Domanda del libro di testo
Identify each statement as true or false: (b) Li+ is smaller than Li.
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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 26b
Using only the periodic table, arrange each set of atoms in order of increasing radius. b. In, Sn, As
Guida verificata passo dopo passo1
Identify the position of each element on the periodic table: Indium (In), Tin (Sn), and Arsenic (As) are all located in period 5, but in different groups.
Recall the periodic trend: Atomic radius increases as you move down a group and decreases as you move across a period from left to right.
Compare the elements based on their group positions: In (Group 13), Sn (Group 14), and As (Group 15).
Since all elements are in the same period, the atomic radius decreases from left to right across the period.
Arrange the elements in order of increasing atomic radius: As, Sn, In.
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Atomic Radius
Atomic radius is a measure of the size of an atom, typically defined as the distance from the nucleus to the outermost electron shell. It 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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Percorso guidato
02:02
Atomic Radius
Periodic Trends
Periodic trends refer to predictable patterns in the properties of elements as you move across or down the periodic table. Key trends include atomic radius, ionization energy, and electronegativity. Understanding these trends helps in predicting the behavior of elements and their compounds, including how they compare in size.
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00:38Periodic Trends
Element Classification
Elements in the periodic table are classified into groups and periods based on their properties. For example, In (Indium), Sn (Tin), and As (Arsenic) belong to different groups, with Indium and Tin being metals and Arsenic being a metalloid. This classification affects their atomic radii and helps in understanding their relative sizes.
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01:39Element Classification Example
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Using only the periodic table, arrange each set of atoms in order from largest to smallest: (a) Ar, As, Kr (b) Cd, Rb, Te (c) F, O, N.
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For each set of atoms and ions, pick the smallest one.
a. I, I+, I−
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Identify each statement as true or false: (a) Cations are larger than their corresponding neutral atoms.
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The experimental Bi─I bond length in bismuth triiodide, Bil3, is 2.81 Å. Based on this value and the data in Figure 7.7, predict the atomic radius of Bi.
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Domanda del libro di testo
Estimate the As¬I bond length from the data in Figure 7.7 and compare your value to the experimental As ¬I bond length in arsenic triiodide, AsI3, 2.55 Å.
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