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Kelly09
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i am stuck on this question and people are giving me different answers. Ok which period 3 element has the following succesive ionization energies: 1800,3000,3600,5800,13200
Ionization energy is the amount of energy required to remove an electron from an atom or molecule, resulting in the formation of a positively charged ion.
Period 3 ionization energy is higher than the previous two periods due to the increased number of protons in the nucleus and the smaller atomic radius. This makes it more difficult to remove an electron from the outermost energy level.
The increase in ionization energy across period 3 is due to the increasing number of protons in the nucleus, which leads to a stronger attraction between the nucleus and the electrons in the outermost energy level. This makes it more difficult to remove an electron and increases the ionization energy.
The trend of ionization energy within a period 3 group is that it generally decreases as you move down the group. This is because the outermost electrons are farther from the nucleus, making them easier to remove.
The shielding effect, which is the repulsion between electrons in different energy levels, decreases the effective nuclear charge experienced by the outermost electrons. This results in a decrease in ionization energy as you move down the group in period 3.