) H_3_C – Cliii. Can be classified into primary, secondary, and tertiary 1. Primarya. Halide is bonded to one carbon that is bonded to one other carbon2. Secondary a. Halide is bonded to one carbon that is bonded to two other carbons3. Tertiarya. Halide is bonded to one carbon that is bonded to three other carbonsiv.d. Alcoholsi. Hydroxyl group is bound to an sp^3 hybridized carbonii. Ex.) methanol, ethanol iii. Subclasses1. Primarya. Hydroxyl group is bounded to carbon which is bonded to one other carbon2. Secondarya. Hydroxyl group is bounded to carbon which is bonded to two other carbons3. Tertiarya. Hydroxyl group is bounded to carbon which is bonded to three other carbons4.e. Ethersi. Oxygen bound to two carbons1. Both sides do not have to be symmetrical2. R-O-Rf. Aminesi. Amino group ii. Nitrogen bonded to a primary, secondary, tertiary carbons by a single bondiii. Sub class1. Simplest amine is ammoniaa. Breaks the rule because there is no carbon2. Primarya. Nitrogen is bonded to 1 carbon and 2 hydrogen3. Secondarya. Nitrogen is bonded to 2 carbons and 1 hydrogen4. Tertiarya. Nitrogen is bonded to 3 carbons and 0 hydrogen5.g. Aldehydes and Ketonesi. Carbonyl group – Carbon double bonded to Oxygenii. Aldehydes1. Carbonyl group bonded to one hydrogen and one carbon2. Exception – formaldehyde3. CH_3_CHOa. CHO is a give away for aldehydesiii. Ketones1. Carbonyl group bonded to two carbons2. Do not have to be symmetric 3. Ex.) acetoneiv.h. Carboxylic Acidsi. Contains carbonyl group bonded to an OH and a Carbonii. Ex.) acetic acidiii.i. Estersi. Derivative of carboxylic acidii. Replaces the H with a carboniii.j. Amidesi. Derivative of carboxylic acidii. Replace OH with an amineiii.k. Nitritesi. Nitrogen triply bonded to a carbonIV. Physical propertiesa. Solid, liquid, and gas statesb. Melting point and boiling pointc. Physical properties are dictated by intermolecular forcesV. Intermolecular forcesa. Ion-Ioni. Strong electrostatic forces between positive and negative chargesii. Solid states require high energy to break bonds1. Causes high melting and boiling pointsb. Vander Waals Forcesi. Forces between molecules (interactions)ii. Dipole- Dipole1. Some molecules are polar (have a permanent dipole)2. They orient so + of one molecule aligns with – of another3. Causes strong interactions with each other4. Increases melting and boiling pointc. Hydrogen bondsi. Strong interactions between heteroatom with Hydrogen and heteroatom with one lone pair (O,N,F)ii. Weaker than covalent bonds, but stronger than dipole-dipole iii. When more hydrogen bonds are bonded together they become much stronger which explains the increase in boiling points in compounds such as H_2_O** all images were found on google