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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
Using only the periodic table below, write the expected ground-state electron configurations for
a.) As
b.) Lv
c.) Tungsten
d.) the halogen with electrons in the 6p atomic orbitals.
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- 8. Hund's rule states that a) in the same orbital only 2 electron of opposite spin are possible b) we cannot know the exact position of an electron c) the p orbital must always be filled before the s orbital d) each electron tends to occupy an empty orbital before occupying an orbital which contains another electron 9. Which of the following sets of quantum numbers are impossible? Explain your choice a) (1,0, 0, -½) d) (4,3,-2, +½) b) (3,0,1, +½) e) (3,2,1,1) c) (2,2,1, +½)arrow_forward» Question 2 of 41 Write the complete ground-state electron configuration of copper. For multi-digit superscripts or coefficients, use each number in succession. 1s²2s²2p63s²3pº4s²3d⁹ Incorrect, 1 attempt remaining Recall that a completely full or half-full d-subshells are more stable than a partially filled d subshell. Consider how the s-orbital electrons will help fill the degenerate d-subshells to obtain this stability. Learn More in OpenStax 0 Periodic Table III O Retry <arrow_forward18. Which of the following electron configurations is correct? a) Ga: [Kr]4s²3d04p! b) Mo: [Kr]5s²4d c) Ca: [Ar]4s'3do d) Br: [Ar]4s²3d04p³arrow_forward
- Objectives: a) Define Aufbau principle, Pauli Exclusion Principle, and Hund's Rule. b) List and describe the four quantum numbers. c) Count valence electrons d) Write electron configurationsarrow_forwardHow many 3d electrons would be predicted in the ground state for the following elements? a.) niobium b.) ruthenium c.) osmiumarrow_forward
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