The molecule shown here is difluoromethane (CH2F2), which isused as a refrigerant called R-32. (a) Based on the structure, howmany electron domains surround the C atom in this molecule?(b) Would the molecule have a nonzero dipole moment? (c) Ifthe molecule is polar, which of the following describes the directionof the overall dipole moment vector in the molecule:(i) from the carbon atom toward a fluorine atom, (ii) from thecarbon atom to a point midway between the fluorine atoms,(iii) from the carbon atom to a point midway between the hydrogenatoms, or (iv) from the carbon atom toward a hydrogenatom?

The molecule shown here is difluoromethane (CH2F2), which isused as a refrigerant called R-32. (a) Based on the structure, howmany electron domains surround the C atom in this molecule?(b) Would the molecule have a nonzero dipole moment? (c) Ifthe molecule is polar, which of the following describes the directionof the overall dipole moment vector in the molecule:(i) from the carbon atom toward a fluorine atom, (ii) from thecarbon atom to a point midway between the fluorine atoms,(iii) from the carbon atom to a point midway between the hydrogenatoms, or (iv) from the carbon atom toward a hydrogenatom?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter7: Covalent Bonding

Section: Chapter Questions

Problem 76QAP: In each of the following molecules, a central atom is surrounded by a total of three atoms or...

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The molecule shown here is difluoromethane 1CH2F22, which isused as a refrigerant called R-32. (a) Based on the structure, howmany electron domains surround the C atom in this molecule?(b) Would the molecule have a nonzero dipole moment? (c) Ifthe molecule is polar, which of the following describes the directionof the overall dipole moment vector in the molecule:(i) from the carbon atom toward a fluorine atom, (ii) from thecarbon atom to a point midway between the fluorine atoms,(iii) from the carbon atom to a point midway between the hydrogenatoms, or (iv) from the carbon atom toward a hydrogenatom? [Sections 9.2 and 9.3]9.5
(a) Is the molecule BF3 polar or nonpolar? (b) If you react BF3to make the ion BF32-, is this ion planar? (c) Does the moleculeBF2Cl have a dipole moment?
Ethyl acetate, C4H8O2, is a fragrant substance used both as asolvent and as an aroma enhancer. Its Lewis structure is (a) What is the hybridization at each of the carbon atomsof the molecule? (b) What is the total number of valenceelectrons in ethyl acetate? (c) How many of the valence electronsare used to make s bonds in the molecule? (d) Howmany valence electrons are used to make p bonds? (e) Howmany valence electrons remain in nonbonding pairs in themolecule?
Consider the Lewis structure shown below.(a) Does the Lewis structure depict a neutral molecule or anion? If it is an ion, what is the charge on the ion? (b) What hybridizationis exhibited by each of the carbon atoms? (c) Arethere multiple equivalent resonance structures for the species?(d) How many electrons are in the p system of the species?
The substance chlorine monoxide, ClO(g), is important inatmospheric processes that lead to depletion of the ozonelayer. The ClO molecule has an experimental dipole momentof 1.24 D, and the Cl¬O bond length is 1.60 Å. (a)Determine the magnitude of the charges on the Cl and Oatoms in units of the electronic charge, e. (b) Based on theelectronegativities of the elements, which atom would youexpect to have a partial negative charge in the ClO molecule?(c) Using formal charges as a guide, propose the dominantLewis structure for the molecule. (d) The anion ClOexists.What is the formal charge on the Cl for the best Lewisstructure for ClO-?
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 structure of caffeine is shown below. (a) Complete the Lewis structure. (b) How many pi bonds are present in caffeine? How many sigma bonds? (c) Identify the hybridization of the carbon atoms. (d) What is the value of the O-C-N angle?
The lactic acid molecule, CH3CH(OH)COOH, gives sourmilk its unpleasant, sour taste. (a) Draw the Lewis structurefor the molecule, assuming that carbon always forms fourbonds in its stable compounds. (b) How many π and howmany σ bonds are in the molecule? (c) Which CO bond isshortest in the molecule? (d) What is the hybridization ofatomic orbitals around the carbon atom associated withthat short bond? (e) What are the approximate bond anglesaround each carbon atom in the molecule?
The bond length in the HCl molecule is 1.27 Å. (a) Calculate the dipole moment, in debyes, that results if the charges on theH and Cl atoms were 1+ and 1- respectively. (b) The experimentally measured dipole moment of HCl(g) is 1.08 D. Whatmagnitude of charge, in units of e, on the H and Cl atoms leads to this dipole moment?
(a) How does a polar molecule differ from a nonpolar one? (b) Atoms X and Y have different electronegativities. Will the diatomic molecule X—Y necessarily be polar? Explain. (c) What factors affect the size of the dipole moment of a diatomic molecule?
A useful solvent that will dissolve salts as well as organic compounds is the compound acetonitrile, H3CCN. It is present in paint strippers.(a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule.(b) Identify the hybrid orbitals used by the carbon atoms in the molecule to form σ bonds.(c) Describe the atomic orbitals that form the π bonds in the molecule. Note that it is not necessary to hybridize the nitrogen atom.
The O¬H bond lengths in the water molecule (H2O) are0.96 Å, and the H—O—H angle is 104.5°. The dipole momentof the water molecule is 1.85 D. (a) In what directionsdo the bond dipoles of the O—H bonds point? In what directiondoes the dipole moment vector of the water moleculepoint? (b) Calculate the magnitude of the bond dipoleof the O—H bonds. (Note: You will need to use vector addition to do this.) (c) Compare your answer from part (b)to the dipole moments of the hydrogen halides (Table 8.3).Is your answer in accord with the relative electronegativityof oxygen?