Answer the following questions about the Lewis structure for the organic molecule CH3CH2CH2CN (see examples in Chapter 10) There are valence electrons. The molecule has single bonds, double bonds, and triple bonds. The three central C atoms on the left have REDS and the shape at each of these is The central C on the right has REDS and the shape is The AENC-N = 0.49 which is only slightly polar and we will consider it to be nonpolar. %3D Since there is only slightly polar covalent bond, the molecule is mostly а. О b. 1 С. 2 d. 3 е. 4 f. 5 g. 8 h. 10 i. 12 j. 14 k. 16 I. 18 m. 20 n. 24 О. 28 р. 30 q. 32 r. 34 S. 36 t. diatomic u. pyramidal v. linear w. monoatomic ions x. tetrahedral y. trigonal planar z. bent aa. 120° bb. 180° dd. 109.5° cc. no bond angles, no central atom nonpolar ее. polar ff. gg. ionic hh. C and C

Answer the following questions about the Lewis structure for the organic molecule CH3CH2CH2CN (see examples in Chapter 10) There are valence electrons. The molecule has single bonds, double bonds, and triple bonds. The three central C atoms on the left have REDS and the shape at each of these is The central C on the right has REDS and the shape is The AENC-N = 0.49 which is only slightly polar and we will consider it to be nonpolar. %3D Since there is only slightly polar covalent bond, the molecule is mostly а. О b. 1 С. 2 d. 3 е. 4 f. 5 g. 8 h. 10 i. 12 j. 14 k. 16 I. 18 m. 20 n. 24 О. 28 р. 30 q. 32 r. 34 S. 36 t. diatomic u. pyramidal v. linear w. monoatomic ions x. tetrahedral y. trigonal planar z. bent aa. 120° bb. 180° dd. 109.5° cc. no bond angles, no central atom nonpolar ее. polar ff. gg. ionic hh. C and C

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 10RQ: Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, IF5, and SCl6....

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Define formal charge and explain how to calculate it. What is the purpose of the formal charge? Organic compounds are composed mostly of carbon and hydrogen but also may have oxygen, nitrogen, and/or halogens in the formula. Formal charge arguments work very well for organic compounds when drawing the best Lewis structure. How do C, H, N, O, and Cl satisfy the octet rule in organic compounds so as to have a formula charge of zero?
7.50 Chemical species are said to be isoelectronic if they have the same Lewis structure (regardless of charge). Consider these ions and write a Lewis structure for a neutral molecule that is isoelectronic with each of them, (a) CN , (b) NH4+ . (c) CO32
Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, IF5, and SCl6. These 12 compounds arc all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structure. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule docs not.) See Exercises 115 and 116 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.
7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?
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