Page 4 of 4are created1016 words214. For a bent molecule with three atoms, what is the relationship between the partial charges and thedirection of the molecular dipole?15. Why is it important to take both the polarity of the bonds and the shape of the molecule intoconsideration when determining the polarity of the molecule?IX English (United States)#3BOCT19the electronegatively anI$4Accessibility: InvestigateUA%5Ais closer toFocusMacBook Pro|||< 6:E6P13less than 2.A&GE78O150%Deпо

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Answered: 14. For a bent molecule with three…

14. For a bent molecule with three atoms, what is the relationship between the partial charges and the direction of the molecular dipole?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

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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Concept explainers

Quantum Mechanical Treatment of the Valence Bond Theory

Quantum mechanical treatment of valence bond theory refers to the relationship established between the quantum mechanical theory and the valence bond theory to describe the chemical bonding in a particular molecule.

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Page 4 of 4
are created
1016 words
2
14. For a bent molecule with three atoms, what is the relationship between the partial charges and the
direction of the molecular dipole?
15. Why is it important to take both the polarity of the bonds and the shape of the molecule into
consideration when determining the polarity of the molecule?
IX English (United States)
#
3
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OCT
19
the electronegatively an
I
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4
Accessibility: Investigate
U
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%
5
A
is closer to
Focus
MacBook Pro
|||
< 6
:E
6
P
13
less than 2.
A
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7
8
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150%
De
по

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7.97 Consider the structure shown below for as well as any other important resonance structures. (a) What is the expected O—N—O bond angle in this structure? (b) The molecule contains N—O bonds of two different lengths. How many sborter N—O bonds would be present?
What is meant by a chemical bond? Why do atoms form bonds with each other? Why do some elements exist as molecules in nature instead of as free atoms?
The percent ionic character of a bond can be approximated by the formula 16+3.52 , where is the magnitude of the difference in the electronegativities of the atoms (see Fig. 3.18). Calculate the percent ionic character of HF, HCl, HBr, HI, and CsF, and compare the results with those in Table 3.7.
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?
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?
Which of the following statements is false concerning bonding? Elements with extremely different electronegativities tend to form ionic bonds with each other. In an N—O bond. electron density is greater near the O atom. An N—O bond is an example of a polar covalent band. In general, chemical bonds form to minimize energy. The bond in KBr is formed by sharing electrons.
Predict die molecular structure and bond angles for each molecule or ion in Exercises 88 and 94. a. POCl3, SO42, XeO4, PO43, ClO4 b. NF3, SO32, PO33, ClO3 c.ClO2, SCl2, PCl2 d. Considering your answers to parts a, b, and c. what conclusions can you draw concerning the structures of species containing the same number of atoms and the same number of valence electrons? (O3), sulfur dioxide, and sulfur trioxide.
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.
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