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• Organic


  Deals with the chemistry of carbon
• There are over 16 million known organic molecules
• Organic Chemistry


  • Study of molecules with carbon atoms
  • The study of the structure, properties, composition, reactions, and preparation of carbon-containing compounds
  • Includes chemicals extracted from living things and man-made polymers like plastics
  • Carbon-centric

  
• Carbon


  • Makes 4 bonds
  • Catenates or bonds with itself
• Urea


  • Main nitrogen containing part of urine that comes from the body's metabolic breakdown of urine
  • Can be used as a fabric dye mordant which makes the dye lasts longer and enhances the color
  • In Ancient Rome, people sell their urine to earn money
• Friedrich Wohler


  • Isolated yttrium, beryllium, and titanium
  • Discovered organic matter on meteorites
  • Synthesized urea from ammonium cyanate, an inorganic salt
• Lewis Structure


  Illustrate what atoms are connected and show all bonds and lone pairs in the molecule

  
• Molecular Formula


  Tells the atoms and how many atom there is in the molecule
• Condensed Structural Formula


  Simplifies the molecule in which the hydrogens are grouped next to the hydrogens they are bonded to
• Skeletal or Line-angle formula


  Only shows the bonds and the atoms that are not carbon and their connected hydrogens

  
• Heteroatoms


  • Atoms in organic compounds other than carbons and hydrogens
  • Always show the hydrogens attached to them in the skeletal formula

  
• Functional groups


  Parts of the organic compound that are not carbon atoms or have double and triple bonds

  
• Retinal


  Molecule in our eyes responsible for turning light into nerve signals
• International Union of Pure and Applied Chemistry (IUPAC)


  The guiding organization for chemical nomenclature
• IUPAC Systematic Naming Steps

  1. Find the longest carbon chain and give it a root name

  2. Identify the highest priority functional group and add its suffix to the root name

  3. Identify the types of substituents and their positions on the carbon chain, then add a numbered prefix to the root name
• Hydrocarbons


  • Simplest organic molecules
  • Only have hydrogens and carbons
• Types of Hydrocarbons

  • Alkanes (-ane)
  • Alkenes
  • Alkynes
  • Aromatics
• Substituents

  The halogens (chlorine, bromine, iodine) and carbon chains that replace the hydrogens in the longest carbon chains
• Heteroatom


  • Generally increases the reactivity of organic compounds
  • Can make up functional groups
• R group


  Represents the rest of the chain that is not part of the functional group
• Alcohol (-ol)


  • Most useful and common compounds in nature
  • Ethanol - type of alcohol commonly found in alcoholic compounds
  • Methanol - simplest alcohol, commonly called as wood alcohol
• Ether

  • The common name "ether" refers to one of the first chemicals in medicine that was regularly used to anesthezise patients before surgery
  • Diethyl ether - Anesthesia ether
  • Trivial (common) naming of ether - Name the two carbons chains on both sides of the oxygen, add the suffix -yl, arrange alphabetically, add the word "ether" at the end
• Carbonyl groups

  • Aldehydes (-al)
  • Ketones (-one)
  • Carboxylic acids (-oic acid)
  • Carboxylic acid derivatives - Esters, Acid chlorides, Anhydrides, Amides
• Amine


  Nitrogen attached to the R groups with one lone pair
• Nitrile


  • Also known as cyano-groups
  • Triple bond between a nitrogen and a carbon, with potential chains attached to the carbon
• Phenyls


  • Benzene rings
  • 6 carbon ring with alternating single and double bonds
• Functional Groups of Highest to Lowest Priority

  • Carboxylic Acids
  • Aldehydes
  • Ketones
  • Alcohol
  • Alkenes / Alkynes
  • Alkanes
• Organic compounds


  Can be plotted on a 3D Cartesian Coordinate System with X, Y, and Z axes

  
• Lewis structures


  • Created in 1916
  • Helped think about how atoms and electrons are arranged in a molecule
• Valence Shell Electron Pair Repulsion Theory (VSEPR)


  • First proposed in 1957
  • Started to explain the observed 3D shapes of molecular structures
  • The theory that the 3D shape of a molecule is determined by a central atom's lone pairs of electrons and the other atoms it's bonded to

  
• 5 VSEPR electron pair geometry

  • Linear
  • Trigonal planar
  • Tetrahedral
  • Trigonal bipyramidal
  • Octahedral
• Molecular shapes


  • Describe how atoms in a molecule relate to each other and pretend that lone pairs are invisible
  • Bent molecular shape - Ex: water

  
• Orbital names and shapes

  • s orbital
  • p orbital
  • d orbital
  • f orbital

  
• Orbital hybridization


  • The idea that one can mix an s-orbital's spherical shape and p-orbital's 3D figure-eight shape to make two hybrid atomic orbitals that look like both
  • 1 s + 1 p = 2sp
  • 1 s + 2 p = 3sp²
  • 1 s + 3 p = 4sp³
  • Helps explain the 3D geometries predicted by VSEPR

  
• Methane

  Tetrahedral shape
• Sigma bonds


  • Chemical bonds that are made by the direct overlap of two orbitals that point at each other
  • Has orbitals that overlap end to end
• Valence Bond Theory


  Based on the idea of overlapping orbitals
• Ethene

  • Trigonal planar
  • All double bonded molecules have 1 sigma bond and 1 pi bond
• Ethyne


  • Linear
  • All triple bonded molecules have 1 sigma bond and 2 pi bonds
• Pi bond


  Bonds where the orbitals line up next to each other and sort of overlap sideways