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Na has a smaller first ionization energy compared to Cl as ionization energy increases across a row on the periodic table. This is because as you move across a row the numbers of protons and electrons increase making the attraction between the two greater as well. This makes it increasingly hard to remove an electron from elements like Cl.
The periodic trends show that ionization energy increases when moving left to right. This is because when moving left to right across a period, atomic radius decreases, so electrons are more attracted to the nucleus. With this in mind, since Na is further left, it will have a lower ionization energy than Al.
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