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The subshell with the lowest effective nuclear charge is typically the 1s subshell. This is because electrons in the 1s subshell are closest to the nucleus and experience a significant amount of shielding from other electrons, which can result in a lower effective nuclear charge for outer subshells. However, when considering only the 1s electrons, they experience the full nuclear charge but are also influenced by electron-electron repulsions, making the effective nuclear charge feel lower for electrons in higher subshells.
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What is the principal shell is the lowest that may contain a d-subshell?
The principal shell that is the lowest to contain a d-subshell is the third shell, or n=3. In this shell, the d-subshell begins to appear, specifically in the 3d sublevel. The d-subshell can be found in principal energy levels n=3 and higher (n=4 for 4d, n=5 for 5d, etc.).
What is the predicted order of first ionization energies from highest to lowest for aluminum phosphorus silicon and sulfur?
The predicted order of first ionization energies from highest to lowest is sulfur, phosphorus, silicon, and aluminum. This trend can be attributed to the increased effective nuclear charge and smaller atomic radius in sulfur compared to the others, leading to stronger attraction for the outer electrons. Phosphorus follows due to its similar group properties, while silicon and aluminum have lower ionization energies due to their larger atomic sizes and lower effective nuclear charge.
What is the order of increasing ionization between lead cesium and barium?
The order of increasing ionization energy among lead (Pb), barium (Ba), and cesium (Cs) is cesium < barium < lead. Cesium, being in Group 1, has the lowest ionization energy due to its larger atomic radius and lower effective nuclear charge. Barium, an alkaline earth metal, has a higher ionization energy than cesium but lower than lead, which is a post-transition metal with a higher effective nuclear charge and smaller atomic radius. Thus, the increasing order is Cs < Ba < Pb.
What makes isoelectronic biggest or smallest?
Isoelectronic species are atoms or ions that have the same number of electrons, resulting in similar electronic configurations. The size of these species can vary based on their nuclear charge; species with a higher positive charge (more protons) will attract electrons more strongly, resulting in a smaller radius. Conversely, species with a lower nuclear charge will be larger due to reduced attraction on the electron cloud. Therefore, within a set of isoelectronic species, the one with the highest nuclear charge is the smallest, while the one with the lowest charge is the largest.
Which atom has the lowest ionization energy in period 3?
In Period 3 of the periodic table, sodium (Na) has the lowest ionization energy. This is because ionization energy generally increases across a period due to increasing nuclear charge, which holds the electrons more tightly. Sodium, being the first element in Period 3, has a relatively low nuclear charge compared to the other elements in the same period, making it easier to remove its outermost electron.
Arrange the atoms icreasing order effective nuclear charge by the electron n3 electron shell K Mg P Rh Tithe explain basis for your order?
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What is the principal shell is the lowest that may contain a d-subshell?
The principal shell that is the lowest to contain a d-subshell is the third shell, or n=3. In this shell, the d-subshell begins to appear, specifically in the 3d sublevel. The d-subshell can be found in principal energy levels n=3 and higher (n=4 for 4d, n=5 for 5d, etc.).
What is the predicted order of first ionization energies from highest to lowest for aluminum phosphorus silicon and sulfur?
The predicted order of first ionization energies from highest to lowest is sulfur, phosphorus, silicon, and aluminum. This trend can be attributed to the increased effective nuclear charge and smaller atomic radius in sulfur compared to the others, leading to stronger attraction for the outer electrons. Phosphorus follows due to its similar group properties, while silicon and aluminum have lower ionization energies due to their larger atomic sizes and lower effective nuclear charge.
Based on the periodic table which element would be expected to have the lowest ionization energy?
Francium would be expected to have the lowest ionization energy, as it is located in the alkali metal group at the bottom left of the periodic table. Alkali metals typically have the lowest ionization energies due to their large atomic size and low effective nuclear charge.
What element of lowest atomic number contains a half filled d subshell at ground state?
The element with the lowest atomic number that contains a half-filled d subshell at its ground state is scandium (atomic number 21). The electron configuration of scandium at ground state is [Ar] 3d^1 4s^2, where the 3d subshell is half-filled with one electron.
What is the order of increasing ionization between lead cesium and barium?
The order of increasing ionization energy among lead (Pb), barium (Ba), and cesium (Cs) is cesium < barium < lead. Cesium, being in Group 1, has the lowest ionization energy due to its larger atomic radius and lower effective nuclear charge. Barium, an alkaline earth metal, has a higher ionization energy than cesium but lower than lead, which is a post-transition metal with a higher effective nuclear charge and smaller atomic radius. Thus, the increasing order is Cs < Ba < Pb.
What Element has lowest atomic number that contains a complete d sub shell at ground state?
The element with the lowest atomic number that has a complete d subshell at its ground state is Titanium (element 22). In its ground state, Titanium's electron configuration is [Ar] 3d2 4s2, which means the 3d subshell is completely filled with 2 electrons.
What makes isoelectronic biggest or smallest?
Isoelectronic species are atoms or ions that have the same number of electrons, resulting in similar electronic configurations. The size of these species can vary based on their nuclear charge; species with a higher positive charge (more protons) will attract electrons more strongly, resulting in a smaller radius. Conversely, species with a lower nuclear charge will be larger due to reduced attraction on the electron cloud. Therefore, within a set of isoelectronic species, the one with the highest nuclear charge is the smallest, while the one with the lowest charge is the largest.
Which atom has the lowest ionization energy in period 3?
In Period 3 of the periodic table, sodium (Na) has the lowest ionization energy. This is because ionization energy generally increases across a period due to increasing nuclear charge, which holds the electrons more tightly. Sodium, being the first element in Period 3, has a relatively low nuclear charge compared to the other elements in the same period, making it easier to remove its outermost electron.
What element has the LOWEST Ionization Energy Electron Affinity and Electronegativity?
The element with the lowest ionization energy, electron affinity, and electronegativity is francium (Fr). Francium is an alkali metal located at the bottom of Group 1 in the periodic table, which gives it a very low tendency to attract electrons and hold onto its own. Its large atomic size and low effective nuclear charge contribute to these low values, making it the least electronegative element.
Why is transfer of electron from 2s subshell to 1s subshell not possible?
Transfer of an electron from a higher energy orbit (2s) to a lower energy orbit (1s) is not possible because it would violate the energy conservation principle. Electrons naturally occupy the lowest available energy levels in an atom, following the Aufbau principle. This means electrons will only move to higher energy levels if they absorb energy, not by transferring between lower and higher energy levels.
What does cost effective mean?
Cost-effective is the principal of going for the lowest cost.
