1C_Lecture_2 Ch13 Bonding General Concepts

1C_Lecture_2 Ch13 Bonding General Concepts - Chapter 13...

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Chapter 13 Bonding: General Concepts o Types of Bonding o Electronegativity o Lewis Structures o Strength/Length of Covalent Bonds o Shapes of Molecules (VSEPR) o Polar Molecules 1 Big Idea: Bonds are formed from the attraction between oppositely charged ions or by sharing electrons. Only the valence electrons participate in bonding. The shape of the molecules maximize the distance between areas of high electron density.
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Chapter 13: Bonding: General Concepts Electronegativity 2
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Chapter 13: Bonding: General Concepts Electronegativity The dividing line between ionic and covalent bonds is hazy. Ionic Character: The extent to which ionic structures contributes to the resonance of a molecule or ion. 3 Difference in Electronegativity Type of Bond > 1.8 Mostly Ionic 0.4-1.8 Polar Covalent < 0.4 Mostly Covalent 0 Non-polar Covalent
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Chapter 13: Bonding: General Concepts Electronegativity How does the difference in electronegativity effect the properties of compounds? NaCl MgCl 2 AlCl 3 SiCl 4 PCl 3 S2Cl 2 Cl 2 ionic polar-covalent covalent 4
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Chapter 13: Bonding: General Concepts Electronegativity 5 Note: The larger the anion the easier it is to distort the electron cloud.
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Chapter 13: Bonding: General Concepts Lewis Structures Formal charge and oxidation numbers both give us information about the number of electrons around an atom in a compound. Formal Charge Exaggerates Covalent Character
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This note was uploaded on 09/09/2011 for the course CHEM 1C taught by Professor Hooker during the Spring '06 term at UCSB.

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1C_Lecture_2 Ch13 Bonding General Concepts - Chapter 13...

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