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Dichlorobenzene, C6H4Cl2, exists in three forms (isomers)
called ortho, meta, and para:
Which of these has a nonzero dipole moment? Explain.
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- Dichloroethylene (C2H2Cl2) has three forms (isomers), eachof which is a different substance. (a) Draw Lewis structures ofthe three isomers, all of which have a carbon–carbon doublebond. (b) Which of these isomers has a zero dipole moment?(c) How many isomeric forms can chloroethylene, C2H3Cl,have? Would they be expected to have dipole moments?Dichlorobenzene, C6H4Cl2, exists in three forms (isomers)called ortho, meta, and para:Which of these has a nonzero dipole moment?Consider a molecule with formula AX3. Supposing the A¬Xbond is polar, how would you expect the dipole moment ofthe AX3 molecule to change as the X¬A¬X bond angle increasesfrom 100° to 120°?
- 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 p2p 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?Acetylsalicylic acid, better known as aspirin, has the Lewisstructure (a) What are the approximate values of the bond angles labeled1, 2, and 3? (b) What hybrid orbitals are used about thecentral atom of each of these angles? (c) How many s bondsare in the molecule?The bond between carbon and hydrogen is one of the most important typesof bonds in chemistry. The length of an H¬C bond is approximately 1.1 Å.Based on this distance and differences in electronegativity, do you expect thedipole moment of an individual H¬C bond to be larger or smaller than that ofan H¬I bond?
- 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?Ozone, O3, has a small dipole moment of 0.54 D (1D= 3.34x10-30 coulumb meters). How can a molecule with only one kind of atom have a dipole moment? What is the lewis structure that cooresponds to O3? What is or are the hybridizations of the oxygen atoms? What are the formal charges of each oxygen?Consider the Lewis structure for glycine, the simplest aminoacid: (a) What are the approximate bond angles about each of thetwo carbon atoms, and what are the hybridizations of the orbitalson each of them? (b) What are the hybridizations ofthe orbitals on the two oxygens and the nitrogen atom, andwhat are the approximate bond angles at the nitrogen? (c)What is the total number of σ bonds in the entire molecule,and what is the total number of π bonds?
- Consider the following XF4 ions: PF4-, BrF4-, ClF4+, and AlF4-.(a) Which of the ions have more than an octet of electronsaround the central atom? (b) For which of the ions will theelectron-domain and molecular geometries be the same?(c) Whi ch of the ions wi l l have an oc t ahedralelectron-domain geometry? (d) Which of the ions willexhibit a see-saw molecular geometry?The AF, species are shown as follows, BF;; CF4; NF3; OF2. (i) Draw the Lewis structure for each of the above AF, species. (ii) Determine the molecular geometry for each of the above AF, species. (iii) Arrange the AFn species in the order of increasing bond angle. Explain your answer. (iv) Determine the hybridisation of the central atom for BF3 and NF3 respectively.Does COS have a dipole moment? Explain.