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Which is true about ionisation energy and its trends found in the periodic table
Accepted Answer
Ionization energy is the minimum energy required to remove an electron from a gaseous atom or ion in its ground electronic state. Here's a summary of trends in the periodic table:
Increases across a period: As you move from left to right across a period, the ionization energy generally increases. This is because the atomic radius decreases, leading to a stronger attraction between the nucleus and the outermost electrons.
Decreases down a group: As you move down a group, the ionization energy generally decreases. This is because the atomic radius increases, resulting in a weaker attraction between the nucleus and the outermost electrons.
It's important to note that there are exceptions to these trends due to factors like electron configuration and shielding effects.
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