This means the outermost electron is more loosely held down the group and so less energy is required to remove it. Thus, 1 st IE decreases down the group. We can use these three properties to explain the trend in first ionisation energy: 1 st IE decreases down the group: this is because the number of filled shells increases down the group, increasing shielding and the distance between the nucleus and the outermost electrons, for very similar effective nuclear charge.
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