7-A - Chapter 7 Covalent Bonding Chemistry 5th Edition...

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C h a p t e r 7 Covalent Bonding Chemistry 5th Edition McMurry/Fay
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2 Electronegativity χ = (E i + E ea )/2 Usually converted to a unitless number between 0 and 4. Low χ form cation High χ form anion
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3 Electronegativity Bond polarity is due to electronegativity differences between atoms. Pauling Electronegativity: is expressed on a scale where F = 4.0
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4 Electronegativity Pauling Electronegativities Pauling Electronegativities
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5 Electronegativity Predicting χ 1. Increases across periods 2. Decreases down groups 3. Very low for noble gases.
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6 Electronegativity % Ionic Character: As a general rule for two atoms in a bond, we can calculate an electronegativity difference (∆EN ) : ∆EN = EN(Y) – EN(X) for X–Y bond. If ∆EN < 0.5 the bond is covalent. If ∆EN < 2.0 the bond is polar covalent. If ∆EN > 2.0 the bond is ionic.
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7 The Covalent Bond Covalent bonds are formed by sharing at least one pair of electrons.
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The Covalent Bond Every covalent bond has a characteristic length that leads to maximum stability.
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This note was uploaded on 02/29/2012 for the course CHM 111 taught by Professor Colyer during the Summer '08 term at Wake Forest.

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7-A - Chapter 7 Covalent Bonding Chemistry 5th Edition...

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