lonization energy (E;) is the amount of energy required to remove an electron from a neutral gaseous atom or gaseous ion. Electrons are attracted to the positively charged nucleus; therefore removing an electron requires energy. The process is endothermic, and so ionization energies have a positive value. The first ionization energy (Ei1) is the energy associated with the removal of an electron from the neutral gaseous atom. The reaction is represented for the generalized atom X as Part A Based on position in the periodic table and electron configuration, arrange these elements in order of decreasing Rank the elements from highest to lowest ionization energy. To rank items as equivalent, overlap them. • View Available Hint(s) X-X+ +e Reset Help The amount of energy required to remove an electron is related to the effective nuclear charge and the stability of the electron configuration of the atom. It therefore shows periodic variation generally increasing from left to right in a period and from bottom to top of a group. In general, metals have lower E values than nonmetals. Exceptions to this general trend from left to right occur when a completely filled s subshell or half-filled p subshell is encountered. These stable configurations have larger than expected E values. OPSAI Na K Highest ionization energy Lowest ionization energy
lonization energy (E;) is the amount of energy required to remove an electron from a neutral gaseous atom or gaseous ion. Electrons are attracted to the positively charged nucleus; therefore removing an electron requires energy. The process is endothermic, and so ionization energies have a positive value. The first ionization energy (Ei1) is the energy associated with the removal of an electron from the neutral gaseous atom. The reaction is represented for the generalized atom X as Part A Based on position in the periodic table and electron configuration, arrange these elements in order of decreasing Rank the elements from highest to lowest ionization energy. To rank items as equivalent, overlap them. • View Available Hint(s) X-X+ +e Reset Help The amount of energy required to remove an electron is related to the effective nuclear charge and the stability of the electron configuration of the atom. It therefore shows periodic variation generally increasing from left to right in a period and from bottom to top of a group. In general, metals have lower E values than nonmetals. Exceptions to this general trend from left to right occur when a completely filled s subshell or half-filled p subshell is encountered. These stable configurations have larger than expected E values. OPSAI Na K Highest ionization energy Lowest ionization energy
Principles of Instrumental Analysis
7th Edition
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Chapter6: An Introduction To Spectrometric Methods
Section: Chapter Questions
Problem 6.9QAP: Cesium is used extensively in photocells and in television cameras because it has the lowest...
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