The atomic radius, the distance from the nucleus to the outermost electron shell, is determined by nuclear charge, electron shell count, and inner electron shielding. It is commonly measured in picometers (pm) or angstroms (Å).
Step 1: Define Silver's Atomic Radius.Silver (Ag), a transition metal with atomic number 47, has the electron configuration \( [\text{Kr}] \, 4d^{10} \, 5s^1 \). This indicates a filled \( 4d \)-subshell and a single electron in its outermost \( 5s \)-orbital. Factors influencing its atomic radius include: Metallic bonding: Delocalized electrons in silver's metallic bonds contribute to a relatively large atomic radius. Shielding effect: Inner \( [\text{Kr}] \) electrons reduce the nuclear charge experienced by the outer electron, resulting in a larger radius.
Step 2: Reference Atomic Radius Values.Experimental data and periodic trends establish the atomic radius of silver as:\[\text{Atomic radius of Ag} = 144 \, \mathrm{pm}.\]
Step 3: Compare with Options.Comparing this value to the provided options:- Option (1) \( 144 \, \mathrm{pm} \) aligns with the established atomic radius of silver.
Conclusion:The atomic radius of silver (Ag) is \( \mathbf{144 \, \mathrm{pm}} \), matching option \( (1) \).