Domanda del libro di testo
True or false? c. S2− is larger than K+.
3
views
Ch.7 - Periodic Properties of the Elements
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
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 34
Arrange each of the following sets of atoms and ions in order of increasing size. Se2−,Te2−, Se
Guida verificata passo dopo passo1
Identify the periodic trend: Atomic and ionic size increases as you move down a group in the periodic table.
Recognize that Se and Te are in the same group (Group 16) with Te below Se, so Te is larger than Se.
Consider the effect of gaining electrons: Anions are larger than their neutral atoms because the added electrons increase electron-electron repulsion.
Compare the sizes: Se is smaller than Se²⁻ because Se²⁻ has gained electrons, increasing its size.
Arrange the atoms and ions in order of increasing size: Se < Se²⁻ < Te²⁻.
Risposta video verificata per un problema simile:
Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
2mConcetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
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.
Video consigliato:
Percorso guidato
02:02
Atomic Radius
Ionic Radius
The ionic radius refers to the size of an ion in a crystal lattice. Cations (positively charged ions) are smaller than their parent atoms due to the loss of electron shells and increased effective nuclear charge, while anions (negatively charged ions) are larger due to the addition of electrons, which increases electron-electron repulsion in the outer shell.
Video consigliato:
Percorso guidato
02:47Ionic Radius
Comparison of Ions and Atoms
When comparing the sizes of atoms and ions, it is essential to consider their charge and position in the periodic table. For example, Se2− and Te2− are both anions, with Te2− being larger due to its position below Se in the periodic table. In contrast, neutral Se is smaller than both anions, as it has fewer electrons and less electron-electron repulsion.
Video consigliato:
Percorso guidato
2:38Atomic Mass Comparison Example
Pratica correlata
Domanda del libro di testo
Consider S, Cl, and K and their most common ions. (a) List the atoms in order of increasing size.
681
views
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.
2
views
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.
664
views
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?
2
views