Don't used Ai solution and hand raiting www.awy.aleks.com/alekscgi/x/Isl.exe/16_u-lgNsikr7j8PGeneral Chemistry ReviewDeciding whether a Lewis structure satisfies the octet ruleDecide whether these proposed Lewis structures are reasonable.proposed Lewis structureIs the proposed Lewis structure reasonable?OYes.:NEN:-:0:N-O-:Z:Cl:O No, it has the wrong number of valence electrons.The correct number is: ☐ONo, 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 manytimes as necessary. For example, if two oxygen atoms don't satisfy the octet rule, enter "O,O".×D

Approach to solving the question:Lewis octet theory.Valence electrons on different atoms. Detailed…

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Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter12: Chemical Bonding

Section: Chapter Questions

Problem 33E

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Similar questions

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.
These are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.
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.
Write Lewis structures for the following: (a) ClF3 (b) PCl5 (c) BF3 (d) PF6
The molecules BH3 and SF6 and the ion SO42 exist and are stable. Draw a Lewis structure of each,and comment on whether they are exceptions to Lewis’ octet rule.
White phosphorus (P4) consists of four phosphorus atoms arranged at the corners of a tetrahedron. Draw the valence electrons on this structure to give a Lewis diagram that satisfies the octet rule.
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 ____.
The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.
7.47 Which of the species listed has a Lewis structure with only one lone pair of electrons? F2 , CO32 , CH4 , PH3
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+
Two possible Lewis diagrams for sulfine (H2CSO) are (a) Compute the formal charges on all atoms. (b) Draw a Lewis diagram for which all the atoms in sulfine have formal charges of zero.
On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be covalent, polar covalent, or ionic. msp;a.SSb.SHc.SK

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