'Bond energy' diaporamas de présentation

Covalent Bonding

Covalent Bonding. Chap. 9. Why does it form?. Why does it form?. Octet rule . An atom will gain, lose, or share electrons in order to get a full set. Why does it form?. Octet rule Stability/Minimum energy. Why does it form? What is a molecule?. Molecule = covalent compound.

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WHO Training Workshop on Pharmaceutical Quality, G MP and Bioequivalence with a focus on artemisinines

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CH 8: Bonding

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Chapter 17 Free Energy and Thermodynamics

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The Quantum Mechanical Model of the Atom

The Quantum Mechanical Model of the Atom. Chapter 7. The nature of light. Light is electromagnetic radiation: a wave of oscillating electric & magnetic fields. Wave properties. A wave has wavelength, frequency, and amplitude. Wave properties. Wavelength = ? (lambda), in m

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The hierarchical nature and processes of different levels of ecological systems :

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PH3-SM (PHY3032) Soft Matter Physics 4 October, 2010 Lecture 1: Introduction to Soft Matter

PH3-SM (PHY3032) Soft Matter Physics 4 October, 2010 Lecture 1: Introduction to Soft Matter. What is Condensed Matter?. Phase diagram of carbon dioxide. I mage : http://wps.prenhall.com/wps/media/objects/602/616516/Chapter_10.html.

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University of Ferrara Department of Chemistry and Centre for Structural Diffractometry

Intermolecular Interactions and Molecular Recognition Przesieka, 8-12 June 2010. Syngenta Crop Protection , 4332 Stein, CH, 28 October 2010. H-Bond Patterns in Nature. A Gallery of Functional H-Bonds. Gastone Gilli. University of Ferrara Department of Chemistry and

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Metabolism

Metabolism. Chapter 7. Metabolism. Metabolism : All chemical reactions within organisms that enable them to sustain life. The two main categories are catabolism and anabolism. Metabolism.

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Department of Chemical Engineering

Chemical Activation Reactions of Cyclic Alkane and Ether Ring-Opened Diradicals with O 2 : Thermochemistry, Reaction Paths, Kinetics. Itsaso Auzmendi Murua, Jason Hudzik Joseph W. Bozzelli. 7 th International Conference on Chemical Kinetics, July 10-14, 2011.

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Assist. Prof. Bilge Imer

MSN 504 Phase Transformations & Diffusion in Materials. Assist. Prof. Bilge Imer. Phase.

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Chemical Bonding I: Basic Concepts

Chemical Bonding I: Basic Concepts. Chapter 8. Group. e - configuration. # of valence e -. ns 1. 1. 1A. 2A. ns 2. 2. 3A. ns 2 np 1. 3. 4A. ns 2 np 2. 4. 5A. ns 2 np 3. 5. 6A. ns 2 np 4. 6. 7A. ns 2 np 5. 7. Valence electrons are the outer shell electrons of an

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CHAPTER 2: A tomic structure and interatomic bonding

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Chemistry 445. Lecture 4. Molecular Orbital Theory of diatomic molecules

Chemistry 445. Lecture 4. Molecular Orbital Theory of diatomic molecules. The non-existent He 2 molecule (bond order = 0). BO = (2-2)/2 = 0. The MO diagram for the He 2 molecule is similar to that for the H 2 molecule,

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GEK2507: Physical Questions from everyday Life

GEK2507: Physical Questions from everyday Life. Tutorial 3: Photosynthesis, Blackbody Radiation, Vision and Biopolymers. . Question1: [Light Harvesting Process]

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Covalent Bonding

Covalent Bonding. Bonding models for methane, CH 4 . Models are NOT reality. Each has its own strengths and limitations. Covalent Bonds. Polar-Covalent bonds. Electrons are unequally shared Electronegativity difference between .3 and 1.7. Nonpolar -Covalent bonds.

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Elements,Compounds and Mixtures

Elements,Compounds and Mixtures. Mixtures. Consist of a physical blend of two or more substances. They contain a variable composition Most materials found in nature are mixtures. EX. Air, stew, blood. Mixtures.

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Exothermic and Endothermic Reactions

Exothermic and Endothermic Reactions. Chemical Reactions. All chemical reactions involve bond breaking and bond forming. Energy is needed to break bonds and released when bonds are formed. Chemical reactions are accompanied by a change in energy, mainly in the form of heat. .

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Bond Enthalpy

Bond Enthalpy. Chem 12. D H 0 = 436.4 kJ. H 2 ( g ). H ( g ). +. H ( g ). D H 0 = 242.7 kJ. Cl 2 ( g ). Cl ( g ). +. Cl ( g ). D H 0 = 431.9 kJ. HCl ( g ). H ( g ). +. Cl ( g ). D H 0 = 498.7 kJ. O 2 ( g ). O ( g ). +. O ( g ). O. D H 0 = 941.4 kJ. N 2 ( g ).

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