The Question and answers have been prepared Can you explain this answer? for IIT JAM 2023 is part of IIT JAM preparation. 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'. NaF, KF, MgO and CaO are crystalline solids. CaO has the largest charges and the smallest ions, resulting in the highest lattice energy. MgO has larger charges but smaller ions than KF, resulting in a higher lattice energy. 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. Therefore, the order of increasing lattice energies is: This is because the ions have the same electronic configuration and as they gain electrons they become larger. The sizes of the ions follow the trend: Ca2+ > Mg2+ > K+ > Na+ > F. CaO: Ca2+ and O2-, with charges of 2- and 2. MgO: Mg2+ and O2-, with charges of 2- and 2. NaF: Na+ and F-, both with charges of 1.
The charges of the ions in each compound are: Using this information, we can compare the lattice energies of NaF, KF, MgO, and CaO. Smaller ions with higher charges have stronger attractions and higher lattice energies. In general, the lattice energy of an ionic compound depends on the charge and size of the ions. The higher the lattice energy, the stronger the forces and the more stable the crystal. The lattice energy is a measure of the strength of the forces that hold the ions in a crystal lattice together.
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