Chapt 7 Study Guide - exceptions which can occur with this...

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Study Sheet for Chapter 7 - Covalent Bonding The student must be able to 1. Describe the differences between covalent and polar covalent bonding; know examples of each type. 2. Use electronegativity from the proceeding chapter to predict the type of bond which might be formed. Know the most electronegative elements and the least electronegative ones to be able to use in predicting bond types. 3. Describe what is meant by bond polarity and dipole moments. 4. Use the methods of writing electronic configuration of elements from the proceeding chapter to write the electronic configuration of cations and anions. 5. Describe the ionic size of ions in terms of the periodic table. 6. Draw Lewis electron dot structures to show bonding and lone pairs of electrons in simple covalent compounds and binary ionic compounds. Recognize the "octet" rule and
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Unformatted text preview: exceptions which can occur with this rule. 7. Define what is meant by resonance in a compound. Be able to correctly draw the resonant structures of compounds and ions that exhibit this phenomenon. 8. Use the valence shell electron pair repulsion model (VSEPR) to predict the geometry of simple compounds. 9. Use hybridization of atomic orbitals to predict the bond angles and geometry of simple molecules. Important words/phrases: covalent bonding single bond polar covalent bonding electronegativity dipole moment isoelectronic ions s (sigma) bond p (pi) bond double bond triple bond lone pair bonding pair Lewis dot structure octet rule resonance molecular structure VSEPR model linear trigonal planar tetrahedral trigonal pyramid trigonal bipyramid octahedral square planar...
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This note was uploaded on 09/01/2011 for the course BUSINESS 101 taught by Professor Jones during the Spring '11 term at Southern Nazarene.

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