Organic Chemistry (Laboratory)

• Organic and Inorganic Compounds form one of the primary bases for chemistry
• Organic Chemistry


  Study of organic compounds
• Inorganic Chemistry


  Study of inorganic compounds
• Organic Compounds


  • Always have a carbon atom
  • Almost all contain the carbon-hydrogen or a simple C-H bond
  • Combustible compared with most inorganic compounds
  • Some have no sharp melting points
  • Decompose easily at moderately high temperatures
  • Few of them ionize because of the nature of bonds (covalent) that hold their atoms together in a molecule
  • Mostly non-electrolyte, with few weak electrolytes
  • Practically insoluble in water and other polar solvents
• Elements commonly present in organic compounds

  • Carbon
  • Hydrogen
  • Oxygen
  • Nitrogen
  • Sulfur
  • Halogens (Chlorine, Bromine, Fluorine)
• Important Groups of Organic Compounds Found in Living Things

  • Proteins
  • Carbohydrates (Sugar)
  • Lipids (Fat, Waxes)
  • Nucleic Acid (DNA, RNA)
• Inorganic Compounds


  • Most do not contain the carbon atom
  • More simple than organic compounds
• Exceptions of inorganic compounds containing carbon

  • Carbon dioxide
  • Carbides
  • Carbonates
  • Cyanides
• Qualitative Analysis


  • Analysis of the species present in a given compound
  • Helps scientists know the composition of the compound
  • Detection of various elements present in an organic compound
• Most organic compounds mainly result from activities of a living being
• Inorganic compounds are obtained from natural processes which are not related to any of the life forms on earth or any result of human experiments
• Ignition Test


  1. Combustion reaction occurs when a substance reacts with oxygen to release energy

  2. Methane burns in oxygen, releasing carbon dioxide and water

  3. Formation of carbon dioxide shows the carbon present in the methane has undergone oxidation
• Inorganic Compounds


  • Contain ionic bonds, atoms tightly held together in contrast to organic compounds
  • Do not allow organic compounds to react with oxygen
• Characteristics of combustion


  • Flammability
  • Charring
  • Flame test
  • Combustibility
  • Color (blue - non luminous, yellow - luminous)
• Solubility


  • Determined by temperature, polarity, pressure, molecular size, surface area of solute
  • Like dissolves like
• Miscible


  No layer
• Immiscible


  Has layer
• Diatomic Molecules


  • H2
  • O2
  • N2
  • F2
  • Cl2
  • Br2
  • I2
• Diatomic Molecules


  Share electrons equally, electrically neutral
• Polar Molecules


  Electrons are shared unequally
• Polar Molecules


  • HF
  • HBr
  • HCl
• Nonpolar Molecules


  Hydrocarbons - Nonpolar (Carbon Hydrogen Bonds)
• Nonpolar Hydrocarbons


  • Methane
  • Ethane
  • Ethene
  • Acetylene
• Tetrahedral Lewis Structure


  • SiBr4
  • CCl4
  • CF4
  • GeH4
• All elements in the same column as Phosphorus are nonpolar
• Linear Molecules


  • CO2
  • CS2
  • BeH2
  • BeCl2
  • BeF2
• Trigonal Molecules


  • BH3
  • AlCl3
  • AlBr3
  • AlF3
  • FeBr3
• Octahedral Molecules


  • SeF6
  • SBr6
  • SF6
  • SeCl6
  • SI6
  • SeI6
• Polar Geometry - Bent Shape


  • Water
  • H2S
  • SF2
  • SCl2
  • SeBr2
  • SO2
  • SeO2
• Polar Geometry - Trigonal Pyramidal

  • NH3
  • PH3
  • AsHl3
  • PBr3
  • PCl3
  • NF3
• Polar Geometry - T-shaped


  • IF3
  • ClF3
  • BrF3
  • ICl3
  • BrCl3
  • IF5
  • ClF5
  • BrF5
  • ICl5
  • BrCl5
• Polar Geometry - Seesaw Shape


  • SF4
  • SeCl4
  • SeBr4
  • SeI4
• Polar Molecules


  • CH3F
  • CSO
• Polar Molecules


  • BH2F
• Whenever the outer elements are different, it is safe to assume that it is polar (95%)
• Identical and No lone pairs - Nonpolar
• Identical and with Lone Pairs - polar (90%)
• Different side of lone pair (opposite side) - nonpolar
• Same side of lone pair (one side) - polar
• Electrical Conductivity


  • Easiest way to determine whether a compound can conduct a current is to identify its molecular structure or composition
  • Compounds with Strong Conductivity - dissociate completely into charged atoms or molecules, or ions, when dissolved in water
  • Can move and carry a current effectively
  • Higher concentration = greater conductivity
  • Electrolyte - strong and weak
  • Nonelectrolyte