Please correct answer and don't use hand rating and don't use Ai solution CENThis violates the first rule by breaking a single bond.This violates the second rule by exceeding an octet for a second-row element.This violates neither rule.

Step 1: Solution for (a):- First Rule: This rule is about not breaking single bonds (σ bonds) when…

Answered: CEN This violates the first rule by…

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 27E

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Similar questions

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 ____.
What is the maximum number of atoms to which a central atom in a molecule can bond and still conform to the octet rule? What is the minimum number?
Chloromethane has the Lewis structure _______________________________ The carbon atom is sharing 4 electron pairs. In each shared pair the carbon atom “owns” 1 electron. The number of electrons that “belong” to carbon is ___. Carbon, being a Group ___ element would have 4 , outer shell electrons in the unbonded, neutral state. Therefore, the carbon atom in chloromethane has a formal charge of zero.
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.
Two Lewis structures can be written for nitrosyl fluoride, which contains one nitrogen, one oxygen, and one fluorine atom per molecule. Write the two Lewis structures land assign a formal charge to each atom.
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.
Draw resonance structures for each of these ions: NSO− and SNO−. (The atoms are bonded in the order given in each case, that is, S is the central atom in NSO−.) Use formal charges to determine which ion is likely to be more stable. Explain why the two ions cannot be considered resonance structures of each other.
Sulfur and oxygen form a series of 2 anions including sulfite, SO32, and sulfate, SO42. In addition to these, there are three other more complex anionsdithionite, S2O42, dithionate, S2O62, and tetrathionate, S4O62. Write correct Lewis structures for dithionite, dithionate, and tetrathionate ions.
The “Chemistry in Focus" segment Hiding Carbon Dioxide- discusses attempts at sequestering (storing) underground CO2produced at power plants so as to diminish the: greenhouse effect. Draw all resonance structures of the CO2molecule.
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.
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.HForHClc.HBrorHClb.HClorHId.HIorHBr
hy is there an octet rule (and what does actet mean) in writing Lewis structures?

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CEN This violates the first rule by breaking a single bond. This violates the second rule by exceeding an octet for a second-row element. This violates neither rule.