Question

a. For each pair of compounds, suggest which will have the most exothermic lattice energy.

i. KCl\mathrm{KCl} and BaO\mathrm{BaO} (ionic radii are similar)

ii. MgI2\mathrm{MgI}_2 and SrI2\mathrm{SrI}_2

iii. CaO\mathrm{CaO} and NaCl\mathrm{NaCl} (ionic radii are similar).

b. Place the following compounds in order of increasingly exothermic lattice energy. Explain your answer.

LiF\mathrm{LiF} MgORbCl\quad \mathrm{MgO} \quad \mathrm{RbCl}

Solution

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(a)

(i)

In this exercise, we have to suggest which compound in a pair will have the most exothermic lattice energy KCL\mathrm{KCL} and BaO\mathrm{BaO}:

\star BaO\mathrm{BaO} will have the most exothermic energy

(ii)

MgI2\mathrm{MgI}_{2} and SrI2\mathrm{SrI}_{2}:

\star MgI2\mathrm{MgI}_{2} will have the most exothermic energy

(iii)

CaO\mathrm{CaO} and NaCl\mathrm{NaCl}:

\star CaO\mathrm{CaO} will have the most exothermic energy

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