Answer
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Work Step by Step
a. NaCl, KCl
The compound with the most negative lattice energy in this pair is NaCl.
Explanation:
Lattice energy is the energy released when a gaseous ion is formed from its constituent elements in their standard states. The magnitude of the lattice energy is influenced by the charge and size of the ions involved.
In the case of NaCl and KCl, both compounds have a +1 cation (Na+ or K+) and a -1 anion (Cl-). However, the size of the ions plays a crucial role. The sodium ion (Na+) is smaller than the potassium ion (K+), and the chloride ion (Cl-) is also smaller than the potassium ion (K+). Smaller ions have a higher charge density, which results in stronger electrostatic interactions and a more negative lattice energy.
Therefore, NaCl has a more negative lattice energy compared to KCl.
b. LiF, LiCl
The compound with the most negative lattice energy in this pair is LiF.
Explanation:
Similar to the previous case, the lattice energy is influenced by the charge and size of the ions involved. In this pair, both compounds have a +1 cation (Li+) and a -1 anion (F- or Cl-).
The fluoride ion (F-) is smaller than the chloride ion (Cl-), and the lithium ion (Li+) is also smaller than the chloride ion (Cl-). Smaller ions have a higher charge density, leading to stronger electrostatic interactions and a more negative lattice energy.
Therefore, LiF has a more negative lattice energy compared to LiCl.
c. Mg(OH)2, MgO
The compound with the most negative lattice energy in this pair is MgO.
Explanation:
In this case, the compounds have different types of ions. Mg(OH)2 has a +2 cation (Mg2+) and two -1 anions (OH-), while MgO has a +2 cation (Mg2+) and a -2 anion (O2-).
The lattice energy is primarily determined by the charge of the ions. The higher the charge, the stronger the electrostatic interactions and the more negative the lattice energy. The oxide ion (O2-) has a higher charge than the hydroxide ion (OH-), leading to a more negative lattice energy for MgO compared to Mg(OH)2.
Therefore, MgO has a more negative lattice energy compared to Mg(OH)2.
d. Fe(OH)2, Fe(OH)3
The compound with the most negative lattice energy in this pair is Fe(OH)3.
Explanation:
In this case, both compounds have a +2 cation (Fe2+) and multiple -1 anions (OH-). However, the number of anions differs between the two compounds.
Fe(OH)3 has three hydroxide ions (OH-), while Fe(OH)2 has two hydroxide ions (OH-). The higher the number of anions, the more negative the lattice energy due to the increased electrostatic interactions.
Therefore, Fe(OH)3 has a more negative lattice energy compared to Fe(OH)2.
e. NaCl, Na2O
The compound with the most negative lattice energy in this pair is Na2O.
Explanation:
In this case, NaCl has a +1 cation (Na+) and a -1 anion (Cl-), while Na2O has a +1 cation (Na+) and a -2 anion (O2-).
The lattice energy is primarily determined by the charge of the ions. The higher the charge, the stronger the electrostatic interactions and the more negative the lattice energy. The oxide ion (O2-) has a higher charge than the chloride ion (Cl-), leading to a more negative lattice energy for Na2O compared to NaCl.
Therefore, Na2O has a more negative lattice energy compared to NaCl.
f. MgO, BaS
The compound with the most negative lattice energy in this pair is MgO.
Explanation:
In this case, both compounds have a +2 cation (Mg2+ or Ba2+) and a -2 anion (O2- or S2-). However, the size of the ions plays a
