2. The molecule LiH has a simple electronic structure. The H atom would like to gain an electron to fill its is subshell, but the Li atom would similarly like to fill its 2s subshell. Based on the atomic structure of H and Li, which would you expect to dominate in the desire for an additional electron? Are the electronegativity values of Table 9.6 consistent with this?

2. The molecule LiH has a simple electronic structure. The H atom would like to gain an electron to fill its is subshell, but the Li atom would similarly like to fill its 2s subshell. Based on the atomic structure of H and Li, which would you expect to dominate in the desire for an additional electron? Are the electronegativity values of Table 9.6 consistent with this?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter7: Covalent Bonding

Section: Chapter Questions

Problem 76QAP: In each of the following molecules, a central atom is surrounded by a total of three atoms or...

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What aspect of the following Lewis structure indicates that the concept of coordinate covalency is needed to explain the bonding in the molecule?
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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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On the basis of the electronegativity values given in Fig. 12.3. indicate which is the more polar bond in each of the following pairs. msp;a.OClorOBrc.PSorPOb.NOorNFd.HOorHN
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