why nuclear charge is more in group 15 than group 14 the explain
Answers
Answer:
While ionization energy is the energy change incurred from losing an electron, electron affinity is the energy change incurred from gaining an electron.
Cl(g) + e-→Cl-(g)
For most atoms, this is a negative quantity - or energy is released. For some elements, however, this is not the case. Most notably, noble gases have a positive electron affinity, meaning it actually requires input of energy to add another electron.
In general, electron affinity increases (or becomes more negative) from left to right across a period. This is due to increasing effective nuclear charge, which more readily pulls these new electrons in.
In general, electron affinity decreases (or becomes less negative) from top to bottom down a group. This change is not as drastic as we see across a period, however. This is due to a balance between increasing atomic radii and decreasing electron-electron repulsions. As we move down a group, the atomic radii increases, meaning these electrons are farther away from the nucleus and thus experience less of an electron-nucleus attraction. Along with this, however, because the valence shells are larger as atomic radii increases, the electrons in those valence shells do not have to be as close to one another and so they do not experience electron-electron repulsions as much. So a lower electron-nucleus attraction is counterbalanced by lower electron-electron repulsions.
Explanation:
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Answer:
because according to periodic table when we go down in a group the no of electrons increases along with the charges