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Chapter 8: Problem 45

Explain which of these ions is larger, and why: \(\mathrm{Cu}^{+}\) or \(\mathrm{Cu}^{2+}\).

Short Answer

Expert verified
The \(\mathrm{Cu}^{2+}\) ion is larger than the \(\mathrm{Cu}^{+}\) ion.

Step by step solution

01

Atomic and Ionic Structure

Atoms are made up of a nucleus, containing protons and neutrons, surrounded by electrons in energy levels. When an atom loses an electron to form a positive ion (\(\mathrm{Cu}^{+}\) or \(\mathrm{Cu}^{2+}\)), the remaining electrons are drawn closer to the nucleus as there are less electrons to counteract the positive charge of the protons in the nucleus.
02

Comparing the Cation Sizes

In \(\mathrm{Cu}^{+}\), one electron has been removed, making it smaller than the neutral copper atom. For \(\mathrm{Cu}^{2+}\), two electrons are removed. This increases the effective nuclear charge felt by the remaining electrons, pulling them closer to the nucleus, and consequently reducing the radius of the ion even further. Therefore, we can deduce that \(\mathrm{Cu}^{2+}\) is smaller than \(\mathrm{Cu}^{+}\).
03

Conclusion

The \(\mathrm{Cu}^{2+}\) ion is smaller than the \(\mathrm{Cu}^{+}\) ion due to the increased effective nuclear charge following the loss of two electrons, which pulls the remaining electrons closer to the nucleus and reduces the size of the ion.

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Most popular questions from this chapter

Indicate whether these elements exist as atomic species, molecular species, or extensive three dimensional structures in their most stable state at \(25^{\circ} \mathrm{C}\) and \(1 \mathrm{~atm},\) and write the molecular or empirical formula for the elements: phosphorus, iodine, magnesium, neon, arsenic, sulfur, carbon, selenium, and oxygen.

What do we mean when we say that two ions or an atom and an ion are isoelectronic?

Use the third period of the periodic table as an example to illustrate the change in first ionization energies of the elements as we move from left to right. Explain the trend.

Define valence electrons. For representative elements, the number of yalence electrons of an element is equal to its group number. Show that this is true for the following elements: \(\mathrm{Al}, \mathrm{Sr}, \mathrm{K}, \mathrm{Br}, \mathrm{P}, \mathrm{S}, \mathrm{C}\).

The \(\mathrm{H}^{-}\) ion and the He atom have two \(1 \mathrm{~s}\) electrons each. Which of the two species is larger? Explain.
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