midterms orgchem

• ORGANIC CHEMISTRY


  - Study of chemistry of compounds of carbon

  - Study of compounds containing carbon that is

  chemically bonded to hydrogen

  - Synthesis, identification, modeling, and chemical

  reactions of such compounds
• CARL WILHELM SCHEELE (1769)


  [person] Organic compounds were isolated from nature in the pure state
• ANTOINE LAVOISIER (1784)


  [person] Analytical methods were developed for determination of elemental composition
• JONS JAKOB BERZELIUS (1807)


  - Among the first to differentiate inorganic from organic

  compounds

  - Believed organic chemicals found in nature contained

  a special "vital force" that directed their natural

  synthesis

  - Impossible to accomplish a laboratory synthesis of

  the chemicals
• FRIEDRICH WOHLER (1828)


  - Father of Organic Chemistry

  - Discovered urea could be synthesized in the

  laboratory by heating ammonium cyanate
• FRIEDRICH AUGUST KEKULE &

  ARCHIBALD SCOTT COOPER (1858)


  - Understanding about the structures of organic

  chemistry began with a theory of bonding called

  valence theory

  - Carbon is tetravalent
• JACOBUS VAN'T HOFF & JOSEPH LE BEL (1874)

  [person]

  - 4 bonds of carbon are not oriented randomly but have

  specific spatial directions

  - 4 atoms to which carbon is bonded sit at the corners

  of a regular tetrahedron, with carbon in the center
• ALEXANDER OPARIN (1923)


  - In theory, organic chemistry may have its beginning

  with the big bang

  - Components of ammonia, nitrogen, carbon dioxide,

  and methane combined to form amino acids
• STANLEY MILLER (1950)


  Performed an experiment in the laboratory that

  verified Oparin's
• C, H

  C, H, O

  C, H, O, N

  C, H, O, N, S

  C, H, O, N, S, P

  COMPOSITION OF ORGANIC COMPOUNDS:

  hydrocarbons: _, _

  carbohydrates and lipids: _ , _ , _

  amino acids and proteins: _, _, _, _

  more amino acids and protein: _, _, _, _, _

  nucleic acids RNA DNA: _, _, _, _, _, _
• CARBON


  - Normally forms 4 covalent bonds

  - No unshared pair of electrons
• NITROGEN


  - Normally forms 3 covalent bonds

  - No unshared pair of electrons
• OXYGEN


  - Normally forms 2 covalent bonds

  - Has 2 pairs of unshared electrons
• HYDROGEN


  - Forms 1 covalent bond

  - No unshared pair of electrons
• HALOGEN (GROUP 7A)


  - Normally forms 1 covalent bond

  - Has 2 unpaired electrons
• expanded structural formula


  a structural formula that shows all atoms in a molecule and all bonds connecting the atoms

  
• condensed structural formula


  a structural formula that uses groupings of atoms, in which central atoms and the atoms connected to them are written as a group, to convey molecular structural information

  
• skeletal structure formula


  a structural formula shows the arrangement and bonding of carbon atoms present but does not show the hydrogen atoms attached to the carbon atoms
• line-angle structural formula


  a structural representation in which a line represents a carbon-carbon bond and a carbon atom is understood to be present at every point where two lines meet and at the ends of lines

  
• INORGANIC COMPOUNDS


  type of bond: Most have ionic bonds

  states: Solids with high MP

  solubility in water: Many are soluble

  solubility in organic solvents: Almost all are insoluble
• ORGANIC COMPOUNDS


  type of bond: Almost entirely covalent

  states: May be gases, solids, or liquids with low MP

  solubility in water: Most are insoluble

  solubility in organic solvents: Most are soluble
• INORGANIC COMPOUNDS


  electrical conduction: Aqueous solutions conduct electricity

  reactions: Often very fast

  ability to burn: Very few burn

  acidity: Strong acids

  alkalinity: Strong bases
• ORGANIC COMPOUNDS


  electrical conduction: Do not conduct electricity

  reactions: Usually slow

  ability to burn: Almost all burn

  acidity: Weak acids

  alkalinity: Weak bases
• Catenation

  - Ability to bond to itself

  - Due to number and strength of carbon bonds

  - Leads to formation of multitude of chemically

  and thermally stable chains, ring, and branched compounds
• Heteroatoms

  - are atoms other than C or H

  - Includes O,N, S, P and halogens
• FUNCTIONAL GROUPS


  - Specific combination of bonded atoms that reacts in a

  characteristic way

  - Has own pattern of reactivity

  - Where reaction of organic compounds takes place
• FUNCTIONAL GROUPS


  - Characterize major families of organic compounds

  - Sites of predictable behaviors and determine physical

  properties of compound
• alcohol


  functional group:

  -OH

  e.g.: ethanol
• amine


  functional group:

  -NH2

  e.g.: ethanamine
• aldehyde


  functional group:

  -CHO

  e.g.: ethanal
• ketone


  functional group:

  -CO-

  e.g.: acetone
• carboxylic acid


  functional group:

  -COOH

  e.g.: acetic acid
• ester


  functional group:

  -COOR

  e.g.: ethyl acetate
• functional groups


  The chemistry of every organic molecule, regardless of size and complexity, is determined by the ___ it contains
• oxygen, hydrogen


  REDOX REACTION:

  - When oxidized, carbon often form additional bonds to

  ___

  - When reduced, carbon often form additional bonds to

  ___
• ADDITION REACTION


  - Unsaturated reactant becomes a saturated product

  - A pi bond breaks, and 2 C atoms (or 1 C and 1 O) are

  bonded to more atoms in the product
• HYDROGENERATION


  - Hydrogen is added to alkene to produce alkane

  - Hydrogen is added to alkyne to produce alkene

  or alkane

  - Usually with transitional metal catalyst
• HYDRATION REACTION


  Water is added to alkene in the presence of heat

  and a strong acid acting as a catalyst
• Markovnikov's Rule


  H+ from water will add to the carbon that

  originally had more H+
• ELIMINATION REACTION

  - Saturated reactant becomes an unsaturated product

  - A pi bond forms, with the 2 C atoms bonded to fewer

  atoms in the product