Answer: The ground-state electronic configuration of
1) [tex]Ru^{2+}=[Kr]4d^6[/tex]
2) [tex]W^{3+]=4f^{14}5d^3[/tex]
Explanation: The electronic configuration of elements is defined as the distribution of electrons around the nucleus of that element. It depends on the atomic number of the element.
Atomic number of the element = Number of electrons.
Atomic number = 44
Number of electrons = 44
Electronic configuration of Ru-element = [tex][Kr]4d^75s^1[/tex]
To form [tex]Ru^{2+}[/tex], 2 electrons are released from the neutral Ru-element.
So, the electronic configuration of [tex]Ru^{2+}=[Kr]4d^6[/tex]
Atomic number = 74
Number of electrons = 74
Electronic configuration of W-element = [tex][Xe]4f^{14}5d^46s^2[/tex]
To form [tex]W^{3+}[/tex], 3 electrons are released from the neutral W-element.
So, the electronic configuration of [tex]W^{3+}=[Xe]4f^{14}5d^3[/tex]
Ru ²⁺ :[Kr] 4d⁶
W ³⁺ : [Xe] 4f¹⁴5d³
The Atomic Number (Z) indicates the number of protons in an atom of an element. If the atom is neutral then the number of protons will be equal to the number of electrons. So the atomic number can also indicate the number of electrons.
This energy level is expressed in the form of electron configurations.
Charging electrons in the sub shell use the following sequence:
1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.
Writing the electron configuration can be abbreviated using the electron configuration of the noble gas in brackets because it has the same configuration
It is in group 8B and period 5 with atomic number 44
So the electron configuration:
1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s¹, 4d⁷
This configuration includes an exception to the Aufbau rule which is that Electrons occupy orbitals of the lowest energy level, which should be 5s² 4d⁶ (exceptions occur mainly in the transition group), so that with the configuration of the noble gases from Kr [1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶], the Ru element can be written:
Ruthenium-Ru: [Cr] 5s¹4d⁷
Because it releases 2 electrons to form Ru²⁺ ions, the configuration becomes
Ru ²⁺ :[Kr] 4d⁶
It is in group 6B and period 6 with atomic number 74
So the electron configuration:
1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s²4f¹⁴5d⁴
Because according to Xe configuration [1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶] it can be written:
W: [Xe] 6s²4f¹⁴5d⁴
Because it releases 3 electrons to form a W³⁺ ion, the configuration becomes (electrons with the largest n , 6s and 5d, the electrons are removed first):
W ³⁺ : [Xe] 4f¹⁴5d³
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