CH9(3-5)Nov10FA08a

CH9(3-5)Nov10FA08a - Chemistry 109 University of Nebraska...

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Chemistry 109 University of Nebraska – Lincoln FALL 2008 ANNOUNCEMENTS Chemjam Times Monday: Henz 124 6:00 pm Tuesday: HAH 110 6:00 and 7:30 pm Exam Thursday
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Born-Haber Cycle ΔH 0 lattice = ΔH o f – (ΔH o sub + ΔH o BE + ΔH o IE1 +ΔH o IE2 + 2ΔH o EA ) ΔH o lattice = -1123 kJ –(148 kJ + 159 kJ + 738 kJ + 1450 kJ +2(-328 kJ)) ΔH o lattice =
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Born-Haber Cycle Given the following information, calculate the electron affinity for fluorine: K(s) K(g) ΔH o sub = 90 kJ K(g) K + (g) + e - ΔH o IE = 419 kJ F 2 (g) 2F(g) ΔH o BE = 159 kJ K(s) + 1/2F 2 (g) KF(s) ΔH f = -569 kJ K + (g) + F - (g) KF(s) ΔH o lattice = -821 kJ KF(s)
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Lattice energy _________ as atomic size increases r Q Q E - + = κ Lattice energy __________ as ionic charge increases Trends in Lattice Energy
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Lattice Energy Notice that the magnitude of the ______________ dominates the entire multistep process of the Born-Haber cycle! What does this mean? Ionic solids exist only because the lattice energy drives the energetically ____________ electron transfer. It takes energy to form ions but this is more than regained when they attract each other and form the solid (note that for Li + (g) + F - (g) LiF(s) ΔH 0 lattice = -1050 kJ while for LiF(s) Li + (g) + F - (g) ΔH 0 = +1050 kJ)
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Energetics of Ionic Compounds 1. Why doesn’t potassium form K 2+ cations or fluorine
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CH9(3-5)Nov10FA08a - Chemistry 109 University of Nebraska...

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