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CHEM 111 (69)
Lecture

EN trends, ionic and covalent bonds, Lewis structures, basic process (single bonds), higher bond orders

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Department
Chemistry
Course
CHEM 111
Professor
Dana Johnson
Semester
Fall

Description
11 October Clicker question from Friday What is the molecular formula for vitamin C from the information that was provided? A. C H3O 4 3 B. C H6O 8 6 C. C H5O 7 5 D. C H1O 1.3 1 E. I didn’t do it Molar mass of vit. C 176.12 g / mol Mass of vit. C is 1.000 g Mass of CO – 2.5 g Mass of H O2– 0.41 g Mass of C = 12.01 / 44.01 x 1.5 g = 0.409 g Mass of H = 1.008 / 18.016 x 0.41 g = 0.046 g Mass of O = 1.000 g – 0.409 g – 0.046 g = 0.545 g Moles of C = 0.409 g x 1 mol / 12.01 g = 0.0341 moles Moles of H = 0.046 g x 1 mol / 1.008 g = 0.0456 moles Moles of O = 0.545 g x 1 mol / 16 g = 0.0341 moles C 0.0341 / 0.0.0456 / 0.00.0341 / 0.0341 C 1 1.33 1 3 C 3 4 3 Compare to molar mass (3 x 12.01) + (4 x 1.008) + (3 x 16) = 88 176.12 / 88 =2 C 6 8 6 EN trends Pauling’s scale puts F at the top with a value of 4.0 Inversely related to atomic size Electrons pulled by larger Z effmaller size Atom behaves the same in a bond Partial charges result (δ+ and δ-) Generally increases as you move up and to the right Ionic and covalent bonds Form a continuum Cutoff between the two labels is arbitrary Usually made using ΔEN Lewis structures Way to visualize bonding relationships in a molecule Built up from Lewis dot symbols Based on the octet rule Basic process (single bonds) Place least electro
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