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If the atom is neutral then, the total number of electrons is the same as the number of protons. We calculate for the total number of electrons given the compressed electron configuration,
   number of electrons of Xenon (Xe) = 54
The total number of electrons after Xenon,
   = 2 + 14 + 7 = 23

Adding up all the number of electrons, we have,
   total number of electrons = 54 + 23 = 77

The identity of this element is Iridium (Ir). This element belongs to the class of Group 9. This is the transition metal. 
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Answer:

The element belongs to d-block of the periodic table and it will be a transition metal. The metal is Iridium.

Explanation:

The given element has electronic configuration [tex]\rm [Xe] 6s^24f^{14}5d^7[/tex].

The electronic configuration ends as 2 electrons in s orbital, 14 electrons in f orbital and 7 electrons in d orbital.

So, the last electron comes in d orbital. The element will belong to d-block where transition elements are placed in the periodic table.

Therefore, the element belongs to d-block of the periodic table and it will be a transition metal. To be precise, the atomic number of the element will be [tex]23+54=77[/tex] and the element will be Iridium.

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https://brainly.com/question/13372254?referrer=searchResults

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