< >=ASU Physics, BS | Major Map | ASU Degree SearchO ELECTRONIC STRUCTURE AND CHEMI...Deducing n and I from a subshell labelsubshell1sAA3dComplete the table below by filling in the principal quantum number nand angular momentum quantum number / for each electron subshelllisted.4fExplanationprincipalquantum number nCheckwww-awa.aleks.com00A ALEKS - Andrew Herrera - Learnangular momentumquantum number /0/3Andrew?扁alloArⒸ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility =O ELECTRONIC STRUCTURE AND CHEMI...Deducing n and I from a subshell labelJural momentum quantum number Toi cachi ciecLION SUpsniemaltalisteu.subshell1s3d4f4sExplanationprincipalquantum number nCheck00angular momentumquantum number /0X0/3Andrew?oloAr© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

General representation of subshell: nl n = principal quantum numberl = angular momentum quantum…

Answered: subshell 1s 3d 4f 45 principal quantum…

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subshell 1s 3d 4f 45 principal quantum number n angular momentum quantum number / 0 0 0 X

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter5: Quantum Mechanics And Atomic Structure

Section: Chapter Questions

Problem 6P: Using Table 5.2, write down the mathematical expression for the 2px wave function for an...

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For the Li atom, the energy difference between the ground state and the first excited state, in which the outermost electron is in a 2p orbital, is 2.961019J . In the Li2+ ion, the energy difference between the 2s and 2p levels is less than 0.00002 of this value. Explain this observation.
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.)
In the Brackett series, nlo=4. (a) Calculate the wavelength in nanometers of a transition from n=6 to n=4. (b) In what spectral region are these lines formed?
Suppose that the spin quantum number had three allowed values (ms=0,+12,12) . Give the atomic numbers of the first three noble-gas atoms in this case.
What are the values of E, L, and Lz for an F8+ atom whose electron has the following wavefunctions, listed as n,l,ml? a 1,0,0 b 3,2,2c 2,1,1d 9,6,3.
The helium ion He+ is a one-electron system whose wave functions and energy levels are obtained from those for H by changing the atomic number to Z=2 . Calculate the average distance of the electron from the nucleus in the 2s orbital and in the 2p orbital. Compare your results with those in Problem 11 and explain the difference.
A particle of mass m is placed in a three-dimensional rectangular box with edge lengths 2L, L, and L. Inside the box the potential energy is zero, and outside it is infinite; therefore, the wave function goes smoothly to zero at the sides of the box. Calculate the energies and give the quantum numbers of the ground state and the first five excited states (or sets of states of equal energy) for the particle in the box.
Chapter 3 introduced the concept of a double bond between carbon atoms, represented by C=C , with a length near 1.34 Å. The motion of an electron in such a bond can be treated crudely as motion in a one-dimensional box. Calculate the energy of an electron in each of its three lowest allowed states if it is confined to move in a one-dimensional box of length 1.34 Å. Calculate the wavelength of light necessary to excite the electron from its ground state to the first excited state.
Using a simple particle-in-a-box model for the multiple bonding in 1,2-butadiene (see Example 4.7) and the n=2 wave function for the weakest bound electron, calculate the probability of finding the electron in an 0.1 interval centered midway between the two inner carbon atoms (that is, the center is at x=2.11 , so this interval is from x1=2.06 to x2=2.16 ). Then calculate the probability of finding the electron in an 0.1 interval centered midway between an end carbon atom and the carbon atom that is double-bonded to it in the Lewis dot structure. (You may calculate the appropriate integrals or estimate the relevant areas under the curve graphically.) Then recalculate the probabilities by approximating the integral as |( x 0)|2x , where x0 is evaluated in the middle of the range from x1 to x2 . Finally, explain why you can’t approximate the integral needed for Problem 37(a) in this way.
In a FranckHertz experiment on sodium atoms, the first excitation threshold occurs at 2.103 eV. Calculate the wavelength of emitted light expected just above this threshold. (Note: Sodium vapor lamps used in street lighting emit spectral lines with wavelengths 5891.8 and 5889.9 Å.)
Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
The maximum in the blackbody radiation intensity curve moves to shorter wavelength as temperature increases. The German physicist Wilhelm Wien demonstrated the relation to be max1/T . Later, Planck’s equation showed the maximum to be max=0.20hc/kt . In 1965, scientists researching problems in telecommunication discovered “background radiation” with maximum wavelength 1.05 mm (microwave region of the EM spectrum) throughout space. Estimate the temperature of space.