17,18 - Chemistry 11500 Lecture 17 & 18 Reading:...

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1 Chemistry 11500 Reading: Sections 9.5, 10.3, 12.3, 13.1, 13.3, 13.5 and add 13.7 to your reading!
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This week in chemistry Attend lecture, lab, and recitation Homework due on Friday Lab: Where’s the iron? Read Chapter 8 in lab manual Read sections 3.5 and pp 273-274 in book
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Where’s the Iron? Read Chapter 8 and review Appendix E in the lab manual. Determine the concentration of iron (Fe 3+ ) in broccoli and compare your results to data on the internet.
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Solubility of Ethanol E10 - a gasoline blend with 10% ethanol is widely used to reduce carbon monoxide emissions and to boost octane ratings. Corona (beer): contains 4.5% ethanol How can ethanol be soluble in gasoline and also soluble in water?
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Chemical Structure To understand solubility we must look at the structure and intermolecular forces. IMFs are NOT covalent bonds, but IMFs are weak forces that hold one molecule to another. Strong interaction with water Strongish interaction with hydrocarbons CH 3 CH 2 OH
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Polar Bond Many IMFs result from polar covalent bonds , an uneven distribution of electrons between atoms in a bond: F
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Dipole Moment Combine the effect of 3-D shape with bond polarity to get the dipole moment of the molecule overall. F μ = 1.94 D D = Debye
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Dipole Moment • Example: CO 2 vs. CO
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Dipole Moment Example H 2 O μ = 1.85 D D = Debye
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__________________________________________ CH 3 OH methanol infinitely miscible CH 3 CH 2 OH ethanol infinitely miscible CH 3 (CH 2 ) 2 OH propanol infinitely miscible CH 3 (CH 2 ) 3 OH butanol 9 g/100g H 2 O CH 3 (CH 2 ) 4 OH pentanol 2.7 g/100g H2O CH 3 (CH 2 ) 5 OH hexanol 0.6 g/100g H2O CH 3 (CH 2 ) 6 OH heptanol 0.18 g/100g H2O
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IMFs: (attractions involving dipoles)
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IMFs: (electrostatic attractions)
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solo Which of the following atoms is the most electronegative? A.
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17,18 - Chemistry 11500 Lecture 17 & 18 Reading:...

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