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NaF, KF, MgO and CaO are crystalline solids. They have NaCl structure. Their lattice energies vary in the order
- a)NaF < KF < MgO < CaO
- b)KF < NaF < CaO < MgO
- c)MgO < CaO < NaF < KF
- d)CaO < MgO < KF < NaF
Correct answer is option 'B'. Can you explain this answer?
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NaF, KF, MgO and CaO are crystalline solids. They have NaCl structure....
The lattice energy is a measure of the strength of the forces that hold the ions in a crystal lattice together. The higher the lattice energy, the stronger the forces and the more stable the crystal.
In general, the lattice energy of an ionic compound depends on the charge and size of the ions. Smaller ions with higher charges have stronger attractions and higher lattice energies.
Using this information, we can compare the lattice energies of NaF, KF, MgO, and CaO.
The charges of the ions in each compound are:
- NaF: Na+ and F-, both with charges of 1-
- KF: K+ and F-, both with charges of 1-
- MgO: Mg2+ and O2-, with charges of 2- and 2-
- CaO: Ca2+ and O2-, with charges of 2- and 2-
The sizes of the ions follow the trend: Ca2+ > Mg2+ > K+ > Na+ > F-. This is because the ions have the same electronic configuration and as they gain electrons they become larger.
Therefore, the order of increasing lattice energies is:
a) NaF < kf="" />< mgo="" />< />
This is because the charges of the ions are the same for NaF and KF, but the ions in KF are larger, resulting in weaker attractions and lower lattice energy. MgO has larger charges but smaller ions than KF, resulting in a higher lattice energy. CaO has the largest charges and the smallest ions, resulting in the highest lattice energy.
In general, the lattice energy of an ionic compound depends on the charge and size of the ions. Smaller ions with higher charges have stronger attractions and higher lattice energies.
Using this information, we can compare the lattice energies of NaF, KF, MgO, and CaO.
The charges of the ions in each compound are:
- NaF: Na+ and F-, both with charges of 1-
- KF: K+ and F-, both with charges of 1-
- MgO: Mg2+ and O2-, with charges of 2- and 2-
- CaO: Ca2+ and O2-, with charges of 2- and 2-
The sizes of the ions follow the trend: Ca2+ > Mg2+ > K+ > Na+ > F-. This is because the ions have the same electronic configuration and as they gain electrons they become larger.
Therefore, the order of increasing lattice energies is:
a) NaF < kf="" />< mgo="" />< />
This is because the charges of the ions are the same for NaF and KF, but the ions in KF are larger, resulting in weaker attractions and lower lattice energy. MgO has larger charges but smaller ions than KF, resulting in a higher lattice energy. CaO has the largest charges and the smallest ions, resulting in the highest lattice energy.
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Community Answer
NaF, KF, MgO and CaO are crystalline solids. They have NaCl structure....
Lattice energy varies with varies in oxidation state as oxidation state increases lattice energy increase for same oxidation state, as radius between postive and negative atom incrases lattice energy decreases
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NaF, KF, MgO and CaO are crystalline solids. They have NaCl structure. Their lattice energies vary in the ordera)NaF < KF < MgO < CaOb)KF < NaF < CaO < MgOc)MgO < CaO < NaF < KFd)CaO < MgO < KF < NaFCorrect answer is option 'B'. Can you explain this answer?
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