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.HAHH-CN Cy―N=Cy―0H-Cx-NC,=0:HHBIn structure B, the formal charge of N is +1.The oxidation state of N is different for each structure.Structures B and C are nonequivalent resonance structures.In structure C, the formal charge of O is -1.On the basis of formal charges, structure B is more important than structure A.The total charge on this species is -1.00000CC

Step 1: Formal charge = valence electrons - Non valence electrons - Bonding electrons/2Formal charge…

Answered: Which of the following statements…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter7: Covalent Bonding

Section: Chapter Questions

Problem 68QAP: Consider the pyrosulfate ion, S2O72-. It has no sulfurâ€“sulfur nor oxygenâ€“oxygen bonds. (a) Write...

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Write the Lewis symbols for each of the following ions: (a) As3 (b) I (c) Be2+ (d) O2 (e) Ga3+ (f) Li+ (g) N3
The n-propyl cation can be formed from a molecule such as When the C–Cl bond is broken so that both electrons leave with Cl, the fragments formed are The carbon atom that had been attached to Cl is now sharing ____ electron pairs. In each shared pair the carbon atom owns ____ electron. The number of electrons that belong to carbon is ____. The formal charge on the carbon atom is ____. The correct Lewis structure for the n-propyl cation is
Write the Lewis symbols of the ions in each of the following ionic compounds and the Lewis symbols of the atom from which they are formed: (a) MgS (b) Al2O3 (c) GaCl3 (d) K2O (e) Li3N (f) KF
Define the term lattice energy. Why, energetically, do ionic compounds form? Fig. 3-8 illustrates the energy changes involved in the formation of MgO(s) and NaF(s). Why is the lattice energy of MgO(s) so different from that of NaF(s)? The magnesium oxide is composed of Mg2+ and O2 ions. Energetically, why does Mg2+O2 form and not Mg+O? Why doesnt Mg3+O3 form?
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. + A B On the basis of formal charges, structure B is more important than structure A. The oxidation state of N is different for each structure. In structure C, the formal charge of O is -1. Structures B and C are nonequivalent resonance structures. In structure B, the formal charge of N is +1. The total charge on this species is -1. H -NC₂=0:
Covalent bonds: H―HC―HO―HO═O C≡O Bond energy (kJ/mol):4364154654981080Calculate the enthalpy change (H, in kJ/mol) for the following reaction and indicate whether the reaction is exothermic or endothermic.(*BE for C═Oin CO2)(a) CH4(g)+ H2O(g)CO(g)+ 3H2(g);
I need this solution, Calculate the Enthalpy Change (ΔH) from average bond energies, which have been listed below in KJ/mol, for the following reaction and identify the nature of the reaction: CH3COOH + CH3OH → CH3COOCH3 + H2O [C‒H: 413; C‒C: 347; C=O: 745; C=C: 614; Cl‒Cl: 239, C‒O: 358; O‒H: 467
Arrange these resonance forms of OCN" in order of most plausible Lewis structure to least plausible Lewis structure: A B C [ö-c=N:] [•0=c=ÿ•] [:ö=c=N:] [:0=c-N:] Most plausible Lewis structure 1 3 Least plausible Lewis structure
Calculate the enthalpy of reaction for the equation using the bond energy values given. CH4 +202 CO₂ + 2H₂O → Bond Energy Bond Bond Bond Energy (kJ/mol) Lewis Structures (kJ/mol) C-H 413 O-H 463 H 0-0 146 0=0 498 H-C-HÔ=0 C-C 346 C=C 602 C-O 358 C=O 799 H H o=c=0; ΔΗχη = [ ? ] kJ .O. rxn Enter a + or - sign AND the magnitude in your answer. Enter
a. Use bond energy values to estimate AH for the following reaction. CEN ΔΗ = C - N H - H C-H N - H ΔΗ = b. Use bond energy values to estimate AH for the following reaction. H-F N - H H-C=N (g) + 2 H₂(g): NEN (891 kJ/mol) (305 kJ/mol) (432 kJ/mol) (413 kJ/mol) (391 kJ/mol) N - N (160. kJ/mol) (565 kJ/mol) (391 kJ/mol) (941 kJ/mol) (154 kJ/mol) F-F kJ H- kJ H C- H H -N(g) H H (g) +2F2(g) → N=N(g) + 4HF(g) H
We can draw three inequivalent Lewis structures for the selenite ion, Se032-. The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. Formal Charge Se 01 02 03 Se || :0: A 0° 2- Se :0: 2. The best Lewis structure for SeO32- i: ✓ B 2. O Se :0: C 12-
Consider the NCO anion. the following three Lewis structures can be drawn for it: Structure 1 Structure 2 Structure 3 [N=C=0] [:N=C_Q] [:N—c=0:] Based on the formal charges determined in the previous three questions, which of these three resonance structures would you predict to be the most stable? Structure 1 Structure 2 Structure 3 Structures 2 and 3 (equally stable) All three structures are equally stable, because all three satisfy the octet rule.

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