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Chapter 1 Organic Chemistry

Chemistry 20. Chapter 1 Organic Chemistry. Organic Compounds. H: 0.9% Ti: 0.6% Others: 0.9%. Organic Compounds. Chemistry of Carbon (H, O, N, S, Halogens, and P). C one of the 116 elements. Organic Compounds. Isolation from nature (animal and plant). (extract-isolate-purify).

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Chapter 1 Organic Chemistry

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  1. Chemistry 20 Chapter 1 Organic Chemistry

  2. Organic Compounds

  3. H: 0.9% Ti: 0.6% Others: 0.9% Organic Compounds Chemistry of Carbon (H, O, N, S, Halogens, and P). C one of the 116 elements

  4. Organic Compounds Isolation from nature (animal and plant) (extract-isolate-purify) Obtained by: Synthesis in lab Organic compounds: 10 million Inorganic compound: 1.7 million Compounds in living systems are organic: Biochemistry

  5. Organic Compounds First organic compound that is synthesized in lab. Wöhler (1828)

  6. Organic Compounds • Typical organic compounds: • Contain carbon • Have covalent bonds • Have low melting points • Have low boiling points • Are flammable (all burn) • Are soluble in nonpolar solvents • May be gases, liquids or solids C3H8 Propane

  7. Organic Compounds

  8. Structural Formula (Lewis Structure) • shows the atoms present in a molecule as well as • the bonds that connect them.

  9. VSEPR Model VSEPR: Valence-Shell Electron-Pair Repulsion method Bond angle: angle between two atoms bonded to a central atom. Each region of electron likes to be as far away as possible from the others.

  10. Regions of electron density Four regions of electron density around an atom:

  11. Bond Angles & Geometric Structures Linear molecules 2 regions Trigonal planar molecules 3 regions Tetrahedral arrangement 4 regions

  12. Tetrahedral Electron Pair Geometry (Tetrahedral arrangement)

  13. Tetrahedral Electron Pair Geometry Unshared electron paires CH4 NH3 H2O

  14. Carbon:normally forms four covalent bonds and has no unshared pairs of electrons. • Hydrogen: forms one covalent bond and no unshared pairs of electrons. • Nitrogen: normally forms three covalent bonds and has one unshared pair of electrons. • Oxygen: normally forms two covalent bonds and has two unshared pairs of electrons. • A Halogen: normally forms one covalent bond and has three unshared pairs of electrons. C H N . . . . . O = . . . . . Cl . .

  15. Functional groups • An atom or group of atoms within a molecule that shows a characteristic set of predictable physical and chemical properties. • A way to classify organic compounds into families. • They determine the chemical and physical properties of a compound. • They undergo the same types of chemical reactions. • A way to name organic compounds.

  16. Functional groups

  17. Alkanes, Alkenes, and Alkynes • Alkanes:contain single bonds between carbon atoms. • Alkenes:contain one or more double bonds. • Alkynes:contain one or more triple bonds. C C C C C C

  18. Alcohols and Ethers O H • Alcohols: contain the hydroxyl (-OH) functional group. • Ethers: an oxygen atom is bonded to two carbon atoms. C O C C C O C C

  19. Aldehydes and Ketones • Aldehydes: contain a carbonyl group (C=O), which is a carbon atom with a double bond to an oxygen atom. • Ketones:the carbon of the carbonyl group is attached to two other carbon atoms. O C C H O C C C

  20. Carboxylic acids and Esters • Carboxylic acids:contain the carboxyl group (-COOH), which is a carbonyl group attached to a hydroxyl group. • Esters: the hydroxyl group of a carboxylic acid is replaced by a carbon • atom. O C H O O C C O C

  21. NR Amines and Amides • Amines: the functional group is a nitrogen atom. • | • — N — • Amides: the hydroxyl group of a carboxylic acid is replaced by a nitrogen group. N N C C C O C N

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