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

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...

See similar textbooks

Similar questions

1. How many f orbitals can have the value n=3? Answer 2. How many electrons in an atom can have the following designations? n=5 and ml=2? Answer W3. hat is the short hand electron configurations for Bi? When writing your answer do not put in any spaces ex: [He]2s22p1.
None
← → C tab esc Aktiv Chemistry 2 app.101edu.co Provide the quantum numbers and related information for the following orbital, 3d. What is the maximum number of electrons in the entire shell? 1 0: F1 Q A 300 (8) X 2 OCT 25 F2 + W S #3 80 F3 E - D $ 4 Question 17.e of 24 F4 R % 5 LL CZEN F5 MacBook Air T 6 F6 G & Y 7 4 F7 1 D 4 7 +/- H 8 U
5c ASALP
It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy (in kJ) for a mole of hydrogen atoms, making the assumption that ionization is thetransition from n = 1 to n = 00(infinity)
pject) - ketelk@oreg X Blank 2 E Chemistry: Atoms First 2e xo Chem101 Osu MyOreg A app.101edu.co M Gmail O YouTube Question 18 of 47 What is the wavelength of light (in nm) emitted when an electron transitions from n = 5 to n = 2 in a hydrogen atom? Submit an answer to three signficant figures. MacBook Air
Edit View History Bookmarks Profiles Tab Mopu!M Help se Info x EChemistry x 3.1 Electro x 3.3 Develo x o Chem101 X p.101edu.co YouTube News Question 27 of 47 Which of the following sets of quantum numbers is not allowed? A)n 2, { = 0, ml = 0 C)n 2, { = 2, ml = 2 D) n = 3, { = 1, ml = -1 E) n =4, { = 2, mł = 1
How can we compute the ionization energy of hydrogen atom?