Organic chemistry 1

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Organic chemistry 1

• Lecturer
• Dr Taghreed M.M.Z

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Organic chemistry

• References which may be helpful
• T.W. Graham Solomons Organic Chemistry Sixth
  Ed., 1996, John Wiley, New York.
• L.G.Wade, JR. "Organic chemistry" third ed.,1995,
  Prentice Hall international, Inc., USA
• Robert. V. Hoffman Organic Chemistry An
  intermediate Text Second Ed., , Wiley
  enterscience, New Jersey.
• Edward E.Burgoyne "A short course in organic
  chemistry"
• Howard, N. "Schaum 's outline of theory and
  problems of organic chemistry" third
  edition,1999, McGraw-Hill, New York.
• R.T.Morrison and R.N.Boyd "organic chemistry"
  fifth ed., 1987,Allyn and Bacon, Inc.,Boston.

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Course objectives

• Have an idea about structural theory of organic
  compound.
• Know main functional groups of organic compounds
• Know main physical and chemical characteristics
  of different functional groups.
• Have an idea about different reaction mechanisms
  involved in organic reactions.
• Get experimental experience in dealing and
  identifying organic compounds.
• Know some important applications of organic
  chemistry in our daily life.

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Course overview

• Structure and chemical bonds
• Important organic compounds will be studied
  (physical and chemical characteristics, methods
  of preparation) such as the following
• Alkanes and Alkyl halides
• Alkenes and Alkynes
• Alcohols and ethers
• Carbonyl compounds
• Aldehydes and ketones
• Carboxylic acids an their derivatives

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Exams and activities

• Mid-term exam 20 points
• Attendance and activities 10 points
• Lab 30 points
  
• Final exam 90 points

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Carbon compounds and chemical bonds

• Definition Organic chemistry is the chemistry of
  compounds containing carbon and hydrogen.
• What is so special about carbon?
• Applications of organic chemistry
• ? Medicine ? Petroleum industry
  Environmental issues
• ? Textile industry ? Human metabolism Plastics
  and polymer
• ? Petrochemicals ? Genetic science.

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Main characteristics of organic compounds

• ? Organic compounds are flammable and can easily
  be decomposed to gases in case they do not
  contain metals in their structure.
• ? In general chemical reactions of organic
  compounds are slow.
• ? Some organic compounds contain high amount of
  halogens e.g. (X F, CL, Br, I,).
• ? Organic compounds have a high content of
  halogens tend to be less flammable

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The Structural Theory of Organic Compounds

• Principal quantum number, (n) n1,2,3
• Angular momentum number (m)0 to (n-1)
• Magnetic quantum number (?) (- ? to ?)
• Spin quantum number(-1/2 to ½)

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The Structural Theory of Organic Compounds

• Orbital (atomic)- An orbital is a three
  dimensional region around the nucleus where there
  is a high probability of finding an electron.
• n1 1s

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The Structural Theory of Organic Compounds

• n2 2s 2p

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Important rules for electronic configuration

• Orbitals are filled in the order of increasing
  energy.
• Each orbital can only be occupied by a maximum of
  two electrons and must have different spin
  quantum numbers (Opposite spin) .
• The most stable arrangement of electrons in
  orbitals is the one that has the greatest number
  of equal spin quantum number (Parallel spins).

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The order of which orbitals are filled
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Electron configuration

• Definition of atomic number-Z of an element is
  the number of protons within the nucleus of an
  atom if that element in a neutral atom, the
  number of protons and electrons are equal and the
  atomic number number of electrons.

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Electron configuration

• Example Write the electron configuration of
  period 2 of periodic Table
• Atom Li Be B C N O F Ne
• Atomic number 3 4 5 6 7 8 9 10

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Types of chemical bonds

• The ionic "electrovalent" bond, formed by the
  transfer of one or more electrons from one atom
  to another to create ions.
• The covalent bond, a bond that results from
  sharing of electrons.
• "The central idea in their work (ionic, covalent
  bond) on bonding is that atoms without the
  electronic configuration of a noble gas generally
  react to produce such a configuration"

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Ionic bond "electrovalent bond"

• Electronegativity- is a measure of the ability
  of an element to accept electrons.
• Li Be B C N O F (period 2)
• Increasing electronegativity
• F Cl Br I (group)
• Decreasing electronegativity

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Ionic bond "electrovalent bond"
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Ionic bond "electrovalent bond"
Helium configuration
Neon Configuration
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Ionic bond "electrovalent bond"

• Ionic bonds form between metals and nonmetals.
• Ionic compounds tend to be crystalline solids
• High melting points may reach 1000?C
• Soluble in water their solution conduct
  electricity because the ion can carry the current
  through the solution .

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Covalent Bonds

• Covalent bonding occurs because the atoms in the
  compound have a similar tendency for electrons
  (generally to gain electrons). This most commonly
  occurs when two nonmetal bond together. Because
  both of the nonmetals will want to gain electrons
  the elements involved will share electrons in an
  effort to fill their valence shell.

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Covalent Bonds