Answer:
C. Barium (Ba) has more energy shells for electrons than magnesium (Mg).
Even B could be correct, but nucleus doesn't repel electrons, but it attracts electrons. Electrons repel electrons
Step-by-step explanation:
Barium and Magnesium are both in Group II
Down the group, nuclear charge increases due to increase in atomic number (addition of protons). But the screening/shielding effect increases down the group since electrons are added to the different energy levels. But the increase in screening effect outweighs the increase in nuclear charge
As a result, Effective nuclear Charge decreases hence atomic radius increases from Barium to Magnesium
- Nuclear charge is the force of attraction by the nucleus towards incoming electrons (nuclear attraction)
Glossary:
- Screening/shielding effect is the tendency of electrons repel the incoming electrons.
- Effective nuclear charge is the overall nuclear attraction of an atom.