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Hello students.
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In this question we have to determine the quantum numbers for electrons in various species.
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In the first case, the electronic configuration of rubidium atom is krypton 5 s1.
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The outermost electron is in 5 s orbital as there is only one electron present in the outermost electron in the outermost electron is in 5 s orbital.
00:33
Or the valence shell which is 5 s the principal quantum number would be 5 the azimuthal quantum number for s orbital is 0 the magnetic quantum number for s orbital is 0 and the spin value for this electron is plus half in the next case the electronic configuration for sulfur negative atom is neon 3s2 3p 5 when an additional electron is added to the orbit the electron comes into the 3p orbital and has a fully filled sub shell p orbital has three different orbitals in which electrons are first singly field and then only pairing is done.
01:48
The n value, which is the principal quantum number for the electron, is 3.
01:54
The azimuthal quantum number for p orbital is 1.
02:00
The magnetic quantum number would be equal to minus 1.
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This is because the electron has entered in the orbital with minus 1 value.
02:15
The spin of the incoming electron is minus half.
02:21
In the next case, we have been asked about the silver atom.
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The atomic configuration of silver atom is krypton 4d10 5s1.
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The electronic configuration for the ionized silver would be equal to krypton 4d10 as the 5s electron is ionized...