Atomic Radius Increase Up Periodic Table: Why?

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SUMMARY

The atomic radius increases up the periodic table due to the effect of electron shielding and the geometry of higher orbitals. As protons increase, inner electrons shield the nucleus, preventing outer electrons from experiencing the full nuclear charge. This results in a larger atomic radius despite the increased number of protons. Additionally, the eccentric geometry of higher orbitals contributes to the overall size of the atom.

PREREQUISITES
  • Understanding of atomic structure and electron configuration
  • Knowledge of electron shielding effects
  • Familiarity with periodic trends in chemistry
  • Concept of orbital geometry and its implications
NEXT STEPS
  • Research the concept of electron shielding in detail
  • Explore periodic trends, focusing on atomic radius and ionization energy
  • Study the geometry of atomic orbitals and their impact on atomic size
  • Examine the relationship between nuclear charge and electron behavior
USEFUL FOR

Chemistry students, educators, and professionals interested in atomic theory and periodic trends will benefit from this discussion.

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If an atom with more protons have tighter electron orbitals than atoms with fewer protons, why doesn't the "atomic radius" decrease up the periodic table? Instead it increases, why is this?
 
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Shielding. The inner electrons shield the nucleus from the outer electrons, so they do not have the full nuclear potential.

Furthermore, higher orbitals have very eccentric geometry which is included in what we define as the "size" of an atom.

Zz.
 

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