Fulminate ion (CNO) Carbon, nitrogen, and oxygen form two different polyatomic ions: cyanate ion (NCO) and fulminate ion (CNO). Write Lewisstructures for each anion, including near-equivalent resonance structures (do not add any arrows between structures) and indicatingformal charges. The isocyanate ion also has two near-equivalent structures, but the formal charge on the nitrogen attom cannot bereduced to zero:Cyanate ion (NCO)

Let's explore the Lewis structures for the cyanate ion (NCO-) and the fulminate ion (CNO-). These…

Answered: Fulminate ion (CNO) Carbon, nitrogen,…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 51QRT: Several Lewis structures can be written for perbromate ion, , the central Br with all single Br—O...

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Several Lewis structures can be written for perbromate ion, , the central Br with all single Br—O bonds, or with one, two, or three Br=O double bonds. Draw the Lewis structures of these possible resonance structures, and use formal charges to predict which makes the greatest contribution to the resonance hybrid.
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.
Write reasonable Lewis structures for the following species, none of which follow the octet rule. (a) BeCl2 (b) SeO2- (c) ClO3 (d) CH3
Write the Lewis structures for the following species, and indicate whether each is an odd-electron species, an electron-deficient species, or an expanded valence shell species. (a) BI3 (b) IF5 (c) HN2
Formamide, HC(O)NH2, is prepared at high pressures from carbon monoxide and ammonia, and serves as an industrial solvent (the parentheses around the O indicate that it is bonded only to the carbon atom and that the carbon atom is also bonded to the H and the N atoms). Two resonance forms (one with formal charges) can be written for formamide. Write both resonance structures, and predict the bond angles about the carbon and nitrogen atoms for each resonance form. Are they the same? Describe how the experimental determination of the HNH bond angle could be used to indicate which resonance form is more important.
Write reasonable Lewis structures for the following species, none of which follow the octet rule. (a) BF3 (b) NO (c) CO+ (d) ClO3
Draw all the equivalent resonance structures for BrO 3¯ on a piece of paper and then fill in the blanks. Draw the structure in such a way that the formal charge on the central atom is zero. Molecular geometry: Number of equivalent resonance structures: Bond order of Br-O bond(s): (fractions rounded to 2 decimal places, e.g. 1/2 will be 0.50 , 4/3 will be 1.33 and 5/3 will be 1.67) Formal charge on terminal atoms participating in resonance
Which of the following statements concerning the structures below is/are true? You can select more than one, or none, of these statements. N = A N: Z: = N B = Z: :N=N- The total charge on this species is -1. Structure B is the least important structure. For each N in structure B, the formal charge is zero. Structures A and B are equivalent resonance structures. Structures A, B, and C are equivalent resonance structures. Structures A and C are equivalent resonance structures. In structure A, the N atom on the left has a formal charge of zero. C N:
Which of the following statements concerning the structures below is/are true? Formal charges are not shown. You can select more than one, or none, of these statements. (i) (ii) (iii) Ö (iv) The total charge on this species is zero. The formal charge of Cl is -3 in structure (i). CI has an expanded octet in all of these structures. The formal charge of Cl is +1 in structure (iii). Structures (ii), (iii), and (iv) are all unrealistic because, in each, there are too many electrons around O Cl. On the basis of formal charges, structure (i) is the most important structure.
Some chemists believe that satisfaction of the octet ruleshould be the top criterion for choosing the dominant Lewisstructure of a molecule or ion. Other chemists believe thatachieving the best formal charges should be the top criterion.Consider the dihydrogen phosphate ion, H2PO4-, inwhich the H atoms are bonded to O atoms. (a) What is thepredicted dominant Lewis structure if satisfying the octetrule is the top criterion? (b) What is the predicted dominantLewis structure if achieving the best formal charges is the topcriterion?
Complete the following Lewis structures for the CICN molecule by adding dots for unshared valence electrons and indicating formal charges. Evaluate the importance of each structure as a contributor to a resonance hybrid. Cl – C = N, Cl = C – N, Cl = C = N
Write a Lewis structure for the NO3 - ion. Include resonance structures?

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