Shielding or principal quantum number predicts Covalent or Ionic?

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The discussion centers on the comparison of covalency between HgCl2 and CaCl2, concluding that HgCl2 exhibits greater covalent character due to the presence of additional p and s orbital shells in Hg^2+. These extra shells provide significant shielding, affecting the attraction between Hg^2+ and the chlorine atoms. The analysis employs the Bohr model to illustrate how the valence electrons of Hg are positioned further from the nucleus, enhancing their interaction with the chlorine electron cloud in HgCl2 compared to the ionic nature of CaCl2.

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TL;DR Summary: Why is HgCl2 more covalent than CaCl2 via shielding?

Hg^2+ in HgCl_2 has more shells of p-orbitals and s-orbitals than Ca^2+ in CaCl2
- Do those extra p and s shells of Hg^2 in HgCl2 shield the two chlorines in HgCl2 from the effect of Hg^2+'s nucleus attraction, or leave the Hg^2+ valence electrons attracted to the chlorine electron cloud in HgCl2 because by the Bohr model the valence electrons of Hg are further apart from its nucleus and should be closer to the chlorine in HgCl2?
- How can shielding or principal quantum number of the cation explain whether some bond is more covalent or ionic?
 

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