Given below are two statements:
Statement I: 
is the correct order in terms of metallic character.
Statement II: Atomic radius is always greater than the ionic radius for any element.
In the light of the above statements, choose the correct answer from the options given below
Text Solution
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Statement I: Metallic character decreases from left to right across a period and increases down a group. K (Group 1, Period 4) is the most metallic element among these. Mg (Group 2, Period 3) is less metallic than 
(Group 13, Period 3) is less metallic than Mg. B (Group 13, Period 2) is a metalloid with the least metallic character. The order 
correctly represents decreasing metallic character. TRUE.
Statement II: Atomic radius compared to ionic radius depends on whether the ion is a cation or anion. For metals forming cations: atomic radius > cationic radius (e.g., 
). However, for nonmetals forming anions: atomic radius < anionic radius (e.g., 
). The statement claims atomic radius is ALWAYS greater for ANY element, which is incorrect because anions have larger radii than their parent atoms. FALSE.
Correct answer: Statement I is true but Statement II is false.
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