Question

choose the larger atom from each of the following pairs. match the symbols in the left column to the appropriate blanks in the sentences on the right. between i and kr, the larger atom is. between si and sn, the larger atom is. between s and sb, the larger atom is. between b and n, the larger atom is.

Explanation:

Step1: Analyze atomic radius trends

Atomic radius increases down a group (due to more electron shells) and decreases across a period (due to increased nuclear charge pulling electrons closer).

Step2: Compare I and Kr

Iodine (\(I\)) is in period 5, group 17. Krypton (\(Kr\)) is in period 4, group 18. Since \(I\) is in a lower period (more electron shells), \(I\) is larger.

Step3: Compare Si and Sn

Silicon (\(Si\)) is in period 3, group 14. Tin (\(Sn\)) is in period 5, group 14. As \(Sn\) is lower in the group (more electron shells), \(Sn\) is larger.

Step4: Compare S and Sb

Sulfur (\(S\)) is in period 3, group 16. Antimony (\(Sb\)) is in period 5, group 15. \(Sb\) has more electron shells (lower period), so \(Sb\) is larger.

Step5: Compare B and N

Boron (\(B\)) and Nitrogen (\(N\)) are in period 2. \(B\) is in group 13, \(N\) in group 15. Across a period, atomic radius decreases. So \(B\) (left - side) is larger.

Answer:

Between \(I\) and \(Kr\), the larger atom is \(I\).
Between \(Si\) and \(Sn\), the larger atom is \(Sn\).
Between \(S\) and \(Sb\), the larger atom is \(Sb\).
Between \(B\) and \(N\), the larger atom is \(B\).