IN THIS SECTION YOU'LL SEE A MORE THOROUGH DESCRIPTION OF LECTURES AND ASSOCIATED MATERIALS
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ART OF DRAWING ORGANIC MOLECULES
CODE: Bdom1TW
Level: basic, 1st semester
SLIDESHOW: 21 slides, 60-90 min lecture
File size: 3.682 KB, [Microsoft PowerPoint 2003 up];
TEXTBOOK STYLE SCRIPT: 4.846 KB [Office Word, 2003 up]
PROBLEM SHEET: 113 KB [PDF]
Description: Most of the keys to chemical properties are shown in a clear drawing of each compound molecular structure. This is a sort of language the future organic chemist must know and acquire a good hand to draw them. This lecture reviews various ways to depict molecular models on paper or computer screen and provides practical techniques to render clear molecular line drawings now of universal application.
CONTENTS
Molecules and rendering types: from the empirical formula to three dimensional structures
Aliphatics: Explicit hydrogens versus abbreviated line renderings
Branching in aliphatic compounds
Drawing aromatic compounds
Drawing alicyclic compounds and the problem of their non planarity, an introduction
A sophisticated example: cocain
PACKAGE INCLUDES:Microsoft PowerPoint Slide show: 21 slides, (60-90 min lecture) (3.682 KB)
Complete script in textbook format (4.846 KB)
Problem sheet (113 KB) PDF
COST: FREE. DOWNLOAD: SLIDESHOW (4.33 Mb),
SCRIPT (PDF, 1.3 Mb),
PROBLEM SHEET (PDF, 113 kb)
FUNCTIONAL GROUPS IN ORGANIC COMPOUNDS
CODE: Bfog1TW
Level: basic, 1st semester
Slideshow: 24 slides, 45-60 min lecture
SLIDESHOW File size: 1150 KB,
SCRIPT: 484 KB (Office Word),
PROBLEM SHEET: 181 KB (PDF)
Cost: FREE DOWNLOAD FREE SAMPLE
FREE DOWNLOADS: SLIDESHOW (1.15 Mb)
SCRIPT (PDF) (1.2 Mg)
PROBLEM SHEET (PDF)
PRINTABLE LIST OF FUNCTIONAL GROUPS
DESCRIPTION:
Functional groups are the sites where real organic chemistry takes place. It is mandatory for the student and practitioner to become familiar with structures and names of functional groups, a task requiring a lot of memory. However, there is a systematic approach to build and remember functionalities based on adding s and p bonds from C to common “organic” heteroatoms, which this lecture describes.
CONTENTS:
1.- Why this topic is important
2.- What is a functional group after all?
3.- The most common functional groups you cannot do without
4.- Approaching functional groups systematically
5.- The fundamental structures around Carbon
6.- Quick view of functionalities according to structural type
7.- Functional groups of C to C multipole bonds
COVALENT BONDING ON CARBON 1. THE LEWIS-LANGMUIR MODEL
CODE: BLew1TW
Level: basic, 1st semester
Interactive Slideshow:
There are two levels in the same pakage:
Fast track lecture: 21 slides, 45-60 min. 22 pages script with 12 full color figures & schemes
Complete lecture: 31 slides, 90-120 min. 46 pages script with 17 full color figures & schemes
File size SLIDESHOW [Microsoft PowerPoint 2003 up] (5.114Kb);
TEXTBOOK STYLE SCRIPTS: Fast Track script (2.023 kb), complete lecture scipt (2.557 kb)
COST: US $ 49.95 (EUROPE: 33.oo €)
DESCRIPTION
The properties of the C-X covalent bond (X = C, N, O, halogens, S, Si) explain the rich gamut of structural and chemical properties of organic and bioorganic compounds. This is why so much effort has been invested in understanding this singular couple. Among all elements of the Periodic Table, Carbon is particularly rich in the various manners it bonds to other atoms. There are various models that explain aspects of the C-X bond. The Lewis-Langmuir electron-sharing model and the Octet Rule of second row elements was the first to be recognized universally. Although quite deficient, it is still educationally essential to review and understand. This lectured explores the fundamentals of interatomic forces leading to covalent bonds from the Lennart-Jones model of Hydrogen molecule up to methane, and reviews other "dot structures" of small organics.
LECURE CONTENT: (in Fast track version only point 6 is emphasized)
1.- REMINDER: Forming the Lennart-Jones energy diagram
2.- Deviations from the simple interatomic bonding: the carbon compounds
3.- Molecular disturbances in organics as new bonds are formed or destroyed
4.- Common elements other than C & H in organic compounds
5.- Type of bonds around C and theories of covalent bond formation in C
6.- The Lewis-Langmuir idea of electron sharing & covalent bonding
COVALENT BONDING AROUND C. VALENCE-BOND THEORY(PART 1): TETRAVALENT C AND sp3 HYBRID ORBITALS
CODE: BVb1TW
Level: basic, 1st semester
Interactive Slideshow: 21 slides, 45-60 min lecture.
File size: SLIDESHOW (1.336KB) [Microsoft PowerPoint 2003 up];
TEXTBOOK STYLE SCRIPT (101 KB)
COST: US $ 49.95 (EUROPE: 33.oo €)
DESCRIPTION:
Although the Lewis-Langmuir model of covalent bonding provided an intuitive picture of covalent bonding based on shell-electron sharing, it failed to explain some structural features and reactivity of organic compounds. After s, p, and d atomic orbitals were described as solutions of the Schröedinger equation (see Lecture MMot1TW for a more detailed description), and difficulties were found in using them to explain the tetrahedral symmetry of simple organic molecules such as CH4 and other lower hydrocarbons, Linus Pauling devised a smart solution to this problem by ‘hybridizing’ or mixing mathematically s and p orbitals in Carbon. This led to sp3, sp2 and sp linear combinations of atomic orbitals. This is the first of a series of two 60-90 min lectures dealing with this hybridization model of atomic orbitals in full graphic detail, currently very popular and extensively used to explain molecular behavior in qualitative terms. All the same Pauling’s is just a practical model uncapable of a more sophisticated quantitative view now offered by MO theory and ab initio methods.
LECTURE CONTENT
1.- Why the Lewis-Langmuir model does not explain satisfactorily the covalent bond
2.- The Valence Bond Atomic Orbitals (VBAO) from solutions of the Schröedinger equation
3.- The pure atomic orbitals of elements in organics. Properties. Sigma and pi bond formation
4.- Failure of pure VBAOs to portray the correct structure of methane
5.- Pauling's Linear Combination of Atomic Orbitals method (LCAO). Sp3 hibridization and the correct sigma bond around carbon. Methane structure
6.- Building the ETHANE molecule. Correct prediction of structure and free rotation of the single C-C bond
7.- Rotational energy barriers of ethane conformers. An introductory view.
COVALENT BONDING AROUND C. VALENCE-BOND THEORY(PART 2): TRIVALENT AND BIVALENT C. (sp2, and sp hybrids)
CODE: BVb2TW
Level: basic, 1st semester
Interactive Slideshow: 21 slides, 45-60 min lecture.
File size: SLIDESHOW (1.126 KB) [Microsoft PowerPoint 2003 up];
TEXTBOOK STYLE SCRIPT (89 KB)
COST: US $ 49.95 (EUROPE: 33.oo €)
DESCRIPTION:
After the sp3 hybridization model proposed by Linus Pauling explained so successfully the symmetry of tetravalent C compounds such as the lower hydrocarbons, alcohols, amines etc, the trivalent and bivalent C compounds were examined through different hybridization ratios of s and p ‘pure’ atomic orbitals. This Led to new symmetry concepts: Trigonal and linear molecules which are explained in full graphic atomic orbital detail in this presentation, a subject usually confusing to draw with chalk on blackboard or hand flickering. Alkenes (ethylene) Carbonyl-containing compounds (formaldehyde), allenes and alkynes (acetylene) are described in detail including thorough molecular symmetry properties in an interactive 21 slide PowerPoint presentation.
LECTURE CONTENTS
1.- The sp2 hybridization. How the trigonal planar geometry of C comes about
2.- Building a pi bond: ethylene. Properties of the C=C bond: geometry, non-rotation of the C=C bond
3.- Building a carbonyl (C=O): Formaldehyde. The sp2 oxygen.
4.- The sp hybridization. How the linear geometry comes about
5.- Building the triple (s + p + p) bond: Acetylene
6.- Combining sp2 and sp carbons: Allenes, ketenes and their peculiar spatial arrangement
7.- The banana pi bonds
8.- Bond lengths, angles, and energy as a function of hybridization
9.- AO hybridization in second row 'organic' elements N, O, and their combinations with C.
COVALENT BONDING AND MOLECULAR ORBITAL THEORY (MOT) IN ORGANIC COMPOUNDS (PART I).
THE s, p & d ATOMIC ORBITALS IN THE MOT CONCEPTION.
CODE: BVb2TW
Level: basic-CHEMISTRY MAJORS, 1st semester
Interactive Slideshow: 22 slides, 60-90 min lecture.
File size: SLIDESHOW (5.566KB) [Microsoft PowerPoint 2003 up];
TEXTBOOK STYLE SCRIPT (358 KB)
COST: US $ 49.95 (EUROPE: 33.oo €)
AVAILABLE IN DARK AND LIGHT SLIDE BACKGROUNDS.
DESCRIPTION:
The behavior of particles at the molecular, atomic and subatomic levels is explained by quantum theory. Although this theory was first devised in the early 20th century, new developments appear continuously in the literature as compounds contain large numbers of quantum atomic particles governed by complex equations in the Hartree-Fock environment. There is no way to study thoroughly organic chemistry without at least some basic knowledge of how quantum theory introduces the concept of atomic orbital to lodge bonding and non bonding electrons in Carbon and the rest of 1st-3rd row elements found in organic compounds. Nowadays there are some computer programs accessible to most organic chemists to perform sophisticated calculations (MM2, MOPAC, Gaussian...) in molecular structures built using simple software molecular drawing interfaces. One should have a basic idea of what lays behind the curtain. This lecture shows how relatively simple equations lead to an intuitive model of s, p & d atomic orbitals, the consequences of orbital overlap and fundamental properties derived from this, including bond length and bond energy.
CONTENTS
1.- Electrons as quantum wave-particles
2.- Atomic orbitals emerge as solutions of the Schröedinger equation
3.- Shape, electron density distribution and internal structure of Atomic Orbitals as a consequence of their mathematical treatment. A view of Atomic orbitals s, p, d.
4.- Relative size of AOs and its impact on some common properties of the covalent bond: bond length and bond energy.
Pi Conjugation in Organic compounds. Part 1
Code: MCar1TW
Level: Intermediate-CHEMISTRY MAJORS, 1st semester
Interactive Slideshow: 40 slides, 90-120 min lecture.
File size: SLIDESHOW (3.9 Mb) [Microsoft PowerPoint 2003 up];
TEXTBOOK STYLE SCRIPT (587 KB) (PDF)
COST: US $ 59.95 (EUROPE: 39.oo €)
CONTENTS
1.- Conjugation. Definition, from butadiene to alpha,beta-unsaturated ketones
2.- Experimental proof of pi conjugation
3.- Other forms of conjugation: pi bonds and lone electron pairs
4.- Conjugation and relative stability: cross conjugation
5.- Conjugation in carbon transient species C+, C•, C-
DESCRIPTION:
Pi conjugation defines structural and chemical behavior in carbon compounds. This lecture focuses on the two general types of pi conjugation: open and closed or circular. Open conjugation refers to open chained or aliphatic compounds whereas closed conjugation occurs in alicyclic compounds. The latter type may or may not lead to aromaticity. In the first of this two part series of lecture the fundamentals, requirements and limitations of open conjugation are described, from butadiene up, using chiefly the valence bond theory background and some reference only to frontier molecular orbital theory. Conjugation of C=C bonds with other systems such as C=N and C=O bonds and C=C-O: allyl systems are also discussed in detail.
Three quizes are embedded in the PowerPoint presentation for in-class discussion
AN ABRIDGED INTRODUCTORY LEVEL LECTURE FOR NON ORGANIC CHEMISTRY MAJORS IS ALSO INCLUDED, SLIDE SHOW AND ADAPTED SCRIPT
