Compound Lattice Energy (kJ/mol) NaF 930 2978 The energy required to dissociate an ionic solid into gaseous ions (lattice energy) for the compounds NaF and MgF. is shown in the table above. On the basis of Coulomb's law, which of the following best helps to explain the large difference between the lattice energies of NaF and MgF, ? A The solubility of MgF, is less than that of NaF. The electronegativity of Mg is greater than that of Na. The mass of the Mg cation is greater than that of the Na cation. The charge of the Mg cation is larger than that of the Na cation.
Compound Lattice Energy (kJ/mol) NaF 930 2978 The energy required to dissociate an ionic solid into gaseous ions (lattice energy) for the compounds NaF and MgF. is shown in the table above. On the basis of Coulomb's law, which of the following best helps to explain the large difference between the lattice energies of NaF and MgF, ? A The solubility of MgF, is less than that of NaF. The electronegativity of Mg is greater than that of Na. The mass of the Mg cation is greater than that of the Na cation. The charge of the Mg cation is larger than that of the Na cation.
Chapter1: Solubility
Section: Chapter Questions
Problem 1Q
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![Compound
Lattice Energy (kJ/mol)
NaF
930
MgF,
2978
The energy required to dissociate an ionic solid into gaseous ions (lattice energy) for the compounds NaF and MgF, is shown in the table above. On the basis of Coulomb's law, which of the
following best helps to explain the large difference between the lattice energies of NaF and MgF, ?
A
The solubility of MgF, is less than that of NaF.
B)
The electronegativity of Mg is greater than that of Na.
The mass of the Mg cation is greater than that of the Na cation.
D
The charge of the Mg cation is larger than that of the Na cation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F83fbd40b-9e26-4777-b346-6909425aa121%2Fe31d0857-0f55-4c38-adc0-e31d25da2476%2Fdisd4uf_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Compound
Lattice Energy (kJ/mol)
NaF
930
MgF,
2978
The energy required to dissociate an ionic solid into gaseous ions (lattice energy) for the compounds NaF and MgF, is shown in the table above. On the basis of Coulomb's law, which of the
following best helps to explain the large difference between the lattice energies of NaF and MgF, ?
A
The solubility of MgF, is less than that of NaF.
B)
The electronegativity of Mg is greater than that of Na.
The mass of the Mg cation is greater than that of the Na cation.
D
The charge of the Mg cation is larger than that of the Na cation.
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