The lattice energy of RbCl is – 689 kJ/mol , whereas that of SrS is – 2900 kJ/mol . Explain this large difference in lattice energy. Match the items in the left column to the appropriate blanks in the sentences on the right. ResetHelp Lattice energies become less exothermic (less negative) with Blank ionic radii and more exothermic (more negative) with Blank magnitude of ionic charges.target 1 of 14target 2 of 14 Because rubidium is slightly Blankstrontium, and sulfur is slightly Blankchlorine, the ionic radius Blank be used to explain the difference in lattice energy in this case.target
The Correct Answer and Explanation is :
The large difference in lattice energy between RbCl and SrS can be explained by several factors, such as the ionic radii of the ions involved and the magnitude of their ionic charges.
Lattice energies are the energies released when ions in the gas phase come together to form a solid lattice. These energies are affected by two main factors: the size of the ions and the magnitude of their charges. Specifically, the lattice energy becomes less exothermic (less negative) with larger ionic radii and more exothermic (more negative) with larger magnitudes of ionic charges. This is because the electrostatic attraction between ions increases as the charge increases and the size of the ions decreases, leading to a more stable lattice structure.
In the case of RbCl and SrS, there is a significant difference in the ionic radii and charges of the ions involved:
- Rubidium (Rb+) has a larger ionic radius compared to strontium (Sr2+). This means that the distance between the ions in RbCl will be larger, which reduces the strength of the electrostatic forces of attraction, resulting in a lower lattice energy.
- Chlorine (Cl-) has a smaller ionic charge compared to sulfur (S2-). Since sulfur carries a charge of -2, while chlorine carries a charge of -1, the electrostatic attraction in SrS will be stronger than in RbCl, which leads to a higher lattice energy for SrS.
Thus, the lattice energy of RbCl is less negative than that of SrS because rubidium is slightly larger than strontium, and sulfur is slightly more charged than chlorine. The ionic radii and charge magnitudes are the key factors that can explain the difference in lattice energies between these two compounds.
Now, here is a visual representation of the differences in ionic radii and charge magnitudes to further illustrate this concept.
Let me generate the image now.
Here is the image comparing the ionic radii and charge magnitudes of rubidium (Rb+), strontium (Sr2+), chlorine (Cl-), and sulfur (S2-) ions. This visualization highlights the differences in size and charge, which explain why SrS has a much more exothermic lattice energy compared to RbCl.
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