'Delocalized electrons' presentation slideshows

METALS

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Organic Chemistry 6 th Edition Paula Yurkanis Bruice

Organic Chemistry 6 th Edition Paula Yurkanis Bruice. Chapter 7 Delocalized Electrons and Their Effect on Stability, Reactivity, and p K a More About Molecular Orbital Theory. Localized Versus Delocalized Electrons. Benzene Has Delocalized Electrons.

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Chapter 9 Molecular Geometries and Bonding Theories

Chemistry, The Central Science , 10th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten. Chapter 9 Molecular Geometries and Bonding Theories. Molecular Shapes. The shape of a molecule plays an important role in its reactivity

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ORGANIC OPTION -G

ORGANIC OPTION -G. IB Core Option Objective. Electrophilic Addition Reactions G.1.1 Describe and explain the electrophilic addition mechanisms of the reactions of alkenes with halogens and hydrogen halides. Terms. Electrophile : Carbocation : Carbocation stabalization :

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Chemical Bonding

Chemical Bonding. Overview. Bonding and structure explains the properties of a substance!. Giant Covalent Structures. Diamond. Graphite. Structure of Covalent Substances. Covalent substances may exist as: simple molecular structures giant covalent structures Diamond Graphite

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Laboratory 06 MOLECULAR GEOMETRY AND POLARITY

Laboratory 06 MOLECULAR GEOMETRY AND POLARITY. The three dimensional (3D) structure of a molecule. -How its atoms are connected and arranged in space. Molecular geometry. Boiling point, Freezing point, Chemical reactivity. Polar. Non Polar. Reactivity. Toxicity.

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Worksheet: Chapter 12 Homework Key

Worksheet: Chapter 12 Homework Key. 1. Determine whether the bond formed between each of the elements listed below would be ionic or covalent based on the metallic/nonmetallic nature of the elements involved.

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Metallic Bond

Metallic Bond. IB. The Periodic Table of Elements. Periodic Table. Formation of metallic bond. the metal atoms "lose" one or more of their outer electrons These electrons become delocalized, and free to move throughout the entire metal.

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Metallic Bonding

Metallic Bonding. Metallic Bonding. Observations of the physical properties of metals have led chemists to develop theories to explain these observations. Physical Properties of Metals. For example, electrical conductivity requires the presence of charged particles that are free to move.

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Midterm 2 Review

Midterm 2 Review. Line Structures. Problem 1: Draw the line structure of HOCH 2 CH 2 CCHCOOH. What is the hybridization of each atom. We will do this on the worksheet. .

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Chemistry Second 9 weeks 3

Chemistry Second 9 weeks 3. Review Ionic. http://www.khanacademy.org/video/ionic--covalent--and-metallic-bonds?playlist=Chemistry 0 to 6:11 is ionic compound review http://www.chemlecture.com/GC1/bonding.introduction/bonding.introduction.html. Class Today. Metallic Bonding.

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Bonds NonMusical Chairs Review

Bonds NonMusical Chairs Review. 1. Which bond type (covalent, ionic, or metallic) conducts electricity as a solid or a liquid? 2. Which bond type (covalent, ionic, or metallic ) conducts electricity only as a liquid, and not in the solid form?

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HL4-5

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Metallic Bonding

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Bonding

Bonding. Chemical Bond- force that holds 2 atoms together. Octet Rule - Atoms want to achieve the configuration of a noble gas 8 valence electrons = Very Stable! Atoms will either lose or gain valence electrons in order to get 8 in the outermost energy level

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Metallic bond

Metallic bond. Metals. Made up of closely packed cations surrounded by electrons Outer electron clouds of the metal ions overlap Share their electrons to form a sea of electrons. Metallic Bond. The electrostatic attraction of the delocalized electrons for the positively charged metal ions

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Delocalized Electrons: Resonance

Delocalized Electrons: Resonance. When writing Lewis structures for species like the nitrate ion, we draw resonance structures to more accurately reflect the structure of the molecule or ion. Delocalized Electrons: Resonance.

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Metallic Bond

Metallic Bond. IB. Formation of metallic bond. the metal atoms "lose" one or more of their outer electrons These electrons become delocalized, and free to move throughout the entire metal. These negative delocalized electrons hold the metal cations together strongly.

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Metallic Bonds

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Metallic Bonding

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