Why do the first ionisation energies of the atoms in group 1 decrease as the atomic number increases?
Answer:
Atomic radius increases down the group. So outermost electrons are further away from nucleus, and nuclear attraction decreases as a result. Therefore first IE decreases down Group 1.
The ionization energy of an atom is the amount of energy required to separate an electron from the neutral atom. It is the energy needed to overcome the force of attaction, Fc, between the nucleus and the electron that is farthest from it. In groups, ionization energy decreases when atomic number increases because the added energy levels shield the power of the nuclear charge making it easier to remove outmost electrons.
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