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What is the shorthand electron configuration of Xe ?

Answer
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Hint: We know that the elements which are known by the terms mentioned in the options. We have to identify the element from the given electronic configuration Look at the electronic configuration and find out in which orbital the valence electrons are present. Find out how many electrons are present in the valence shell to get the answer.

Complete answer:
Xenon is element 54,in the noble gases (last) column. To get the short-handed electron configuration, look at the noble gas in the row above xenon. This would be krypton. This is the base that we use to form the configuration. So far, we have [Kr].
Now, let's look at the row for Xenon. Since it is in row 5, we will be filling the 5s and 5p orbitals. Remember that the d orbitals start at 3d in row 4, so we will be filling the 4d orbitals. Starting from left to right, we fill in 2 electrons for the s orbitals. Since we haven't gotten to xenon yet, we need to fill in the d orbitals. This will be 10 electrons. We need to fill in the p orbitals to complete the configuration. We will fill all 6 electrons in. Now we got the electron configuration for xenon. The complete electronic configuration is 1s22s22p63s23p64s23d104p65s24d105p6.
 We can see that the 5d orbital is incompletely filled. This indicates that the given element belongs to d-block and not s-block. So, this element is not an alkaline earth metal. It has the valence shell 6s which means the element belongs to the sixth period. We know that lanthanides are present in the sixth period.  [Kr] 4d105s25p6 here, 4d orbitals are lower in energy than 5s, so 4d electrons are typically listed before 5s electrons.

Note:
Remember that the given element has completely filled 4f orbitals and 3 electrons left to complete 5d orbitals, which means, this element is not a lanthanide and thus, not a rare earth element. This element has a vacant 6p orbital, so it is not an inert gas element. So, three out of four options are eliminated. Therefore, our answer should be the transition element which is correct because d-block elements are transition elements.