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Chapter 9: Problem 82

An ion that is isoelectronic with \(\mathrm{Se}^{2-}\) is (a) \(\mathrm{S}^{2-} ;\) (b) I \(^{-}\) (c) \(\mathrm{Xe} ;\) (d) \(\mathrm{Sr}^{2+}.\)

Short Answer

Expert verified
Among the given options, only \(\mathrm{Sr}^{2+}\) is isoelectronic with \(\mathrm{Se}^{2-}\).

Step by step solution

01

Identify the electron count of \(\mathrm{Se}^{2-}\)

The atomic number of Selenium (Se) is 34, which means a neutral Selenium atom has 34 electrons. When the Selenium atom gains 2 more electrons it becomes \(\mathrm{Se}^{2-}\) ion with a total of \(34+2=36\) electrons.
02

Compare with option (a) \(\mathrm{S}^{2-}\)

The atomic number of Sulfur (S) is 16, which means a neutral Sulfur atom has 16 electrons. When the Sulfur atom gains 2 more electrons it becomes \(\mathrm{S}^{2-}\) ion with a total of \(16+2=18\) electrons. So option (a) \(\mathrm{S}^{2-}\) is not isoelectronic with \(\mathrm{Se}^{2-}\).
03

Compare with option (b) \(\mathrm{I}^{-}\)

The atomic number of Iodine (I) is 53, which means a neutral Iodine atom has 53 electrons. When the Iodine atom gains 1 more electron it becomes \(\mathrm{I}^{-}\) ion with a total of \(53+1=54\) electrons. So, option (b) \(\mathrm{I}^{-}\) is not isoelectronic with \(\mathrm{Se}^{2-}\).
04

Compare with option (c) \(\mathrm{Xe}\)

Xenon (Xe) is a noble gas and has an atomic number of 54. This means a neutral Xenon atom has 54 electrons. So, option (c) \(\mathrm{Xe}\) is not isoelectronic with \(\mathrm{Se}^{2-}\).
05

Compare with option (d) \(\mathrm{Sr}^{2+}\)

The atomic number of Strontium (Sr) is 38, which means a neutral Strontium atom has 38 electrons. When the Strontium atom loses 2 electron it becomes \(\mathrm{Sr}^{2+}\) ion with a total of \(38-2=36\) electrons. So, option (d) \(\mathrm{Sr}^{2+}\) is isoelectronic with \(\mathrm{Se}^{2-}\).

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Most popular questions from this chapter

Sketch a periodic table that would include all the elements in the main body of the table. How many "numbers" wide would the table be?

Explain why the first ionization energy of \(\mathrm{Mg}\) is greater that of \(\mathrm{Na},\) whereas the second ionization of Na is greater than that of Mg.

For the following groups of elements, select the one that has the property noted: (a) the largest atom: \(\mathrm{Mg}, \mathrm{Mn}, \mathrm{Mo}, \mathrm{Ba}, \mathrm{Bi}, \mathrm{Br}.\) (b) the lowest first ionization energy: \(\mathrm{B}, \mathrm{Sr}, \mathrm{Al}, \mathrm{Br}\) \(\mathrm{Mg}_{\ell} \mathrm{Pb}.\) (c) the most negative electron affinity: \(\mathrm{As}, \mathrm{B}, \mathrm{Cl}\) \(\mathrm{K}, \mathrm{Mg}, \mathrm{S}.\) (d) the largest number of unpaired electrons: \(\mathrm{F}, \mathrm{N}, \mathrm{S}^{2-}, \mathrm{Mg}^{2+}, \mathrm{Sc}^{3+}, \mathrm{Ti}^{3+}.\)

Concerning the incomplete seventh period of the periodic table, what should be the atomic number of the element (a) for which the filling of the \(6 d\) subshell is completed; (b) that should most closely resemble bismuth; (c) that should be a noble gas?

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