P Course Homee MasteringChemistry: Post Lectur Xv?assignmentProblemlD=146110541&offset-nextFree Article Rewrite,EssayTyper 6 6 Assignment Hel.sm...O Hire/Pay Sumeone.O Get RegisCHM 1045Part DHow would the d orbital in the n5 sholl compare to the d,2 orbital in the n = 3 subshell?A. The contour of the orbital would extend further out along the z and y axcs.B. The valueC The radial probabdity function would nclude two more nodosD. The orientaion of tho orbital would be rotated 45° along the xy plane.E The me value would be the samo.f would increase by 2Drag the appropriate items to their respective bins.> View Available Hint(s)Reset HelpTrueFalscF10F11F12PriScScr LkSysRqB.

How would the d or bital in the n 5 sholl compare to the d-ya orbital in tho = 3 subshall? A The contour of ere orbital would extend further out along the z und y axes. B. Tho value ul E would increase by 2. C The radial prohablity lunction would nclude two more nodos D. The orientabon of the orbital would be rotatod 45° alang the xy plane. F The me valuo would be the same

How would the d or bital in the n 5 sholl compare to the d-ya orbital in tho = 3 subshall? A The contour of ere orbital would extend further out along the z und y axes. B. Tho value ul E would increase by 2. C The radial prohablity lunction would nclude two more nodos D. The orientabon of the orbital would be rotatod 45° alang the xy plane. F The me valuo would be the same

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

Chapter7: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 180CP: Answer the following questions, assuming that ms, could have three values rather than two and that...

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Which of the subshells described in the previous question contain degenerate orbitals? How many degenerate orbitals are in each?
(a) The nitrogen atom has one electron in each of the 2px , 2py , and 2pz orbitals. By using the form of the angular wave functions, show that the total electron density, 2(2px)+2(2py)+2(2pz) , is spherically symmetric (that is, it is independent of the angles and ). The neon atom, which has two electrons in each 2p orbital, is also spherically symmetric. (b) The same result as in part (a) applies to d orbitals, thus a filled or half-filled subshell of d orbitals is spherically symmetric. Identify the spherically symmetric atoms or ions among the following: F , Na, Si, S2,Ar+ , Ni, Cu, Mo, Rh, Sb, W, Au.
When metallic sodium is dissolved in liquid sodium chloride, electrons are released into the liquid. These dissolved electrons absorb light with a wavelength near 800 nm. Suppose we treat the positive ions surrounding an electron crudely as defining a three-dimensional cubic box of edge L, and we assume that the absorbed light excites the electron from its ground state to the first excited state. Calculate the edge length L in this simple model.
Identify the element that corresponds to each of the simplified photoelectron spectral data given below. (Energy data taken from D. A. Shirley, R. L Martin, S. P. Kowalczyk. F. R. McFeely, and L. Ley: Core-electron binding energies of the first thirty elements, Physical Review B, Vol. 15, pp. 544-552, 1977.) (a) There are peaks at energies of 64.8 and 5.4 eV, corresponding to 2 and 1 electrons, respectively. (b) There are peaks at energies of 3614, 384, 301, 40.9, 24.7, and 4.34 eV, corresponding to 2, 2, 6, 2, 6, and 1 electrons, respectively. (c) There are peaks at energies of 4494, 503, 404, 56.4, 33.6, 8.01, and 6.65 eV, corresponding to 2, 2, 6, 2, 6, 1, and 2 electrons, respectively.
Identify the element that corresponds to each of the simplified photoelectron spectral data given below. (Energy data taken from D. A. Shirley, R. L. Martin, S. P. Kowalczyk. F. R. McFeely, and L Ley: Core-electron binding energies of the first thirty elements Physical Review B, Vol. 15, pp. 544-552, 1977.) (a) There are peaks at energies corresponding to 1079, 70.8, 38.0, 5.14 eV, corresponding to 2, 2, 6, and 1 electrons, respectively. (b) There are peaks at energies corresponding to 4043, 443, 351, 48.4, 30.1, and 6.11 eV, corresponding to 2, 2, 6, 2, 6, and 2 electrons, respectively. (c) There are peaks at energies corresponding to 5475, 638, 524, 77, 47, 12. and 7.3 eV, corresponding to 2, 2, 6, 2, 6, 3, and 2 electrons, respectively.
Answer the following questions, assuming that ms, could have three values rather than two and that the rules for n, l, and ml are the normal ones. a. How many electrons would an orbital be able to hold? b. How many elements would the first and second periods in the periodic table contain? c. How many elements would be contained in the first transition metal series? d. How many electrons would the set of 4f orbitals be able to bold?
Spectroscopic studies show that Na can have electrons in its 1s, 2s, 2p, and 3s Hartree orbitals, and that Zeff(3s)=1.84 . Using data from Problem 13, compare the energies of the Na 3s orbital, the Li 2s orbital, and the H 1s orbital.
Consider the orbitals shown here in outline. (a) What is the maximum number of electrons contained in an orbital of type (x)? Of type (y)? Of type (z)? (b) How many orbitals of type (x) are found in a shell with n=2? How many of type (y)? How many of type (z)? (c) Write a set of quantum numbers for an electron in an orbital of type (x) in a shell with n=4, of an orbital of type (y) in a shell with n=2. Of an orbital of type (z) in a shell with n=3. (d) What is the smallest possible n value for an orbital of type (x)? Of type (y)? Of type (z)? (e) What are the possible I and ml values for an orbital of type (x)? Of type (y)? Of type (z)?
What is the maximum number of orbitals that can be identified by each of the following sets of quantum numbers? When none is the correct answer, explain your reasoning. (a) n = 4, = 3 (b) n = 5 (c) n = 2, = 2 (d) n = 3, = 1, m = 1
Estimate the probability of finding an electron which is excited into the 2s orbital of the H atom, looking in a cubical box of volume 0.751036m3 centered at the nucleus. Then estimate the probability of finding the electron if you move the volume searched to a distance of 105.8 pm from the nucleus in the positive z direction. (Note that since these volumes are small, it does not matter whether the volume searched is cubical or spherical.)
Until recently, it was thought that Ca was unstable, and that the Ca atom therefore had a negative electron affinity. Some new experiments have now measured an electron affinity of +2.0kJmol1 for calcium. What is the longest wavelength of light that could remove an electron from Ca ? In which region of the electromagnetic spectrum does this light fall?
Using data from Problems 13 and 15, calculate the average distance of the electron from the nucleus in the Na 3s orbital, the Li 2s orbital, and the H 1s orbital. Explain the trend in your results.