chm115_lecture15

chm115_lecture15 - Chemistry 115 Lecture 15 Outline Chapter...

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22-1 Chemistry 115 Lecture 15 Outline Chapter 8 Intro to Bonding Lewis Dot Structures EXAM 2: Thursday, March 10, 8pm Elliot Hall of Music Chapters 5, 6, 7, 8 (Lewis dots) Recitation: Chapter 8: Lewis dot structures Exam 2 preparation (review Chapters 5-8)
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15-2 Chapter 8 – Chemical Bonding Chemical bonding is a key to understanding the microscopic aspects that determine materials properties. We’ll talk about three types of bonding 1. Ionic Bonding -electrostatic forces that hold ions together 2. Covalent Bonding – shared electrons between atoms 3. Metallic Bonding – metal nuclei “floating” in a sea of electrons. A key to understanding bonding is to know what the Valence electrons are doing, i.e, those electrons in the outer orbital shell of the atoms.
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15-3 The three models of chemical bonding
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Lewis electron-dot structures Depicts the valence electrons Use A group number to place dots around the atoms Pair up the dots until they are all used For metals , number of dots = number of electrons it loses For non-metals , the number of unpaired electrons tells you the number of bonds it can form. .. .. ·F: Cu· Na· Question: What are the Lewis dot structures for sodium, fluorine and copper(I)? 15-4
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Ionic Bonds Involves a transfer of electron(s) from metal to non-metal and the formation of a solid ionic compound Li [He]2s 1 + F [He]2s 2 2p 5 Li + 1s 2 (or [He]) + F - [He]2s 2 2p 6 or [Ne] Can also show this with Lewis dots: .. .. .. .. Li· + ·F: Li + + :F: - Note that the F- ion has an octet of electrons – very stable. Li + also has a closed shell ([He]).
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