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Chapter 9: Problem 20

Is it possible for two different atoms to be isoelectronic? two different cations? two different anions? a cation and an anion? Explain.

Short Answer

Expert verified
Yes, it is possible for two different atoms, cations, anions, and a cation and an anion to be isoelectronic. All these species can achieve the same electronic configuration and, thus, are considered isoelectronic.

Step by step solution

01

Understanding Isoelectronic Species

Isoelectronic species are those which have the same number of electrons or the same electronic configuration. It does not depend on the type of atom or ion, be it an atom, cation, or anion.
02

Comparing Two Different Atoms

As different atoms can share the same electronic configuration when they gain or lose electrons to achieve stable configuration, they can indeed be isoelectronic. For example, neon (a neutral atom) and fluoride ion (F-) are isoelectronic as they both have 10 electrons and share the same electronic configuration.
03

Comparing Two Different Cations

Similarly, two different cations can also be isoelectronic. Sodium ion (Na+) and magnesium ion (Mg2+) being examples, as they both have 10 electrons after losing electrons.
04

Comparing Two Different Anions

Two different anions can also be isoelectronic. For instance, sulfide ion (S2-) and chloride ion (Cl-) both have 18 electrons after gaining electrons to obtain stable configuration.
05

Comparing a Cation and an Anion

A cation and an anion can also be isoelectronic. An example is that of potassium ion (K+) and chloride ion (Cl-), both of which have 18 electrons.

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Most popular questions from this chapter

The element whose atoms have the electron configuration \([\mathrm{Kr}] 4 d^{10} 5 \mathrm{s}^{2} 5 p^{3}(\mathrm{a})\) is in group 13 of the periodic table; (b) bears a similarity to the element Bi; (c) is similar to the element \(\mathrm{Te} ;\) (d) is a transition element.

Give the symbol of the element (a) in group 14 that has the smallest atoms; (b) in period 5 that has the largest atoms; (c) in group 17 that has the lowest first ionization energy.

Explain the important distinctions between each pair of terms: (a) actinide and lanthanide element; (b) covalent and metallic radius; (c) atomic number and effective nuclear charge; (d) ionization energy and electron affinity; (e) paramagnetic and diamagnetic.

Explain why the several periods in the periodic table do not all have the same number of members.

A method for estimating electron affinities is to extrapolate \(Z_{\text {eff }}\) values for atoms and ions that contain the same number of electrons as the negative ion of interest. Use the data in the table on the next page to answer the questions that follow. $$\begin{array}{lll} \hline \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} & \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} & \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} \\ \hline \text { Ne: 2080 } & \text { F: 1681 } & \text { O: } 1314 \\ \text { Na }^{+}: 4565 & \text { Ne }^{+}: 3963 & \text { F }^{+}: 3375 \\ \text { Mg }^{2+} \text { : 7732 } & \text { Na }^{2+}: 6912 & \text { Ne }^{2+}: 6276 \\ \text { A1 }^{\text {3 }^{+}: 11,577} & \text { Mg }^{3+}: 10,548 & \text { Na }^{3+}: 9540 \\ \hline \end{array}$$ (a) Estimate the electron affinity of \(F\), and compare it with the experimental value. (b) Estimate the electron affinities of \(\mathrm{O}\) and \(\mathrm{N}\) (c) Examine your results in terms of penetration and screening.
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