None proposed Lewis structureYes.H-O-HN-N:Z:: Cl=0Is the proposed Lewis structure reasonable?No, it has the wrong number of valence electrons.The correct number is:No, it has the right number of valence electrons but doesn't satisfy theoctet rule.The symbols of the problem atoms are:*Yes.No, it has the wrong number of valence electrons.The correct number is:No, it has the right number of valence electrons but doesn't satisfy theoctet rule.The symbols of the problem atoms are:*Yes.No, it has the wrong number of valence electrons.The correct number is:No, it has the right number of valence electrons but doesn't satisfy theoctet rule.The symbols of the problem atoms are:*☐If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as manyExplanationCheck2024 McGraw Hill T

Proposed Lewis structureIs the proposed Lewis structure reasonableYesTotal valence electrons= H…

Answered: proposed Lewis structure Yes. H-O-H N-N…

Living by Chemistry

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ISBN:9781464142314

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Publisher:Angelica M. Stacy

ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 3STP

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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?
A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain.
It is impossible to draw a legitimate Lewis structure of a neutral NH4 molecule. Hypothetically,how many valence electrons would such a neutral NH4 molecule have ifit could exist? a. The +1 cation, NH4+ , does exist. How many valence electrons does one NH4+ ion have? b. Draw the Lewis structure for NH4+
In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.
Draw Lewis diagrams for the following compounds. In the formula the symbol of the central atom is given first. (Hint: The valence octet may be expanded for the central atom.) (a) PF5 (b) SF4 (c) XeO2F2
Acrylonitrile is the building block of the synthetic fiber Orlon. Acrylonitrile Which carbon-carbon bond is shorter? Which carbon-carbon bond is stronger? Which bond is the most polar? What is the partial negative end of that bond?
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.
On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be ionic, covalent, or polar covalent. msp;a.HOc.HHb.OOd.HCl
In each of the following diatomic molecules. which end of the molecule is positive relative to the other end? msp;a.hydrogenfluoride,HFb.chlorinemonofluorideClFc.iodinemonofluorideICl
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
Fill in the blanks in each line of the following table that involves characteristics of various bonds between nonmetals. The first line is already completed as an example.
For each of the following numbers of electrons, give the formula of a positive ion that would have that number of electros, and write the complete electros configuration for each ion. msp;a.10electronsc.18electronsb.2electronsd.36electrons

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