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Chapter 6: Problem 9

Predict which is larger: the \(\mathrm{O}^{2-}\) ion or the \(\mathrm{F}^{-}\) ion. Explain your reasoning.

Short Answer

Expert verified
The \(\mathrm{O}^{2-}\) ion is larger than the \(\mathrm{F}^{-}\) ion. This is due to a combination of naturally larger atomic radius of Oxygen plus the increase in size caused by the addition of two electrons (as opposed to one in the case of \(\mathrm{F}^{-}\) ), which increases electron-electron repulsion and therefore the overall size of the ion.

Step by step solution

01

Understand the effect of charge on the size of ions

Adding electrons to an atom forms a negatively charged ion, or anion. An increase in the electron count causes a natural increase in electron-electron repulsion, which causes the ion to expand and thus increase in size.
02

Compare the atomic radii

Oxygen and Fluorine are next to each other on the periodic table, with Oxygen coming first. Given the same energy level, atoms increase in size from right to left. Therefore, an oxygen atom is larger than a fluorine atom.
03

Factor in the charge effect

O^2- has gained two extra electrons, further increasing its size due to increased electron-electron repulsion. F^- has gained one electron, so while it too is bigger than its atom, it will not have expanded as much as O^2-. This is because the electron-electron repulsion impact isn't as strong as in O^2-.

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Most popular questions from this chapter

Why does the core charge increase moving from left to right across a period in the periodic table - for example, from boron to carbon to oxygen?

What are three characteristics of an atom (or ion) that must be considered in determining its relative radius?

What trend in atomic radius is observed moving from left to right across a period? Explain why this trend exists.

\(\mathrm{F}\) and \(\mathrm{F}^{-}\) have identical core charges and the valence shell is \(\mathrm{n}=2\) in both cases. Explain why the radius of \(\mathrm{F}^{-}\) is larger than the radius of \(\mathrm{F}\).

What trend in atomic radius is observed moving down a group in the periodic table? Explain why this trend exists.
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