Compare these two structures.[0=C=N] [0=C—N:Determine whether the two represent resonance contributors of a single species or depict different substances. If two structures are not resonance contributors,explain why. Select the single best answer.O The two structures are resonance contributors of the same species.The two structures are not resonance contributors because they contain different numbers of electrons.The two structures are not resonance contributors because they contain different bond orders.O The two structures are not resonance contributors because they contain bond orders having integer values.The two structures are not resonance contributors because each structure is present in its most stable (lowestenergy) configuration.The two structures are not resonance contributors because they have different arrangements of atoms.XŚ

If the Lewis structure of a molecule or ion cannot be explained by a single structure then more than…

Compare these two structures. [0=C=N_0=C—N: Determine whether the two represent resonance contributors of a single species or depict different substances. If two structures are not resonance contributors, explain why. Select the single best answer. O The two structures are resonance contributors of the same species. O The two structures are not resonance contributors because they contain different numbers of electrons. O The two structures are not resonance contributors because they contain different bond orders. O The two structures are not resonance contributors because they contain bond orders having integer values. The two structures are not resonance contributors because each structure is present in its most stable (lowest energy) configuration. O The two structures are not resonance contributors because they have different arrangements of atoms. X

Compare these two structures. [0=C=N_0=C—N: Determine whether the two represent resonance contributors of a single species or depict different substances. If two structures are not resonance contributors, explain why. Select the single best answer. O The two structures are resonance contributors of the same species. O The two structures are not resonance contributors because they contain different numbers of electrons. O The two structures are not resonance contributors because they contain different bond orders. O The two structures are not resonance contributors because they contain bond orders having integer values. The two structures are not resonance contributors because each structure is present in its most stable (lowest energy) configuration. O The two structures are not resonance contributors because they have different arrangements of atoms. X

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

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.114QE: Formamide, HC(O)NH2, is prepared at high pressures from carbon monoxide and ammonia, and serves as...

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In the following pair, determine whether the two represent resonance contributors of a single species or depict different substances. If two structures are not resonance contributors, explain why. Select the single best answer. :N-N=N: and :N-N=N: The two structures are resonance contributors of the same species. The two structures are not resonance contributors because they contain different numbers of electrons. The two structures are not resonance contributors because they contain different bond orders. The two structures are not resonance contributors because they contain bond orders having integer values. The two structures are not resonance contributors because each structure is present in its most stable (lowest energy) configuration.
SO < SO2< SO32-( a) Match each species with the number of covalent bonds predicted by Lewis structures to exist between an S atom and an O atom bonded to this S atom. (Hint: Average the number of bonds between S and an attached oxygen atom in a particular position using all of your resonance structures for the species that you are working on.)SO32- : is it 1.00, 1.33, 1.50, 2.00, 3.00 (b) Match each species with the correct formal charge on the central S atom. SO32- : is it -1.00 , -0.67 , -0.50, 0.00, +1.00, or +2.00 ? (c) Match each species with the average formal charge on an outside oxygen atom predicted by Lewis structures. SO32- : is it -1.00 , -0.67 , -0.50, 0.00, +1.00, or +2.00 ?
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:
Should 100% sure of answer. Draw the Lewis structure of HBrO₃ (by following the octet rule on all atoms) and then choose the appropriate pair of molecular geometries of the two central atoms. Your answer choice is independent of the orientation of your drawn structure.
Consider a molecule AB6, where element A has 6 valence electrons and B has 7 valence electrons. If the ΔEn for each bond = 1.2, predict the shape, bond hybridization and polarity (polar or non-polar) of the molecule. Your answer should follow the format: a) number of total electrons for bonding; b) Steric Number and Lone Pairs; c) name of shape based on the VSEPR chart, d) bond hybridization and e) molecular polarity.
A resonance hybrid is a structure that can be depicted by more than one valid Lewis structure. part1: Draw the major resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons. part2: Draw the second most important resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons. part3: Draw the least important resonance contributor for fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized and should include all nonzero formal charges and all nonbonding electrons.
A resonance hybrid is a structure that can be depicted by more than one valid Lewis structure. part1: Draw the major resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons. part2: Draw the second most important resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons.
Does CH3COCH3 has molecular resonance? If so, show all possible forms.
Molecules containing a single atom of nitrogen, carbon, and oxygen can gain an electron to form an anion.All non-bonding electrons and nonzero formal charges should be included in the structure. What is the most stable resonance structure if nitrogen is the central atom in the CNO– ion? What is the most stable resonance structure if carbon is the central atom in the NCO– ion? What is the most stable resonance structure if oxygen is the central atom in the CON– ion?
Three resonance structures for the cyanate ion, OCN are shown. :0—C=N: Structure 31 :0=C-N: Structure 1 :0=C=N Structure 2 Select all of the true statements: All of the structures are equivalent since they all obey the octet rule. Structure 1 is not very likely because of the large formal charges. Structure 2 is a better resonance form than structure 3 because the negative formal charge is on the most electronegative element. Structure 3 is a better resonance form than structure 2 because the negative formal charge is on the most electronegative element. Structure 3 is not a valid Lewis structure because carbon doesn't obey the octet rule.
Create 3 different lewis structures that are not resonance structures for a compound. Note that the compound much have 4 carbon atoms, 1 oxygen atom, 1 nitrogen atom, 6-10 hydrogen atoms. The formula for the 3 compounds do not need to be exactly the same. Consider also: 1st compound: There must be 1 carbon atom with tetrahedral geometry around it. 2nd compound: There must be 1 carbon with trigonal planar geometry 3rd compound: There must be 1 carbon with linear geometry around it. Encircle those carbons mentioned. Make sure that lone pairs are visible.
Draw out the Lewis structures for H₂CO3, HCO3, and CO32-. Then determine the maximum number of equivalent resonance structures for each species. Note that carbon is the central atom in all three cases. If the molecule contains hydrogen atoms they are attached to oxygen atoms. Only count the best structures. For example, A structure with really bad formal charges should not be counted. The molecule H₂CO3 has The molecule HCO3 has The molecule CO3²- has equivalent Lewis structures. equivalent Lewis structures. equivalent Lewis structures.