8. Write all the possible quantum sets for electron with the following restrictions. If no sets can be written state that and why. A. n=2 & l=1 B. n=3 & l=0 C. n= 4 & 1=3 & s= ½ D. n=6 & 1 =1 & m = -1 %3D E. n=2 &1 = 2 F. n=3 &1=2 & mj =-3

8. Write all the possible quantum sets for electron with the following restrictions. If no sets can be written state that and why. A. n=2 & l=1 B. n=3 & l=0 C. n= 4 & 1=3 & s= ½ D. n=6 & 1 =1 & m = -1 %3D E. n=2 &1 = 2 F. n=3 &1=2 & mj =-3

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter2: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 161CP: The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase....

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Question

8. Write all the possible quantum sets for electron with the following
restrictions. If no sets can be written state that and why.
A. n=2 & l=1
B. n=3 & l=0
C. n= 4 & 1=3 & s= ½
D. n=6 & 1 =1 & m = -1
%3D
E. n=2 &1 = 2
F. n=3 &1=2 & mj =-3

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Step 2- A. n = 2, l = 1

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Step 3: B. n = 3, l = 0.

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Step 4: C. n = 4, l = 3, s = +1/2

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Step 5: D. n = 6, l = 1, ml = -1

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Step 6: E. n = 2, l = 2

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Similar questions

The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase. All the lines result from electronic transitions from excited states to the n = 3 state. (See Exercise 160.) a. What electronic transitions correspond to lines A and B? b. If the wavelength of line B is 142.5 nm, calculate the wavelength of line A.
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?
How do 2p orbitals differ from each other? How do 2p and 3p orbitals differ from each other? What is a nodal surface in an atomic orbital? What is wrong with lp, ld, 2d, lf, 2f, and 3f orbitals? Explain what we mean when we say that a 4s electron is more penetrating than a 3d electron.
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?
Although no currently known elements contain electrons in g orbitals in the ground state, it is possible that these elements will be found or that electrons in excited states of known elements could being orbitals. For g orbitals, the value of l is 4. What is the lowest value of n for which g orbitals could exist? What are tile possible values of ml? How many electrons could a set of g orbitals hold?
What is the maximum number of electrons that can occupy a f subshell (l = 3)?
What are the allowed values for each of the four quantum numbers: n, l, ml, and ms?
• identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.
Consider an electron for a hydrogen atom in an excited state. The maximum wavelength of electromagnetic radiation that can completely remove (ionize) the electron from the H atom is 1460 nm. What is the initial excited state for the electron (n = ?)?
How far from the nucleus in angstroms (1 angstrom =11010 m) is the electron in a hydrogen atom if it has an energy of 8.721020 J?
Imagine a world in which the rule for the l quantum number is that values start with 1 and go up to n. The rules for the n and mi quantum numbers are unchanged from those of our world. Write the quantum numbers for the first two shells (i.e., n = 1 and n = 2).
6.29 A mercury atom emits light at many wavelengths, two of which are at 435.8 and 546.1 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) lf a transition between the two higher energy states could be observed, what would be the frequency of the light?

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