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Chapter 9: Problem 38

Neither \(\mathrm{Co}^{2+}\) nor \(\mathrm{Co}^{3+}\) has \(4 \mathrm{s}\) electrons in its electron configuration. How many unpaired electrons would you expect to find in each of these ions? Explain.

Short Answer

Expert verified
\(\mathrm{Co}^{2+}\) has 1 unpaired electron and \(\mathrm{Co}^{3+}\) has 0 unpaired electrons.

Step by step solution

01

Determine electron configuration of neutral atom

The atomic number of Cobalt is 27, meaning it has 27 electrons in its neutral state. The electron configuration of a neutral Co atom will be \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^7\).
02

Determine electron configuration of \(\mathrm{Co}^{2+}\) ion

The \(\mathrm{Co}^{2+}\) ion is formed by removing two electrons from the neutral Co atom. Electrons are removed from the highest energy level down, so they are removed from the 4s orbital first, then the 3d orbital. The electron configuration for \(\mathrm{Co}^{2+}\) will be \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^7\). Thus, \(\mathrm{Co}^{2+}\) has 1 unpaired electron in the 3d orbital.
03

Determine electron configuration of \(\mathrm{Co}^{3+}\) ion

The \(\mathrm{Co}^{3+}\) ion is formed by removing three electrons from the neutral Co atom. Again, electrons are removed from the highest energy level down. The electron configuration for \(\mathrm{Co}^{3+}\) will be \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^6\). Here all the electrons in the 3d orbital are paired, so there are no unpaired electrons.

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Most popular questions from this chapter

The \(\mathrm{Na}^{+}\) ion and the Ne atom are isoelectronic. The ease of loss of an electron by a gaseous Ne atom, \(I_{1}\) has a value of \(2081 \mathrm{kJ} / \mathrm{mol} .\) The ease of loss of an electron from a gaseous \(\mathrm{Na}^{+}\) ion, \(I_{2}\), has a value of \(4562 \mathrm{kJ} / \mathrm{mol} .\) Why are these values not the same?

Indicate the smallest and the largest species (atom or ion) in the following group: Al atom, F atom, As atom, \(\mathrm{Cs}^{+}\) ion, \(\mathrm{I}^{-}\) ion, \(\mathrm{N}\) atom.

How would you expect the sizes of the hydrogen ion, \(\mathrm{H}^{+},\) and the hydride ion, \(\mathrm{H}^{-},\) to compare with that of the H atom and the He atom? Explain.

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 atom \(^{119} \mathrm{Sn}\), indicate the number of (a) protons in the nucleus; (b) neutrons in the nucleus; (c) \(4 d\) electrons; (d) 3s electrons; (e) 5 \(p\) electrons; (f) electrons in the valence shell.
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