Domanda del libro di testo
Why is the ionization energy of Ca higher than K, but lower than that of Mg?
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Ch.4 Atoms and Elements
Timberlake13th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9780134421353
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TOC.tableOfContents
- Ch.1 Chemistry in Our Lives11
- Ch.2 Chemistry and Measurements80
- Ch.3 Matter and Energy54
- Ch.4 Atoms and Elements51
- Ch.5 Nuclear Chemistry42
- Ch.6 Ionic and Molecular Compounds57
- Ch.7 Chemical Quantities and Reactions41
- Ch.8 Gases29
- Ch.9 Solutions51
- Ch.10 Acids and Bases and Equilibrium65
- Ch.11 Introduction to Organic Chemistry: Hydrocarbons78
- Ch.12 Alcohols, Thiols, Ethers, Aldehydes, and Ketones83
- Ch.13 Carbohydrates54
- Ch.14 Carboxylic Acids, Esters, Amines, and Amides90
- Ch.15 Lipids61
- Ch.16 Amino Acids, Proteins, and Enzymes84
- Ch.17 Nucleic Acids and Protein Synthesis83
- Ch.18 Metabolic Pathways and ATP Production67
Timberlake13th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9780134421353Non è quello che usi tu?Cambia libro di testo
Capitolo 4, Problema 110
Why is the ionization energy of Cl lower than F, but higher than that of S?
Guida verificata passo dopo passo1
Ionization energy is the energy required to remove an electron from a neutral atom in the gaseous state. It depends on factors such as nuclear charge, electron shielding, and atomic radius.
Fluorine (F) has a smaller atomic radius than chlorine (Cl), meaning its valence electrons are closer to the nucleus and experience a stronger electrostatic attraction. This makes it harder to remove an electron from F, resulting in a higher ionization energy compared to Cl.
Chlorine (Cl) has a larger atomic radius than F, so its valence electrons are farther from the nucleus and experience slightly less attraction. This makes it easier to remove an electron from Cl, giving it a lower ionization energy than F.
Sulfur (S) has a larger atomic radius than Cl and also has one more electron in its valence shell. The additional electron increases electron-electron repulsion, which slightly reduces the effective nuclear attraction on the outermost electrons. This makes it easier to remove an electron from S, resulting in a lower ionization energy compared to Cl.
In summary, the ionization energy trend is influenced by atomic radius, nuclear charge, and electron shielding. F has the highest ionization energy due to its small size and strong nuclear attraction, Cl has a lower ionization energy than F but higher than S due to its intermediate size and shielding effects, and S has the lowest ionization energy among the three due to its larger size and increased electron repulsion.
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Ionization Energy
Ionization energy is the energy required to remove an electron from an atom in its gaseous state. It reflects the strength of the attraction between the nucleus and the electrons. Generally, ionization energy increases across a period due to increasing nuclear charge and decreases down a group due to increased electron shielding.
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Percorso guidato
02:13
Periodic Trend: Ionization Energy (Simplified) Concept 1
Atomic Structure and Electron Configuration
The atomic structure of an element, including its electron configuration, plays a crucial role in determining its ionization energy. Fluorine (F) has a higher ionization energy than chlorine (Cl) because it has a smaller atomic radius and fewer electron shells, leading to a stronger attraction between the nucleus and its outermost electron.
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01:08The Electron Configuration: Condensed
Electron Shielding
Electron shielding occurs when inner-shell electrons repel outer-shell electrons, reducing the effective nuclear charge felt by the outer electrons. In the case of sulfur (S), the additional electron shells compared to chlorine lead to greater shielding, resulting in a lower ionization energy for sulfur than for chlorine, despite sulfur being further down the periodic table.
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01:23Electronic Structure: Electron Spin Concept 1
Pratica correlata
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Write the name and symbol of the element with the following atomic number:
h. 92
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Domanda del libro di testo
Give the symbol of the element that has the
a. largest atomic size in Group 1A (1)
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Give the symbol of the element that has the
e. most metallic character in Group 2A (2)
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Give the symbol of the element that has the
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Domanda del libro di testo
Indicate if each of the following statements is true or false:
d. The proton and the electron have about the same mass.
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