Domanda del libro di testo
Arrange each of the following sets of atoms and ions in order of increasing size. Se2−,Te2−, Se
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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 35c
True or false? c. S2− is larger than K+.
Guida verificata passo dopo passo1
Identify the ions involved: \( \text{S}^{2-} \) and \( \text{K}^+ \).
Understand that \( \text{S}^{2-} \) is a sulfide ion, which has gained 2 electrons, and \( \text{K}^+ \) is a potassium ion, which has lost 1 electron.
Consider the electron configuration: \( \text{S}^{2-} \) has the electron configuration of \( \text{Ar} \) (18 electrons), and \( \text{K}^+ \) also has the electron configuration of \( \text{Ar} \) (18 electrons).
Recognize that both ions are isoelectronic, meaning they have the same number of electrons.
Compare the nuclear charge: \( \text{S}^{2-} \) has a lower nuclear charge (16 protons) compared to \( \text{K}^+ \) (19 protons), which means \( \text{S}^{2-} \) is larger due to less effective nuclear attraction on the same number of electrons.
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Ionic Radius
Ionic radius refers to the size of an ion in a crystal lattice. Cations, like K+, are smaller than their neutral atoms due to the loss of electrons, which reduces electron-electron repulsion and allows the remaining electrons to be pulled closer to the nucleus. Conversely, anions, such as S2−, are larger than their neutral atoms because the addition of electrons increases repulsion among them, causing the electron cloud to expand.
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02:47
Ionic Radius
Charge and Size Relationship
The charge of an ion significantly influences its size. Anions (negatively charged ions) are generally larger than their neutral atoms due to increased electron repulsion, while cations (positively charged ions) are smaller due to decreased electron-electron repulsion. This relationship is crucial for comparing the sizes of different ions, as the charge directly affects the ionic radius.
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01:53Formal Charge
Comparison of Ions
When comparing the sizes of different ions, it is essential to consider both their charges and the number of electrons. In this case, S2− has gained two electrons, resulting in a larger size, while K+ has lost one electron, making it smaller. Understanding these differences allows for accurate comparisons between ions, such as determining whether S2− is larger than K+.
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06:17Ion Formation
Pratica correlata
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Consider S, Cl, and K and their most common ions. (a) List the atoms in order of increasing size.
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Domanda del libro di testo
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.
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Domanda del libro di testo
Consider S, Cl, and K and their most common ions. (b) List the ions in order of increasing size. (c) Explain any differences in the orders of the atomic and ionic sizes.
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Domanda del libro di testo
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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Domanda del libro di testo
Write the electron configurations for the following ions, and determine which have noble-gas configurations.
a. Ru3+
b. As3−
c. Y3+
d. Pd2+
e. Pb2+
f. Au3+
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