Organic Chemistry CHE111 Fall 2023-2024 PDF

Field of Basic Sciences Organic Chemistry CH E1 1 1 3 Credit hours: lecture (2 Cr. Hr) + laboratory (1 Cr. Hr) Nanoscience and Technology Molecular Biotechnology Petroleum...

Field of Basic Sciences Organic Chemistry CH E1 1 1 3 Credit hours: lecture (2 Cr. Hr) + laboratory (1 Cr. Hr) Nanoscience and Technology Molecular Biotechnology Petroleum Mining and Geology Lecture one: Introduction Dr Ahmed Swilem [email protected] Fall 2023-2024  Course Grading Grade Distribution Assessment Measures Weight Attendance 20 % Course activities (Quizzes, Assignments, Presentations, etc.) Lab 30 % Midterm Exam 10 % Final Exam 40 % Total 100 % Note: To pass a course: - Student must earn 60 % as a whole grade. - Student must earn at least 30% of its final exam mark (i.e. 12/40).  Grading System Marks % Collected Grade Points More than 97% A+ 4 93% to less than 97% A 4 89% to less than 93% A- 3.7 84% to less than 89% B+ 3.3 80% to less than 84% B 3.0 76% to less than 80% B- 2.7 73% to less than 76% C+ 2.3 70% to less than 73% C 2.0 67% to less than 70% C- 1.7 64% to less than 67% D+ 1.3 60% to less than 64% D 1.0 Less than 60% F 0.0  Course Content □ Introduction □ Formula weights, Avogadro’s number, empirical formulas from analyses □ Bonding and molecular structure □ Acids and bases □ Alkanes □ Alkenes and alkynes □ Stereoisomerism □ Alkyl halides □ Alcohols, ethers, aldehydes and ketones □ Carboxylic acids □ Aromatic compounds □ Polymers  Learning Resources Organic Chemistry, 11th Edition, By Francis Carey and Robert Giuliano and Neil Allison and Susan Bane. McGraw Hill Higher Education, 2020. ISBN10: 1260148920, ISBN13: 9781260148923. Introduction to organic chemistry, Fourth Edition by William Brown and Thomas Poon, John Wiley and Sons 2011. ISBN 978-0-470-38467-1 Organic Chemistry, 9th Edition by T. W. Graham Solomons and Craig B. Fryhle, John Wiley and Sons, 2008. ISBN 978-0-471-68496-1 Introduction What is Organic Chemistry? ▪ Literally, the term “organic” means “derived from living organisms”. ▪ Organic chemistry was originally the study of compounds extracted from living organisms and their natural products. ▪ It was believed that only living organisms possessed the “vital force” necessary to create organic compounds (vitalism). ▪ This concept started to change in 1828 after Friedrich Wöhler showed that it was possible to make urea (a constituent of urine) by evaporating an aqueous solution of the inorganic compound ammonium cyanate:  What is Organic Chemistry? ▪ The modern definition of organic chemistry is the chemistry of compounds containing carbon. ▪ Carbon Compounds are everywhere around us in food, flavors, fragrances, medicines, cosmetics, plastics, fibers, paints, adhesives and of course in our bodies (DNA and proteins). 11-cis-retinal Absorbs light and allows vision  Why Carbon? 1. Carbon can form strong covalent bonds to other carbon atoms and other elements as: hydrogen, nitrogen and oxygen. 2. Carbon can form chains and rings.  Principles of atomic structure Pure substances are either Elements or Compounds.  Principles of atomic structure ATOM ▪ It is the smallest unit of ordinary matter that forms a chemical element. ▪ An atom consists of a dense, positively charged nucleus containing protons and neutrons and a surrounding cloud of electrons. ▪ Each proton of the nucleus bears one positive charge; electrons bear one negative charge. Neutrons are electrically neutral; they bear no charge. ▪ Protons and neutrons have nearly equal masses (approximately 1 atomic mass unit each) and are about 1800 times as heavy as electrons. Most atom mass comes from the mass of the nucleus; (electrons atomic mass is negligible).  Principles of atomic structure Electronic Structure of Atom ▪ Electrostatic forces keep the electrons moving around the nucleus. These are the forces that pull negatively-charged and positively-charged particles towards each other. ▪ In nature, most atoms are stable. A stable atom has the same number of electrons as protons.  Principles of atomic structure ▪ Each element is distinguished by 2 numbers. ▪ The Atomic Number (Z) a number equal to the number of protons in its nucleus. Because an atom is electrically neutral, the atomic number also equals the number of electrons surrounding the nucleus. ▪ The Mass Number (A) is the total number of protons and neutrons in an atom.  Principles of atomic structure Volume of the atom ▪ Most of the volume of an atom comes from the electrons. ▪ The volume of an atom occupied by the electrons “electron cloud” is about 10,000 times larger than that of the nucleus. ▪ Electron Cloud contributes very little to the mass of the atom, but make up most of the volume of the atom.  Principles of atomic structure Isotopes They are two or more types of atoms that have the same atomic number and position in the periodic table, and that differ in mass numbers due to different numbers of neutrons in their nuclei. Isotopes of Hydrogen  GROUP 1 18 1 Alkali Metals Non-metals 78 Atomic Number 2 H He 1 PERIO Pt Alkaline Earth Metals Halogens Symbol D Hydrogen 1.008 2 Transition Metals Noble Gases 13 14 15 16 17 Helium 4.003 3 4 5 6 7 8 9 10 Platinum Name Li Be B C N O F Ne Other Metals Lanthanides 195.1 Average Atomic Mass 2 Metalloids Actinides Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon 6.94 9.012 10.81 12.01 14.01 16.00 19.00 20.18 11 12 13 14 15 16 17 18 3 Na Mg Al Si P S Cl Ar Sodium 22.99 Magnesium 24.31 3 4 5 6 7 8 9 10 11 12 Aluminium 26.98 Silicon 28.09 Phosphorus 30.97 Sulfur 32.06 Chlorine 35.45 Argon 39.95 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 4 K Potassium Ca Calcium Sc Scandium Ti Titanium V Vanadium Cr Mn Fe Chromium Manganese Iron CoCobalt Ni Nickel Cu Zn Ga Ge As Copper Zinc Gallium Germanium Arsenic Se Selenium Br Bromine Kr Krypton 39.10 40.08 44.96 47.88 50.94 52.00 54.94 55.85 58.93 58.69 63.55 65.39 69.72 72.64 74.92 78.96 79.90 83.79 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 5 Rb Sr Rubidium Strontium Y Yttrium Zr Nb Mo Zirconium Niobium Molybdenum Tc Technetium Ru Rh Pd Ag Cd Ruthenium Rhodium Palladium Silver Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon 85.47 87.62 88.91 91.22 92.91 95.96 (98) 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3 55 56 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 6 Cs Ba Caesium Barium 57-71 Lanthanides Hf Hafnium Ta Tantalum W Tungsten Re Os Rhenium Osmium Ir Iridium Pt Platinum Au Hg Gold M e rcury Tl Thallium PbLead Bi Bismuth Po Polonium At Rn Astatine Radon 132.9 137.3 178.5 180.9 183.9 186.2 190.2 192.2 195.1 197.0 200.5 204.38 207.2 209.0 (209) (210) (222) 87 88 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 7 Fr Ra Francium Radium 89-103 Actinides Rf Db Sg Bh Hs Mt Ds Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Rg Roentgenium Cn Nh Copernicium Nihonium Fl Flerovium Mc Lv Moscovium Livermorium Ts Tennessine Og Oganesson (223) (226) (265) (268) (271) (270) (277) (276) (281) (280) (285) (284) (289) (288) (293) (294) (294) 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 La Ce Lanthanum Cerium Pr Nd Pm Sm Eu Gd Tb Dy Ho Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium D ysprosium Holmium Er Tm Yb Lu Erbium Thulium Ytterbium Lutetium 138.9 140.1 140.9 144.2 (145) 150.4 152.0 157.2 158.9 162.5 164.9 167.3 168.9 173.0 175.0 89 90 91 92 93 94 95 96 97 98 99 100 101 102 103 Ac Th Pa Actinium Thorium Protactinium U Uranium Np Pu Am Cm Bk Neptunium Plutonium Americium Curium Berkelium Cf Californium Es Fm Md No Einsteinium Fermium Mendelevium Nobelium Lr Law rencium (227) 232.0 231.0 238.0 (237) (244) (243) (247) (247) (251) (252) (257) (258) (259) (262) American Chemical Society www.acs.org/outreach