Consider molecules A and B. (a) In which moleculewould you expect the C-CI bond to be stronger? (b) Inwhich molecule would you expect the C-CI bond to beshorter? (c) In which molecule would you expect thereto be the greater concentration of negative charge on theCl atom? Explain..CICIAB

We will consider both structures one by one -: A. Structure A In structure (A) C-Cl bond is formed…

Answered: Consider molecules A and B. (a) In…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter9: Chemical Bonds

Section: Chapter Questions

Problem 9.94QE

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Three resonance structures are possible for dinitrogen monoxide, N2O. (a) Draw the three resonance structures. (b) Calculate the formal charge on each atom in each resonance structure. (c) Based on formal charges and electronegativity, predict which resonance structure is the most reasonable.
Benzene is commonly regarded as a resonance hybrid ofthe two Kekule structures. but other possible structures canalso contribute. Draw three other structures in which thereare only covalent n bonds (al lowing for bonding betweensome non-adjacent C atoms) and two structures in whichthere is one ionic bond. Why may these structures be ignoredin simple descriptions of the molecule?
A benzene molecule can be modeled as six carbon atoms arrangedin a regular hexagon in a plane. At each carbon atom, one of threeradicals NH2, COOH, or OH can be attached. How many suchcompounds are possible? (Make no distinction between single anddouble bonds between the atoms.)
The compound SF3N has been synthesized.(a) Draw the Lewis diagram of this molecule, supposingthat the three fluoride atoms and the nitrogen atomsurround the sulfur atom. Indicate the formal charges.Repeat, but assume that the three fluorine atoms andthe sulfur atom surround the nitrogen atom.(b) From the results in part (a), speculate about whicharrangement is more likely to correspond to the actualmolecular structure.
I waasnt sure about the sigma and pi bonds sentence. Would they not be broken because they are present in all bonds, no matter the type of IMF?
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?
the actual molecule of which this is a Lewis stricture, which of the labeled distances can change?
What would happen to the energy of the s1s MO if theH atoms in H2 were pulled apart to a distance twice as longas its normal bond length?
Mothballs are composed of naphthalene, C10H8, a moleculethat consists of two six-membered rings of carbonfused along an edge, as shown in this incomplete Lewisstructure:(a) Draw all of the resonance structures of naphthalene.How many are there? (b) Do you expect the C¬C bondlengths in the molecule to be similar to those of C¬Csingle bonds, C“C double bonds, or intermediate betweenC¬C single and C“C double bonds? (c) Not allof the C¬C bond lengths in naphthalene are equivalent.Based on your resonance structures, how many C¬Cbonds in the molecule do you expect to be shorter thanthe others?
The diagram that follows shows the highest-energy occupiedMOs of a neutral molecule CX, where element X is in thesame row of the periodic table as C. (a) Based on the numberof electrons, can you determine the identity of X? (b) Wouldthe molecule be diamagnetic or paramagnetic? (c) Considerthe π2p MOs of the molecule. Would you expect them to havea greater atomic orbital contribution from C, have a greateratomic orbital contribution from X, or be an equal mixtureof atomic orbitals from the two atoms?
Benzene is commonly regarded as a resonance hybrid of the two Kekule structures, but other possible structures can also contribute. Draw three other structures in which there are only covalent π bonds (allowing for bonding between some non-adjacent C atoms) and two st ructu res in which there is one ionic bond. Why may these structures be ignored in simple descriptions of the molecule?
Consider the following ion: BrO3−. What is the electronic geometry of BrO3−? What is its molecular shape? e) Does BrO3− have a dipole moment? Briefly justify your answer. f) On average, would you expect IO3− to have longer or shorter bonds than BrO3−? Briefly explain your answer.

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Consider molecules A and B. (a) In which molecule would you expect the C-CI bond to be stronger? (b) In which molecule would you expect the C-CI bond to be shorter? (c) In which molecule would you expect there to be the greater concentration of negative charge on the Cl atom? Explain. .CI CI A B