Nitrogen oxides are pollutants and common by-products of power plants and automobiles.NO, can react with the NO in smog, forming a bond between the N atoms.:0:productDraw the structure of the resulting compound, including formal charges.SelectDrawRingsMoreEraseNUse the table of bond energies to predict the energy of the bond in NO.O about 200 kJ/molO about 400 kJ/molO about 600 k/molUse the same table to predict the energies of the bonds in NO,.O both are about 400 kJ/molO one is about 200 kl/mol and the other is about 600 k/molO both are about 600 kl/molO both are about 200 kl/moltvAaMacBook Air Multiple BondsBondkJ/molO=0498C=C611*C=C835*C=0745*C=O1077N=O607*N=N418*N=N941C=N615*C-N891*C=S477**indicates an energy that is an average for that type of bond in several different molecules.Single BondsHydrogenCarbonHalogensNitrogenEnergyBond (kJ/mol) Bond (kJ/mol) Bond (kJ/mol) Bond (kJ/mol) Bond (kJ/mol) Bond (kJ/mol)ОхудenSulfurEnergyEnergyEnergyEnergyEnergyH-H436C-HS-HS-OS-F410*N-H390*O-H460*340*Br-F234H-O460*C-O350*N-O200*142*265*Br-Cl219H-F569C-F450*N-F270*O-F180*310*Br-Br194H-CI432C-CI330*N-CI200*O-CI200*S CI250*Br-I179H-Br366C-Br270*N-Br240*O-Br210S-Br210C-F251H-I298C-I240*N-I159*O-I220*S-I170*CI-CI243H-C410*C-C350*N-C300*OC350*S-C260*F-F157C-NC-SH-N390*300*N-N240*O-N200*S-NI-F280H-S340*260*N-SO-S265*S-S225I-I153

Nitrogen oxides are pollutants and common by-products of power plants and automobiles. NO, can react with the NO in smog, forming a bond between the N atoms. :0: N= - EN• product > Draw the structure of the resulting compound, including formal charges. Select Draw Rings More Erase N Use the table of bond energies to predict the energy of the bond in NO. about 200 kJ/mol about 400 kJ/mol about 600 kJ/mol Use the same table to predict the energies of the bonds in NO,. both are about 400 kJ/mol one is about 200 k/mol and the other is about 600 k/mol both are about 600 k/mol both are aboutl 200 k/mal O000

Nitrogen oxides are pollutants and common by-products of power plants and automobiles. NO, can react with the NO in smog, forming a bond between the N atoms. :0: N= - EN• product > Draw the structure of the resulting compound, including formal charges. Select Draw Rings More Erase N Use the table of bond energies to predict the energy of the bond in NO. about 200 kJ/mol about 400 kJ/mol about 600 kJ/mol Use the same table to predict the energies of the bonds in NO,. both are about 400 kJ/mol one is about 200 k/mol and the other is about 600 k/mol both are about 600 k/mol both are aboutl 200 k/mal O000

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter4: Molecular Structure And Orbitals

Section: Chapter Questions

Problem 123CP: Carbon monoxide (CO) forms bonds to a variety of metals and metal ions. liS ability to bond to iron...

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Similar questions

9.77 When a reaction is exothermic, is the sum of bond energies of products or of reactants greater?
Which of the following statements is false concerning bonding? Elements with extremely different electronegativities tend to form ionic bonds with each other. In an N—O bond. electron density is greater near the O atom. An N—O bond is an example of a polar covalent band. In general, chemical bonds form to minimize energy. The bond in KBr is formed by sharing electrons.
The major industrial source of hydrogen gas is by the following reaction: CH4(g)+H2O(g)CO(g)+3H2(g) Use bond energies to predict E for this reaction.
7.97 Consider the structure shown below for as well as any other important resonance structures. (a) What is the expected O—N—O bond angle in this structure? (b) The molecule contains N—O bonds of two different lengths. How many sborter N—O bonds would be present?
Draw Lewis structures for BrO4-, SiH4, PCl4, CH2Cl2 and BF4-.(a) Which species is/are likely to be paramagnetic?(b) What reaction(s) would occur for the paramagnetic species? (c) By VSEPR, suggest the molecular geometry of each species.
Methane burns in oxygen to form carbon dioxide and watervapor. Hydrogen sulfide burns in oxygen to form sulfur dioxideand water vapor. Use bond energies to deter-mine the heat of each reaction per mole of O₂(assume Lewisstructures with zero formal charges; BE of S=O is 552 kJ/mol).
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxnΔHrxn° for the equation C2H4 (g) + HBr (g) --> C2H5Br (g) Average molar bond enthalpies. (?bond)(Hbond) Bond ??⋅???−1kJ⋅mol−1 Bond ??⋅???−1kJ⋅mol−1 O−HO−H 464464 C≡NC≡N 890890 O−OO−O 142142 N−HN−H 390390 C−OC−O 351351 N−NN−N 159159 O=OO=O 502502 N=NN=N 418418 C=OC=O 730730 N≡NN≡N 945945 C−CC−C 347347 F−FF−F 155155 C=CC=C 615615 Cl−ClCl−Cl 243243 C≡CC≡C 811811 Br−BrBr−Br 192192 C−HC−H 414414 H−HH−H 435435 C−FC−F 439439 H−FH−F 565565 C−ClC−Cl 331331 H−ClH−Cl 431431 C−BrC−Br 276276 H−BrH−Br 368368 C−NC−N 293293 H−SH−S 364364 C=NC=N 615615 S−SS−S 225225
Using Lewis symbols and Lewis structures, diagram the formationof SiCl4 from Si and Cl atoms, showing valence-shellelectrons. (a) How many valence electrons does Si have initially?(b) How many valence electrons does each Cl haveinitially? (c) How many valence electrons surround the Siin the SiCl4 molecule? (d) How many valence electrons surroundeach Cl in the SiCl4 molecule? (e) How many bondingpairs of electrons are in the SiCl4 molecule?
The standard heat of formation of CaBr2 is -675 kJ/mol. The first ionization energy of Ca is 590 kJ/mol, and its second ionization energy is 1145 kJ/mol. The heat of sublimation of Ca3Ca(s)¡Ca( g)4 is 178kJ>mol. The bond energy of Br2 is 193 kJ/mol, the heat of vaporization of Br2(l ) is 31 kJ/mol, andthe electron affinity of Br is -325 kJ>mol. Calculate the lattice energy of CaBr2.
Suppose there is an element X which occurs naturally as X2(g).X2(g) + 2O2(g) → X2O4(g)ΔHof of O(g) is 249 kJ/molΔHof of X(g) is 458.5 kJ/molΔHof of X2O4(g) is 31 kJ/molThe X-X single bond energy is 116 kJ/molUse the above data to estimate the average bond energy in X2O4. Give your answer to the nearest 1 kJ/mol.
(a) Describe the molecule xenon trioxide, XeO3, usingfour possible Lewis structures, one each with zero, one,two, or three Xe¬O double bonds. (b) Do any of theseresonance structures satisfy the octet rule for every atomin the molecule? (c) Do any of the four Lewis structureshave multiple resonance structures? If so, how many resonancestructures do you find? (d) Which of the Lewisstructures in part (a) yields the most favorable formalcharges for the molecule?
The cyanate ion (OCN-) and the fulminate ion (CNO-) share the same three atoms but have vastly different properties. The cyanate ion is stable, while the fulminate ion is unstable and forms explosive compounds. The resonance structures of the cyanate ion were explored in Example 5.6. Draw Lewis structures for the fulminate ion—including possible resonance forms—and use formal charge to explain why the fulminate ion is less stable(and therefore more reactive) than the cyanate ion.