Calcium and chlorine combine to form CaCl_2,b | vedclass

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Question

(C) The formation of an ionic compound depends on the total energy change,which includes the energy required to ionize the metal and the lattice energ

Vedclass · Accepted Answer

The lattice energy of $CaCl_{(s)}$ is less exothermic than that of $CaCl_{2(s)}$.

Vedclass · Answer

(C) The formation of an ionic compound depends on the total energy change,which includes the energy required to ionize the metal and the lattice energy released upon the formation of the crystal lattice. For $Ca^{2+}$,the sum of the first and second ionization energies is relatively low due to the stable noble gas configuration achieved. However,the lattice energy of $CaCl_{2(s)}$ is significantly higher (more negative) than that of $CaCl_{(s)}$ because the $Ca^{2+}$ ion has a higher charge density and forms a more stable crystal lattice with two $Cl^-$ ions. Therefore,the formation of $CaCl_{2(s)}$ is energetically more favorable than $CaCl_{(s)}$.

Calcium and chlorine combine to form $CaCl_2$,but they do not form $CaCl$. This is because:

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