How would the d,2_2 orbital in the n = 5 shell compare to the d,2 12 orbital in the n 3 shell? 1. The orbital in the n = 5 shell is bigger than the orbital in the n = 3 shell. 2. The value of / would increase by 2 for the n = 5 shell. 3. The value of / for both orbitals would be the same. 4. The orientation of the n = 5 orbital would be rotated 45° along the xy plane. 5. The me value for both orbitals would be the same. %3D Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help P Pearson r Copyright O2020 Pearson Education Inc. All rights reserved. I Terms of Use I P

How would the d,2_2 orbital in the n = 5 shell compare to the d,2 12 orbital in the n 3 shell? 1. The orbital in the n = 5 shell is bigger than the orbital in the n = 3 shell. 2. The value of / would increase by 2 for the n = 5 shell. 3. The value of / for both orbitals would be the same. 4. The orientation of the n = 5 orbital would be rotated 45° along the xy plane. 5. The me value for both orbitals would be the same. %3D Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help P Pearson r Copyright O2020 Pearson Education Inc. All rights reserved. I Terms of Use I P

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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Bohr's model of the atom is a system consisting of a small, dense nucleus surrounded by orbiting electrons. How does Bohr's model explain spectral emission lines? Bohr developed a formula (shown below) that predicted the wavelength of a photon given off when an electron moves from one orbit to another orbit. His formula worked well to explain spectral emission lines in the hydrogen atom. Calculate the wavelength of light that would be emitted for the orbital transition of n = 2 to n = 1. Submit an answer to four significant figures ninitial Mfinal = R Rm = 1.09678 x 107 m-'
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How many nodes are there in the 1s, 2p, and 3d orbitals? How many nodes are in a 4f orbital? Match the words in the left column to the appropriate blanks in the sentences on the right. a node two nodes four three more less five two Reset Help The 1s orbital does not have any nodes. The 2p orbitals have the 3d orbitals have a cloverleaf shape, with lobes of electron density around the nucleus and two perpendicular nodal planes. The f orbitals are even more complex. The number of nodes (and nodal planes) depends on the specific orbital, but there will be than for s, p, or d orbitals. at the nucleus. Four of
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