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rdgt3000
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which atom has a larger atomic radius: K+ or Ar ?
Which Atom Has a Larger Atomic Radius: K+ or Ar?
- Thread starter rdgt3000
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- Atomic Atomic radii
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SUMMARY
The discussion centers on the comparison of atomic radii between the potassium ion (K+) and argon (Ar). Despite both having the same number of electrons, K+ has fewer protons (19) compared to argon (18), leading to a larger ionic radius for K+. The general periodic trend indicates that as the atomic number increases, the atomic radius decreases when the outermost electron shell remains constant. Therefore, K+ exhibits a larger radius than Ar due to its lower nuclear charge.
PREREQUISITES- Understanding of atomic structure and electron configuration
- Familiarity with periodic trends in atomic and ionic radii
- Knowledge of nuclear charge and its effect on atomic size
- Basic concepts of ions and their formation
- Research the concept of nuclear charge and its impact on atomic size
- Study periodic trends in atomic and ionic radii across different groups and periods
- Explore the differences between cations and anions in terms of size
- Learn about the factors influencing atomic radius, such as electron shielding and effective nuclear charge
Chemistry students, educators, and anyone interested in atomic structure and periodic trends will benefit from this discussion.
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