Based on considerations we have discussed in class relative to ion-dipole interactions, rank the following ions in terms of increasing hydration energy. Na+, Rb+, Li +, K + lowest ï¿(1)/(2) ï¿(1)/(2) highest
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Some ions are sketched below. Rank them in increasing order of size of hydration enthalpy ΔHhyd. That is, select 1 next to the ion with the smallest ΔHhyd, select 2 next to the ion with the next bigger ΔHhyd, and so on. Note for advanced students: please compare the absolute magnitude of ΔHhyd. For example, if ΔHhyd = -1 kJ/mol for the first ion and ΔHhyd = -2 kJ/mol for the second ion, then the first ion has the smaller ΔHhyd and the second ion has the bigger ΔHhyd.
Ishu S.
Very lost on how to read this problem please help thank you!
David C.
Alkali metals form hydrated compounds. The hydration enthalpies of alkali metals are in the sequence of : (a) $\mathrm{Rb}^{+}>\mathrm{Li}^{+}>\mathrm{Na}^{+}>\mathrm{K}^{+}>\mathrm{CS}^{+}$ (b) $\mathrm{CS}^{+}>\mathrm{Rb}^{+}>\mathrm{K}^{+}>\mathrm{Na}^{+}>\mathrm{Li}^{+}$ (c) $\mathrm{L}^{+}>\mathrm{Na}^{+}>\mathrm{K}^{+}>\mathrm{Rb}^{+}>\mathrm{CS}^{+}$ (d) $\mathrm{K}^{+}>\mathrm{Na}^{+}>\mathrm{Li}^{+}>\mathrm{Rb}^{+}>\mathrm{CS}^{+}$
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