Domanda del libro di testo
Pick the correct word to complete the sentence: The larger the atom, the (smaller/larger) its first ionization energy.
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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 47b
Which element in the periodic table has the largest first ionization energy?
Guida verificata passo dopo passo1
Understand that ionization energy is the energy required to remove an electron from an atom in the gaseous state.
Recall that ionization energy generally increases across a period (from left to right) on the periodic table due to increasing nuclear charge and decreasing atomic radius.
Remember that ionization energy generally decreases down a group (from top to bottom) because of increasing atomic radius and electron shielding.
Identify that the element with the largest first ionization energy will be located at the top right corner of the periodic table, excluding the noble gases.
Conclude that among the elements, the one with the largest first ionization energy is likely to be a halogen or a non-metal in the second period.
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Ionization Energy
Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It is a key indicator of how strongly an atom holds onto its electrons. Generally, ionization energy increases across a period in the periodic table due to increasing nuclear charge and decreases down a group due to increased distance from the nucleus and electron shielding.
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Percorso guidato
01:19
Ionization Energy
Periodic Trends
Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. For ionization energy, the trend shows that it increases from left to right across a period and decreases from top to bottom in a group. Understanding these trends helps in predicting the ionization energies of different elements.
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Percorso guidato
00:38Periodic Trends
Noble Gases
Noble gases, located in Group 18 of the periodic table, are known for their high ionization energies and low reactivity due to their full valence electron shells. Among the elements, helium has the highest first ionization energy, followed closely by neon. Their stable electron configurations make them less likely to lose electrons, contributing to their high ionization energies.
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00:44Noble Gas Compounds Example
Pratica correlata
Domanda del libro di testo
Identify each statement as true or false.
a. Ionization energies are always negative quantities.
b. Oxygen has a larger first ionization energy than fluorine.
c. The second ionization energy of an atom is always greater than its first ionization energy.
d. The third ionization energy is the energy needed to ionize three electrons from a neutral atom.
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Domanda del libro di testo
Which element has the highest second ionization energy: Li, K, or Be?
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Domanda del libro di testo
Would a neutral K atom or a K+ ion have a more negative value of electron affinity?
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