Anomalous 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 principle. The reason the anomalies are observed is the unusual stability of both half-filled andcompletely filled subshells. This behavior can be explained with an example of the chromium 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 as1s? 2s? 2pº 3s? 3p 4s? 3d4 . However, by moving an electron from the 4s orbital to the 3d orbital you obtain a half-filled 3d orbital. This half-filled orbital is more stable than the combination of the filled 4s orbital and the partially filled 3d orbital.Thus, the observed electron configuration of the Cr atom is 1s? 2s 2p® 3s² 3p® 4s' 3d³.Part DAg has an anomalous electron configuration. Write the observed electron configuration of Ag.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)

The atomic number of Ag is 47. So the electronic configuration of Ag is 1s2, 2s2, 2p6, 3s2, 3p6,…

Part D Ag has an anomalous electron configuration. Write the observed electron configuration of Ag. Express your answer in complete form in order of orbital filling. For example, 1s° 25° should be entered as 15^225^2. • View Available Hint(s)

Part D Ag has an anomalous electron configuration. Write the observed electron configuration of Ag. Express your answer in complete form in order of orbital filling. For example, 1s° 25° should be entered as 15^225^2. • View Available Hint(s)

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...

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I am trying to learn noble gas electron configurations, but I am confused because I am seeing different orders of doing the notations than what I was seeing when doing the ground state (normal) electron configurations. For example, I was trying to do the noble gas electron configuration for cadmium, and using the chart I came up with: [Kr] 5s^2 4d^10 But then, I wanted to check to make sure that I was right so I googled it, and it was a different answer?? It flipped it around and said that the correct configuration was: [Kr] 4d^10 5s^2 So then I was super confused and watched a video to see if they would explain why you do it in a different way, but then the guy in the video did it the way I originally did it!? And so I kept looking and now I am seeing two different answers online. It seems whenever a noble gas electron configuration involves anything from D block, they put D block first in the configuration. But then again, some people aren’t doing it this way. Could somebody…
C Express your answer in complete form in the order of orbital filling as a string without blank space between orbitals. For example, 1s22s21s22s2 should be entered as 1s^22s^2.
F− Express your answer in complete form, in order of increasing orbital. For example, 1s22s2 would be entered as 1s^22s^2.
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