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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Suppose an atom with its nucleus at the origin has an electron in a 1s orbital. Complete each row of the table below by deciding how PA, the probability of finding the electron at point A, compares to PB, the probability of finding the electron at point B. This sketch is about 200 pm wide. The coordinate (x, y, and z) axes are also shown. You can rotate the sketch for a better view of the orbital by dragging the slider with your mouse. point A 10 pm to the left of the nucleus, along the -x axis. 10 pm in front of the nucleus, along the -y axis. Continue 10 pm to the right of the nucleus, along the +x axis. point B 10 pm behind the nucleus, along the +y axis. 10 pm below the nucleus along the -z axis. 10 pm above the nucleus, along the +z axis. compare PA to PB OP PA P OPA B O PA
03. When an electron makes a transition from the n = 3 to the n = 2 hydrogen atom Bohr orbit, the energy differ- ence between these two orbits (3.0 × 10-¹⁹J) is emitted as a photon of light. The relationship between the energy of a photon and its wavelength is given by E = hc/λ, where E is the energy of the photon in J, h is Planck's constant (6.626 × 10-34 J·s), and c is the speed of light (3.00 × 108 m/s). Find the wavelength of light emitted by hydrogen atoms when an electron makes this transition
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OWLV2 | Online teaching and X 0mySigTau xb Login | bartleby M COMM.1113: FUND OF ORA X G what food has C- Google Se X + com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take [References] Assume that a hydrogen atom's electron has been excited to the n = 3 level. How many different wavelengths of light can be emitted as this excited atom loses energy? different wavelengths Submit Answer Try Another Version 3 item attempts remaining
. A student was asked to write the electron configuration for a number of elements on an exam. Here is a sample of some of their answers: a) Ne s2 b) 1s22s3 c) [Kr] 4s1 Select any 2 of the answers above, and explain what is wrong. What element do you think they were describing? Write the correct electron configuration for that element.
Ionization energy is the energy needed to eject an electron from an atom. Compute the ionization energy of a hydrogen atom in its second excited state (n = 3). E = J
Suppose an atom with its nucleus at the origin has an electron in a 2p, orbital. Complete each row of the table below by deciding how P A' the probability of finding the electron at point A, compares to P the probability of finding the electron at point B. B' point A point B compare PA to PB O 'A Р. A В A В P = P 100 pm behind the nucleus, along the +y axis. 100 pm to the left of the nucleus, along the -x axis. A В Р. > Р. A В P Р A В
Consider a hydrogen atom in the ground state. What is the energy of its electron? E = Now consider an excited-state hydrogen atom. What is the energy of the electron in the n = 3 level? E3 = PAGES · O J J
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The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. For an electron in the 2p orbital shown above, enter a possible value for each quantum number. n = 1 = Give ONE example. Give ONE example. Though a given electron only has one value for ▸ possible mi, there are my values for electrons in 2p orbitals. m₁ = mg =
i 1 Z I 1 1 X 1 This sketch is about 1800 pm wide. The coordinate (x, y, and z) axes are also shown. You can rotate the sketch for a better view of the orbital by dragging the slider with your mouse. Suppose an atom with its nucleus at the origin has an electron in a 3d, orbital. Complete each row of the table below by deciding how PA the probability c finding the electron at point A, compares to PB, the probability of finding the electron at point B. point A 200 pm in front of the nucleus, along the -y axis. 200 pm above the nucleus, along the +z axis. 200 pm to the right of the nucleus, along the +x axis. point B 200 pm behind the nucleus, along the +y axis. 200 pm below the nucleus along the -z axis. 200 pm to the left of the nucleus, along the -x axis. compare PA to PB B O P P A PA PA PB P P A B
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