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Which is the correct order of ionic sizes (At. No. : Ce = 58, Sn = 50, Yb = 70 and Lu = 71) [AIEEE-2002]
a)Ce>Sn>Yb>Lu
b)Sn>Ce>Lu>Yb
c)Lu>Yb>Sn>Ce
d)Sn>Yb>Ce>Lu
Correct answer is option 'A'. Can you explain this answer?
Verified Answer
Which is the correct order of ionic sizes (At. No. : Ce = 58, Sn = 50,...
The answer is a.
Generally as we move from left to right in a period, there is regular decrease in atomic radii and in a group as the atomic number increases the atomic radii also increases. Thus the atomic radius of Sn should be less than lanthanides. La > Sn. But due to lanthanide contraction, in case of lanthanides there is a continuous decrease in size with increase in atomic number. Hence the atomic radius follow the given trend:
Ce > Sn > Yb > Lu. 
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Which is the correct order of ionic sizes (At. No. : Ce = 58, Sn = 50,...
4+ < sn4+="" />< yb3+="" />< />
b)Ce3+ < sn4+="" />< yb3+="" />< />
c)Lu3+ < yb3+="" />< sn4+="" />< />
d)Lu3+ < yb3+="" />< ce4+="" />< />

The correct order of ionic sizes is:

c) Lu3+ < yb3+="" />< sn4+="" />< />

This is because as we move across a period in the periodic table, the ionic size decreases due to an increase in effective nuclear charge. Among the given elements, Lu and Yb belong to the same period, but Lu has a greater nuclear charge than Yb, so Lu3+ has a smaller size than Yb3+. Sn4+ has a larger size than Yb3+ because it has a greater number of shells. Ce4+ has the largest size among the given ions due to its f-block contraction effect, which makes its size larger than expected. Therefore, the correct order is Lu3+ < yb3+="" />< sn4+="" />< ce4+.="" />
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Which is the correct order of ionic sizes (At. No. : Ce = 58, Sn = 50,...
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Which is the correct order of ionic sizes (At. No. : Ce = 58, Sn = 50, Yb = 70 and Lu = 71) [AIEEE-2002]a)Ce>Sn>Yb>Lub)Sn>Ce>Lu>Ybc)Lu>Yb>Sn>Ced)Sn>Yb>Ce>LuCorrect answer is option 'A'. Can you explain this answer?
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