Chapter 3, Part 1 homeworkAnimation-Electron ConfigurationsAnomalous electron configurationsSome atoms, such as some transition metals and some elements in the lanthanide and actinide series, do not adhere strictly to Hund's rule and Pauli's prireason the anomalies are observed is the unusual stability of both half-filled and completely filled subshells. This behavior can be explained with an exampchromium atom. Using Hund's rule and Pauli's principle, you can write the expected electron configuration of the Cr atom that strictly follows these rules a1s2 2s? 2p6 3s2 3p 4s2 3d However, by moving an electron from the 4s orbital to the 3d orbital you obtain a half-filled 3d orbital. This half-filled orbitathan the combination of the filled 4s orbital and the partially filled 3d orbital. Thus; the observed electron configuration of the Cr aton is 1s² 2s² 2p® 3s²Part DMo has an anomalous electron configuration. Write the observed electron configuration of Mo.Express your answer in complete form in order of orbital filling. For example, 1s² 2s should be entered as 1s^225^2.> View Available Hint(s)SubmitPrevious Answerso 77°F Partly cloudyChpprt scdelete&backspace6.8TYUG HJ KpauseB N M

Electronic configuration of molybdenum

us, the observed eléctron configuration of the Cr atom is 1s 2s 2p" 3s Part D Mo has an anomalous electron configuration. Write the observed electron configuration of Mo. Express your answer in complete form in order of orbital filling. For example, 1s 2s should be entered as 1s^22s^2. > View Available Hint(s) Submit Previous Answers 77°F Partly cloudy A

us, the observed eléctron configuration of the Cr atom is 1s 2s 2p" 3s Part D Mo has an anomalous electron configuration. Write the observed electron configuration of Mo. Express your answer in complete form in order of orbital filling. For example, 1s 2s should be entered as 1s^22s^2. > View Available Hint(s) Submit Previous Answers 77°F Partly cloudy A

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter12: Atoms And Molecules

Section: Chapter Questions

Problem 12.1E: In the Stern-Gerlach experiment, silver atoms were used. This was a good choice, as it turned out....

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Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and an orbital (as described by the more modern, wave mechanical picture of the atom).
Section 11.6 uses a "firefly" analogy to illustrate how the wave mechanical modal for the atom differs from Bohr’s. model. Explain this analogy.
In the Stern-Gerlach experiment, silver atoms were used. This was a good choice, as it turned out. Using the electron configuration of silver atoms, explain why silver was a good candidate for being able to observe the intrinsic angular momentum of the electron. Hint: Dont use the aufbau principle to determine the electron configuration of Ag, because its one of the exceptions. Look up the exact electron configuration in a table.
What type of electron orbital (i.e., s, p, d, or f) is designated by (a) n=3,l=1,m l =1?(b) n=5,l=0,m l =0? (c) n=6,l=4,m l =4?
Suppose that the spin quantum number could have the values 12,0 and 12 . Assuming that the rules governing the values of the other quantum numbers and the order of filling sublevels were unchanged, (a) what would be the electron capacity of an s sublevel? a p sublevel? a d sublevel? (b) how many electrons could fit in the n=3 level? (c) what would be the electron configuration of the element with atomic number 8? 17?
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)?
Using a periodic table or Table 12.1, find the elements whose electron configurations do not follow the aufbau principle strictly. Comment on any relationship between these elements or their place within the periodic table.
Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
Chromium(IV) oxide is used in making magnetic recording tapes because it is paramagnetic. It can be described as a solid made up of Cr4+ and O2 . Give the electron configuration of Cr4+ in CrO2 , and determine the number of unpaired electrons on each chromium ion.
Spectroscopic studies show that Li can have electrons in its 1s, 2s, and 2p Hartree orbitals, and that Zeff(2s)=1.28 for the 1s22s1 configuration. Estimate the energy of the 2s orbital of Li. Calculate the average distance of the electron from the nucleus in the 2s orbital of Li.
Which atom would be expected to have a half-filled 4s subshell?