Atomic radii of fluorine and neon in angstroms units are respectively:
Correct answer: B. 0.72 and 1.60
- A. 1.60 and 1.60
- B. 0.72 and 1.60
- C. 0.72 and 0.72
- D. None of these
Explanation
The atomic radius of Fluorine is its covalent radius, which is small (~0.72 Å). For Neon, a noble gas that doesn't form covalent bonds, the van der Waals radius is measured, which is significantly larger (~1.60 Å) as it represents the distance between non-bonded atoms.
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About Periodic Properties and Trends
Periodic properties arise from electron configuration and effective nuclear charge, producing trends in atomic and ionic radius, ionization energy, electron affinity, electronegativity, metallic character and reactivity. Comparisons run across periods and down groups, with attention to common exceptions. The topic also relates these trends to the behavior of s-block and p-block elements.
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