Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Sr and Se b. Ba and Cl c. Na and S d. Al and O
Ch.9 - Chemical Bonding I: The Lewis Model
Chapter 9, Problem 44
Rubidium iodide has a lattice energy of -617 kJ/mol, while potassium bromide has a lattice energy of -671 kJ/mol. Why is the lattice energy of potassium bromide more exothermic than the lattice energy of rubidium iodide?
Verified Solution
Video duration:
4mThis video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Lattice Energy
Lattice energy is the amount of energy released when gaseous ions combine to form an ionic solid. It is a measure of the strength of the forces between the ions in an ionic compound. A more negative lattice energy indicates a more stable ionic compound, as it reflects a greater release of energy upon formation.
Recommended video:
Guided course
00:49
Lattice Energy
Ionic Size and Charge
The size and charge of the ions involved in an ionic compound significantly influence lattice energy. Smaller ions can pack more closely together, leading to stronger electrostatic attractions and higher lattice energy. Additionally, ions with higher charges produce stronger interactions, resulting in more exothermic lattice energies.
Recommended video:
Guided course
01:53
Formal Charge
Comparative Analysis of Ionic Compounds
When comparing ionic compounds like rubidium iodide and potassium bromide, it is essential to consider the specific ions involved. Potassium (K+) and bromide (Br-) ions are smaller and have higher charge density compared to rubidium (Rb+) and iodide (I-), which contributes to the greater lattice energy of potassium bromide, making it more exothermic than rubidium iodide.
Recommended video:
Guided course
02:11
Ionic Compounds Naming
Related Practice
Textbook Question
992
views
1
rank
Textbook Question
Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Ca and N b. Mg and I c. Ca and S d. Cs and F
1732
views
Open Question
What is the trend in the lattice energies of alkaline earth metal oxides? Here are the lattice energies (in kJ/mol): MgO -3795, CaO -3414, SrO -3217, BaO -3029.
Textbook Question
The lattice energy of CsF is -744 kJ/mol, whereas that of BaO is -3029 kJ/mol. Explain this large difference in lattice energy.
2194
views
Textbook Question
Use the Born–Haber cycle and data from Appendix IIB, Chapter 8 and this chapter to calculate the lattice energy of KCl. (ΔHsub for potassium is 89.0 kJ/mol.)
849
views
1
rank
2
comments
Textbook Question
Use the Born–Haber cycle and data from Appendix IIB and Table 9.3 to calculate the lattice energy of CaO. (ΔHsub for calcium is 178 kJ/mol; IE1 and IE2 for calcium are 590 kJ/mol and 1145 kJ/mol, respectively; EA1 and EA2 for O are -141 kJ/mol and 744 kJ/mol, respectively.)
2604
views
2
comments