The following do not represent valid ground-state electron configurations for an atom either because they violate the Pauli exclusion principle or because orbitals are not filled in order of increasing energy. Indicate which of these two principles is violated in each example or whether both or neither are violated. Drag the appropriate items to their respective bins. Reset Help Ne]3s²3d [Xe]6s25dª |1s 2s²3s' Only the Pauli exclusion principle is violated Both the Pauli exclusion Only the order of filling by energy is violated Neither the Pauli exclusion principle and the order of filling by energy are violated principle nor the order of filling by energy is violated

The following do not represent valid ground-state electron configurations for an atom either because they violate the Pauli exclusion principle or because orbitals are not filled in order of increasing energy. Indicate which of these two principles is violated in each example or whether both or neither are violated. Drag the appropriate items to their respective bins. Reset Help Ne]3s²3d [Xe]6s25dª |1s 2s²3s' Only the Pauli exclusion principle is violated Both the Pauli exclusion Only the order of filling by energy is violated Neither the Pauli exclusion principle and the order of filling by energy are violated principle nor the order of filling by energy is violated

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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Identify the 4 quantum numbers that can represent the last electron added to a Sr atom (use the Aufbau Principle)
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Identify the neutral element represented by this excited‑state electron configuration, then write the ground‑state electron configuration for that element. excited state: 1s22s12p03s1
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How many different values of ml are possible when the principal quantum number is n = 32? Group of answer choices 65 0 63 62
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What is wrong with the following set of quantum numbers? n = 2, l = 1, ml = -2, ms = +1/2 A. ml must be greater than or equal to l. B. l must be greater than or equal to n. C. l has a maximum value of n–1. D. ms must be 0 or 1. E. ml only has values equal to -l,0,+l
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