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 25
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.
Guida verificata passo dopo passo1
Identify the position of each element (F, O, N) on the periodic table. Note that they are located in the second period.
Understand that atomic size decreases across a period from left to right due to the increase in the number of protons in the nucleus, which pulls the electrons closer.
Locate the elements in the periodic table: Nitrogen (N) is in Group 15, Oxygen (O) is in Group 16, and Fluorine (F) is in Group 17.
Since atomic size decreases from left to right across a period, the order from largest to smallest atomic size in the second period for these elements is N > O > F.
Arrange the atoms accordingly based on their atomic size: Nitrogen (N) is the largest, followed by Oxygen (O), and Fluorine (F) is the smallest.
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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 radius generally decreases across a period from left to right due to increased nuclear charge, which pulls electrons closer to the nucleus. Conversely, it increases down a group as additional electron shells are added, resulting in larger atomic sizes.
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02:02
Atomic Radius
Periodic Trends
Periodic trends refer to the predictable patterns observed 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, such as their size, reactivity, and bonding characteristics.
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00:38Periodic Trends
Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. While it primarily influences bonding behavior, it is also related to atomic size; smaller atoms with higher electronegativity tend to have stronger attractions for electrons. This concept is important for understanding how elements interact and form compounds.
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02:10Electronegativity Trends
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Identify each statement as true or false: (a) Cations are larger than their corresponding neutral atoms.
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Using only the periodic table, arrange each set of atoms in order of increasing radius. b. In, Sn, As
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Which of the following statements about the bonding atomic radii in Figure 7.7 is incorrect? (i) For a given period, the radii of the representative elements generally decrease from left to right across a period. (ii) The radii of the representative elements for the n = 3 period are all larger than those of the corresponding elements in the n = 2 period. (iii) For most of the representative elements, the change in radius from the n = 2 to the n = 3 period is greater than the change in radius from n = 3 to n = 4. (iv) The radii of the transition elements generally increase moving from left to right within a period. (v) The large radii of the Group 1 elements are due to their relatively small effective nuclear charges.
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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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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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