Consider the 4 Lewis structures given here, it is the ion NSO". [Ns-+] [s] [sso] [s0]" N=S=Ö (B) (C) (D) (A) 1- One of the figures is not a resonance structure to the other three. That is 2- The formal charge of the sulfur is in all correct resonance structures. 3- Based on the electronegativity character of N, O, and S, the probable Lewis structure is figure 4- The positive charge means one electron is missing from the total of initial valence electrons

Consider the 4 Lewis structures given here, it is the ion NSO". [Ns-+] [s] [sso] [s0]" N=S=Ö (B) (C) (D) (A) 1- One of the figures is not a resonance structure to the other three. That is 2- The formal charge of the sulfur is in all correct resonance structures. 3- Based on the electronegativity character of N, O, and S, the probable Lewis structure is figure 4- The positive charge means one electron is missing from the total of initial valence electrons

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter9: Chemical Bonds

Section: Chapter Questions

Problem 9.72QE: Write all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure...

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Write all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?
Based on the concept of formal charge, what is the central atom in (a) HCN (do not include H as a possibility)? b) NOCI (Cl is always a terminal atom)?
Incomplete Lewis structures for the nitrous acid molecule,HNO2, and the nitrite ion, NO2-, are shown here. (a) Completeeach Lewis structure by adding electron pairs as needed.(b) Is the formal charge on N the same or different in thesetwo species? (c) Would either HNO2 or NO2- be expected toexhibit resonance? (d) Would you expect the N=O bond inHNO2 to be longer, shorter, or the same length as the N¬Obonds in NO2?
Consider the formate ion, HCO2", which is the anion formed when formic acid loses an H* ion. The H and the two O atoms are bonded to the central C atom. (a) Draw the best Lewis structure(s) for this ion. (b) Are resonance structures needed to describe the structure? Explain briefly (c) Would you predict that the C-O bond lengths in the formate ion would be longer or shorter relative to those in CO2? Explain briefly
Incomplete Lewis structures for the nitrous acid molecule,HNO2, and the nitrite ion, NO2-, are shown here. (a) Completeeach Lewis structure by adding electron pairs as needed.(b) Is the formal charge on N the same or different in thesetwo species? (c) Would either HNO2 or NO2- be expected toexhibit resonance? (d) Would you expect the N“O bond inHNO2 to be longer, shorter, or the same length as the N¬Obonds in NO2-? [Sections 8.5 and 8.6]
In the vapor phase, BeCl2 exists as a discrete molecule. (a) Draw the Lewis structure of this molecule, using only single bonds. Does this Lewis structure satisfy the octet rule? (b) What other resonance structures are possible that satisfy the octet rule? (c) On the basis of the formal charges, which Lewis structure is expected to be dominant for BeCl2?
#6. Consider the Lewis structure below where X is an element from the third period (Na-Ar). (a) Identify the central atom, X, when n = - -1. (b) Determine the formal charge on X. (c) Draw a Lewis structure so that the formal charge on X is equal to +1. :Ö: [+] n-
There are many Lewis structures you could draw for sulfuricacid, H2SO4 (each H is bonded to an O). (a) WhatLewis structure(s) would you draw to satisfy the octet rule?(b) What Lewis structure(s) would you draw to minimizeformal charge?
Cyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.
The hypochlorite ion, ClO-, is the active ingredient inbleach. The perchlorate ion, ClO4-, is a main componentof rocket propellants. Draw Lewis structures for both ions. (a) What is the formal charge of Cl in the hypochlorite ion?(b) What is the formal charge of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (c) What is theoxidation number of Cl in the hypochlorite ion? (d) Whatis the oxidation number of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (e) In a redox reaction,which ion would you expect to be more easily reduced?
Draw Lewis diagrams for the following ions. In the formula the symbol of the central atom is given first. (Hint:The valence octet may be expanded for the central atom.)(a) BrO4 - (b) PCl6 - (c) XeF6+
Three possible Lewis structures for the thiocyanate ion, NCS-, are (a) Determine the formal charges in each structure.(b) Based on the formal charges, which Lewis structure is the dominant one?