Show the orbital-filling diagram for N (nitrogen). Order subshells by energy, with the lowest-energy subshell at the left.Drag the appropriate labels to their respective targets.View Available Hint(s)ResetHelp1L11s2s2p3sЗрG1G1G1G1G1G1G1G1G1G2G2G2G2G2 Part CShow the orbital-filling diagram for S (sulfur). Order subshells by energy, with the lowest-energy subshell at the left.Drag the appropriate labels to their respective targets.View Available Hint(s)HelpReset1L11s2s2p3sЗрG1G1G1G1G1G1G1G1G1G2G2G2G2G2

The orbital filling diagram for nitrogen atom is given by,

Answered: Show the orbital-filling diagram for N…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter11: Quantum Mechanics: Model Systems And The Hydrogen Atom

Section: Chapter Questions

Problem 11.82E

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Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
Spectroscopic studies show that Li can have electrons in its 1s, 2s, and 2p Hartree orbitals, and that Zeff(2s)=1.28 for the 1s22s1 configuration. Estimate the energy of the 2s orbital of Li. Calculate the average distance of the electron from the nucleus in the 2s orbital of Li.
How many nodal planes exist for a 5d orbital? (a) 0 (b) 1 (c) 2 (d) 3
For the Li atom, the energy difference between the ground state and the first excited state, in which the outermost electron is in a 2p orbital, is 2.961019J . In the Li2+ ion, the energy difference between the 2s and 2p levels is less than 0.00002 of this value. Explain this observation.
Show the orbital-filling diagram for NN (nitrogen). Order subshells by energy, with the lowest-energy subshell at the left. Drag the appropriate labels to their respective targets.
Show the orbital-filling diagram for S (sulfur). Order subshells by energy, with the lowest-energy subshell at the left. Drag the appropriate labels to their respective targets.
Determine the Γred for the six H 1s orbitals in B2H6. Rationalize the χ value for each operation Please answer very soon will give rating surely
Using complete subshell notation (1s2, 2s², 2p6, and so forth), predict the electron configuration of each of the following i, N³, ii, Ca²+, iii, Cr²+ Note please solve within 30 minutes. Asap.
Of the following choices which electron configuration(s) (in its ground state) is (are) not possible? Answer(s): _______________ a. 1s2 2s2 2p3 b. [Ne] 3s2 3p8 c. [Kr] 5s2 4d10 5p2 d. [Ar] 4s2 3d7 e. All choices are possible
Two possible electron configurationsfor an Li atom are shown here. (a) Doeseither configuration violate the Pauliexclusion principle? (b) Does eitherconfiguration violate Hund’s rule? (c)In the absence of an external magneticfield, can we say that one electron configurationhas a lower energy than theother? If so, which one has the lowestenergy?
Give the EXPECTED abbreviated electron configuration for the ground state of the element shown below and the number of unpaired electrons expected to be in the highest energy subshell for.Enter your answer with subshells in increasing energy order, without superscripts and with spaces between subshells.Example: vanadium (V) = [Ar] 4s2 3d3Abbreviated Electron ConfigurationCobalt (Co): Answer Answer Unpaired ElectronsZirconium (Zr): Answer Answer Unpaired ElectronsTerbium (Tb): Answer Answer Unpaired Electrons
Is it true that the smaller the azimutal quantum number the more penetrating the orbitals? If yes/no why?

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