Textbook Question
Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Sr and P b. Ba and S c. Sr and Se d. Rb and I
Ch.10 - Chemical Bonding I: The Lewis Model
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 10, Problem 48
Arrange these compounds in order of increasing magnitude of lattice energy: CaO, NaBr, CsI, BaS.
Verified step by step guidance1
Understand that lattice energy is the energy required to separate one mole of an ionic solid into its gaseous ions. It is influenced by the charge of the ions and the distance between them.
Recall that lattice energy increases with increasing charge of the ions and decreases with increasing ionic radius (distance between ions).
Identify the charges of the ions in each compound: CaO (Ca²⁺ and O²⁻), NaBr (Na⁺ and Br⁻), CsI (Cs⁺ and I⁻), BaS (Ba²⁺ and S²⁻).
Compare the ionic radii: Cs⁺ and I⁻ are larger than Na⁺ and Br⁻, and Ba²⁺ and S²⁻ are larger than Ca²⁺ and O²⁻.
Arrange the compounds by considering both the charges and the ionic radii: CsI < NaBr < BaS < CaO.
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. Higher lattice energy indicates stronger ionic bonds, which typically results from smaller ions with higher charges.
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00:49
Lattice Energy
Ionic Size and Charge
The size and charge of the ions in a compound significantly influence lattice energy. Smaller ions can pack more closely together, leading to stronger electrostatic attractions. Additionally, ions with higher charges produce stronger interactions, resulting in greater lattice energy compared to those with lower charges.
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Trends in Lattice Energy
Lattice energy trends can be predicted based on the ionic compounds' composition. Generally, for compounds with similar ionic charges, lattice energy increases with decreasing ionic size. For example, comparing compounds like NaBr and CsI, NaBr has a higher lattice energy due to the smaller size of Na+ compared to Cs+.
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