Question on structure of Atom

[Dhamnekar Win,odd]

An x-ray photoelectron spectroscopy experiment with an unidentified element, X, displays an emission spectrum with four distinct kinetic energies:

 

[math] 5.9 \times 10^{-17} J, 2.53 \times 10^{-18} J,[/math]

[math]2.59 \times 10^{-20} J, 2.67 \times 10^{-20} J [/math] (Assume the incident light has sufficient energy to eject any electron in the atom.)

(a)Name all of the possible ground state atoms that could yield this spectrum.

(b)Calculate the binding energy of an electron in the 2p orbital of element X if the x-rays used for the spectroscopy experiment had an energy of [math] 2.68 \times 10^{-16} J[/math]

(c)Consider both the filled and unfilled orbitals of element X. Determine the number of: (1) total nodes in a 4d orbital (2)angular nodes in the [math]2p_y[/math] orbital (3)degenerate 5p orbitals

How to answer all these questions?

Edited November 17, 2021 by Dhamnekar Win,odd

[Bufofrog]

Let me be the first to ask, how far have you gotten?  You will receive help here, not just the answers.

[Dahiru saidu]

14 hours ago, Dhamnekar Win,odd said:

An x-ray photoelectron spectroscopy experiment with an unidentified element, X, displays an emission spectrum with four distinct kinetic energies:

 

[math] 5.9 \times 10^{-17} J, 2.53 \times 10^{-18} J,[/math]

[math]2.59 \times 10^{-20} J, 2.67 \times 10^{-20} J [/math] (Assume the incident light has sufficient energy to eject any electron in the atom.)

(a)Name all of the possible ground state atoms that could yield this spectrum.

(b)Calculate the binding energy of an electron in the 2p orbital of element X if the x-rays used for the spectroscopy experiment had an energy of 2.68×10−16J

(c)Consider both the filled and unfilled orbitals of element X. Determine the number of: (1) total nodes in a 4d orbital (2)angular nodes in the 2py orbital (3)degenerate 5p orbitals

How to answer all these questions?

I don't know 

 

[swansont]

I work better in electron-Volts, so 

5.9e-17J = 368.25 eV (x-ray)

2.53e-18J = 15.8 eV (ultraviolet)

2.59e-20J = 0.161 eV (infrared)

2.67e-20J = 0.167eV

Note that these are 3 quite different energy scales (spectroscopically speaking). What transitions would be involved in emitting a photon that has several hundred eV, around 15 eV, and around 0.1 eV?

You're asked for what atoms could give you this spectrum, so you musty have access to spectroscopy data to do the comparisons

 

 

 

[Dhamnekar Win,odd]

Answers:

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Edited November 18, 2021 by Phi for All
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[Phi for All]

1 hour ago, Dhamnekar Win,odd said:

Answers:

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