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Chapter 6: Problem 68

\(\mathrm{Mg}^{2+}\) is a smaller cation than \(\mathrm{Na}^{+}\) and also carries more positive charge. Which of the two species has a larger hydration energy (in \(\mathrm{kJ} / \mathrm{mol}\) ) ? Explain.

Short Answer

Expert verified
Mg2+ has a larger hydration energy than Na+ because it is smaller and carries a larger positive charge, leading to stronger interactions with water molecules.

Step by step solution

01

Analyzing the size and charge of ions

In the case given within the problem, Magnesium (Mg2+) is a smaller cation than Sodium (Na+) and also carries more positive charge. Thus, according to the properties of ionic sizes and charges, Mg2+ can form stronger bonds with water molecules and hence has a higher hydration energy.
02

End conclusion

As Mg2+ is smaller and has a greater charge in comparison to Na+, it is able to form stronger ionic bonds with the water molecules. Therefore, the hydration energy of Mg2+ is greater than the hydration energy of Na+.

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Most popular questions from this chapter

A 3.53-g sample of ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\) was added to \(80.0 \mathrm{~mL}\) of water in a constantpressure calorimeter of negligible heat capacity. As a result, the temperature of the water decreased from \(21.6^{\circ} \mathrm{C}\) to \(18.1^{\circ} \mathrm{C}\). Calculate the heat of solution \(\left(\Delta H_{\mathrm{soln}}\right)\) of ammonium nitrate.

Which of the following standard enthalpy of formation values is not zero at \(25^{\circ} \mathrm{C} ? \mathrm{Na}(s), \operatorname{Ne}(g)\) \(\mathrm{CH}_{4}(g), \mathrm{S}_{8}(s), \mathrm{Hg}(l), \mathrm{H}(g)\)

A gas expands and does \(P-V\) work on the surroundings equal to \(325 \mathrm{~J}\). At the same time, it absorbs \(127 \mathrm{~J}\) of heat from the surroundings. Calculate the change in energy of the gas.

The average temperature in deserts is high during the day but quite cool at night, whereas that in regions along the coastline is more moderate. Explain.

Determine the amount of heat (in kJ) given off when \(1.26 \times 10^{4} \mathrm{~g}\) of ammonia are produced according to the equation $$\begin{aligned}\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow & 2 \mathrm{NH}_{3}(g) \\ & \Delta H_{\mathrm{rxn}}^{\circ}=-92.6 \mathrm{~kJ} / \mathrm{mol} \end{aligned}$$ Assume that the reaction takes place under standardstate conditions at \(25^{\circ} \mathrm{C}\).
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