Multiple Choice
Based on the periodic table, which statement correctly compares mercury and tin?
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9. Electrons in Atoms and the Periodic Table
Periodic Trend: Atomic Radius (Simplified)
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Periodic Trend: Atomic Radius (Simplified) Which element has the greatest atomic radius?
A
F
B
Cl
C
Na
D
Cs
Verified step by step guidance1
Understand that atomic radius generally increases as you move down a group (column) in the periodic table because additional electron shells are added, making the atom larger.
Recognize that atomic radius generally decreases as you move from left to right across a period (row) due to increasing nuclear charge pulling electrons closer to the nucleus.
Identify the positions of the given elements: F (fluorine) is in period 2, group 17; Cl (chlorine) is in period 3, group 17; Na (sodium) is in period 3, group 1; Cs (cesium) is in period 6, group 1.
Compare the elements based on their group and period: since Cs is in the same group as Na but much lower down the periodic table, it has more electron shells and thus a larger atomic radius.
Conclude that among the listed elements, Cs has the greatest atomic radius because it is the furthest down the group, outweighing the effects of group and period trends.
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