Organic Chemistry: Introduction PDF
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This document provides an introductory overview of organic chemistry. It defines organic chemistry, differentiating it from inorganic chemistry, and explores key concepts like functional groups and different types of hydrocarbons. The document also covers important topics such as hybridization, geometry, and expressing formulas.
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ORGANIC CHEMISTRY: Introduction ORGANIC CHEMISTRY (OLD) Deals with matter that is obtained ONLY from living organisms Based on the VITAL FORCE THEORY Disproved by FRIEDRICH WOHLER Able to synthesize UREA from inorganic compounds (NEW) Deals with CARBON a...
ORGANIC CHEMISTRY: Introduction ORGANIC CHEMISTRY (OLD) Deals with matter that is obtained ONLY from living organisms Based on the VITAL FORCE THEORY Disproved by FRIEDRICH WOHLER Able to synthesize UREA from inorganic compounds (NEW) Deals with CARBON and its derivatives (NEW) Study of HYDROCARBONS WHAT’S THE DIFFERENCE? ORGANIC INORGANIC Source Primarily LIVING Primarily NON-LIVING CONTAINS CARBON ALL ELEMENTS (w/ or Constituent (also H, O, N, S, P, X) w/out carbon) Bond COVALENT IONIC Polarity NONPOLAR/POLAR ELECTRONEGATIVITY Ability to ATTRACT electrons IONIC = WEAKER bond by two atoms of extremely different EN; they are transferring electrons COVALENT = STRONGER bond by two atoms of same/similar EN; they are sharing electrons How to determine if COVALENT or IONIC? EN < 0.4 = COVALENT, NONPOLAR EN is 0.4 – 1.8 = COVALENT, POLAR EN ≥ 1.8 = IONIC COVALENT vs IONIC? C – C → 2.55 – 2.55 → 0 (NON-POLAR, COVALENT) O – H → 3.5 – 2.2 → 1.3 (POLAR, COVALENT) Na – Cl → 3.16 – 0.93 → 2.23 (IONIC) PROPERTIES OF CARBON 1) STABILITY C = Group IVA = 4 valence e- C = 1s2 2s2 2p2 = 4 valence e- OCTET RULE = for atom stability = 8 valence e- C needs 4 valence e- → 4 bonds → TETRAVALENT 2) CATENATION (form bonds with itself; also Si) 3) HYBRIDIZATION (atomic orbitals fuse → new, hybridized orbitals) 4) ISOMERISM HYBRIDIZATION Atomic orbitals FUSE to form new, hybridized orbitals ______ bond = _______ bond; essential for ___________ ____ bond = _______ & ________ bond HYBRIDIZATION 4 = sp3 Lone Pair + Sigma Bond 3 = sp2 2 = sp GEOMETRY VSEPR Rule (Valence Shell Electron Pair Repulsion) e- pairs located in bonds repel to affect the geometry of the bonds in a molecule Steric # = lone pair + sigma bond GEOMETRY GEOMETRY Steric # = lone pair + sigma bond EXPRESSING FORMULAS KEKULE/EXPANDED (atoms + bonds) CONDENSED (atoms) SKELETAL (bonds) EXPRESSING FORMULAS KEKULE/EXPANDED (atoms + bonds) CONDENSED (atoms ONLY) SKELETAL (bonds ONLY) BASIC TERMINOLOGY OUTLINE/SKELETON = LINEAR vs BRANCHED vs CYCLIC BASIC TERMINOLOGY IF CYCLIC: Number of ring members Number of rings = monocyclic, bicyclic, tricyclic, etc. Composition of rings = carbocyclic vs heterocyclic BASIC TERMINOLOGY SATURATION = SATURATED vs UNSATURATED If UNSATURATED: CUMULATED = adjacent CONJUGATED = distance of between one single bond ISOLATED = distance of AT LEAST 2 single bond FUNCTIONAL GROUPS Set of atoms that divides organic compounds into different “types/classes” Called FUNCTIONAL because it literally affects the properties/reactivity of the compound in general 2 TYPES: HYDROCARBON = ONLY C-H bonds HYDROCARBON DERIVATIVES = primarily C-H, but with other types of atoms HYDROCARBONS ALKANES ALKENES ALKYNES ARENES AKA paraffins AKA olefins AKA acetylene AKA aromatics Follows Huckel’s CnH2n+2 CnH2n CnH2n-2 rule SATURATED UNSATURATED 𝐶5 𝐻12 𝐶4 𝐻8 𝐶10 𝐻20 𝐶4 𝐻6 𝐶6 𝐻10 HYDROCARBON DERIVATIVES OXYGEN Alcohol Ether Aldehyde Ketone Carboxylic Acid Ester Anhydride HYDROCARBON DERIVATIVES NITROGEN Amine Amide SULFUR Thiol Thioether Thioester HYDROCARBON DERIVATIVES HALOGEN Alkyl Halide Aryl Halide Acyl Halide
