The atomic radius of an element is defined as the distance from the nucleus to the outermost shell of electrons. This size is influenced by several factors, including the nuclear charge, the number of electron shells, and the shielding effect from inner electrons. It is typically measured in picometers (pm) or angstroms (Å).
Step 1: Define the Atomic Radius of Silver.
Silver (Ag) is a transition metal with an atomic number of 47. The electron configuration of silver is , meaning that silver has a filled -subshell and a single electron in its outermost -orbital. The atomic radius is influenced by: Metallic bonding: The metallic bonding in silver results in a relatively large atomic radius, as the electrons are delocalized. Shielding effect: The inner electrons in the core shield the outer electron from the full nuclear charge, allowing for a larger radius.
Step 2: Reference Values for Atomic Radius.
According to experimental data and periodic trends, the **atomic radius** of silver is:
Step 3: Comparison with Options.
When we compare this value to the given options:
- Option (1) matches the known value for the atomic radius of silver.
Conclusion:
Thus, the atomic radius of silver (Ag) is , which corresponds to option .