Consider the Lewis structure for the polyatomic oxyanion shown here, where X is an element from the third period (Na-Ar). By changing the overall charge, n, from 1- to 2- to 3- we get three different polyatomic ions. For each of these ions a. identify the central atom, X; b. determine the formal charge of the central atom, X; C. draw a Lewis structure that makes the formal charge on the central atom equal to zero. . :Ö: :0––0: :Ọ: n

Consider the Lewis structure for the polyatomic oxyanion shown here, where X is an element from the third period (Na-Ar). By changing the overall charge, n, from 1- to 2- to 3- we get three different polyatomic ions. For each of these ions a. identify the central atom, X; b. determine the formal charge of the central atom, X; C. draw a Lewis structure that makes the formal charge on the central atom equal to zero. . :Ö: :0––0: :Ọ: n

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter2: Lewis Structures

Section: Chapter Questions

Problem 20CTQ

See similar textbooks

Similar questions

Represent the bonding in SF2 (FUSUF) with Lewis diagrams. Include the formal charges on all atoms. The dimer of this compound has the formula S2F4. It was isolated in 1980 and shown to have the structure F3SUSF. Draw a possible Lewis diagram to represent the bonding in the dimer, indicating the formal charges on all atoms. Is it possible to draw a Lewis diagram for S2F4 in which all atoms have valence octets? Explain why or why not.
On the left side of Figure 3.6, label the areas shown with a dotted line where... one bond can form. one bond can form.
The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.
Based on the concept of formal charge, what is the central atom in (a) HCN (do not include H as a possibility)? b) NOCI (Cl is always a terminal atom)?
Draw a curve that describes the energy of a system with H and Cl atoms at varying distances. Then, find the minimum energy of this curve two ways. (a) Use the bond energy found in Table 8.1 to calculate the energy for one single HCl bond (Hint: How many bonds are in a mole?) (b) Use the enthalpy of reaction and the bond energies for H2 and Cl2 to solve for the energy of one mole of HCl bonds. H2(g)+Cl2(g)2HCl(g)Hrxn=184.7kJ/mol
Explain why this Lewis structure for CO is not as valid as the Lewis structure you drew in theprevious question even though it has no “hot spots” of + or charge (formal charges).
Define formal charge and explain how to calculate it. What is the purpose of the formal charge? Organic compounds are composed mostly of carbon and hydrogen but also may have oxygen, nitrogen, and/or halogens in the formula. Formal charge arguments work very well for organic compounds when drawing the best Lewis structure. How do C, H, N, O, and Cl satisfy the octet rule in organic compounds so as to have a formula charge of zero?
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
1. What is the formal charge on each atom in CH3Cl and the Lewis structure for it? 2. What is the formal charge on each atom in PH4 nd the Lewis structure for it? 3. What is the formal charge on each atom in HNO3 and the Lewis structure for it?
Draw possible Lewis structures and using formal charge determine the best one for [AsSiSe]-. Show FC for ALL structures and then explain why you chose the one that is best.
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxnΔ⁢Hrxn° for the equation NH3(g)+2O2(g)⟶HNO3(g)+H2O(g)NH3⁢(g)+2⁢O2⁡(g)⟶HNO3⁢(g)+H2O(g) The bonding in the molecules is shown.
4.Examine the model and real structures for SO2. A.In what way does the central atom violate the octet rule? When is it possible for molecules to have this exception to the octet rule? B.Calculate the difference in the bond angle between the real and model structure? Is this difference larger or smaller than the difference observed for H2O? Why is the deviation between the real and model structure different for SO2compared to H2O? The deviation for H2O is 5 degrees