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The smaller the atomic radius in an element, the more ionization energy it will have. So when you go across the periodic table, the IE will decrease.
Considering the definition of ionization energy, in a group, the ionization energy increases upwards and in the same period, in general, it increases as you shift to the right.
Ionization energy is the energy required to separate an electron from a gaseous atom, isolated and in a ground state. Electrons are attracted to the nucleus, so it is necessary to provide energy to separate them. You should keep in mind that the electrons of the last layer are always lost, because they are the weakest attracted to the nucleus.
In a group, the ionization energy increases upwards because when passing from one element to the bottom, it contains one more layer of electrons. Therefore, the valence layer electrons, being further away from the nucleus, will be less attracted to it and it will cost less energy to pluck them.
In the same period, in general, it increases as you shift to the right. This is because the elements in this way have a tendency to gain electrons and therefore it will cost much more to tear them off than those on the left which, having few electrons in the last layer will cost them much less to lose them.
In summary, in a group, the ionization energy increases upwards and in the same period, in general, it increases as you shift to the right.
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