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The noble gases, however, do not follow the general trend for electron affinities. They are small atoms and do follow the general trend for ionization energies. The major exception to this rule are the noble gases. Therefore, the small atoms tend to gain electrons and tend not to lose electrons. Since they are small, they have high ionization energies and high electron affinities. Small atoms, in general, are the opposite. Therefore, they tend to lose electrons and do not tend to gain electrons. Large atoms have low ionization energy and low electron affinity. This is because both electron affinity and ionization energy are highly related to atomic size.
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The general trend in the electron affinity for atoms is almost the same as the trend for ionization energy. Overall, the Periodic Table shows the general trend similar to the one below.Įlectron Affinities for Period 4 Main Group Elements Nonmetals Tend to Have the Highest Electron Affinity Electron affinity of all of the elements in the second period is less than the ones below them due to the fact that the elements in the second period have such small electron clouds that electron repulsion is greater than that of the rest of the family. For instance, the electron affinity for oxygen is less than the electron affinity for sulfur. This phenomenon is observed in other families as well. Electron affinity for fluorine is less than chlorine most likely due to the electron-electron repulsions that occur between the electrons where n = 2. There is an exception to this when it involves certain small atoms. Therefore, as the atoms in a family get larger, the electron affinity gets smaller. When an electron is added to a large atom, less energy is released because the electron cannot move as close to the nucleus as it can in a smaller atom.
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For example, an atom of chlorine is smaller than iodine or, an atom of oxygen is smaller than sulfur. Remember that the atoms located within a family but lower on the periodic table are larger since there are more electrons filling more energy levels. Table 10.10: Electron Affinities for Group 17Īs you can see, the electron affinity generally decreases (becomes less negative) going down a group because of the increase in size of the atoms. Take a look at Table 10.10, the electron affinity for the Halogen family. Let's look at the electron configurations of a few of the elements and the trend that develops within groups and periods. Electron affinity is defined as the energy released when an electron is added to a gaseous atom or ion. When an atom gains an electron, energy is given off and is known as the electron affinity. The Energy Process When an Electron is Added to an Atom Ītoms can gain or lose electrons. Describe the trend for electron affinity on the Periodic Table.And now, the final periodic trend we will study is how an atom can gain an electron and the trends that exist in the Periodic Table. We have talked about atomic structure, electronic configurations, size of the atoms and ionization energy. The final periodic trend for our discussion is electron affinity. 3 Nonmetals Tend to Have the Highest Electron Affinity.2 The Energy Process When an Electron is Added to an Atom.