Taking into account the definition if ionic radius, as the atomic number of the metals of Group 1 increases, the ionic radius increases.
The ionic radius is, like the atomic radius, the distance between the center of the nucleus of the atom and the most distant stable electron, but referring not to the atom, but to the ion.
An ion is a chemical species with a charge, either positive or negative, and they originate because the elements try to resemble the closest noble gas, since they have a superior stability because their energy levels are complete.
So, the ionic radius is the radius that an atom has when it has lost or gained electrons, acquiring the electronic structure of the closest noble gas.
The effective nuclear charge is the charge that the nucleus should have so that, in the absence of other electrons, the attraction of the nucleus on the considered electron would be the same as the net attraction that the electron experiences in the real atom.
As the atomic number of the elements in a group increases, the number of occupied levels increases, while the effective nuclear charge on the outermost electron is the same. So the ionic radius increases as a group on the periodic table descends because a shell of electrons is added to the atoms.
In summary, as the atomic number of the metals of Group 1 increases, the ionic radius increases.
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