Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Transcribed Image Text:III
Structure and Bonding
Drawing the second best resonance structure
3/5
Shown below is the major resonance structure for a molecule. Draw the second best resonance structure of the molecule. Include all non-zero formal charges.
H H
H
xx
H
C
H
Click and drag to
start drawing a
structure.
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- Carbon monoxide (CO) is an example of an overall neutral molecule (netcharge=0) that hasnon-zero formal charges. Draw a Lewis structure of carbon monoxide (CO).arrow_forwardBased 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)?arrow_forwardThe 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.arrow_forward
- A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain.arrow_forwardThe percent ionic character of a bond can be approximated by the formula 16+3.52 , where is the magnitude of the difference in the electronegativities of the atoms (see Fig. 3.18). Calculate the percent ionic character of HF, HCl, HBr, HI, and CsF, and compare the results with those in Table 3.7.arrow_forwardPlease draw all Lewis dot structures for each species below. Ifthere is more than one, please circle which you’d argue is thebest structure. Also denote the formal charges for each atom.arrow_forward
- rd Font Paragraph Styles Edit SO2 NO2 PF3 Sil4 Crude Sketch Calculations (# of valence electrons, # of bonds, etc. Lewis Structure # electron groups, electron group geometry 以 D, Focus 目 目 圈 18 2428 words P Type here to search 梦 。 85°F A O hparrow_forwardPrevious Page 5 of 16 Next O References Use the References to access important values if needed for this question. The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. :CI: :ci: :CI-P-CI: Based on the Lewis structure given, the formal charge on the central phosphorus atom is 453 F 4/21/2 FLV Type here to search prt sc delete home en fio 11 esc & + backspace lock %23 81 9. %24arrow_forwardGive a clear handwritten answer with explanationarrow_forward
- Draw the second best resonance structurearrow_forwardNhy is resonance structure A and resonance structure B not the same structure? If you rotate the molecule like a spicket handle (l. e. clockwise with the C at the center and the R group remaining in place as you look down the C - R bond) wouldn't you get the same thing? Why are these not equivalent structures? Resonance structure A t Resonance structure B Actual structurearrow_forwardWhich of these best descibe formal charge? Select all that apply. The difference between the number of electrons around an atom in the free state and the number of electrons assigned to the atom in the Lewis structure an atom in a chemical compound. O The formal charge of each atom is calculated by subtracting the number of valence electrons in the neutral atomfrom the number of electrons assigned to the atom. O Can be used to help determine the most reasonable distribution of electrons in a molecule or ion. O The charge that an atom in a molecule or ion would have if all atoms had the same electronegativity.arrow_forward
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