O REPRESENTATIONS OF ORGANIC MOLECULES Identifying isomers and resonance structures Determine the relationship between Structure A and Structure B in each row of the table. Structure A Structure B Relationship isomers :0: н н : H .C. TH. H. resonance structures H. H H HH H o neither isomers нн HH H- -Ċ-NEN: -Ċ-H O resonance structures H O neither O isomers ö=N=ö O resonance structures o neither

O REPRESENTATIONS OF ORGANIC MOLECULES Identifying isomers and resonance structures Determine the relationship between Structure A and Structure B in each row of the table. Structure A Structure B Relationship isomers :0: н н : H .C. TH. H. resonance structures H. H H HH H o neither isomers нн HH H- -Ċ-NEN: -Ċ-H O resonance structures H O neither O isomers ö=N=ö O resonance structures o neither

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 53QRT

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A paper published in the research Journal Science in 2007 (S. Vallina and R. Simo, Science, Vol. 315, p. 506, January 26, 2007) reported studies of dimethylsulfide (DMS), an important green-house gas that is released by marine phytoplankton. This gas represents the largest natural source of atmospheric sulfur and a major precursor of hygroscopic (i.e., cloud-forming) particles in clean air over the remote oceans, thereby acting to reduce the amount of solar radiation that crosses the atmosphere and is absorbed by the ocean. (a) Sketch the Lewis structure of dimethylsulfide, CH3SCH3, and list the bond angles in the molecule. (b) Use electronegativities to decide where the positive and negative charges lie in the molecule. Is the molecule polar? (c) The mean seawater concentration of DMS in the ocean in the region between 15 north latitude and 15 south latitude is 2.7 nM (nanomolar). How many molecules of DMS are present in 1.0 m3 of seawater?
See the Attached compound A. Ques: Label the strongest C–H bond.
Consider Lewis formulas A, B, and C:(a) Are A, B, and C constitutional isomers, or are they resonance contributors? (b) Which have a negatively charged carbon? (c) Which have a positively charged carbon? (d) Which have a positively charged nitrogen? (e) Which have a negatively charged nitrogen? (f) What is the net charge on each? (g) Which is a more stable structure, A or B? Why? (h) Which is a more stable structure, B or C? Why? (i) What is the CNN geometry in each according to VSEPR?
#1: What is the formal charge of bromine in the structure of bromate, BrO3-? a) 0 b) +1 c) +2 d) -1 #2: Carbonate (CO32-) has three resonance structures. Choose the stayement that best expains the meaning of those 3 resonance structures. a) Carbonate consists of two single CO bonds and one double CO bond. b) Carbonate consists of one single structure which is an average of the three resonance structures. c) Carbonate quickly flips back and forth between three structures. d) Three different structures for carbonate coexist. #3: When compaing a carbon-carbon double bond (C==C) and a carbon-carbon single bond (C-C), the double bond is a) longer and shorter b) longer and weaker c) shorter and stronger d) shorter and weaker
The partial Lewis structure that follows is for a hydrocarbonmolecule. In the full Lewis structure, each carbon atomsatisfies the octet rule, and there are no unshared electronpairs in the molecule. The carbon—carbon bondsare labeled 1, 2, and 3. (a) How many hydrogen atomsare in the molecule? (b) Rank the carbon–carbonbonds in order of increasing bond length. (c) Whichcarbon—carbon bond is the strongest one?
1. Conjugated radicals, ions, or molecules are more stable than non-conjugated ones, why? 2. Charge separation decreases stability, why? 3. Structures in which all of the atoms have a complete valence shell of electrons are especially stable and make large contributions to the hybrid, why?
(a) Compare the bond enthalpies (Table 8.3) of the carbon–carbon single, double, and triple bonds to deduce an averageπ -bond contribution to the enthalpy. What fraction ofa single bond does this quantity represent? (b) Make a similarcomparison of nitrogen–nitrogen bonds. What do youobserve? (c) Write Lewis structures of N2H4, N2H2, and N2,and determine the hybridization around nitrogen in eachcase. (d) Propose a reason for the large difference in yourobservations of parts (a) and (b).
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.
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).
Which of the following would you expect to be more favorable energetically? Explain. a. an H2 molecule in which enough energy is added to excite one electron from the bonding to the antibonding MO b. two separate H atoms
Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?
The bond energy of a C—C single bond averages 347 kJ mol-1; that of a CC triple bond averages 839 kJ mol-1. Explain why the triple bond is not three times as strong as a single bond.