Suppose that any given kind of bond, such as 0-H, has a characteristic electric dipole. That is, suppose that elec- tric dipole moments can be assigned to bonds just as bond energies can be. Both are usefully accurate approxi- mations. Consider the water molecule H `H Show that if MOH is the dipole moment of the OH bond, then the dipole moment of water is µ(H2O) = 2µ0H cos (0/2). What is the dipole moment µoH if µ(H,O) is 1.86 D?

Suppose that any given kind of bond, such as 0-H, has a characteristic electric dipole. That is, suppose that elec- tric dipole moments can be assigned to bonds just as bond energies can be. Both are usefully accurate approxi- mations. Consider the water molecule H `H Show that if MOH is the dipole moment of the OH bond, then the dipole moment of water is µ(H2O) = 2µ0H cos (0/2). What is the dipole moment µoH if µ(H,O) is 1.86 D?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

In the following molecule H₂C CH3 the OH has a +1 charge.
Which of the following statements concerning the structures below is/are true? Formal charges are not shown. You can select more than one, or none, of these statements. H A H H-CN Cy ―N=Cy―0 H-Cx-NC,=0: H H B In structure B, the formal charge of N is +1. The oxidation state of N is different for each structure. Structures B and C are nonequivalent resonance structures. In structure C, the formal charge of O is -1. On the basis of formal charges, structure B is more important than structure A. The total charge on this species is -1. 00000C C
Please help me with the answer
The azide ion, N3, is a symmetrical ion, all of whose contributing structures have formal charges. Draw three important contributing Lewis structures for this ion. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all nonbonding electrons. Show the formal charges of all atoms in the correct structure. Q Q Q ? ⒸNNNITY [] + F g i с H N S P Br CI | X Press [TAB] to move to the next option. Press (ALT+A) to get to the bonds and More
Draw three resonance structures for the chlorate ion, Clo -. show formalcharges.
Two possible Lewis structures for the cyanate ion are shown below, with formal charges (FC) calculated for each atom. One structure has carbon as the central atom and the other has a nitrogen as a central atom. By considering formal charges, which arrangement of atoms is the best, and therefore most likely structure for cyanate? FC: -1 0 0 FC: -1 +1 -1 |:0—C=N:1 STRUCTURE A STRUCTURE B Structure A Structure B Both are equally likely QUESTION 19 Two possible Lewis structures for the thiocyanate ion are shown below, with formal charges (FC) calculated for each atom. One structure has carbon as the central atom and the other has a nitrogen as a central atom. By considering formal charges, which arrangement of atoms is the best, and therefore most likely structure for thiocyanate? FC: 00-1 FC: -1 +1 -1 Ec: STRUCTURE A STRUCTURE B O Structure A Structure B
Hello, I want the answer in clear handwriting, please. In which of the following molecules is it necessary to invoke charge-separated resonance structures in order that the central atom obeys the octet rule: (a) H2S; (b) HCN; (c) SO2; (d) AsF5; (e) [BF4]¯; (f) CO2; (g) BRF3.
Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. substance A B C D chemical symbol, chemical formula or Lewis structure H : Cl H Nb Cl5 - N | H : Cl: C : Cl: -D - H · Η Cl I C-H I H boiling point ✓ (Choose one) | (highest) 2 3 4 (lowest) (Choose one) (Choose one) ✓
Carbon monoxide (CO) has a very small dipole moment (0.122) despite having a polar C-O bond. Using resonance structures, please explain this conclusion.
Propane and chlorine react in the presence of UV light to give 2-chloropropane other things: Assuming that the reaction is carried out at a temperature where everything is gaseous, estimate the enthalpy change of reaction from the following bond enthalpies. Bond enthalpy (kJ mol-1) C-H +413 CI-CI +243 C-Cl +346 H-CI +432 C-C +348
A neutral diatomic molecule has a dipole moment of 1.1 D and a bond length of 1.85 Å. What is the magnitude of the charge on each atom? State your answer in units of e (the electron charge). Recall that 1 D = 0.208 eÅ.
For the carbonate ion (CO32-), there are 3 resonance structures. For any given structure what would the formal charge be for an oxygen that has a single bond to the central carbon atom?