QuestionAugust 19, 2025

4. Explain why the lattice energy-the amount of energy necessary to break apart the lattice-of MgCl_(2) is greater than the lattice energy of NaCl. Coulomb's low which you may use in your answer, is F_(c)=k(q_(1)q_(2))/(r^2)

4. Explain why the lattice energy-the amount of energy necessary to break apart the lattice-of MgCl_(2) is greater than the lattice energy of NaCl. Coulomb's low which you may use in your answer, is F_(c)=k(q_(1)q_(2))/(r^2)
4. Explain why the lattice energy-the amount of energy necessary to break apart the lattice-of MgCl_(2) is greater than the lattice energy of NaCl. Coulomb's low which you may use in your answer, is F_(c)=k(q_(1)q_(2))/(r^2)

Solution
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Answer

The lattice energy of MgCl_2 is greater than that of NaCl due to higher ionic charges and smaller ionic radii, resulting in stronger electrostatic forces. Explanation 1. Identify the charges MgCl_2 has Mg^{2+} and Cl^{-} ions, while NaCl has Na^{+} and Cl^{-} ions. The charge on Mg^{2+} is greater than that on Na^{+}. 2. Apply Coulomb's Law **Coulomb's Law** states F_{c} = k\frac{q_{1}q_{2}}{r^{2}}. Higher charges (q_1, q_2) result in stronger forces. MgCl_2 has a higher product of charges compared to NaCl. 3. Consider ionic radii Mg^{2+} is smaller than Na^{+}, leading to a smaller distance r between ions in MgCl_2, increasing the force according to Coulomb's Law.

Explanation

1. Identify the charges<br /> $MgCl_2$ has $Mg^{2+}$ and $Cl^{-}$ ions, while $NaCl$ has $Na^{+}$ and $Cl^{-}$ ions. The charge on $Mg^{2+}$ is greater than that on $Na^{+}$.<br />2. Apply Coulomb's Law<br /> **Coulomb's Law** states $F_{c} = k\frac{q_{1}q_{2}}{r^{2}}$. Higher charges ($q_1$, $q_2$) result in stronger forces. $MgCl_2$ has a higher product of charges compared to $NaCl$.<br />3. Consider ionic radii<br /> $Mg^{2+}$ is smaller than $Na^{+}$, leading to a smaller distance $r$ between ions in $MgCl_2$, increasing the force according to Coulomb's Law.
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