chm115_lecture140

chm115_lecture140 - Chemistry 115 Lecture 14 Outline Review...

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22-1 Chemistry 115 Lecture 14 Outline Review Hess’s Law (see end of Lecture 13) Chapter 8 Intro to Bonding Lewis Dot Structures Ionic Bonding Recitation: Chapter 8: Ionic bonds Lewis dot structures Exam 2 preparation (review Chapters 5-8)
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22-2 Example problem (2007 Exam 2) 21. Calculate the enthalpy change for the following reaction: NO(g) + O(g) NO 2 (g) from the following information: NO(g) + O 3 (g) NO 2 (g) + O 2 (g) H = -198.9 kJ O 3 (g) 1.5 O 2 (g) H = -142.3 kJ ½ O 2 (g) O(g) H = 247.5 kJ a) -551.6 kJ b) -304.1 kJ c) 153.8 kJ d) 438.4 kJ e) none of these is correct
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22-3 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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22-4 The three models of chemical bonding
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22-5 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.
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