Domanda del libro di testo
True or false? c. S2− is larger than K+.
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Ch.7 - Periodic Properties of the Elements
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 7, Problema 36b
In the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation–anion distances are 2.01 Å (Li–F), 2.82 Å (Na–Cl), 3.30 Å (K–Br), and 3.67 Å (Rb–I), respectively. b. Calculate the difference between the experimentally measured ion–ion distances and the ones predicted from Figure 7.8.
Guida verificata passo dopo passo1
Identify the experimentally measured cation–anion distances for each ionic compound: LiF (2.01 Å), NaCl (2.82 Å), KBr (3.30 Å), and RbI (3.67 Å).
Refer to Figure 7.8 to find the predicted ion–ion distances for each of the ionic compounds based on the ionic radii of the cations and anions involved.
Subtract the predicted ion–ion distance from the experimentally measured distance for each compound to find the difference.
Express the differences in distances for each compound in Ångströms (Å).
Review the differences to understand any trends or discrepancies between the experimental and predicted values.
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Ionic Bonding
Ionic bonding occurs when atoms transfer electrons, resulting in the formation of charged ions. Cations (positively charged) and anions (negatively charged) attract each other due to electrostatic forces, creating ionic compounds. Understanding this concept is crucial for analyzing the properties and distances between ions in compounds like LiF, NaCl, KBr, and RbI.
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01:49
Chemical Bonds
Cation-Anion Distances
Cation-anion distances refer to the measured distances between the centers of cations and anions in an ionic compound. These distances can be influenced by factors such as ionic size, charge, and the lattice structure of the compound. Analyzing these distances helps in understanding the stability and strength of ionic bonds in different compounds.
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00:31Cation Solubility
Experimental vs. Predicted Values
In chemistry, comparing experimental measurements with predicted values allows for the validation of theoretical models. In this context, the experimentally measured ion-ion distances can be compared to those predicted from established models or figures, such as Figure 7.8. This comparison helps identify discrepancies that may arise from factors like ionic radii or lattice energy.
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05:50Experimental Error
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In the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation–anion distances are 2.01 Å (Li–F), 2.82 Å (Na–Cl), 3.30 Å (K–Br), and 3.67 Å (Rb–I), respectively. c. What estimates of the cation–anion distance would you obtain for these four compounds using neutral atom bonding atomic radii? Are these estimates as accurate as the estimates using ionic radii?
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Write the electron configurations for the following ions, and determine which have noble-gas configurations.
a. Ru3+
b. As3−
c. Y3+
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