chm115_lecture140

chm115_lecture140 - 22-1Chemistry 115Lecture 14...

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Unformatted text preview: 22-1Chemistry 115Lecture 14 OutlineReview Hess’s Law (see end of Lecture 13)Chapter 8Intro to BondingLewis Dot StructuresIonic BondingRecitation:Chapter 8: Ionic bondsLewis dot structuresExam 2 preparation (review Chapters 5-8)22-2Example problem (2007 Exam 2)21. Calculate the enthalpy change for the following reaction:NO(g) + O(g) NO2(g)from the following information:NO(g) + O3(g) NO2(g) + O2(g)∆H = -198.9 kJO3(g) 1.5 O2(g)∆H = -142.3 kJ½ O2(g) O(g)∆H = 247.5 kJa) -551.6 kJb) -304.1 kJc) 153.8 kJd) 438.4 kJe) none of these is correct22-3Chapter 8 – Chemical BondingChemical bonding is a key to understanding the microscopic aspects that determine materials properties.We’ll talk about three types of bonding1. Ionic Bonding -electrostatic forces that hold ions together2. Covalent Bonding – shared electrons between atoms3. 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.22-4The three models of chemical bonding22-5Lewis electron-dot structuresDepicts the valence electronsUse A groupnumber to place dots around the atomsPair up the dots until they are all usedFor metals, number of dots = number of electrons it losesFor non-metals, the number of unpaired electrons tells you the number of bonds it can form....
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This note was uploaded on 02/05/2011 for the course CHM 115 taught by Professor Towns during the Fall '08 term at Purdue.

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chm115_lecture140 - 22-1Chemistry 115Lecture 14...

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