Domanda del libro di testo
(a) What is the general relationship between the size of an atom and its first ionization energy?
573
views
Ch.7 - Periodic Properties of the Elements
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 7, Problema 41b
(b) Which element in the periodic table has the largest ionization energy? Which has the smallest?
Guida verificata passo dopo passo1
1. Ionization energy is the energy required to remove an electron from an atom or ion. It is an indication of how tightly an atom holds onto its electrons. The larger the ionization energy, the harder it is to remove an electron.
2. In general, ionization energy increases from left to right across a period (horizontal row) in the periodic table. This is because as you move across a period, the number of protons in the nucleus increases, which means the positive charge of the nucleus increases. This stronger positive charge pulls the electrons in the atom closer to the nucleus, making them harder to remove.
3. Ionization energy also generally decreases from top to bottom down a group (vertical column) in the periodic table. This is because as you move down a group, the electrons are further from the nucleus and are therefore easier to remove.
4. Therefore, the element with the largest ionization energy is typically found in the top right corner of the periodic table (excluding the noble gases). This is because it is furthest to the right (so it has a high nuclear charge) and at the top (so the electrons are close to the nucleus).
5. Conversely, the element with the smallest ionization energy is typically found in the bottom left corner of the periodic table. This is because it is furthest to the left (so it has a low nuclear charge) and at the bottom (so the electrons are far from the nucleus).
Risposta video verificata per un problema simile:
Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
2mConcetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Ionization Energy
Ionization energy is the energy required to remove an electron from an atom or ion in its gaseous state. It is a key indicator of how strongly an atom holds onto its electrons. Generally, ionization energy increases across a period from left to right due to increasing nuclear charge and decreases down a group as the distance between the nucleus and the outermost electrons increases.
Video consigliato:
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. Key trends include ionization energy, electronegativity, and atomic radius. Understanding these trends helps in predicting the behavior of elements, including which will have the highest or lowest ionization energies.
Video consigliato:
Percorso guidato
00:38Periodic Trends
Noble Gases and Alkali Metals
Noble gases, located in Group 18 of the periodic table, typically have the highest ionization energies due to their stable electron configurations. In contrast, alkali metals in Group 1 have the lowest ionization energies because they have a single electron in their outermost shell, which is easily removed. This distinction is crucial for identifying the elements with the largest and smallest ionization energies.
Video consigliato:
Percorso guidato
00:44Noble Gas Compounds Example
Pratica correlata
Domanda del libro di testo
Identify each statement as true or false:
(a) Ionization energies are always endothermic.
(b) Potassium has a larger first ionization energy than lithium.
(c) The second ionization energy of the sodium atom is larger than the second ionization energy of the magnesium atom.
(d) The third ionization energy is three times the first ionization energy of an atom.
675
views
Domanda del libro di testo
Based on their positions in the periodic table, predict which atom of the following pairs will have the smaller first ionization energy: (a) Br, Kr (b) C, Ca (c) Li, Rb (d) S, Ge (e) Al, B.
731
views
Domanda del libro di testo
Which element has the highest second ionization energy: Li, K, or Be?
721
views