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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Ch.7 - Periodic Properties of the Elements
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 7, Problema 33a
Consider S, Cl, and K and their most common ions. (a) List the atoms in order of increasing size.
Guida verificata passo dopo passo1
Identify the most common ions for sulfur (S), chlorine (Cl), and potassium (K). Sulfur commonly forms S^2-, chlorine forms Cl^-, and potassium forms K^+.
Recall that cations (positively charged ions) are generally smaller than their neutral atoms due to loss of electrons which reduces electron-electron repulsion and allows the nucleus to pull the remaining electrons closer. Anions (negatively charged ions) are generally larger than their neutral atoms because the addition of electrons increases electron-electron repulsion, causing the electron cloud to expand.
Compare the charges of the ions: K^+ (a cation), Cl^- (an anion), and S^2- (an anion with a higher negative charge than Cl^-).
Understand that the size of ions increases as the magnitude of the negative charge increases. Therefore, among anions, those with higher negative charges are larger because they have more electrons for the same number of protons in the nucleus.
Arrange the ions in order of increasing size based on the above understanding: K^+ (smallest), Cl^-, S^2- (largest).
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Atomic Radius
The atomic radius is a measure of the size of an atom, typically defined as the distance from the nucleus to the outermost electron shell. Atomic size generally increases down a group in the periodic table due to the addition of electron shells, while it decreases across a period from left to right due to increased nuclear charge, which pulls electrons closer to the nucleus.
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02:02
Atomic Radius
Ionic Size
Ionic size refers to the size of an ion, which can differ significantly from the neutral atom. Cations (positively charged ions) are smaller than their parent atoms because they lose one or more electrons, reducing electron-electron repulsion and allowing the remaining electrons to be pulled closer to the nucleus. Conversely, anions (negatively charged ions) are larger than their parent atoms due to the addition of electrons, which increases repulsion among electrons.
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00:50Ionic Salts
Periodic Trends
Periodic trends are patterns observed in the periodic table that describe how certain properties of elements change across periods and down groups. For atomic and ionic sizes, the trend shows that as you move from left to right across a period, the size decreases, while moving down a group increases the size. Understanding these trends is essential for predicting the relative sizes of atoms and their ions.
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00:38Periodic Trends
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