P Org Topic 1

• Organic Chemistry 


  Study of carbon and Carbon-related compounds.
• "Organic Chemistry" Comes from the word ORGANISM.
• Friedrish Wohler


  A German chemist, that disproved "Vitalism Theory".
• In 1828, A German chemist disproved the "Vitalism Theory", called Wohler Synthesis. He was able to Isolate UREA from an inorg compound, AMMONIUM CYANATE.
• Organic Compounds

  • Do not dissolve on water
  • Dissolve in organic solvents like ether, alcohol, benzene, cloroform
  • Low melting point, decompose on heating
  • Inflammable
  • Covalent, non-electrolytes
• Inorganic Compounds

  • Dissolve in water
  • Do not dissolve in Organic solvents
  • High melting point and boiling point, does not decompose on heating
  • Non inflammable
  • Ionic, Electrolytes
• Ability to Catenate - Catenation


  Carbon atoms link together to form chains of varying lenght, branched chains, and rings of different sizes
• Uniqueness of Carbon

  It is able to form 4 covalent bonds (Tetravalent), with other carbon or other elements.
• Atomic Structure 


  Erwin Schrödinger
• Elements - Fundamental building blocks of all substances

  • Atoms: Smallest particle of an element
  • Neutron: Neutral subatomic particle
  • Proton: Positively Charged subatomic particle (+1 charge)
  • Electron: Negatively Charged subatomic particle (-1 charge, weightless)
  • Nucleus: Center of an atom; contains proton and neutrons
• Isotopes - Atoms that have the same number of protons but differing numbers of neutrons and different mass number.
• Mass Number


  Number if proton plus neutrons
• Atomic Number 


  Number of Protons in Nucleus
• Carbon-12

  • Stable
  • Most Dominant
  • 98.9%
  • 6 Protons
  • 6 Neutrons
• Carbon-13

  • stable
  • 1.1%
  • 6 Protons
  • 7 Neutrons
• Carbon-14

  • <0.1%
  • Unstable
  • Radioactive
  • 6 Protons
  • 8 neutrons
• Atomic Structure Orbitals

  • Region if space where is a Certain probability of finding an electron
  • Can hold 2 electrons
  • also known as WAVE FUNCTION
• S - Spherical

  P - Dumbbell

  d - Cloverleaf

  f Complex
• Distribution of Orbitals within shells

  • Each shell contains subshells known as ATOMIC ORBITALS
  • Electrons are said to Occupy orbitals in an atom
• (Subshells -

  S, P, D, F)

  (No. of orbital of equal energy -

  1, 3, 5 , 7)

  (Maximum number of electrons -

  2, 6, 10, 14)
• Aufbau Principle


  "Build Up"

  States that electrons fill lower energy atomic orbitals before filling higher energy ones.
• Pauli's Exclusion Principle


  Maximum of 2 electron per orbital with opposite spin.
• Hund's Rule


  Fill the orbitals singly before they pair up. (One at a time)
• Principal QN - To determine the size of the particle

  Symbol - n

  Values- 1, 2, 3
• Azimuthal or Angular -Subshell or sublevel, determines the shape

  Symbol - l

  Values - 0 to (n-1)
• Magnetic - Orbitals, determine orientation

  Symbol - m or mL

  Values – -1 to +1
• Spin - Direction of spin or orientation

  Symbol - S or ms

  values — -1/2 to +1/2
• Electron Configuration 


  Symbolic notation of the manner which electron of its atom are distributed over different atomic orbitals

  It is where the electrons are around a nucleus
• Chemical Bonding 


  Joining of two atoms in a stable arrangement
• Octet rule


  (Tendency Among Atoms)

  Atoms react in a way that achieve valence of eight valence electrons.
• Ionic bond


  (Transfer of electron) N + NM

  Bond between anion and cation

  May lose or gain enough electron to acquire a completely filled valencr shell
• Covalent bond


  Sharing of electron

  NM+NM/NM+METALLOID
• Lewis Structure


  Electron Dot Structure

  Valence shell electrons of an atom are represented as dot
• Kekule Structure


  Line Bond Structure

  Each shared electron is represented by line between the atom symbols
• Lone pair electrons or non-bonding electrons


  Pair of valence electrons that are used for bonding
• Multiple bond


  When 2 atoms share more than 1 pair electrons
• Electronegativity


  Measure of the ability of an atom to attract
• Solid Line


  Represents bond in the plane of page
• Heavy weighed Line


  Bonds coming out of the page, toward the viewer
• Dashed Line


  Bonds preceding back behind page, away from the viewer