In what row and group of the periodic table would you find the element with the electron configuration [Kr]5s²4d¹⁰5p² A) row 4, group 4A B) row 4, group 5A C) row 5, group 4A D) row 5, group 5A E) none of the above

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The electron configuration shows that the element has 4s, 4p, 4d, and 5s orbitals filled with electrons. This corresponds to the fifth row of the periodic table. The presence of Kr (krypton) in the electron configuration suggests that the element is in the same group as krypton, which is group 18 or the noble gases. However, since the electron configuration also shows the presence of s, p, and d orbitals in the valence shell, the element is not one of the noble gases. This narrows down the possible groups to 3A, 4A, and 5A. The electron configuration also shows that the element has one electron in the 5s orbital, which is the highest energy level. This suggests that the element is an alkali metal or an alkaline earth metal, both of which have valence electrons in the s orbital. Among the possible groups, the only one that includes alkali metals and alkaline earth metals is group 4A. Therefore, the element is most likely in row 5 and group 4A, which corresponds to the element Ge (germanium).

In What Row and Group of the Periodic Table Would