Drag the electrons with the quantum numbers m=0, m =-1/2 into the"electron counter".3d个个个个个4s3s 13p 11 125122p 1 1 1IsSubmitUndoElectron CounterReset

Step 1:The magnetic quantum number (ml) indicates the total number of orbitals in a subshell and the…

Answered: Drag the electrons with the quantum…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 141QRT

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Similar questions

Give the possible values of a. the principal quantum number, b. the angular momentum quantum number, c. the magnetic quantum number, and d. the spin quantum number.
6.85 The visible lines in the hydrogen atom emission spectrum arise from transitions with a final state with n = 2. In what spectral region should we expect to find transitions that have a final state of n = 1 ? Explain your reasoning using an energy level diagram similar to the one in Problem 6.26.
A photoemissive material has a threshold energy, Emin = 5 1019 J. Will 300. nm radiation eject electrons from the material? Explain.
Neutrons are used to obtain images of the hydrogen atoms in molecules. What energy must be imparted to each neutron in a neutron beam to obtain a wavelength of 10.0 pm? Obtain the energy in electron volts (eV) (1 eV = 1.602 1019 J).
Light with a wavelength of 405 nm fell on a strontium surface, and electrons were ejected. If the speed of an ejected electron is 3.36 105 m/s, what energy was expended in removing the electron from the metal? Express the answer in joules (per electron) and in kilojoules per mole (of electrons).
According to a relationship developed by Niels Bohr, for an atom or ion that has a single electron, the total energy, En, of an electron in a stable orbit of quantum number n is En = [Z2/n2] (2.179 1018 J) where Z is the atomic number. Calculate the ionization energy for the electron in a ground-state He+ ion.
State which of the following sets of quantum numbers would be possible and which impossible for an electron in an atom. a n = 2, I = 0, mi = 0, ms=+12 b n = 1, I = 1, mi = 0, ms=+12 c n = 0, I = 0, mi = 0, ms=12 d n = 2, I = 1, mi = 1, ms=+12 e n = 2, I = 1, mi = 2, ms=+13
How far from the nucleus in angstroms (1 angstrom =11010 m) is the electron in a hydrogen atom if it has an energy of 8.721020 J?
What are the allowed values for each of the four quantum numbers: n, l, ml, and ms?
Imagine a world in which the rule for the l quantum number is that values start with 1 and go up to n. The rules for the n and mi quantum numbers are unchanged from those of our world. Write the quantum numbers for the first two shells (i.e., n = 1 and n = 2).
6.29 A mercury atom emits light at many wavelengths, two of which are at 435.8 and 546.1 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) lf a transition between the two higher energy states could be observed, what would be the frequency of the light?
A bright violet line occurs at 435.8 nm in the emission spectrum of mercury vapor. What amount of energy, in joules, must be released by an electron in a mercury atom to produce a photon of this light?

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Drag the electrons with the quantum numbers m=0, m =-1/2 into the "electron counter". 3d个个个个个 4s 3s 1 3p 11 1 25 12 2p 1 1 1 Is Submit Undo Electron Counter Reset