The electron being removed from an Al atom is a 3 p electron, which is shielded by the two 3 s electrons as well as all the inner core electrons. The electron being removed from a Mg atom is a 3 s electron, which is only shielded by the inner core electrons.
Since there is a greater degree of electron shielding in the Al atom, it is slightly easier to remove the valence electron and its ionization energy is less than that of Mg. This is despite the fact that the nucleus of the Al atom contains one more proton than the nucleus of the Mg atom. There is another anomaly between Groups 15 and Atoms of Group 16 O, S, etc. In a nitrogen atom, there are three electrons in the 2 p sublevel and each is unpaired.
In an oxygen atom, there are four electrons in the 2 p sublevel, so one orbital contains a pair of electrons. It is that second electron in the orbital that is removed in the ionization of an oxygen atom. Since electrons repel each other, it is slightly easier to remove the electron from the paired set in the oxygen atom than it is to remove an unpaired electron from the nitrogen atom.
Use the link below to answer the following questions:. Skip to main content. The Periodic Table. Search for:. Electron Shielding Learning Objectives Define electron shielding. Explain sublevel shielding. This states that the position and the velocity of an object cannot both be measured exactly, at the same time, and since we can determine the velocity of the electron, knowing the location with certainty is not possible.
The main reason behind this is that as soon as you "look" at the electron, using whatever method available, you will by the very nature of looking at it, alter its position. Chrome will not alter MacAfee software easily.
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If you have a nonmodifiable risk factor for a disease what should you do? Study Guides. Trending Questions. Therefore, it becomes more and more difficult to remove the valence shell electron. Hence, ionization energy increases with increase in nuclear charge. In this section we shall see, how nuclear charge affects ionization energy?
In this section we shall see, how penetration effect affects ionization energy? How does penetration effect affect ionization energy?
In this section we shall see, how electron configuration affects ionization energy? How does electron configuration affect ionization energy? The electronic configuration of an atom may also affect the value of its ionization energy. Half filled and completely filled shells are found to possess extra stability. The atoms having completely filled shells are said to possess stable electronic configuration. The atoms having filled shells also show an extra stability. Such atoms possess a tendency to lose the valence electron and consequently have higher values of ionization energies.
Helium possesses a stable electronic configuration 1s 2. In it the K shell is completely filled. This is why the ionization energy of helium is much greater than that of hydrogen. Other gases also possess completely filled shells with stable configuration ns 2 np 6. Therefore the noble gases have very high values of ionization energy. Elements like Be, Mg etc. Therefore these elements also have higher ionization energies.
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