Domanda del libro di testo
Choose the element with the more negative (more exothermic) electron affinity from each pair. c. P or S
Ch.9 - Periodic Properties of the Elements
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 9, Problema 85b
Choose the element with the more negative (more exothermic) electron affinity from each pair. b. C or F
Guida verificata passo dopo passo1
Understand the concept of electron affinity: Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gaseous state. A more negative electron affinity indicates a greater tendency to accept an electron.
Consider the periodic trend: Electron affinity generally becomes more negative across a period from left to right due to increasing nuclear charge, which attracts electrons more strongly.
Identify the position of the elements in the periodic table: Carbon (C) is in group 14 and period 2, while Fluorine (F) is in group 17 and period 2.
Compare the elements based on their positions: Since both elements are in the same period, the trend suggests that the element further to the right (Fluorine) will have a more negative electron affinity.
Conclude based on the trend: Fluorine, being to the right of Carbon in the same period, is expected to have a more negative (more exothermic) electron affinity.
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Electron Affinity
Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gas phase. A more negative electron affinity indicates that the process is more exothermic, meaning energy is released when the atom gains an electron. This property is crucial for understanding how easily an atom can accept an electron and form an anion.
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01:34
Electron Affinity
Trends in Electron Affinity
Electron affinity varies across the periodic table, generally increasing (becoming more negative) from left to right and decreasing from top to bottom. This trend is due to the increasing nuclear charge and decreasing atomic radius, which enhance the attraction between the nucleus and the added electron. Understanding these trends helps predict the electron affinity of different elements.
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01:42Electron Affinity Trends
Comparison of Carbon and Fluorine
When comparing carbon (C) and fluorine (F), fluorine has a significantly more negative electron affinity than carbon. This is because fluorine, being more electronegative, has a stronger tendency to attract additional electrons, resulting in a more exothermic process. This comparison illustrates the importance of electronegativity in determining electron affinity.
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02:11Oxyacid Strength Comparison
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Consider this set of ionization energies.
IE1 = l000 kJ/mol
IE2 = 2250 kJ/mol
IE3 = 3360 kJ/mol
IE4 = 4560 kJ/mol
IE5 = 7010 kJ/mol
IE6 = 8500 kJ/mol
IE = 27,I00 kJ/mol
To which third-period element do these ionization values belong?