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Chapter 8: Problem 45

Explain which of the following cations is larger, and why: \(\mathrm{Cu}^{+}\) or \(\mathrm{Cu}^{2+}\)

Short Answer

Expert verified
The cation Cu2+ is smaller than the Cu+ cation. This is because when copper loses electrons to form ions, the effective nuclear charge increases causing the size of the atom to decrease. Therefore, Cu2+ which has lost two electrons will be smaller than Cu+, which has lost one electron.

Step by step solution

01

Understanding the atomic structure of Copper (Cu)

Copper is represented by the symbol Cu. In its neutral state, copper has 29 protons and 29 electrons. The electron configuration of copper is [Ar] 3d10 4s1.
02

Analyzing the cations

Cu+ means that the copper atom has lost one electron, giving it a charge of +1. Therefore, the Cu+ ion has 28 electrons. The Cu2+ ion has lost two electrons, meaning it has 27 electrons with a +2 charge. Both Cu+ and Cu2+ have more protons than electrons, which means a greater pull on the remaining electrons. Therefore, each remaining electron is more strongly attracted to the nucleus, hence the atomic radius reduces.
03

Comparing the sizes of the Copper ions

When moving from Cu+ to Cu2+, one electron is lost which reduces the electron-electron repulsion and increases the effective nuclear charge. Therefore, Cu2+ is smaller than Cu+ due to the decrease in size that accompanies the loss of an electron. This is because the remaining electrons in Cu2+ are significantly more attracted to the nucleus, and thus the overall atomic size decreases.

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Most popular questions from this chapter

Explain, in terms of their electron configurations, why \(\mathrm{Fe}^{2+}\) is more easily oxidized to \(\mathrm{Fe}^{3+}\) than \(\mathrm{Mn}^{2+}\) is to \(\mathrm{Mn}^{3+}\)

The first and second ionization energies of \(\mathrm{K}\) are 419 kJ/mol and \(3052 \mathrm{~kJ} / \mathrm{mol}\), and those of Ca are \(590 \mathrm{~kJ} / \mathrm{mol}\) and \(1145 \mathrm{~kJ} / \mathrm{mol},\) respectively. Compare their values and comment on the differences.

Element \(\mathrm{M}\) is a shiny and highly reactive metal (melting point \(\left.63^{\circ} \mathrm{C}\right)\), and element \(\mathrm{X}\) is a highly reactive nonmetal (melting point \(-7.2^{\circ} \mathrm{C}\) ). They react to form a compound with the empirical formula MX, a colorless, brittle white solid that melts at \(734^{\circ} \mathrm{C} .\) When dissolved in water or when in the molten state, the substance conducts electricity. When chlorine gas is bubbled through an aqueous solution containing MX, a reddish-brown liquid appears and \(\mathrm{Cl}^{-}\) ions are formed. From these observations, identify \(\mathrm{M}\) and \(\mathrm{X}\). (You may need to consult a handbook of chemistry for the melting-point values.)

How does atomic radius change (a) from left to right across a period and (b) from top to bottom in a group?

Explain why, for isoelectronic ions, the anions are larger than the cations.
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